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St. Mary’s College Science Department
Year 10 Science
St. Mary’s College Science Department
Year 10 Science
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M. Logue
St. Mary’s College Science Department
Year 10 Science
Pupil Name
Date
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St. Mary’s College Science Department
Year 10 Science
Welcome back to your third year at St. Mary’s College.
Hopefully you enjoyed your summer holidays and are ready to work hard
again this year. This is an important year for you because how you do will
help decide what GCSE science course you will follow next year. So it is
important to work hard and do your very best.
In 3 rd Year you will be learning about a variety of topics including
variation among humans, materials and their properties, the atom,
chemical reactions and forces and movement.
The full list of your topics is below…
September to Hallowe’en – Cells and Variation
Hallowe’en to Christmas – Force and Movement
January to Mid-term – Materials and Energy
Mid-term to Easter – Chemical Reactions
April/ May – The Atom
June – Numeracy in Science/ Careers
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St. Mary’s College Science Department
Year 10 Science
Topic 1 – Cells and Variation
In this topic you will be learning about the main organs in our bodies and
their functions (jobs).
You will then learn about variation (the differences between humans) and
how this happens.
First though you need to be very clear about the difference between
things which are alive, dead and non-living.
Look at the pictures below and decide which things are alive, dead and
non-living…
Basically things that are dead must have died so they must have been
alive at some point – for example the dead leaf. The robot was never alive
so we describe it as ‘non-living’
Living things must be able to do ‘living processes’. There are 7 living
processes which all living things should be able to do.
We remember them by using ‘MRS. GREN’
M – movement (moving from place to place or moving on one spot)
R – respiration (burning our food to get energy from it)
S – Sensing (being able to detect the world around)
G – Growing (getting more cells and getting bigger)
R – Reproducing (having babies or making seeds like plants)
E – Excretion (getting rid of waste - peeing and pooing)
N – Nutrition (eating or getting energy from food)
Homework 1
Learn the 7 living processes and what they mean
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St. Mary’s College Science Department
Year 10 Science
Next you will be learning about the main organs in human bodies.
Look at the locations of the main organs in the body below. You will need
to know these – and be able to identify them on an unlabelled diagram.
The table on the next page gives the jobs of the main organs in the body.
See if you can think of a rhyme to help you
remember the main organs of the body –
Brain, Lungs, Heart, Liver, Stomach, Small
Intestine, large Intestine, Bladder
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St. Mary’s College Science Department
Year 10 Science
Name of Organ
Brain
Job
Controls all other organs and emotions
Heart
Pumps blood to all parts of the body and all cells
Lungs
Take oxygen from the air and put it in the blood
Stomach
Digests food – breaks it into smaller pieces for absorption into the
blood‐stream
Liver
Removes toxins (poisons) from our body
Small Intestine
Absorbs nutrients from our food and into our bodies
Large Intestine
Absorbs water from our food and into our bodies
Homework 2
Learn the locations and jobs of the main organs of the body.
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St. Mary’s College Science Department
Year 10 Science
Next you are going to look a little closer at what makes up all our organs –
tiny cells
Every part of the body is made up of cells but these are too small to see
with just your eyes. You need a microscope in order to see cells. You are
going to use a microscope to look at the cells from an onion (which is a
living thing too).
First look at the parts of a microscope.
You will need to know the parts of the microscope for your Christmas
Exam.
You have no End of Unit Test for this topic.
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St. Mary’s College Science Department
Year 10 Science
Now you will prepare a slide of onion cells so you can use a microscope to
look at them.
Follow the method below…
Peel off a very thin layer of onion skin
Lay the onion skin on a glass slide (no creases or overlaps)
Add a few drops of iodine on top of the onion skin to dye it
Place a cover slip on top of the onion skin slide
Place on the microscope stage
Adjust microscope to see onion cells clearly
Hopefully you will see something that looks a little like the image below.
In this diagram you can see the
actual parts of each onion cell.
You will learn more about the
parts of cells later.
Onion cells under a microscope
Homework 3
Write a method for how you prepared and observed onion cells under a
microscope.
Extension Homework
The eye-piece lens in a microscope has a magnification of x10 and the
three objective lenses have magnifications of x10, x40 and x100.
What is the largest magnification you can get and what is the smallest
magnification you can get?
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St. Mary’s College Science Department
Year 10 Science
The last part of this short topic is to learn about the parts of cells and
their jobs.
Animal Cell
Plant Cell
The tables below show the jobs of the different parts of a cell.
Animal Cell
Name of part of
cell
Nucleus
Cell membrane
Cytoplasm
Job
Controls what the cell does
Controls what enters and leaves the cell
Jelly like substance which fills the cell, gives
the cell its shape and where chemical reactions
take place
Plant Cell
Name of part of
cell
Nucleus
Cell membrane
Cytoplasm
Cell Wall
Chloroplasts
Vacuole
Job
Controls what the cell does
Controls what enters and leaves the cell
Jelly like substance which fills the cell, gives
the cell its shape and where chemical reactions
take place
Gives the cell shape/structure and protection
Contain chlorophyll which absorbs sunlight to
allow the cell to do photosynthesis (make food)
Large empty space to store materials and
waste
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St. Mary’s College Science Department
Year 10 Science
Finally look at the diagrams of animal and plant cell beside each other and
notice the parts that are in both cells and the parts that are only found
in plant cells.
Living, nonliving
and dead
Homework 4
Living
processes –
MRS GREN
Using a
microscope to
look at onion
cells
Topic 4
‘Major Body
Organs’
Major organs
in the body
and their jobs
Cells – parts
of animal and
plant cells
Revise all the things you have
learned in this topic so far.
The mind map on the right will
help you focus on the right
areas to study.
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St. Mary’s College Science Department
Year 10 Science
Next you will be learning about variation.
To begin with, look carefully at your partner and list as many of their
physical attributes as you can (look for things that can be different
between you and your partner) – for example – eye colour, hair colour,
shape of nose, dimples, hair length etc.
Now do the same with the pictures of
the kittens below…
A B C
In particular you should list the
differences in the colour of fur,
the size of ears, the colour of
eyes etc.
D E F
Activity
If you have time the teacher might give you out sets of model animals.
In groups you should try to list their differences. This is good practice for
noticing differences between different animals and will also help you when you
have to do this for humans…
The differences between animals (whether they are the same species of
different species) is called ‘Variation’
Variation is the range of differences there are between different
animals and plants.
Among humans these differences might include …
eye colour, hair colour, shape of nose, dimples, arm length, height, weight,
scars, ear lobes and many other things.
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St. Mary’s College Science Department
Year 10 Science
Look at the butterflies below and identify all the different
characteristics
Now we will concentrate on the variation between humans for a while….
It is important first to note that there are two main reasons for the
variation between us all.
1. Our genes
2. The environment
The variation between us which is caused by our genes (which we get from
our biological parents) is called ‘Inherited’ variation.
The variation between us which is caused by the environment in which we
live is called ‘Environmental’ variation.
The table below gives some examples of each type of variation…
Examples of inherited
variation in humans
Eye colour
Hair colour (natural)
Ear lobe
Widow’s peak
Ability to roll your tongue
Examples of environmental
variation in humans
Scar
Accent
Language
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St. Mary’s College Science Department
Year 10 Science
Of course there are some examples of variation in humans which are
partly genetic but also affected by the environment – for example weight
and skin colour.
Homework 5
Copy out the list of features below and write I after those you think are
inherited and write E after those you think are environmental…
shape of nose neat hand writing freckles
hair colour hair length scars
skill at languages an accent eye colour being good at sport
blood group
size of feet
Extension Homework
1. What features do you think you have inherited from your…
a. Mother
b. Father
2. Fred and George Weasley (pictured below) are identical twins.
What features do you think they have inherited from their parents?
What features do you think are the result of their environment?
Fred
George
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St. Mary’s College Science Department
Year 10 Science
Activity
1. Copy out and complete…
We _________many features from our parents.
Other things like being able to ride a bike, we _________ during our
lifetime.
We say that they are due to the ____________.
2. Aine has just come back from two weeks holiday in Spain. Do you think
her sun-tan is inherited? Explain your answer.
3. Meabh says that being red-haired and being good at sport are both
inherited. Do you agree? Explain your answer.
Next you are going to learn about ‘continuous’ and ‘discontinuous’
variation…
Continuous Variation is any difference which has lots of different
possible values and which varies gradually.
Often forms of continuous variation can be measured and given a
numerical value.
Examples of continuous variation in humans would be height, weight, arm
length, length of foot etc. All of these have many, many possible values.
Discontinuous variation is any difference which is more clear cut such as
eye colour, hair colour,
blood group or can you roll
your tongue or not. With
discontinuous variation
there are normally a fairly
small number of different
possible values.
For example with eye colour
the possible values are
blue, brown, green (only a
few possibilities).
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St. Mary’s College Science Department
Year 10 Science
If we do a survey of heights in a class of girls we would probably get 25
different heights, all slightly different so a bar chart would have 25
different bars and wouldn’t be very useful.
Instead it is better to group the heights into categories so we can see
better the spread of different heights in the class including which is the
most common range. Look at the bar chart below for a class of pupils’
heights.
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St. Mary’s College Science Department
Year 10 Science
On the other hand if the data is for discontinuous variation such as which
blood group people are then you can simply draw a normal bar chart for
each of the possible values – in this case A, B, AB and O
Now you are going to use data for different forms of variation in your
class to draw bar charts.
First you need to collect the data…
Eye Colour
Blue
Brown
Green
Hazel
Grey
Number of pupils
Height Range Number of pupils
150 – 154 cm
155 – 159 cm
160 – 164 cm
165 – 169 cm
170 – 174 cm
Activity
Numeracy in Science
Now draw a bar chart for eye colour and a bar chart for heights of pupils in
your class. Good Luck!
Extension Activity
Numeracy in Science – Very difficult
Now collect another set of data about discontinuous variation in your class –
for example – can each girl roll her tongue or not or does each girl have a
large ear-lobe or not. Draw a pie chart to show this data.
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St. Mary’s College Science Department
Homework 6
Year 10 Science
Numeracy in Science
Some pupils did a survey on the size of the fruit from the foxglove plant.
Here are their results…
Length of
fruit (mm)
Number
collected
20 21 22 23 24 25 26 27 28 29
4 6 14 22 30 26 18 12 12 3
a. Draw a bar chart of their results.
b. What sort of variation does this bar chart show?
Activity
Numeracy in Science
Now that you have had some practice in displaying data about variation you will
display data for your class for the following types of variation…
Left handed or right handed
Shoe size
Length of index finger
Hair colour
First collect the data (the teacher might help with this), then display the data
in the most appropriate way – bar chart, pie chart etc.
Homework 7
Numeracy in Science
Continue and finish the bar charts / pie charts for the data you collected in
class.
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St. Mary’s College Science Department
Year 10 Science
Extension Homework
Numeracy in Science
Look at the bar chart below for the different heights in a class and answer the
questions which follow…
a. What is the most common height range in the class?
b. How many pupils are at least 150 cm tall?
c. What is the least common height range in the class?
d. How many pupils are in the range between 135 cm to 139 cm?
Next you are going to learn about why there is such variation between us.
First you should know that all the information about us is actually present
in every single cell of our bodies.
Earlier in the unit you learned about the parts of an animal cell. The
nucleus contains information about you – eye colour, blood group etc.
Basically the nucleus contains all the genetic information about all your
inherited characteristics.
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Year 10 Science
The diagram below shows the cell and also a close up of the nucleus and
the chromosomes inside it…
So the nucleus of every cell contains chromosomes
which, in turn, are made of genes.
You have 23 pairs of chromosomes and each pair
contains millions of genes.
Each pair of genes gives information about one of your characteristics –
for example – you have a pair of genes to determine your eye colour, a
different pair of genes determines whether or not you have large earlobes
etc.
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St. Mary’s College Science Department
Year 10 Science
The diagram below shows the 23 pairs of chromosomes that each human
has inside the nucleus of every cell.
So chromosomes are basically thread-like structures made up of lots of
individual genes which contain information about your features.
You get these from your biological parents. The instructions for a new
baby are found in two places – the egg cell of the mother and the sperm
cell of the father. In both cases the instructions are in the nucleus of
these cells.
Although all other cells contain 46 chromosomes in their nuclei, sperm
cells and egg cells only contain 23 each. This is because they will join
together during fertilisation to make the embryo that grows into a new
baby.
23
23 chromosomes
in an egg cell
46
46 chromosomes
in a fertilised
23
23 chromosomes
in a sperm cell
egg cell
Activity
Look at the image of chromosomes above and answer these questions…
1. Are all the chromosomes the same size and shape?
2. How many are there?
3. What do you think the x and y chromosomes are for?
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St. Mary’s College Science Department
Year 10 Science
Homework 8
1. Copy and complete…
Inside the nucleus of each cell there are thread-like structures called
_________. These are made up of _______. These ______ contain
instructions to control how the ____ works. They also contain information
which is _____ from one generation to the next.
2. How many chromosomes are there in a human sperm cell or egg cell?
How many are there inside other human cells?
Why do you think these numbers are different?
Extension Homework
Research what genes are, what they do and what they are made of. Write your
findings in a paragraph in your exercise book.
Find out what DNA stands for?
Next you are going to learn more
about genes and how your
characteristics are passed on to
you from your biological parents…
In the nucleus of each of your cells are 23 pairs of
chromosomes.
Each chromosome is made up of lots of sections called
genes.
Every gene holds one piece of information about you – for example – eye
colour might be on one gene, hair colour on a different gene, tonguerolling
ability on another gene.
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Remember though that you have 23 pairs of chromosomes.
This means that for every feature you actually have two genes – one
passed on to you from your mother and another one from your father.
So what happens if the eye colour gene from your mother gives different
information from the eye colour gene from your father?????
What do you think would happen if a blue eyed woman has a baby with a
brown eyed man?
Does their child have one blue eye and one brown eye?
The answer is No.
One of the genes has to ‘get its way’ and be dominant. This gene is called
the ‘dominant’ gene. The other gene (the one which doesn’t get its way) is
called the ‘recessive’ gene.
Let’s look at an example to make things more clear…
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Year 10 Science
Aobhe’s mum has blue eyes. Both of her mum genes for eye colour indicate
blue eyes. We use the symbol b (lower case letter b) for the blue eye gene.
Aobhe’s dad has brown eyes. One of his eye colour genes indicates brown
eyes (B for brown eye gene) and his other eye colour gene indicates blue eyes
(b).
Numeracy in Science
So why or how does Aobhe have blue eyes?
To answer this we need to look at the possibilities.
A punnet square can help us do this.
If Aobhe’s mum has blue eyes, then both her genes for eye colour must
indicate blue eyes (because the blue eye gene is recessive and if a brown eye
gene was present it would dominate and she would have brown eyes). So
Aobhe’s mum’s eye colour genes are b and b.
Aobhe’s dad has brown eyes but we know that he has a blue eye gene and a
brown eye gene so he has B and b.
We now use a punnet square to look at the possibilities for their children…
Dad
B
b
b
Bb
bb
Mum
b
Bb
bb
So if you look at each section
within the punnet square, you can
see the 4 different possibilities
for combinations of genes from
mum and dad. Bb means that the
brown gene will dominate and that
child will have brown eyes but bb
means that the child has two blue
eye genes and so will have blue
eyes.
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St. Mary’s College Science Department
Year 10 Science
Now look at another example…
Orlaith has dyed her hair orange for a Hallowe’en party. You have to try to
figure out what colour(s) her hair could have been originally.
Orlaith’s mum has two genes for hair colour – one of these is a gene to
indicate red hair and this gene is recessive. We give it the symbol b.
Her mum’s other gene for hair colour indicates brown hair and has the
symbol B.
Orlaith’s dad also has two different genes for hair colour – b and B.
(These different types of gene are called ’alleles’).
We can use a punnett square to figure out the different possibilities for
Orlaith’s original hair colour.
Like in the previous example look at
each section within the punnet
Dad
Mum
square, you can see the 4 different
B
b
possibilities for combinations of
genes from mum and dad. BB means
B
that the child would have 2 Brown
BB Bb
hair genes and so would have brown
hair. Bb means that the brown hair
b Bb
bb gene will dominate over the red hair
gene and that child will also have
brown hair but bb means that the
child has two red hair genes and so
will have red hair.
The different types of genes for a feature are called ‘alleles’.
The combination of the two alleles is called your Genotype – for example Bb
or bb.
The actual feature you have – for example – brown hair or blue eyes is called
your Phenotype.
Homozygous means the two alleles are the same type – eg. bb or BB
Heterozygous means the two alleles are different – eg. Bb
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St. Mary’s College Science Department
Year 10 Science
Homework 9
1. The Black fur gene (B) in guinea pigs is dominant over the white fur gene
(b). Complete a punnett square to find out the chances of the baby
guinea pigs have black fur and white fur when the parents have the
genes BB and Bb.
2. The tongue rolling gene (T) is dominant over the non-tongue rolling gene
(t). If Nicola’s mum has the genes Tt and her dad has the genes tt what
is the chance of Nicola …
a. Being able to roll her tongue
b. Not being able to roll her tongue
3. In purple people eaters, one-horn is dominant and no horns is recessive.
Draw a Punnet Square showing the cross of a purple people eater that is
hybrid for horns (2 different types of gene) with a purple people eater
that does not have horns.
Extension Homework
1. Black fur (B) in guinea pigs is dominant over white fur (b). Find the
probability of a baby guinea pig having white fur if one of its parents is
homozygous white fur and the other is heterozygous black fur.
2. Now find the probability of a baby guinea pig having white fur if both its
parents are homozygous white fur.
3. Let's say that in seals, the gene for the length of the whiskers has two
alleles. The dominant allele (W) codes long whiskers & the recessive
allele (w) codes for short whiskers.
a) What percentage of offspring would be expected to have short
whiskers from the cross of two long-whiskered seals, one that is
homozygous dominant and one that is heterozygous?
b)
b) If one parent seal is pure long-whiskered and the other is shortwhiskered,
what percent of offspring would have short whiskers?
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St. Mary’s College Science Department
Year 10 Science
Activity
Now you can use the knowledge you have gained about using punnett squares to
try this task…
Your task is to discover the identity of Georges’ parents.
First, however, a few necessary pieces of information for you to complete your
task…
You will be completing punnett squares on three characteristics: number of eyes,
fur colour, and number of horns.
Three eyes are dominant (E), and two eyes are recessive (e).
Blue fur is dominant (F), and purple fur is recessive (f).
Two horns are dominant (H), and one horn is recessive (h).
Georges’ characteristics are: blue fur, three eyes, and one horn.
Below you will find the names of each of the families, the characteristics of each
of the parents, and blank punnett squares to copy into your exercise books and
then fill in.
Good Luck!
Possible Family Number 1: The Venetians
• The mother is Ee, ff, and Hh.
• The father is ee, ff, and Hh.
Eyes Fur Horns
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St. Mary’s College Science Department
Year 10 Science
Possible Family Number 2: The Neptunes
• The mother is ee, Ff, and hh.
• The father is EE, Ff, and Hh.
Eyes Fur Horns
Topic 2 – Force Possible and Movement Family Number 3: The Plutonians
1) The mother is Ee, ff, and Hh.
Topic
• The
3
father
Materials
is Ee,
and
FF,
Energy
and HH.
Eyes Fur Horns
Topic 4 – Chemical Reactions
Topic 5 – The Atom
Only one of these families could possibly be
Georges’ true parents.
Which family is it?
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Year 10 Science
Extension Questions…
1. In cats, long hair (L) is dominant over short hair (l).
Complete a punnett square to show a cross between two short-haired
cats.
What is the probability that the parents will produce a short-haired
kitten?
2. For Flower colour in roses Purple is dominant (P) and White is
recessive (p)
Draw and fill in a punnett square to show the different possibilities for
the offspring of a PP father and a PP mother.
What colour(s) are the parents?
What colour(s) are the children?
3. For dimples in humans the Dimples gene is dominant (D) and the Nodimples
gene is recessive.
Draw and complete a punnett square to show the probabilities for the
children of parents where the mum has no dimples and the dad is
heterozygous for dimples.
Homework 10
1. In Noombats, yellow bellies (Y) are dominant over green bellies (y).
a. Complete a punnett square to show a cross between a purebred yellow
bellied noombat and a noombat that is a hybrid for belly colour.
b. What is the probability that the parents will have yellow bellied
offspring?
c. Is it possible for two yellow bellied noombats to have a green bellied
child?
d. Can the yellow bellied parents produce a green bellied child?
e. If yes, explain how and identify what the probability would be.
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St. Mary’s College Science Department
Year 10 Science
Activity
1. For Fur colour in Amazon caterpillars Yellow is dominant (Y) and Green
is recessive (y)
Draw a punnett square to show the different probabilities for the
offspring of a yy father and a YY mother
What colour(s) are the parents?
What colour(s) are the children?
2. For Eye colour in Wombats Green is dominant (G) andYellow is
recessive (g)
Draw and complete a punnett square to show the different
possibilities for the offspring of a Gg father and a GG mother
What color(s) are the parents?
What color(s) are the children?
3. In snapdragon plants red flowers are dominant and white flowers are
recessive.
Draw a punnett square to show the probabilities for the offspring of
two heterozygous parent plants.
Homework 11
1. In pea plants the allele for round seeds (R) is dominant and the allele
for oval seeds (r) is recessive. Complete punnett squares for a cross
between two pea plants with round seeds (homozygous and
heterozygous).
What is the percentage probability of the offspring having round
seeds? Oval seeds?
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St. Mary’s College Science Department
Year 10 Science
Next you are going to learn about how scientists classify living things…
First of all can you answer this…
What do the ox-eye daisy, the dog daisy and the marguerite have in
common?
The answer is… that they are all the
exact same plant!
The name of this plant is different
in different areas.
Can you imagine how this could be
confusing.
very
Imagine if dogs were known by a different name in other places – how
confusing would that be?
Luckily scientists do not normally use the ‘common’ names for living
things.
Instead they use a special system of naming called the ‘binomial system’.
This system gives everything 2 names – the first is called its ‘genus’ and
the second name is called its ‘species’.
Let’s look at an example… how we classify the brown bear…
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St. Mary’s College Science Department
Year 10 Science
This diagram shows the
complete classification
of the brown bear –
from the Kingdom of
animals right down to
its genus and species.
Normally we only state
the genus and species
when naming a living
thing as this is enough
to be clear and avoid
confusion.
This time we are
classifying the leopard.
It is in the animal
Kingdom, its phylum is
Vertebrate or Chordata,
it is a mammal, a
carnivore, a member of
the cat family.
Then finally its genus is
Panthera and it species is
Panthera Pardus.
It is known by scientists
as Panthera Pardus.
Living things are classified because of their shared features.
The more shared features they have the more classes they share.
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St. Mary’s College Science Department
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If you have time your teacher might allow you to play a naming game for
animals…
Playing in pairs one girl holds the cards and looks at each one in turn. Her
partner asks questions about the animal on the card and the only allowed
answers are Yes and No.
Homework 12
Use the internet to carry out research to find out the correct scientific
names for the following animals…
Giraffe, chimpanzee, great white shark, bottle-nose dolphin, ostrich
The next thing you need to learn about is ‘vertebrates’ and ‘invertebrates’
A ‘vertebrate’ is any animal which has a backbone (or an internal
skeleton).
Vertebrates can be split into 5 main categories which can be remembered
by using the name Mr. Fab
Mammals
Reptiles
Mammals
Fish
Reptiles
Fish
Amphibians
Birds
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Here is a summary of the main features of each of
the groups of vertebrate…
Mammals… have fur, feed their young on milk and give
birth to live young (not eggs)
Reptiles… have dry scaly skin, are cold blooded and lay
eggs with hard shells
Fish… have scales and breathe through gills
Amphibians…live on land but lays eggs with soft shells
in water
Birds…have feathers and lay eggs with hard shells
Homework 13
Choose one reptile, fish, amphibian and bird and write a biography of each
using the guidance in the homework above.
Careers in Science
Clinical Geneticist
A clinical geneticist is a type of doctor who specialises in diagnosing and
treating patients with inherited health problems such as Alzheimer’s
Disease, Cystic Fibrosis or Sickle Cell Disease.
A geneticist has to do a degree in Biological Science or Physical Science and
it normally takes about 8 years to be fully qualified.
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Year 10 Science
Literacy in Science
Here is a list of the key words from this topic along with their meanings…
Cell – the small structures of which all living things are made
Nucleus – the part in the middle of a cell which controls the function of the
cell
Chromosome – the string-like structures in the nucleus made up of genes
Gene – the structures in chromosomes made of DNA which contain our
genetic information
Variation – the range of difference between living things
Inherited – passed on from your biological parents
Environmental – obtained through your environment
Continuous – type of variation with lots of possible values (measurable)
Discontinuous – type of variation with only a discreet number of values
Vertebrate – an animal which has a backbone
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Year 10 Science
Topic 2: Forces and Movement
The distance between Derry and Belfast is roughly 115 Kilometres.
But the displacement between Derry and Belfast is 115 Kilometres South-
East.
Basically Displacement is just Distance is a specific direction.
The direction of a displacement is represented by the direction of an
arrow and the length of the arrow represents the distance.
For example:
represents a displacement of 5 Km East
and
represents a displacement of 10 Km West
because the arrow is twice as long and the opposite direction.
Derry
Belfast
The arrow represents a distance of 115 Km
but because it is a specific direction (South-
East), it is called a displacement of 115 Km
South-East.
If you travelled from Derry to Belfast and
back again, the distance is 230 Km but the
displacement is O Km (because you have not
moved in any direction from your starting
point.
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The average Speed of a car can be calculated by using the equation:
Av. Speed = Distance moved
Time Taken
If we measure the distance in metres and measure the time in seconds,
then the units for the Speed are metres per second or m/s for short.
For example:
A car travels from Derry to Belfast (a distance of 115 Km) and it takes 2
hours.
The average Speed is…
115 km
= 57.5km/h
2 hours
Remember: this is just the average speed and the speedometer in the car
would not read 57.5 Km/h all the time during the journey. The car might
slow down or stop at times and might travel even faster at other times.
If we want to know the actual speed at a certain moment we would need
to do the same calculation but do it over a very short distance and time –
say 50 metres over 2 seconds.
0 seconds
2 seconds
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50m
St. Mary’s College Science Department
Year 10 Science
So Speed is the distance travelled in a certain time.
Velocity is the distance travelled in a certain time and in a specific
direction.
In other words, Velocity is the displacement in a certain time.
Displacement (distance
in a specific direction)
Av.Velocity =
Time Taken
(Average speed
in a specific direction)
30 m/s 30 m/s
The red car has the same speed as the green car but it has a different
velocity – because it has a different direction.
Speed is called a scalar quantity because it only has size but Velocity is
called a vector quantity because it has size and direction.
The red car in the picture is
going round the round-about.
Its direction is constantly
changing so its velocity is
changing even though it travels
at the same speed the whole
time.
Velocity depends on the
direction as well as the size of
the speed.
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St. Mary’s College Science Department
Year 10 Science
Now try these questions…
1. A car travels 800 metres in 40 seconds.
a. What is its average speed?
b. Why is its actual speed probably different from its average speed?
2. A car has a steady speed of 10 m/s.
a. How far does it travel in 9 seconds?
b. How long would it take this car to travel 220 metres?
3. Calculate the average speed of these objects…
a. A runner who travels 400 metres in 45 seconds
b. A car which travels 175 miles in 3 hours
c. A Space shuttle which travels 45,750 Km in 2.5 hours
d. A snail which slithers 2 metres in 4 hours
4. A train sets off from Derry at 9am in the morning. It reaches Belfast
which is 150 Km away at 12pm (midday). What is the average speed of
the train?
5. Usain Bolt runs 100m in 10 seconds. David Rudisha runs 800m in 110
seconds. Who has the faster average speed? Who do you think would
win a race over 400 metres? Why?
Homework 1
1. A train has an average speed of 45 Km/h over a three-hour journey.
How far is the journey?
2. A woman in Derry has three hours to make it to an appointment in
Dublin. She gets the bus which travels at an average speed of 60 Km/h.
The distance from Derry to Dublin is 225 Km. Will she make it to her
appointment on time?
Extension Homework
Explain the difference between Distance and Displacement and the
difference between Speed and Velocity?
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St. Mary’s College Science Department
Year 10 Science
Acceleration
When the velocity of an object changes, we say that the object is
accelerating (even if it is only the direction of its travel that changes and
not the actual speed).
Change in Velocity
Acceleration =
Time Taken to change
Acceleration is a vector quantity which means that it has direction as well
as size.
For example:
A car travels from rest (its velocity at the start is 0 m/s) and
accelerates until it is travelling at 5 m/s. It takes the car 2 seconds to do
this. What is its acceleration?
Change in Velocity
Using the equation
Notice the units
of acceleration
are m/s/s or
m/s 2
Acceleration =
Time Taken to change
5 –0 m/s 5m/s
Acceleration = 2s = 2s
Acceleration =
2.5 m/s/s
Another way of writing the equation for acceleration is to write the ‘change in velocity’ as the
final velocity minus the initial velocity.
The equation then looks like this…
v - u
where v = final velocity
Acceleration = t u = initial velocity
and
t = time taken for velocity to change 39
St. Mary’s College Science Department
Year 10 Science
Now try these questions…
1. A train has an acceleration of 3 m/s/s. What does this tell you about its
velocity?
2. A bus has a deceleration of 2 m/s/s. What does this tell you about the
velocity of the bus?
3. A car takes 8 seconds to increase its velocity from 3 m/s to 30 m/s.
What is its acceleration?
4. A motorbike, travelling at 25 m/s takes 5 seconds to come to a halt.
What is its deceleration?
5. An aeroplane has an acceleration of 4 m/s/s. What is its velocity after 5
seconds if it starts from rest?
Homework 2
1. A car starts at a speed of 20 m/s and accelerates up to a speed of 30
m/s. It takes 5 seconds to do this. What is its acceleration?
2. A bus which is travelling at a speed of 25 m/s makes an emergency stop
and comes to a halt in 3 seconds. What is its deceleration?
Extension Homework
1. Carry out research on how the following things help protect you in the
event of a car crash…
a. A seatbelt
b. An air-bag
In particular find out how these things affect the deceleration of the
driver or passenger.
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St. Mary’s College Science Department
Year 10 Science
Now try this activity…
Using a run-way investigate how the slope of the run-way affects the speed
of the trolley which rolls down it.
Method…
1. Set up the run-way on the floor
with one book (from a set of
textbooks) under one end of
the run-way.
2. Hold the trolley at the higher
end and let go.
3. Using a stop-watch time how
long it takes the trolley to
reach the bottom of the run-way.
4. Repeat this process but each time with another extra book under the
end of the run-way.
5. Record all results in a table like the one below…
Number of books under end
of run-way
Time for trolley to reach
bottom of run-way
Homework 3
Write a title, equipment list, method, results table and conclusion for the
experiment you did in class.
Extension Homework
Describe how you could calculate the average speed of the trolley as it
moved down the run-way each time. Do this and add another column to your
results table for Average Speed.
Do you think it went at a constant speed the whole way down? Why/Why not?
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St. Mary’s College Science Department
Year 10 Science
Motion Graphs
We can draw simple graphs of Distance travelled during a certain time.
Different shapes of line on the graph tell us different things about the
movement of the object.
Distance
Distance
Moving with a
steady speed
Not moving
Time
Time
We can also draw graphs of Speed during a certain time.
Speed
Speed
Moving at a steady speed
Accelerating
Time
Time
Notice that a horizontal line means something different depending on if it is a
Distance –Time graph or a Speed –Time graph.
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Practice: Look at the following Distance-Time graphs and for each one describe
the motion of the vehicle from the start until the end of the journey:
A
B
C
D
E
F
A Speed –Time graph can be made up of different types of movement
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Year 10 Science
For example: A car starts from rest, accelerates for a while, then goes at a
steady speed for a while and finally slows down to rest again. The graph of its
movement will look like the one below.
Speed
Accelerating
Moving at a
steady
Slowing down
Time
When you have got a Speed – Time Graph the steepness (gradient) of the line
can tell you the acceleration.
Look at the Speed – Time graph below.
25 m/s
0 m/s
50 150 secs
Time
The speed has increased from 0 m/s up to 25 m/s during the first 50 seconds.
The acceleration can be worked out from the change of speed and the time
needed to change the speed.
The distance travelled can also be found from a Speed-Time graph.
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Year 10 Science
The distance is equal to the area under the graph.
To calculate the area you might have to split it into sections like the three
coloured sections below.
25 m/s
0 m/s
50 150 secs
200 secs
So in the graph above the distance travelled is the area under the graph…
Area of purple triangle = ½ base x perpendicular height
= ½ x 50 x 25
= 625 m
The add the area of the green rectangle = length x breadth
= 100 x 25
= 2500 m
The add the area of the orange triangle =
½ base x perpendicular height
= ½ x 50 x 25
= 625 m
Finally add all three together to get the total area = 3750 m or 3.75 Km
So the distance travelled was 3.75 Km.
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St. Mary’s College Science Department
Year 10 Science
Homework 4
Look at the graph below showing the motion of a car and answer the
questions…
Speed (m/s)
50 m/s
0 m/s
150
50 100 Time (s)
a. Describe what is happening during the first 50 seconds of the journey.
b. Describe what is happening from 50 seconds until 100 seconds.
c. Describe what is happening from 100 seconds until 150 seconds.
d. What is the acceleration during the first 50 seconds?
e. What is maximum speed of the car?
f. What is the deceleration of the car during the last 50 seconds?
g. How far does the car travel during the first 50 seconds of its journey?
Now have a look at these Distance-Time graphs. For each one describe the
h. What is the total distance travelled by the car?
Now look at this Speed-Time graph and answer the questions…
Extension Homework
Distance (m)
a. Describe the motion of
the car in the first 8
seconds?
18
b. How long is the
journey?
c. Describe the motion of
0
8
20
Time (s)
the car from 8 seconds
until 20 seconds.
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St. Mary’s College Science Department
Year 10 Science
A
a. What is the speed of the
car in the first 3 seconds
of its journey?
b. What happens between 3
and 5 seconds?
c. What is the acceleration
between 3 and 5 seconds?
d. What is happening between
5 and 8 seconds?
e. What is the total distance
travelled by the car?
Now look at the next Speed-Time graph and again answer the questions that
follow…
a. What is maximum speed the car reaches during its journey?
b. How long does the journey last?
c. What is happening in the first 10 seconds?
d. What is the deceleration of the car?
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Year 10 Science
Homework 5
Describe in a paragraph the journey of the car shown by the Distance-Time
graph below…
Extension Homework
Describe in a paragraph the
journey of the car shown by
Velocity-Time graph to the right.
the
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Extension Activity
Choose one of the situations described below and draw a Speed-Time graph
to show what is happening…
Then use the graph to find out the total distance travelled and the
acceleration during the different parts of the journey.
a. A bus accelerates from rest (starting speed = 0) up to a speed of 25
m/s in a time of 10 seconds. It then ravels at this steady speed for 50
seconds before slowing down to a stop in the next 20 seconds.
OR
b. A cyclist starts form rest (initial speed = 0) and accelerates to a
speed of 5 m/s in 10 seconds. She then travels at this speed for 10
seconds before accelerating again up to a speed of 15 m/s. She travels
at 15 m/s for 30 seconds before coming to a halt suddenly in 2
seconds.
OR
c. A car is travelling at a steady speed of 40 m/s for 20 seconds and
then slows down to a speed of 30 m/s in a time of 25 seconds as it
enters a town. Finally the car slows down again to a halt in a time of 15
seconds.
OR
d. A woman starts running from a rest position and reaches a speed of 4
m/s in a time of 5 seconds. She then runs at this speed for 50 seconds
before accelerating again up to a speed of 8 m/s in a time of 5
seconds. She runs at this speed for a further 45 seconds before
coming to a stop in a time of 5 seconds.
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Year 10 Science
Friction
You studied Friction in Year 9 so hopefully that will help you with this work.
A car is made to move forward by the force of the engine. But there is also the
force of the air hitting it as it moves. This is called ‘Air resistance’ or ‘Drag’
When the car is accelerating, then the force of the engine must be bigger than
Drag.
When the car is going at a steady speed, then Engine force and Drag must be
equal.
Diagram A
Forward Force of
Engine
Backward Force of
Drag
Diagram B
Forces Balanced =
car travelling at
steady speed
Forward Force of
Engine
Backward Force of
Drag
Forward force of
engine bigger = car
accelerating
There also has to be a force of ‘Friction’ between the tyres of the car and the
ground to allow the car to ‘grip’ the road for steering around corners and for
braking.
Note: The amount of drag on a car or any moving object depends on its surface
area and shape – rockets and jets are ‘streamlined’ with a smoother shape to
reduce the amount of air hitting them so to reduce Drag.
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Homework 6
Copy and complete the table below in your exercise book…
Times when Friction is a
nuisance
Times when Friction is useful
Extension Homework
Use your knowledge of friction to answer the following questions…
(Write out the full sentences in your exercise book)
1. A car driver has to be more careful when driving in winter when it is
icy because the road is more slippery than in summer. This is because
the friction on the road in winter is more than/ less than the
friction in summer.
2. A carpenter finds maple wood easier to cut than oak. This is because
there is… less friction between the maple and the saw / more
friction between the maple and the saw.
3. When a woman pushes a trolley on the tiles it moves more easily than
it does when she pushes it on the carpet. This is because there is
more friction / less friction between the tiles and the trolley.
Do you remember…
There are several ways of reducing friction – for example - lubricating,
stream-lining.
You could research these for more information.
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Year 10 Science
Mass and Weight
Lots of people say ‘weight’ when they should say ‘mass’ and vice-versa.
For example – people say they want to lose ‘weight’ but really they want to lose
‘mass’.
Mass is the amount of matter (stuff) in an object. It is measured in Kilograms
(Kg).
Mass it a scalar quantity – it has no direction!
Every object has a mass and, as you learned earlier in this unit, masses don’t
move unless a resultant force makes them accelerate. In other words objects
are sort of lazy – this is called ‘inertia’ which means ‘laziness’!
Weight is a force – it is the force of the gravity on an object.
So on earth your weight is the size of the earth’s gravity on your mass.
Our earth’s gravity has a force of 10N on every Kg of mass of an object so we
say the earth’s gravity is 10N/Kg.
Notice how
The equation for weight is…
this equation
is like the
Weight = Mass x gravity (acceleration due to gravity)
equation for
(N) (Kg) (m/s/s)
Force, mass
and
acceleration
– so Weight
is a force!
Mass
Size only, no direction
Measured in Kilograms
Never changes
Weight
Size and direction
Measured in Newtons
Changes form planet to planet
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Example:
What is the weight of a man whose mass is 70Kg when he is on the earth
(earth’s gravity = 10N/Kg) and when he is on the moon (moon’s gravity =
1.6N/Kg).
Weight = Mass x acceleration (due to gravity)
So on earth gravity = 10N/Kg
so the man’s weight is
The moon’s gravity is 1.6N/Kg so the
man’s weight is
= 70 x 10 = 70 x 1.6
= 700N = 112N
Now try these questions before you continue…
1) Aoife says her weight is 35 Kg. What is wrong with this statement
and what is her weight really?
2) Explain why a parachute slows down a falling parachutist.
Homework 7
Copy and complete the table below…
Mass of object (Kg) Acceleration due to Weight of object (N)
gravity (N/Kg)
75 10
200 500
140 9.8
27 2700
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Year 10 Science
Forces
Forces are vector quantities – that means that forces have a size and also a
direction. Forces are measured in Newtons (N)
The size of a force is shown by the length of an arrow and its direction is shown
by the direction of the arrow.
Large force to the right
Small force
upwards
Normally objects have more than one force on them and some of the time the
forces on them are balanced.
So none of the objects in these diagrams move or accelerate.
If there are no forces on an object or if the forces on the object are balanced,
then the object will stay as is – either it will stay still as in the diagrams above
or it will continue to move at the same speed like the car below. This is Newton’s
First law!
An object stays at rest or continues to move in a straight line with a constant
speed (uniform velocity) unless an unbalanced force makes it behave
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differently.
St. Mary’s College Science Department
Year 10 Science
This car is travelling at a steady
speed because the forces on it
are balanced.
But what happens if there are two or more forces acting on an object and these
forces are not balanced?
Forward Force of
Engine
Forward force of
engine bigger = car
accelerating
Backward Force of
Drag
The force of the engine is bigger than the force of drag so the car is
accelerating.
When objects are moving, the force of friction (the object rubbing against the
surface it is moving on) always slows down the movement and eventually stops it
altogether.
So friction always opposes (works against) movement).
So we know now that objects do not accelerate (speed up or slow down) on their
own.
They only change their speed if some sort of Force makes them.
Forces cause things to accelerate.
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This is also described in the equation for force, mass and acceleration.
Force = Mass of object x acceleration of object
Or
This
equation is
known as
newton’s 2 nd
Law.
F = m a
Example 1:
What is the force needed to make a train with a mass of 250,000 Kg
accelerate with an acceleration of 0.5 m/s/s?
F = m x a
F = 250,000 x 0.5
F = 125,000 Newtons
So the force needed to
make the train
accelerate at 0.5 m/s/s
is 125,000 Newtons.
Of course a smaller
force could still make
the train move but at a
smaller acceleration
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Example 2:
The mass of the rock is 500 Kg.
The acceleration of the rock is 2
m/s/s.
So the force the girl must be
putting on the rock = mass x
acceleration.
The mass of this rock is only 200
Kg.
The acceleration is still 2 m/s/s.
So this time the girl only needs a
force of 200 x 2 = 400 N.
If the girl wanted to make the rock have a bigger acceleration, she would have
to push it with a bigger force.
If she wanted to give a bigger rock the same acceleration, she would also need a
bigger force.
It is important that we always use the overall resultant force when using the
force, mass, acceleration equation.
Look at the example below.
Forward Force of
Engine = 10,000N
Forward force of
engine bigger = car
accelerating
Backward Force of
Drag = 6000N
A car has a mass of 1000Kg.
What is its acceleration if the force of the engine is 10,000N and the force of air resistance
(drag) is 6000N?
The overall resultant force on the car is 10,000 – 6000 N = 4000N
So we use this resultant force in our equation.
F = m x a
4000 = 1000 x a s
so the acceleration = 4000 ÷ 1000 = 4 m/s/s
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Now try this question…
A bicycle and rider have a total mass of 90Kg and travel along a flat road at a steady speed.
The forward force exerted by the cyclist is 40N.
a) Explain why the cyclist is not accelerating.
b) If the rider increases the forward force to 70N, what is her acceleration?
Summary of balanced and unbalanced forces
Balanced forces have no effect on the movement of an object. If it is still it
will stay still; if it is moving it will continue moving at the same speed and in
the same direction.
Unbalanced forces do affect the movement of an object – unbalanced forces
can cause the object’s velocity to change – it accelerates. The bigger the
resultant force the bigger the acceleration.
The bigger the mass of an object the bigger the force needed to make it
accelerate.
Homework 8
1. A train has a forward force of 200,000N and the mass of the train
is 4000Kg. What is its acceleration?
2. A car’s engine has a driving force of 8,000N and the mass of the
car is 1000Kg. What is its acceleration?
Extension Homework
1. A train is being pushed forward with an engine force of 100,000N. If
the force of air resistance is 20,000N, what is the resultant force on
the train? If the train has a mass of 8000Kg what is the acceleration
of the train?
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Work
Work is done when a force causes something to move.
If you stand and push against a wall it will make you tired but you have not done
any work because there has been no movement.
Or it you hold a pile of books you have not done work unless you have moved
them.
The amount of Work done can be calculated by using this simple formula:
Work Done = Force used x Distance moved in the direction of
force
(Joules) (Newtons) (metres)
This can be shortened to…
W = F x d
You might notice that the unit for ‘Work Done’ is the same unit as for ‘Energy’ –
Joules.
When you do work (use a force to move something) you use up energy.
The more work you do, the more energy you use.
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Look at this example…
How much work is done when a heavy box is dragged 4 metres across the floor
against a frictional force of 45 Newtons.
How much energy is needed to do this work?
4 metres
45 Newtons (friction)
Forward force pulling the
Now look at this question…
A crane does 1200 Joules of useful work when it lifts a load straight up (vertically)
by 60cm.
How heavy is the weight?
Remember… Work Done = Force x Distance moved in the direction of
force
Remember we need to use
metres so we have to
change the 60cm into
metres)
Therefore…
1200 Joules = Force (Weight of load) x 0.6 metres
So if we rearrange the equation…
Force = Work Done ÷ Distance
Force = 1200 ÷ 0.6
Force = 2000 Newtons
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Now try this question…
1. How much work is done by an electric motor pulling a 130 Newton load 6.5
metres up the slope if the tension in the string is 60 Newtons.
Tension in string = 60 N
Electric Motor
Energy and Work are closely related. Energy can be described as the ‘ability to
do work’
So if a machine has 500 Joules of stored energy, this means that it can do 500
Joules of work. Energy and Work are both measured in Joules (J)
You can carry out an experiment to measure the work you do when you walk up
the stairs. Copy and complete the table for your results…
Measurements
Mass of pupil in Kilograms
Weight of pupil in Newtons
(Weight = mass x 10)
Height of each stair
Number of stairs in staircase
Total height of staircase
Calculations
Work Done (=Force x Distance)
or
Work Done = Weight x total height of
staircase
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Homework 9
1. The force from the engine of a car is 25,000N and the car
travels 20,000m. What is the work done?
(Remember to use the equation for Work Done)
2. A crane lifts a load of 10,000N up to a height of 40m. What is
the Work Done?
3. A girl goes up a flight of stairs which is 3m high with her
schoolbag. Her weight is 400N and her schoolbag weighs 25N.
How much work has she done in walking up the stairs?
Extension Homework
1. A man lifts 100 crates of apples from the ground floor up a flight
of 12 stairs.
Each crate has a mass of 25 Kg and each stair is 15 cm high.
How much work has the man done?
Literacy in Science
Here is a list of the key words from this topic along with their meanings…
Displacement – the distance travelled in a specific direction
Velocity – the speed in a specific direction
Acceleration – how quickly an object is changing its speed
Friction – a force between surfaces which always opposes motion
Mass – a measure of the amount of matter (stuff) in an object
Weight – the mass of an object multiplied by the force of gravity
Work – a measure of the amount of energy used to d move an object
(found by multiplying the force needed by the distance the object is
moved)
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Careers in Science
If you study Physics
at A-level and then
at university you
could go on to
become a flight
engineers in the
aerospace industry.
This would involve
figuring out how to
make planes fly more
efficiently and
One job that is connected with the science of force and motion is in the
faster.
aerospace industry. Aerospace engineers help design planes to make
them more efficient and able to fly faster and with less fuel. They need
to know about friction and streamlining as well as balanced forces and
gravity. Salaries for this type of work vary but can reach well over
£60,000 Another per job year. that
you could do that is
connected with
forces and
movement is Sports
Coach.
A coach needs to be
able to calculate
speed and
acceleration and
work out how the
Many athlete sports can be coaches more also need to understand friction and streamlining
in efficient order to and help their athletes run, swim or cycle faster. In fact many
coaches streamlined study . a subject called Sport Science – the science of sport!
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Topic 3: Materials and Energy
Nothing happens or works without ‘Energy’.
You need to be very clear about the difference between ‘forms of energy’ and
‘sources of energy’
‘Forms of energy’ are the different ways which energy can appear – for example
– light energy, heat energy etc.
‘Sources of energy’ are the different places and things that give us energy – for
example – coal, oil, wind and solar.
The table below summarises the main ‘forms of energy’
Form of Energy What is it? Examples of resources (or uses)
Light
Heat
The energy coming out of a
glowing object
The energy coming out of a hot
object
Sun, Stars
Sun, Stars
Sound The energy of particles vibrating Any sound or noise
Movement
(Kinetic) (KE)
Electrical
The energy of any moving object
The energy of moving electrons in
a circuit
Wind, Waves, Tides
None – we have to make it from
other forms of energy
Stored Chemical
Gravitational
Potential
(GPE)
Elastic potential
The energy stored in a substance
that is then released when the
substance is burned
The energy an object has if it is
high above the ground
(because gravity will pull it
downwards and it will then move)
The energy in a stretched spring
or elastic band that then makes it
move when you let it go
Coal, Oil, natural gas, peat (turf)
wood, food, battery
Stored energy in the water in a
dam or reservoir (Hydroelectric)
Clockwork toy, wind-up watch
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This next law is possibly the most important law in all Science. It is called the
‘Law of Conservation of Energy’
Energy cannot be created or destroyed, but it be changed from
one form into a different form / different forms.
Energy Changes can be shown in a diagram called an ‘Energy Transfer Diagram’
Here are some examples…
Chemical
Energy
Kinetic Energy
when she
stretches the
elastic cord
Useful Elastic / Strain
Potential
Energy in the stretched
elastic cord
Stored Chemical
Energy
Useful Heat
Energy coming out
of the lit match
inside the chemicals
in
the head of the
match
Wasted Light
Energy coming out
of the lit match
Stored
Chemical
Energy in
the battery
Kinetic
Energy in
the Moving
hammer
Useful Sound
Energy from the
gong
Stored
Chemical
Energy in the
gas
Useful Heat Energy
coming out of the
Bunsen Burner
Useful Light Energy
coming out of the
Bunsen Burner
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These ‘Energy Transfer Diagrams’ show how one form of energy can be changes
into other forms but they do not show how much of the energy that goes in is
changed into each form that comes out.
For example - in the diagram for the Bunsen Burner we do not know how much of
the Stored Chemical Energy in the gas is actually turned into heat energy and
how much is turned into light energy.
Now try this question…
In your exercise book draw ‘energy transfer diagrams’ for these
situations.
A) A television
B) A gas cooker
C) A roller-coaster
D) A light-bulb
E) A wind-up toy
Remember that
each diagram will
have one arrow
going in but possibly
more than one
coming out!
Homework 1
Draw and fully label Energy Transfer Diagrams for the following
situations…
a. A bow and arrow
b. A loud-speaker
c. A toaster
d. A torch (with a battery inside it)
e. A coal fire
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Sankey Diagrams
Sankey Diagrams are similar to Energy Transfer Diagrams but they are able
to show how much of the energy input is turned into the different types of
energy output.
For example – the Sankey diagram above shows how energy is transferred in a
light bulb. The thickness of each arrow represents the amount of energy
described – ie. the thicker the arrow the more energy it represents.
You can actually draw these Sankey diagrams to scale..
To do this you could decide how many centimetres represents a certain
amount of energy and draw the arrows accordingly.
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Examples to try…
1. Draw a Sankey diagram to represent the following situations…
a. A light bulb turns 100 Joules of electrical energy into 80 Joules
of heat energy and 20 Joules of light energy.
b. A television turns 500 Joules of electrical energy into 200 Joules
of light energy, 100 Joules of sound energy and 200 Joules of
heat energy.
c. Copy the Sankey diagram below into your exercise book. Do you
think this is an ordinary light bulb or an energy efficient light
bulb? Explain your answer.
Homework 2
1. Draw a Sankey diagram for a Bunsen burner which transfers 200
Joules of Stored Chemical energy into 140 Joules of heat energy, 40
Joules of light energy and 20 Joules of sound energy.
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Sources of Energy
‘Sources of energy’ are the different places and things that give us energy – for
example – coal, oil, wind and solar.
Sources of Energy can be put into groups (classified).
One way of doing this is to split them into ‘renewable energy sources’ and ‘nonrenewable
energy resources’
This table summarises what is meant by ‘renewable’ and non-renewable’
Type of Energy
Source
Renewable Energy
sources
Non-renewable
Energy sources
What does this mean?
Can be replaced by
nature within a human
lifetime
Are used faster than
nature can replace them
Examples
Wind
Solar
Wave
Tidal
Geothermal
Hydroelectric
Biomass
Fossil Fuels (Coal, Oil &
Natural gas)
Nuclear Fuel (Uranium)
The tables on the two next pages summarise the main ‘renewable’ and ‘nonrenewable’
energy sources and how they work.
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First look at the renewable energy sources:
Name of energy source
Solar Energy from Solar cells
How it works
Solar cells turn sunlight (solar energy) into electricity.
A lot of solar cells joined together is called a ‘solar
array’
Hydroelectric Power Station
The water is high above the ground so it has
‘gravitational potential energy’. As it flows downhill it
turns a turbine which then turns a generator. The
generator then makes electricity.
Tidal Barrage (Tidal Energy)
A barrier is built in a river estuary (opening to the
sea).
When the tide rises and falls every 12 hours a gate is
opened in the barrier and the water flows through and
turns a turbine as it does. The turbine turns a
generator which makes electricity.
Wave Energy
The wind causes waves on the surface of the water. A
wave machine floats up and down on the waves and this
turns a turbine (by hydraulics) which turns a generator
which then makes electricity.
Wind Turbine
The wind turns the blades which then turn a turbine
which turns a generator. The generator makes
electricity.
Lots of wind turbines in the same area is known as a
wind farm.
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Geothermal Energy
The rocks far below the earth’s surface are hot. Cold
water is pumped down a pipe into the earth. This water
is heated by the rocks and is then pumped upwards
again. When it comes back up it is now hot (sometime
even steam).
Biomass
Some types of plant / tree are fast growing – such a s
willow. These can be harvested (cut down) every 3
years or so and dried out and turned into woodchip
which can be burned instead of fossil fuels.
Another way to use them is to let crops ferment to
make alcohol which can be added to fossils fuels such
as petrol or diesel to make then last longer (gasohol)
Remember:
Sources of energy which cannot be used more than once and which will
eventually run out are known as ‘non-renewable’ energy sources.
Here are the main Non-renewable energy sources…
The fuel is burned in a power station
to make water turn into steam which
then turns a generator which makes
electricity.
Uranium nuclei in a reactor are hit by
neutrons and split (nuclear fission).
This gives out huge amounts of energy
which then turns water into steam
which turns a turbine and then a
generator which makes electricity.
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Advantages and Disadvantages of different energy resources
Energy
Resource
Advantages Disadvantages Other Information
Fossil Fuels
(Coal, Oil,
Natural Gas,
Lignite,
turf)
Nuclear Fuel
(Uranium)
Wind
Turbines /
Wind Farm
Relatively cheap to start
up
Only moderately
expensive to run
Large amount of coal left
in the world (not so much
oil or gas)
Do not produce Carbon
Dioxide (so no
Greenhouse effect)
Do not produce Sulphur
Dioxide (so does not
cause acid rain)
Renewable
Low running cost
Does not use up fossil
fuels
Waves Renewable
Low running cost
Does not use up fossil
fuels
Tides Renewable
Low running cost
Does not use up fossil fuels
Non-renewable
Produces carbon
Dioxide when burned
so contributes to
Global Warming
Produces Sulphur
Dioxide which causes
acid rain
Waste products stay
radioactive for years
afterwards
Expensive to store
nuclear materials
safely
Non-renewable
Dangerous – an
accident could
contaminate an area
for many years
Unreliable
Eyesore / Ugly
Noisy
Can harm birds
Unreliable
Eyesore / Ugly
Dangerous for ships /
boats
Causes problems for
shipping
Destroys habitats for
birds and other
organisms
Coal is the worst
for releasing
Carbon Dioxide and
Natural gas is the
least bad of the
fossil fuels.
Removing Suphur
Dioxide from the
smoke etc is really
expensive
Quite cheap to get
Uranium
Building the actual
Nuclear Power
Station is very
expensive
Shutting down a
Nuclear power
station is very
expensive
Needs a lot of land
Need a lot of
turbines to make
electricity
Tides, unlike the
wind and waves, are
predictable but
they do changes
from day to day and
month to month
Ireland has not got any coal or oil. We do have lots of turf but, if we take that
from out of the ground it damages the environment. We do have Natural gas in
the Irish Sea and we also have Lignite which is sometimes called ‘Brown Coal’.
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Now try these questions…
1. Name three fossil fuels.
2. Which of the following are forms of energy? Sound, Pressure, Force,
Electricity, Heat, Weight
3. Which of these energy resources are renewable? Gas, Hydroelectricity,
Oil, Coal, Wind, Tides
Homework 3
1. A solar powered model aircraft uses solar cells to turn the propellers
and to charge a battery. Complete the following paragraph to describe
how it works…
The solar cells change _________ energy into _________ energy. The
battery then stores __________ energy. As the propellers turn they
change __________ energy into useful __________ energy. As the
model aircraft gets higher it gains more _________
__________energy. The model aircraft crashes to the ground and as it
does it produces wasted heat and _________ Energy.
2. Explain what is meant by ‘renewable energy’.
3. Name the polluting gas that contributes to global warming and is
produced by burning fossil fuels.
Now try this question…
1. For each of the devices or situations shown below, draw an energy
transfer diagram to show the main energy change that is taking place.
Device / Situation
Microphone
Loudspeaker
Electric Iron
Coal in a fire
A weight falling to the ground
Battery powered electric drill
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Efficiency
The efficiency of a machine or device is basically how god it is at doing its job –
changing one type of energy into another useful type.
Calculating the efficiency of a device is a bit like calculating your exam scores –
what percentage of the questions you got right!
For example…
If a light bulb is a 100 Watt bulb, this means that it can change 100 Joules of
electricity per second. (remember:- Watt = Joule per second)
But not all of the 100 Joules of electricity will actually be turned into light. A
lot of it is turned into heat which is really just a waste. It is a bit like the
lightbulb getting it wrong!
Let’s say the lightbulb turns 40Joules into Light and the other 60Joules into
heat energy.
We say that its efficiency is
40/100 (40 Joules out of the 100 Joules of electricity
were turned into useful Light)
which is 40%.
Useful Energy Output
Efficiency =
Total Energy Input
Notice that Efficiency does not have any units – it’s just a percentage (%)
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Now look at this question…
1. An electric kettle has a power rating of 2500W
(it produces 2500 Joules of heat per second)
The kettle takes 160 seconds to boil some water and in this time 360,000
Joules of heat is passed from the kettle into the water.
Calculate the efficiency of the kettle.
Efficiency =
Useful Energy Output
Total Energy Input
The Useful energy output is the energy is the energy that is passed into the
water which is 360,000 Joules.
The total energy input is the 2500 Joules per second for 160 seconds which is
2500 x 160 = 400,000 Joules
360,000
So the efficiency = = 0.9
400,000
To make this a percentage we multiply it by 100
So the Efficiency = 90%
Homework 4
A motor has a power rating of 40 Watts. It lifts a load of 80 Newtons up to a
height of 90cm in 4 seconds. Find its efficiency.
Hint – First find the work done, then the power, then divide the power (useful)
by the power rating (total)
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Gravitational Potential Energy
When any object is lifted upwards, it is being moved against Gravity.
If is then let go, it will move (fall downwards) because of gravity.
So when it is still being held up in the air (before you let it go) we say that it
has the potential to move because of gravity which will pull it down when you let
go.
It has ‘Gravitational potential Energy’ - or GPE for short
The heavier the object the more GPE it has.
The higher up it is the more GPE it has.
Gravitational Potential Energy = Mass x Gravity x Height
(Joules) (Kg) (m/s/s) (m)
Remember before you look at the questions that…
a mass of 1 Kg on earth has a weight of 10 Newtons because Gravity on earth is
10 Newtons per Kg.
Now look at this question…
1. Find the gravitational potential energy of a mass of 500 grams when it
is raised to a height of 240cm.
Hint – be careful about units here
500 grams is 0.5 Kg so the mass is 0.5 Kg
240cm is 2.4m so the height is 2.4 m
Gravity on earth is 10 m/s/s or 10 N/Kg
So…
GPE = 0.5 x 2.4 x 10
So GPE
= 12 Joules
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Now try these questions…
Some of them will help you revise earlier work too!!
2. A man pushes a lawn mower with a force of 60 Newtons. How much work
does he do when he pushes the lawn mower 20m?
3. The electrical energy used by a boiler is 1000kJ (Hint: 1 kJ = 1000 Joules)
The useful energy output is 750 kJ.
a. Calculate the efficiency of the boiler.
b. Suggest what might have happened the energy wasted by the boiler.
4. A car engine has an efficiency of 0.28. How much input chemical energy
must be supplied if the total output useful energy is 140,000 kJ?
5. The power of a motor in an electric car is 3600W. How much electrical
energy
is changed into other forms of energy in 5 minutes?
(Hint: remember to use correct units!!)
Homework 5
1. A crane can produce a maximum output power of 3000W.
It raises a load of mass 1500kg through a vertical height (straight
upwards) of 12 metres.
a. What is the weight of the load?
b. How much useful work does the crane do when it lifts the load up 12m?
c. How long does it take the crane to raise the load 12m?
d. What is the speed of the load as it rises?
(Hint: think back to another equation for speed you studied earlier!!)
2. A barrel of weight 1000N is pushed up a ramp. The barrel rises vertically
40cm when it is pushed 1m along the ramp.
a. Calculate how much useful work is done when the barrel is pushed
along the ramp.
b. Pushing the barrel along the ramp needs 1200 Joules of energy.
Calculate the efficiency of the ramp.
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Kinetic Energy
Kinetic Energy is another way of saying ‘Movement Energy’
Kinetic Energy of a moving object is the energy it has because it is moving.
Kinetic Energy = ½ x mass x velocity 2
This equation can be written in short version as…
K.E. = ½ m v 2
Kinetic Energy is measured in Joules (like all forms of energy).
Now look at these examples of questions…
1. A car which has a mass of 800kg is travelling at a speed of 15 m/s.
What is its Kinetic Energy?
K.E. = ½ m v 2
= ½ x 800 x 15 2
= 90,000 Joules
2. A bullet has a mass of 20g and is travelling at 300m/s.
What is its Kinetic Energy?
K.E. = ½ m v 2
= ½ x 0.02 x 300 2
= 900 Joules
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Now try these questions…
1. Find the speed of a boat if its mass is 1200kg and it has a Kinetic Energy of
9600J.
2. A satellite in space has a mass of 120kg and it orbits the earth at a speed of
3000m/s. Calculate its Kinetic Energy.
3. An oil tanker has a mass of 100,000 tonnes (1 tonne = 1000kg).
Its Kinetic Energy is 200MJ. Calculate its speed.
4. The input power of a small hydroelectric power station is 1 MW
(1,000,000W)
If 18,000,000 kg of water flows past the turbines every hour, find the
average speed of the water.
Homework 6
1. A ball of mass 2kg falls from rest (it is still at the start) from a height
of 5m above the ground. Copy the table below and complete it to show
the gravitational potential energy, the kinetic energy, the speed and the
total energy of the falling ball at different heights above the surface.
Height above the
ground (m)
Gravitational
Potential Energy (J)
Kinetic
Energy
(J)
Total
energy
(J)
Speed
(m/s)
5 0 100 0
4 4.47
64
1.8 64
0 0
2. On planet X an object of mass 2kg is raised 10m above the surface.
At that height the object has a gravitational potential energy of 176J
Details of three planets are given below. Which of these is planet X?
Planet Mercury Venus Jupiter
Gravity on planet (N/kg) 3.7 8.8 26.4
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Materials, their properties and their uses
Now that you have learned about energy you need to learn about some of the
materials we use, what we use them for and how we decide to use certain
materials for certain things.
For example- you probably know that we use glass to make window panes but
have you ever thought about why we use glass for this?
Look at the objects above. Each is made from a different material. Can you
explain why each object is made from the chosen material?
Now look at the following descriptive words and see if any of them appeared in
your explanations…
Literacy in Science
transparent shiny flexible strong
light-weight
hard
doesn’t rust
tough
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The words in the box on the previous page are all ‘properties’ of materials – they
are describing words to describe what the materials are like.
Here is a list of lots of ‘properties’ of materials along with the meanings of the
words…
Literacy in Science
Hard – difficult to scratch
Soft – easily scratched
Tough – does not break easily
Brittle – breaks or shatters very easily
Strong – can hold or carry a lot of weight without breaking
Weak – cannot hold or carry a lot of weight without breaking
Conductor – allows heat or electricity to pass through easily
Insulator – does not allow heat or electricity to pass through easily
High density – particles tighly packed making a small piece of it heavy
Low density – the opposite of high density
Transparent – light can pass through it
Opaque – light doenot pass through it at all
Translucent – some light passes through it (like a bathroom window)
Lustre – shininess
Flexible – bends easily
Rigid – does not bend easily
Malleable – can be shaped easily
Non-malleable – cannot be shaped easily
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Activity
Use the words on the previous page to explain why each of the following
materials is used for the purpose given…
a. Glass is used in window panes
b. Wood is used to make furniture (like science benches)
c. Steel is used to build bridges
d. Plastic is used to make shopping bags
e. Gold is used for jewellery
f. Plastic is used to make rulers
g. Iron is used to make saucepans
h. Copper is used to make electrical wires
Homework 7
Use the ‘properties’ of materials you have learned about to explain why
these materials are used for the purpose given…
a. Rubber is used to make car tyres
b. Iron is used to make magnets
c. Diamond can be used to cut glass or tiles
d. Aluminium is used to make aeroplanes
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Testing the properties of materials
We can carry out experiments to test certain properties of materials.
You will now carry out some of these tests over the next few science lessons.
Experiment 1: Testing the hardness of materials
The test for the hardness of a material is called the ‘scratch test’.
The method is as follows…
1. Hold the material to be tested firmly in one hand.
2. Use an iron nail to scratch the surface of the material (trying to
maintain a steady force).
3. Note the depth of the scratch (if there is a visible scratch).
4. Record results in a table (describing the depth of the scratch)
Name of material
Depth of scratch (none,
shallow, deep, very deep)
The hardness of a material can be more accurately measured in
industry where very precise instruments can measure the depth of
even very small scratches. Materials can then be placed on the Mohs
Hardness Scale
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The next Material test is for strength.
Experiment 2: Testing the strength of materials
1. Attach material to a retort stand.
2. Attach a weight holder to the other end of the material.
3. Hang weights, one by one, onto the weight holder until the material
snaps/ breaks.
4. Record results in a table…
Name of material
Thread
String
Paper
Human hair
Number of weights held
before material snapped
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The strength of a material can
be extremely important.
For example - a bridge must be
made of a very strong material
because it has to be able to hold
a lot of weight without breaking.
Steel used in building skyscrapers
must also be strong so
they don’t collapse.
Homework 8
In an experiment
to test the
strength of
materials the setup
to the right was
used. What things
would need to be
done to ensure the
experiment was
fair.
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Extension Activity Building Bridges
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Next you are going to test materials for electrical conductivity.
Experiment 3: Testing the electrical conductivity of materials
1. Build an electrical circuit with two batteries, one bulb, connecting
leads, crocodile clips and leave a gap in the circuit between the two
crocodile clips.
2. Connect various materials between the crocodile clips and see if the
bulb lights or not.
3. Copy and complete the results table below..
Name of
material
Does the bulb
light up?
(Yes/No)
Is the material a
conductor or an
insulator?
Homework 9
Write up the experiment you did in class – with a title, equipment list, risk
assessment, method, variables, fair test, results and conclusion.
Extension Homework
An ammeter is a device which measures the amount of electrical current
flowing. Explain how you could use an ammeter to improve the experiment you
did in class.
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The next materials test is for thermal conductivity.
Experiment 4: Testing the thermal conductivity of materials
1. Use Vaseline to attach thumb
tacks at the ends of each of the
arms of the thermal conductivity
apparatus.
2. Place the Bunsen Burner
underneath the centre (where all
the arms meet).
3. Light Bunsen Burner and adjust
air-hole to get hot flame.
4. Start stop-watch and time until
the thumb tacks fall off (due to
the Vaseline melting).
5. Record all times in a table.
Material Time for thumb
tack to fall (s)
Homework 10
Write up the experiment you
did in class – with a title,
equipment list, risk assessment,
method, results table and
conclusion.
Extension Homework
Explain why cooking pots have to be made of a metal such as iron or copper
but their handles are usually made of plastic or wood.
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Next you need to investigate how we test the flexibility of materials.
Experiment 5: Testing the flexibility of materials
1. Clamp a metre ruler to the edge of the bench making sure that 80cm
of the ruler extend over the edge.
2. Attach a weight holder to the very end of the metre ruler using
string and blue-tac.
3. Measure the deflection (how far downwards the ruler bends) with the
weight holder attached.
4. Add a weight to the weight holder and again measure the deflection.
5. Repeat when adding 2, 3 and 4 weights to the weight holder.
6. Record all results in a table like the one below…
Number of weights added
(remember that the holder
counts as one weight)
Deflection (cm)
Homework 11
Plot a graph of your results of the experiment you carried out in
class…
Plot the number of weights on the x-axis and the deflection in cm on
the y-axis.
Numeracy in Science
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You have now finished your study of Energy and Materials and you need to
prepare for your End of Unit Assessment…
You can use the revision list below to help you study.
Energy and Materials Revision List
What is energy?
What is the law of conservation of energy?
What are the different types of energy?
What are renewable and non-renewable sources of energy?
What are the equations for Kinetic Energy and Potential Energy?
What are Sankey diagrams?
What is meant by ‘efficiency’ and how is it calculated?
What is meant by the ‘properties’ of a material?
What are the tests for the different properties of materials?
Careers in Science
There is a new course at the University of Ulster in Derry called
‘Renewable Energy Engineering’. To do this course you would need
to study either Science or Technology at A-level or preferably
both! Pupils from St. Mary’s have already done this course and
have really enjoyed it!
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Topic 4: Chemical Reactions
In this topic you will be learning about lots of chemical reactions and why
certain chemicals react. You will also learn about chemical equations.
To start with you need to know that ‘chemical reactions’ are also known as
‘chemical changes’. However, there are two types of ‘change’ – Chemical and
Physical and the first thing you need to know is the difference between them.
Chemical Changes…
Make a new substance
Cannot be easily changed back
Normally show signs of a change
Physical Changes…
Do not make a new substance
(the same substance is just in a
different state or form)
Can be quite easily changed back
Don’t show many signs of a change
apart from perhaps a change of
state
Examples of Chemical changes…
Something burning
Two substances reacting
Examples of Physical Changes…
Something melting, evaporating,
freezing or condensing
Something dissolving in a liquid
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Now try to decide if each of the following changes is a Physical Change or a
Chemical Change.
Copy and complete the table with the title ‘Physical or Chemical Change’ and
then put ticks in the correct boxes…
What is happening? Physical Change Chemical
Change
Chocolate melting on a hot day
Turf burning in a fire
Steam rising from the spout of a kettle
An apple going bad and rotting
An ice lolly melting
Sugar dissolving in a cup of tea
Making toast
Making ice cubes in the freezer
An iron nail rusting
Bread going mouldy
Now look at the pictures below and decide if the changes are physical or
chemical.
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Homework 1
1. Which of these are Physical changes?
a. Adding water to dilutable orange juice
b. Burning petrol in a car engine
c. Getting salt from sea water
d. Making plastic from crude oil
2. Name 5 examples of a Physical change and 5 examples of a chemical
change.
Extension Homework
Explain why each of the following is a chemical change…
a. Burning coal in a fire
b. An iron nail rusting
c. Acid and alkali reacting to form salt and water
Famous Scientist…Leo Baekeland
Leo Baekeland was a Belgian scientist who specialised in Chemistry.
His first invention was a new type of paper for
making photographs. He made a lot of money
selling this and was able to spend time developing
a new material which is considered to be the
world’s first plastic. He spent 3 years and
thousands of failed experiments perfecting this
but his perseverance paid off in the end.
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Before you move on and learn about ‘Chemical Changes’ you should first take a
little while to remind yourself about ‘Physical Changes’.
Take the example of ice melting – this is a physical change.
This means that the ice changes shape or state but that the actual substance
remains the same – water!
The particles that make up the ice may have rearranged themselves because
they have more energy but they have not joined with any other particles from a
different substance – No new substance is made in a Physical change!
So the mass remains the same and the properties of the substance remain the
same.
There is actually a pair of experiments you can do to see for yourself whether
or not the mass of the substance changes during a Physical Change and a
Chemical Change.
Method 1… To see if there is a change of mass during a Physical Change
1. Place an ice cube in a beaker
2. Place the beaker on a mass balance
3. Take a reading for the mas of ice and beaker
4. Leave until half of the ice cube has melted
5. Take another reading for mass
6. Wait until all the ice cube has melted
7. Take another reading for mass
Method 2… To see if there is a change of mass during a Chemical Change
1. Half fill a test tube with Lead Nitrate
2. Pour some Potassium Iodide into a flask
3. Place test tube upright inside flask
4. Put rubber bung on top
5. Tip flask
6. Place flask upright on mass balance
7. Record mass every minute.
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So now you should have noticed that there is no change of mass during a
Physical Change or a Chemical Change
So we can improve our earlier summary…
Chemical Changes…
Make a new substance
Cannot be easily changed back
Normally show signs of a change
NO CHANGE OF MASS
Physical Changes…
Do not make a new substance
(the same substance is just in a
different state or form)
Can be quite easily changed back
Don’t show many signs of a change
apart from perhaps a change of
state
NO CHANGE OF MASS
Examples of Chemical changes…
Something burning
Two substances reacting
Examples of Physical Changes…
Something melting, evaporating,
freezing or condensing
Something dissolving in a liquid
Homework 2
Copy and complete…
In a ______ change no new substance is made. In a _____ change a new
substance is made. In a chemical change the total mass ____ ____ ____. In a
physical change the mass ____ ____ ____. Melting is a _____ change. Burning
is a _____ change.
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So you now know that a CHEMICAL CHANGE is totally different from a Physical
change – IN A CHEMICAL CHANGE A NEW SUBSTANCE IS MADE!
There are certain signs of a chemical change – signs that a chemical reaction
has taken place and that a new substance has been made…
Bubbles
released
Change in
temperature
A smell or gas
released
Difficult to
reverse
Colour
change
A solid precipitate
is formed
You do not see these signs when a Physical Change happens.
So it should not be too hard to spot when two chemicals have reacted with one
another.
Activity
What is the sign of each of the following chemical reactions (chemical
changes). You may give more than one answer for each reaction.
a. Coal burning b. Iron rusting c. making toast from bread
d. Magnesium burning in air e. Potassium Iodide and Lead Nitrate
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Homework 3
Decide which of the following are chemical changes and for each chemical
change write down the signs that it is happening…
a. Making soap from vegetable oil
b. Boiling water
c. Burning natural gas
d. Making aluminium cans from aluminium metal
e. Making coffee by adding water to coffee powder
f. Making glass from sand
g. Baking clay to make pottery
Extension Homework
In an earlier topic you studied ‘Matter’.
Describe what happens the particles in ice when it melts into water.
What happens these particles if the water is then boiled.
Now explain why the mass of ice, water and steam is always the same.
Finally explain why you think this is different from a chemical change.
Summary of the main things you have learned so far…
Substances can undergo two types of change – physical and chemical
Physical changes involve the particles rearranging themselves because of a
change in the amount of energy they have.
Chemical changes involve particles of a substance swapping places or joining
with particles from a different substance.
In a physical change – no new substance is made.
In a chemical change a new substance is made.
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In these next lessons you are going to be learning about lots of different
examples of chemical reactions. You will also get the chance to learn about
chemical equations – which we use to help explain what is actually happening.
First let’s look at one of the most common types of chemical reaction / chemical
change – OXIDATION
Oxidation simply involves Oxygen being added to a chemical (or Hydrogen being
removed).
For example –burning Magnesium in air
Method… Burning Magnesium
1. Cut a length of
Magnesium ribbon of
about 2 cm.
2. Hold the 2cm strip of
Magnesium ribbon in a
pair of tongs.
3. Light a Bunsen Burner
and adjust collar to
open the air-hole.
4. Hold the Magnesium
strip in the hot flame
of the Bunsen Burner
until you see it ignite
into a bright white
light.
5. Observe the substance
that remains after the
burning has stopped.
In this experiment you have made Magnesium react with the Oxygen in the
air. The particles of Magnesium have joined with particles of air to make a
new substance called Magnesium Oxide. This new substance is different from
Magnesium and is also different from Oxygen. It truly is a brand new
substance with its own properties. It even looks completely different – it is a
white powder whereas Oxygen is an invisible gas and Magnesium is a grey
solid.
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Now you are going to do the same experiment again but in a slightly different
way…
Method … Burning Magnesium in a crucible (Combustion)
1. Set up the equipment like in the diagram below…a heat-proof mat
with a tripod on top of it, a ceramic triangle on the tripod and then a
crucible on the ceramic triangle.
2. Weigh a 2cm strip of Magnesium ribbon on a mass balance and then
place it in the crucible.
3. Light the Bunsen Burner and adjust the air-hole to get the hot flame.
4. Place Bunsen Burner under crucible and begin heating strongly.
6. When the Magnesium has
become Magnesium Oxide, leave
the crucible to cool and then
scrape out the Magnesium Oxide
and weigh it again on a mass
balance.
7. Record the new mass.
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From you last experiment you should have found that the mass of the
Magnesium is less than the mass of the Magnesium Oxide. This makes sense
because there are more particles in this new substance – magnesium Oxide than
there are in plain old Magnesium.
+
+
Magnesium Oxygen Magnesium Oxide
You can see from the particle diagram above that Magnesium Oxide should be
heavier than just Magnesium because there are more particles.
Now let’s look at the chemical equation for this ‘chemical reaction’
Mg is the chemical symbol for Magnesium
(You might remember this from Year 9)
O is the chemical symbol for Oxygen
Magnesium Oxide has the formula MgO because each Magnesium atom is now
joined together with one Oxygen atom.
So the chemical equation is…
Mg + O MgO
Extension Work
There is a slight problem with the equation above. Oxygen atoms do not float
about in the air on their own. They are always found in pairs – in molecules.
An Oxygen molecule has the formula O 2
But if we put this formula in the equation, the equation is not balanced.
Mg + O 2 MgO
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Extension Work (continued)
Mg + O 2 MgO
You can see that, in this equation, there are two Oxygen atoms on the left hand
side but only one on the right hand side – this cannot happen – atoms cannot just
disappear!
So we have to balance the equation…
We can’t change the O 2 on the left hand side because Oxygen gas is made up of
molecules of 2 atoms and we can’t change that so instead we make two Oxygen
atoms on the right hand side by putting a 2 in front of the MgO.
Mg + O 2 2MgO
Problem… now the number of Magnesium atoms doesn’t match up – there is only one
atom of Magnesium on the left hand side but there are 2 on the right hand side. So
we now put a 2 in front of the Magnesium atom on the left hand side.
2Mg + O 2 2MgO
Now the equation is completely balanced – the same of number of Oxygen atoms on
both sides and the same number of Magnesium atoms on both sides.
+
+
2 Mg O 2 Mg O
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Homework 4
Grainne heated some magnesium ribbon in air. She measured the mass of solid
before and after heating. Here are her results…
Mass of solid before heating = 0.24 g
Mass of solid after heating = 0.4 g
a. Copy and complete the word equation for this reaction.
Magnesium + _________ = Magnesium Oxide
b. Name the reactants in this reaction.
c. Name the product in this reaction.
d. Explain the results of Grainne’s experiment – mass of solid before and
after heating.
Now you are going to look at another ‘Oxidation’ chemical reaction.
This time it is the oxidation of iron.
Method… Investigation into the rusting of iron
1. Place two small iron nails in
each of three boiling tubes.
2. In one boiling tube place a
pinch of Calcium Chloride
powder. Label this boiling
tube C.
3. In another boiling tube pour
some boiled water to cover
the nails and then pour some
oil on top. Label this boiling
tube B.
4. In the third boiling tube
pour some tap water and
label this boiling tube A.
5. Put rubber bungs in all
three boiling tubes and wait.
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Method… Rusting of Iron (continued)
6. Record your results in a table like the one below…
Boiling
Tube
A
B
C
Conditions (set-up)
Tap water covering half
of nails
Boiled water covering
nails with layer of oil on
top of water
No water and powdered
calcium Chloride
present
Conditions
(Presence of
water/Air)
Water and air
present
Water but no air
Air but no water
Description of
nail after 1 week
You should have noticed that the nails needed both air and water present in
order for the iron in them to ‘react’ with Oxygen and become ‘oxidised’.
The actual reaction that took place when the nails rusted was as follows…
Iron + Oxygen Iron Oxide
This is called a ‘Word Equation’ and is used to state the reactants (the
substances which reacted together) and the products (the new substances that
were made).
Preventing iron from rusting
Iron is a very strong material which is useful for buildings and other
structures such as bridges and even parts of cars and lorries. However, when
it rusts it ‘changes’ into Iron Oxide which is not so useful – Iron Oxide is
flaky and weak.
So it is important sometimes to stop iron from rusting in the first place – to
do this we simply have to keep the Oxygen in the air and water away from it.
There are several ways of doing this.
You should carry out some research to find out 4 ways of preventing rusting.
Then decide which way would be best for preventing the rusting of…
Bicycle chain Iron fence Iron water taps Body of a car
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Homework 5
1. Match up the method of preventing rusting with the situation in which
you would best use this method..
Bicycle chain
Iron fence
Car body
Jewellry
Water tap
Chromium plating
Oiling
Silver plating
Painting
Zinc plating
Extension Homework
Carry out research to find out about how much the ‘Titanic’, which sank
around 100 years ago, has rusted. Write a paragraph on your findings.
Now you are going to learn about a different type of ‘chemical reaction’ called
‘Thermal Decomposition’.
Thermal means ‘to do with heat’
Decomposition means ‘breaking down’ or ‘breaking apart’
So ‘Thermal Decomposition’ means ‘heating a substance and making it break
apart into other new substances’.
Carbon
Copper
Oxygen
+
Copper Carbonate molecules are made
up of one Calcium atom, one Carbon
atom and three Oxygen atoms all
joined together
When heated strongly Copper
Carbonate breaks apart to form
Copper Oxide and Carbon Dioxide.
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You can now carry out an experiment to see the thermal decomposition of
Copper carbonate.
WARNING – Danger
Method… Thermal Decomposition of Copper Carbonate
of Suck-Back
1. Put two spatulas of Copper Carbonate powder into a boiling tube.
2. Place rubber bung with delivery tube on top of boiling tube.
3. Fill another boiling tube about half full of Limewater.
4. Hold the two boiling tubes in retort stands so that the delivery tube
leads right into the Limewater.
5. Position the boiling tube of Copper Carbonate at a slight angle to
reduce the risk of suck-back.
6. Place a Bunsen Burner under the boiling tube of Copper Carbonate and
light it.
7. Heat the Copper carbonate strongly and observe.
You should find that the Copper carbonate changes colour (think of the signs of
a chemical change) from green to black and that the Limewater also changes
colour (from clear to cloudy).
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Explanation of Thermal decomposition of Copper Carbonate
Copper is a brownish orange solid, Carbon is a black solid and Oxygen is a
colourless gas but Copper carbonate is a green powder.
It is a different substance than any of the substances that make it up!
When we heat Copper Carbonate it changes colour from green to black.
This is because it is no longer Copper Carbonate –the solid powder you are
seeing in the boiling tube has changed into Copper Oxide (which is black)
Copper
Carbon
Oxygen
+
Copper Carbonate Copper Oxide Carbon Dioxide
A gas is given off which is Carbon Dioxide. We know it is Carbon Dioxide
because it goes into the Limewater and turns it cloudy – only Carbon Dioxide
turns Limewater cloudy!
Homework 6
Write up the experiment you did in class on the thermal decomposition of
Copper Carbonate.
Include a title, equipment list, risk assessment, method and conclusion.
Extension Homework
What substances would be formed by the Thermal decomposition of…
a. Calcium Carbonate
b. Sodium Carbonate
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So far you have learned about two types of ‘Chemical Reaction’…
1. Oxidation is the addition of Oxygen to another substance. There are two
types of Oxidation – burning and rusting.
2. Thermal Decomposition is the breaking apart of a complicated substance
into other substances when it is heated strongly.
Now you will be learning about some more types of chemical reaction.
The next few reactions you will be learning about all have one thing in common –
they all have some sort of salt as a product.
What is Salt?
Lots of people think that ‘salt’ is the name of one particular substance.
Actually the word ‘salt’ refers to a whole family of substances.
There are lots of different ‘salts’.
For example - the salt that you put on your dinner is called ‘Sodium Chloride’.
However, there are other salts that you eat too – like Potassium Chloride.
All salts are made up of some sort of metal (like Sodium or Potassium) in a
compound with at least one non-metal (like Chlorine or Sulphur).
Here are some examples of the names of some salts…
Sodium Chloride Sodium Sulphate Sodium Carbonate Sodium Nitrate
Potassium Chloride Potassium Sulphate Potassium Carbonate
Magnesium Nitrate Magnesium Sulphate Magnesium Chloride
You can see that every salt contains a metal and a non-metal or combination of
non-metals.
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Making Salts
Method 1 - Reacting acid with metal to make a salt
1. Place 5 test tubes in a test-tube rack and fill each one half full with
dilute Hydrochloric acid.
2. Place a small sample of each of the metals in the test-tubes – one
metal for each test-tube… magnesium, zinc, iron, tin and copper.
3. Observe any changes.
4. Put your results in a table like this one…
Name of metal
Magnesium
Zinc
Iron
Tin
Copper
Reaction with acid
You may have noticed that a gas came out of some of the test-tubes where a
reaction took place.
You can test to confirm which gas this is by lighting a splint and holding it near
the opening of the test-tube as the gas escapes. You can see this on the next
page.
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Testing for Hydrogen Gas
There is a very simple test to confirm if a gas is actually Hydrogen.
Simply collect some of the gar as it comes out of the test-tube (of metal and
acid) and then, still holding the test-tube of gas upside-down, hold a lighted
splint at the opening. If it is Hydrogen gas, you will hear a squeaky pop.
There is also a slightly more complicated way to collect Hydrogen gas which
your teacher might show you.
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Homework 7
Copy and complete…
Acids have a pH number _____ than 7. An acid added to a metal will make a
____ and ____. Hydrogen gas ____ with a ____ splint. Sulphates are made
from ____ acid. Chlorides are made from ____ acid. Nitrates are made
from ____ acid. To make Zinc Chloride we use ____ and ____ acid.
You have now carried out the experiment to make salts by reacting metals with
acid. You should now have a look at the chemical equations for these reactions.
First look at the reaction between Magnesium metal and Hydrochloric acid…
The word equation is as follows…
Magnesium + Hydrochloric Acid
Magnesium Chloride + Hydrogen
The symbol equation is…
Mg + 2HCl MgCl 2 + H 2
Magnesium Chloride is the name of the salt that is produced and hydrogen gas is
also produced and given off.
The equations for the reactions between the other metals and the acid are very
similar.
Also you could use different types of acid to make different types of salt. For
example – if you use Sulphuric acid the salt will be a ‘sulphate’; if you use Nitric
acid the salt will be a Nitrate and if you use Hydrochloric acid the salt will be a
Chloride.
You might have noticed some signs of a reaction when you carried out the
last experiment – bubbles of Hydrogen gas forming, the metal fizzing,
perhaps even some heat being given off. However, the salt that was produced
was actually dissolved in the water from the dilute acid and so you probably
couldn’t actually see it.
Next you are going to make a salt by reacting a metal and acid but you will
then filter and evaporate so you actually obtain the solid salt.
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The salt you are going to make is called Zinc Sulphate.
You might be able to work out which acid and which metal you need to react
together to make this salt….
Zinc metal reacting with Sulphuric acid will make the salt ‘Zinc Sulphate’.
Making Zinc Sulphate using the metal and acid method…
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You should now have made Zinc Sulphate. You should be able to see it as a
powder left behind in the evaporating dish.
Can you answer a few questions about this experiment using the knowledge you
have gained so far in this topic…
Questions…
1. What are the reactants in this reaction?
2. What are the products in this reaction?
3. What are the signs that a chemical reaction has taken place?
Harder Questions…
4. Why do you think you should keep adding the Zinc powder until no more
dissolves?
5. Try to write a word equation for this reaction.
6. Try to write a balanced symbol equation for this reaction.
Homework 8
Name the salts that you would make in the following reactions…
1. Hydrochloric acid with Copper
2. Sulphuric acid with Magnesium
3. Nitric acid with Silver
4. Sulphuric acid with Copper
Extension Homework
1. Write word equations for the reactions in the homework above.
2. Write balanced symbol equations for the reactions also.
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There is another way to make a salt.
This other way is to react an acid with an base. You actually did this in year 8
(although it is so long ago that you might not remember).
You will now carry out this second method.
Method 2 – Reacting an acid with a base to make a salt
1. First add Copper Oxide
to the acid and stir.
2. When no more Copper
Oxide dissolves, filter
the mixture.
3. Carefully evaporate the
filtrate to about half of its
original volume and leave it
to cool.
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Homework 9
1. What are the signs that a chemical reaction has taken place?
2. What substance is left behind in the filter paper?
3. What is the name of the product in this experiment?
4. What are the reactants in this experiment?
Extension Homework
1. Why should you keep adding Copper Oxide until no more dissolves?
2. Write the word equation for this chemical reaction.
Extension Work
The word ‘base’ in science means a certain compound of a metal.
For example any metal oxide (Copper Oxide, Zinc oxide) is a base.
Also any metal Hydroxide (Sodium Hydroxide, Potassium Hydroxide) is a base
Finally any metal carbonate (Copper Carbonate, Calcium carbonate) is a base.
To summarise – a base is the oxide, Hydroxide or the Carbonate of a
metal.
Bases neutralise acids – just like alkalis do.
In fact many bases are also alkalis.
The reactions for bases with acids can be describes as below…
Acid + Metal Oxide Salt + Water
Acid + Metal Hydroxide Salt + Water
Acid + Metal carbonate Salt + Carbon Dioxide + Water
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Next you are going to learn about the chemical reactions between alkali metals
and water…
Demonstration – Alkali metals reactions with water
The teacher will fill a trough with tap water, then add a few drops of an
indicator called Phenolphthalein (which turns pink if an alkali is present).
Next the teacher will add a small piece of the first alkali metal – Lithium.
This will be repeated for some of the other alkali metals including Sodium
and Potassium.
The last three alkali metals cannot be shown to you because they are too
dangerous but you can watch a video showing how they react with water.
Potassium in water is shown
in the image below
This results table describes the reactions
of the first three alkali metals with water.
If Caesium is placed in water the result can be
pretty explosive
Scan the QR code to
watch a video about the
reactions of Caesium,
Rubidium and Francium
with water
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You should now have seen how the ‘alkali metals’ react with water. Hopefully you
also noticed that they all react in a similar way although the reactions do vary in
how violent they are.
You might even have noticed that there is a pattern to how violent the reactions
are. The least reactive is Lithium which is at the top of the ‘Alkali metal’ group
on the Periodic Table. The most reactive is at the bottom of the group.
In other words the alkali metals get more reactive the further down the group
you go.
The word equations for these reactions are all very similar…
Can you write the word equations for Caesium, Rubidium and Francium?
Lithium + Water Lithium Hydroxide + Hydrogen gas
Sodium + Water Sodium Hydroxide + Hydrogen gas
Potassium + Water Potassium Hydroxide + Hydrogen gas
Homework 10
Write a paragraph to describe the reactions of each of the alkali metals –
the first three from your observations of the demonstration carried out by
the teacher and the last three from the video.
Extension Homework
Write balanced symbol equations for the reactions of each of the alkali
metals with water. The first one is done for you.
2 Li + 2 H 2 O 2 LiOH + H 2
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Next you are going to learn about the ‘Reactivity Series’. You have actually
learned a little bit about it already without knowing it – Remember in the last
lesson when you learned that the alkali metals vary in the violence of their
reactions with water; some alkali metals are more reactive than others!
You already know that an iron nail rusts when it is in contact with air and
water. However this reaction takes quite a long time – it is a slow reaction.
On the other hand Magnesium ribbon burns in air very quickly. It is all over in
a few seconds. The reaction between magnesium and Oxygen is very fast.
Some substances are more reactive than others!
To help us remember which elements are more reactive scientists have made
a list of elements in order of their reactivity. This list is called the
‘Reactivity Series’
The ‘Reactivity series’ is a bit like a league table in football.
The league table for the English Premier league for 2016 is below. Leicester
were the best team so they are top of the league. Aston Villa were the worst
team so they are bottom of the league.
In the ‘Reactivity series’ the element at the top is the most reactive and the
one at the bottom is the least reactive.
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Below is the ‘Reactivity Series’ along with a pneumonic (rhyme) to help you
remember it in the correct order…
Try to learn it off by heart.
Now answer these questions…
Which is more reactive from each pair of elements?
a. Sodium and Iron
b. Potassium and Lead
c. Hydrogen and Aluminium
d. Gold and Zinc
e. Magnesium and Lithium
f. Calcium and Sodium
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So what is the point of the ‘Reactivity Series’? How does it help us when doing
chemical reactions?
As well as telling us about how fast elements might react and how ‘reactive’
they are, we can use the positions of the elements in the series to predict
which reactions might actually happen in the first place…
For example - what if we added a piece of Magnesium to a solution of Copper
Sulphate?
The ‘Reactivity Series’ can help us figure out if these two substances would
react or not…
Magnesium and Copper are both metals. Only one of these can be part of a
Sulphate compound. So which one gets to be in the compound? Whichever
one is more reactive and wants it more!!
Magnesium is above Copper in the ‘Reactivity Series’ and so it will ‘displace’
Copper in the Sulphate compound.
Therefore the following reaction will take place…
Magnesium + Copper Sulphate Magnesium Sulphate + Copper
This type of reaction when one metal is ‘displaced’ by another is called a
‘displacement’ reaction.
Now try this question…
A piece of Zinc metal is added to a solution of Magnesium Sulphate.
Will a chemical reaction occur and, if so write the word equation for it?
Answer…
Magnesium is above Zinc in the reactivity series so zinc is not reactive
enough to ‘displace’ Magnesium. Therefore no reaction will take place!
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Now try these questions…
1. A piece of Zinc is added to a solution of Copper Sulphate. Does a
chemical reaction take place and, if so, write the word equation.
2. Look at the following pairs of chemicals which are added together. In
each case decide if a reaction will take place and if so, write the word
equation…
a. Magnesium added to Potassium Iodide
b. Copper added to Zinc Sulphate
c. Sodium added to Iron Sulphate
d. Calcium added to Magnesium Sulphate
Extension Work
Decide in each case if a chemical reaction will take place and, if so, write the
word equation. Also decide for each reaction if it is likely to happen quickly or
more slowly. Explain your answers.
a. Calcium added to Sodium Iodide
b. Magnesium added to Zinc Sulphate
c. Sodium added to Copper Sulphate
d. Calcium added to Magnesium Sulphate
Now you will carry out an experiment to see for yourself how displacement
reactions happen and how they can be predicted (even how quick and violent
they will be can be predicted)…
Fill 12 testtubes with the 4 solutions provided – 3 testtubes of each solution.
Then add a piece of each metal provided to each solution and observe what
happens. Use your observations to fill in the results table below…
Zinc Metal Iron Metal Magnesium Metal Copper Metal
x
x
x
x
Copper
Sulphate
Magnesium
Sulphate
Iron
Sulphate
Zinc
Sulphate
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Homework 11
Write a method for the experiment you carried out in class.
Draw a diagram of the equipemtn as you set it up.
Mention 2 risks during this experiment and what you did to keep yourself and
others safe.
Extension Homework
1. Name the products in each of these chemical reactions…
a. Iron + Sulphuric acid
b. Zinc Carbonate + Sulphuric acid
c. Magnesium Oxide + Nitric acid
d. Sodium Hydroxide + Hydrochloric acid
2. Chemical reactions don’t always happen. Think about the reactivity
series and predict if a reaction will take place in each case…
a. Magnesium + Iron Oxide
b. Zinc Oxide + Copper
c. Copper Sulphate + Zinc
d. Magnesium Sulphate + Copper
Nest you are going to start learning about ‘Rates of reaction’.
The rate of a chemical reaction basically just means how fast it happens.
Some reactions are naturally quicker than others.
However there are things we can do to speed up or slow down chemical
reactions.
Your teacher will show you how to carry out some experiments to see how to
speed up chemical reactions.
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Topic 5: The Atom
Everything is made up of tiny particles called ‘atoms’
We now know that even atoms are made up of even smaller particles inside
them.
You could research the development of our ideas about the atoms – look up the
‘plum pudding model of the atom’ and the ‘Rutherford-Bohr model of the atom’
and see the difference between what we used to believe and what we now know
to be true.
Atoms are actually made up of three even smaller particles inside them –
electrons, protons and neutrons
The planetary model of the atom
(also known as the Rutherford-Bohr model)
An atom is actually made up of three
even smaller particles inside it called
electrons, protons and neutrons.
The way they are arranged is shown in
the diagram to the left – protons and
neutrons bunched together in the centre
in a bundle called the ‘nucleus’ and the
electrons orbiting around this ‘nucleus’.
The table on the next page tells you the
masses and electric charges of each
type of particle within the atom.
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Name of particle
Whereabouts is
Mass of particle
Electric Charge
in atom
it in the atom
(Atomic Mass Units
– AMU)
Proton
Neutron
In the nucleus
(centre bundle)
In the nucleus
(centre bundle)
1 +1
1 0
Electron
Orbiting around
1
-1
the nucleus
1840
All atoms are electrically neutral overall which means they have to have the
same number of + charges as – charges. This means that all atoms have to have
the same number of protons and electrons always!
The number of neutrons is quite often the same too but not always!
Atomic Number and Mass Number
As you may know there are lots of different types of atom and the full list of
all the atoms can be found in the periodic table – you have one in your school
diary.
Homework 1
Learn the mass
and electric
charge of
protons,
neutrons and
electrons.
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All atoms have protons and electrons (and all have the same number of protons
and electrons too!).
Almost all atoms have neutrons – only Hydrogen doesn’t have any neutrons.
The number of protons in an atom is called the ‘Atomic Number’
This will also be the number of electrons because it is always the same as the
number of protons.
The number of particles in the centre bundle – the nucleus – is called the ‘Mass
Number’ – so this is the number of protons + the number of neutrons
Here is an example of one the boxes in the Periodic table:
Mass Number
16
(Number of
particles in
the nucleus)
Symbol of
the atom
Name of
the atom
Oxygen
8
Atomic Number
(number of
protons which is
also the number
of electrons in
the atom)
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The Mass number is given the symbol A
Atomic number is given the symbol Z
So every atom can be written in this way…
A
X
Z
Now try this question…
1. Use the periodic table to find out how many protons, neutrons and electrons
each of the atoms in the table below has.
Name of atom Number of
protons
Number of
electrons
Number of neutrons
(Mass Number – Atomic Number)
(Atomic Number)
Hydrogen
Carbon
Magnesium
Plutonium
Homework 2
Use the periodic table in your school diary to write out the numbers of protons,
neutrons and electrons in all of the first 20 elements – from Hydrogan up to and
including Calcium.
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Isotopes
Normally a particular type of atom – say a Carbon atom – always has the same
number of particles inside it. In fact this is always true for protons and
electrons. But sometimes you can find atoms of Carbon that have a different
number of neutrons from what is usual.
An atom with a different number of neutrons from normal is called an ‘Isotope’
For example - Helium has two different isotopes… Helium - 4 and Helium - 3
4
3
He
He
Helium – 4 Helium – 3
Another example of an atom which has an isotope is Carbon.
12
14
C
C
Carbon - 12 Carbon - 14
How many protons, neutrons and electrons does each isotope of Carbon have?
Homework 3
Use the internet to research 5 elements which have isotopes and write out
the mass numbers of all their isotopes.
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Radiation
The difference between all the atoms listed in the periodic table is basically
their size – how many protons, neutrons and electrons they have in them. Atoms
range in size from the very smallest type which is a Hydrogen atom (only 1
proton and 1 electron) to the very heaviest Actinium which has very many
protons, neutrons and electrons.
Imagine building a tower of building blocks.
When there are only a few blocks in the tower, it is very stable and
doesn’t topple over easily.
But what if there were lots more blocks in the tower?
The tower would start to become quite unstable
and might actually topple over at any time.
Atoms which are very heavy and are therefore unstable are said to be
‘radioactive’
These ‘unstable’ ‘radioactive’ atoms can become stable by getting rid of some of
the particles in their nucleus.
They might ‘fire out’ some particles from their nucleus and when they do, what
comes out is called ‘Nuclear Radiation’
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We now know that there are actually three different types of ‘Nuclear
radiation’ – three different combinations of particles that radioactive atoms
might fire out (emit).
They are called alpha α ,
beta β and
gamma γ
When heavy, radioactive atoms emit this ‘Nuclear Radiation’ is always completely
random – at random times – and we can do nothing to affect this at all.
A heavy, unstable nucleus emitting an alpha particle
There is always some radiation all around us coming from rocks in the ground,
gases in the air and from Space – this is known as ‘Background Radiation’.
When nuclear radiation hits other materials (including living things like us) it can
cause the atoms in that thing to turn into ions (lose electrons).
For this reason Nuclear Radiation is described as being ‘ionising’
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The table below gives more details about the three types of Nuclear radiation.
Type of
Nuclear
Radiation
What is it?
Mass
(AMU)
Charge
Penetrating
Power
Deflection
Ionising
Power
(and symbol)
alpha α
(particles)
A bundle of 2
protons and 2
neutrons
4 +2 Absorbed by
paper (or even
a few cm of
Deflected
slightly by a
magnetic field
Strongly
ionising
air)
beta β
(particles)
Fast moving
electrons 1/1840
-1 Absorbed by
a few mm of
aluminium
Deflected a
lot by a
magnetic field
Slightly
ionising
gamma γ
(waves)
High frequency,
high energy EM
waves
0 0 Only
absorbed by
thick lead
Not deflected
at all
Very weakly
ionising
The diagram below shows clearly the penetrating power of each type of Nuclear
radiation.
Homework 4
Use the information above to explain why the containers which hold
radioactive materials are made of lead.
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Uses of Nuclear Radiation
We have quite a few uses for Nuclear radiation in industry, hospitals and even in
our homes.
Here are a few…
Treating cancer – the radioactive isotope Cobalt – 60 is used to treat
cancerous tumours
Gamma Radiation can be used to irradiate food to keep it fresh – basically
the radiation kills bacteria which would cause the food to go off
Gamma radiation is also used to kill bacteria and other germs on surgical
equipment
Carbon dating – radiation can be used to figure out how old rocks and
fossils are
Beta radiation can be used to measure the thickness of paper or thin
sheets of aluminium
Radiation can be used to monitor the flow of liquids – such as blood in the
blood vessels or water/sewerage in a pipe
Homework 5
Choose one of the
uses of radiation
above and carry
out research into
it and make notes.
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Electronic Configuration
You have now learned about the nucleus (the centre) of atoms. Next you need to
learn a little bit more about the electrons and how they are arranged.
Firstly you should know that the number of electrons in orbit around the nucleus
is always the same as the number of protons in the nucleus.
So an Oxygen atom has 8 protons and 8 electrons.
Next you need to understand that the electrons are not all simply flying around
in the one circle around the nucleus…
Instead the electrons are arranged in specific rings called shells and there are
rules for how many electrons are allowed in each shell.
In the first shell (the one closest to the nucleus) there are only 2 electrons
allowed maximum. In the second shell there is a maximum of 8 electrons allowed
and the same for the third shell.
Below are diagrams showing the electronic configuration of Sodium (Na) and
calcium (Ca).
Notice that the nucei do not show the protons and neutrons (this is just for
handiness)
In a Sodium nucleus, there are 11
protons so there are 11 electrons in the
shells. Look how these are arranged.
In a Calcium nucleus, there are 20
protons so there are 20 electrons in the
shells. Look how these are arranged.
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Class Activity
Use the periodic table in your diary to find the atomic number and mass
number of each of the first 20 atoms and darw a diagram of each one.
You do not have to actually draw the protons and neutrons – just draw a
circle to represent the nucleus and write the number of protons and
neutrons inside it. Then draw in the elctrons in the correct electronic
configuration.
An example is shown here for Sodium
Homework 6
11p
12n
You should
finish all 20
drawings of
atoms for
homework.
For handiness, here is a copy of the part of the Periodic table you need…
H 1
1
He
4
2
Li
7
3
Be
9
4
B 11
5
C 12 6
N 14
7
O 16
8
F 19 9
Ne
20
10
Na
23
11
24
Mg
12
27
Al
13
28
Si
14
31
P
15
S 32
16
37
Cl
17
Ar
40
18
39
K
19
Ca
40
20
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How atoms bond
Think about this –
everything is made out of atoms,
there are around 100 different types of atom listed in the Periodic table,
yet there are thousands of different types of material.
How is that?
The answer is that different types of atom can be joined together to make new
materials!
But how do atoms join together or ‘bond’?
It is all about their electrons.
Remember the rules for electron shells – 2 electrons in the first shell, 8 in the
second and third.
But atoms really like to have their outermost shell full to maximum if possible.
For example an Oxygen atom has 8 electrons so the first shell has 2 and the
second shell has 6.
However, an atom
can have up to 8
electrons in its
second shell so
Oxygen’s second
shell is not full to
maximum
It would be better if
Oxygen could fill its outer
shell – to do this it could
either get rid of the 6
electrons in the second
shell or get two more
electrons from some other
atom to fill its second shell.
It is easier to find two more electrons than to get rid of ( and have to find
ahome for) 6 electrons!
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So where does the Oxygen atom get two more electrons from?
It would be great if it could find an atom that needed to get rid of 2 electrons,
wouldn’t it?
Can you find an atom among the first twenty that you drew that could fill its
outer shell by getting rid of 2 electrons????
Magnesium has 12 electrons which gives an electronic configuration of
2 : 8 : 2
First shell Second shell Third shell
This means that Magnesium could achieve a full outer shell by getting rid of the
2 electrons in its third shell – then its second shell would be its outer shell and
would be full!!
So it would help Magnesium and Oxygen if Magnesium just gave 2 electrons to
oxygen.
Both atoms now have full outer shells as long as they remain together – as long
as they are bonded.
This is called an ionic bond because the atoms have now turned into ions.
An ion is just an atom that has gained or lost electrons.
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If an atom gains an electron, it has gained a negative charge so the atom
becomes a negative ion.
If an atom loses an electron, it has lost a negative charge so the atom becomes
a positive ion.
An atom thought it had lost
an electron and said I will
have to keep my ion that!
Two atoms were walking
down the street and one says
‘I think I’ve lost an electron’.
The other atom asks ‘Are
you sure?’
The first atom says ‘I’m
positive’
You should note that ionic
bonding always happens
between the atoms of a
metal and the atoms of a
non-metal.
Homework 7
Draw diagrams like the one on the
previous page to show how the
following atoms bond…
Calcium and Oxgen
Sodium and Chlorine
Magnesium and Chlorine
Now you have learned about ionic bonding.
There is also another way for atoms to bond.
It is called covalent bonding and it happens between the atoms of 2 nonmetals.
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Covalent Bonding
Remember in ionic bonding how one atoms basically gave electrons to the other.
This was because one atom needed to get rid of an electron to make its outer
shell full and the other needed to gain an electron to make its outer shell full.
But what if both atoms need to gain electrons to make their outer shells full?
The atoms can ‘share’ the electrons…
Let’s look at the example of two Fluorine atoms bonding with each other…
Fluorine atoms have 9 electrons.
(The diagram to the left only
shows the 7 electrons in their
outer shells).
Because the Fluorine atoms have
7 electrons in their outer shells,
they both need one more to
make these outer shells full.
So they simply share one of the electrons – this means both atoms have a full
outer shell (if they both count this shared electron as belonging to each atom.
This is called covalent bonding and it is how the atoms of 2 non-metals bond
with each other.
This diagram to the left shows
how an atom of Hydrogen bonds
with an atom of Fluorine.
They both need one electron to
fill their outer shell (Hydrogen’s
first shell of 1 electron needs to
have 2 and Fluorine’s second shell
of 7 electrons needs to have 8).
So they share an electron which
gives both atoms a full outer shell
of electrons.
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Sometimes an
atom can bond
with two other
atoms in a
covalent bond.
For example –
Oxygen needs two
more electrons to
fill its second
shell.
It can bond with 2 Hydrogen atoms. Each Hydrogen atom has one electron in its
outer shell but if they both share an electron with Oxygen then all three atoms
have full outer shells.
Covalent bonds can happen
between even more than 3 atoms.
The diagram on the left shows
how 4 Hydrogen atoms can bond
in a covalent bond with one carbon
atom. Can you explain how this
covalent bond works.
(Remember – only the outer
electron shell is shown for the
Carbon atom)
So you have now finished your study of how atoms bond. There are a few key
words you should know when talking about atoms.
A group of two or more atoms bonded together is called a molecule.
If the atoms are of the same type, then it is a molecule of an element. If the
atoms are different, then it is a molecule of a compound.
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Topic 6 – Numeracy in Science
You now need to spend some time practicing how to write up experiments
properly and firstly how to deal with data (results).
Dealing with results
Section A – Putting results into tables
You should try these activities for making results tables to deal with data…
1. Here are some results from an
investigation into springs. The
spring was 5cm long at the start
(when there were no weights
hanging on it). When the mass on
the end of the spring was 10g,
the spring was 6cm long. With
20g it was 7cm, with 30g it was
8cm and with 40g it was 9cm
long. The last reading was for 50g. The spring was then 10cm long.
Put these results into a table. There should be two columns in your table.
You should decide the headings for the 2 tables.
2. Draw your own results table to show
the results below…
When the length of the flaps was 2cm,
it took the spinner 1.9 seconds to fall.
Whe they were 2.5cm, it took 2.1
seconds; 3cm took 2.4 seconds and
3.5cm took 2.5seconds. The last result
was 4cm and 2.7 seconds.
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3. Saoirse’s group did an investigation looking at the
effect of temperature on dissolving Copper
Sulphate. Unfortunately they did not design a
results table for their results before starting.
When they temperature was 20 o C it took 205
seconds to dissolve. At 50 o C it took 30 seconds, at
40 o C it took 50 seconds, at 30 o C it
took 110 seconds and at 60 o C it took
20 seconds. Draw a suitable results
table and put in Saoirse’s results.
4. Saoirse’s group then decided to make their results more reliable by
repeating their tests. They took three readings at each temperature.
Results:
20 o C 205 seconds, 220 seconds, 200 seconds
50 o C 30 seconds, 30 seconds, 25 seconds
40 o C 50 seconds, 45 seconds, 45 seconds
30 o C 110 seconds, 105 seconds, 100 seconds
60 o C 20 seconds, 18 seconds, 21 seconds
Sort out these results and present them in a table. Make sure that your
table shows….
All the results
The average time taken to dissolve the Copper Sulphate
Now you have had some practice drawing results tables to make results clearer.
Next you need to practice drawing some graphs to display results in another
format.
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Section B: Drawing Bar charts
1. Put the results in the table on to a bar chart on the squared paper or
graph paper that your teacher gives you.
Type of surface Height ball
bounced (cm)
Carpet 30
Tiles 85
Concrete 80
Wood 70
Felt 40
2. Put the following results on to a bar chart
Number of
paper clips
1 1.9
2 1.6
3 1.3
4 0.8
5 0.6
Time to fall
(seconds)
Now you have finished drawing bar charts.
Next you are going to practice drawing lines of best fit.
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Section C: Line of Best Fit
A line of best fit is not done by joining the dots!!!!!
It is a line that shows us where the perfect results would be if we had done the
experiment perfectly without any errors. Look at the LOBF below to see.
You will notice that the line
is completely straight (not
zig-zag joining up with all the
dots).
You will also notice that it
actually misses some of the
points. This is okay!! The
points are possibly wrong and
the line of best fit shows us
where the points should be.
A line of best fit might be a straight line but it also might be a curve…
The points in this graph clearly need a curved
line of best fit
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Sometimes the line of best fit will miss some of the points – this is okay.
In fact it helps us see which results were not as accurate.
Now you are going to practice plotting graphs, including drawing lines of best
fit.
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Section D: Drawing graphs with lines of best fit
1. Draw a line graph of the results below on the paper your teacher gives
you. (Don’t forget to label the axes)
Load (grams) Extension (cm)
0 0
10 2
20 4
30 6
40 8
50 10
2. Draw a line graph showing the results below.
Remember to use a line of best fit.
Time (seconds) Temperature ( o C)
0 23
60 33
120 42
180 54
240 63
300 74
3. Show the results below on a line graph.
Time (seconds) Volume of gas (cm 3 )
0 0
10 21
20 38
30 52
40 62
50 66
60 68
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Section E: Interpreting graphs
Now you have finished practicing drawing line graphs you will need to learn about
how to interpret and draw conclusions from experiment results and graphs.
The first stage in doing this is to be able to spot patterns from graphs..
Here is an example of how to describe the pattern in a line graph…
Length of spring (cm)
Pattern:
As the load increases, the
length of the spring
increases steadily
Load (g)
Now write the pattern for each of these line graphs…
Acceleration (m/s/s)
Height of bounce (cm)
Force (N)
Height ball is dropped from cm)
Extension (cm)
Load (g)
Volume of gas (cm 3 )
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Section F: Reliability of results
Next you are going to think about the reliability of results.
Sometimes the results from an experiment are not correct and so the pattern
they give you is not reliable.
One way to lessen the effect of bad results is to repeat experiments several
times so that, hopefully, you get good results most of the time.
Look at the examples below and see if you can spot the anomalous (bad) results
which do not fit the pattern.
Question A
1. A group did an investigation to find out
which car rolled best down a slope.
Look at the results they got and work
out the correct order from best to
worst.
Car Distance rolled (cm)
Blue 50
Green 75
Red 60
Black 80
2. The group repeated their tests.
Work out the average and find the order now – from best to worst.
Car Distance rolled (cm) Average
1 st try 2 nd try
Blue 50 80
Green 75 75
Red 60 50
Black 80 60
Has the order changed?
Which order do you think is more reliable – more likely to be correct?
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3. The group did their tests a third time.
Again work out the averages and find the order – from best to worst.
Car Distance rolled (cm) Average
1 st try 2 nd try 3 rd try
Blue 50 80 Car crashed
Green 75 75 75
Red 60 50 55
Black 80 60 75
Has the order changed?
Which car has the most reliable results? Why?
Which car has the least reliable results? Give two reasons why.
How could you make the results for the car in the previous question more
reliable?
Question B
1. Ellie did an experiment to find out which
trainers had the best grip. She raised
the height of the ramp until the trainer
slipped.
Look at her results below and then put
the trainers in order from best grip to
worst grip.
Trainer Height of rampl
before trainer
slipped (cm)
Nike 50
Addidas 46
Puma 44
Air-Max 47
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2. Ellie repeated her tests. Now work out the averages and again put them in
order from best grip to worst grip.
Trainer
Height of rampl before
trainer slipped (cm)
1 st try 2 nd try
Average
Nike 50 45
Addidas 46 44
Puma 44 47
Air-Max 47 49
3. Ellie repeated her tests a third time.
Again work out the averages and put the trainers in order from the best
grip to the worst grip.
Trainer
Height of rampl before trainer
slipped (cm)
1 st try 2 nd try 3 rd try
Average
Nike 50 45 46
Addidas 46 44 44
Puma 44 47 47
Air-Max 47 49 48
Looking at these results which order would you now out the trainers in?
Explain why you have chosed this order.
Now choose two results from the third table that you think are wrong.
What would you advise Ellie to do about these results?
How could Ellie make her results even more reliable?
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Section G: Evaluating evidence and drawing conclusions
The last part of handling data is being able to draw conclusions – this is a bit
like spotting patterns but in this section you have to explain the pattern too.
Try these two questions…
1. A group investigated which material was the best insulator of heat.
Look at their results below
Type of
material
Temperature
of water at
start ( o C)
Temperature
of water after
2 minutes ( o C)
Wool 68 66 2
Cotton 70 68 2
Metal Foil 70 67 3
Polystyrene 72 71 1
Fall in
temperature
( o C)
What conclusion could you make based on these results?
2. A group investigated the effect of temperature on the evaporation of
water from a beaker. As the water evaporated, they measured its mass
on a mass balance.
Look at their results below…
Temperature
of water
( o C)
Mass of water
at start (g)
Mass of
water after
2 minutes (g)
20 50.38 50.38 0.00
21 51.23 51.22 0.01
22 48.32 48.32 0.00
23 49.99 49.98 0.01
24 50.53 50.51 0.02
Loss in mass (g)
Whatb conclusions could you make from these results?
How could you improve the evidence to make a more valid conclusion?
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Experimental write-ups
Now you are going to learn more about how to write up experimental reports
properly.
All reports start with a title.
Mostly the titles begin with… ‘Investigation into how….. ‘
Activity…
Try to write titles for the following experiments…
1. Seanna is try to find out if the steepness of a ramp changes how far a
car will roll on the flat ground after it has gone down the ramp.
2. Erin is doing an experiment where she changes the temperature of
water and dissolves sugar in the water at different temperatures.
She is timing how long it takes the sugar to dissolve in each beaker of
water.
3. Aoife is carrying out an experiment to see if longer wires or shorter
wires let more electrical current pass through them.
Next you need to write the ‘aim’. This is a short statement about what you hope
to find out. Often the ‘aim’ sounds quite like the ‘title’…. My aim is to find out
how….
Activity…
Write aims for the three experiments outlined above.
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Next in an experimental write-up you need to consider what equipment you will
need to use and list all the pieces of equipment and describe what each one is
used for.
Activity…
Write equipment lists for experiments 1 and 2 on the previous page.
At this point you normally write a risk assessment.
There are some different ways to do this but all have certain things in common.
Below is an example of the headings you might use…
Hazard
Type of
risk
How serious
is the risk/
How likely is
it to happen
(Scale: 1-5)
How bad
would it be
if it
happened
(Scale: 1-5)
Steps you
will take
to prevent
it from
happening
Steps you
will take if
it does
happen
anyway
Activity…
Write risk assessments for experiment 1 and 2 on the previous page.
At this point you should consider the variables in the experiment.
‘Variables’ means any factor which can change or be changed – either things you
can control or things you deliberately keep unchanged (Fair test) or things you
measure.
You need to identify all the variables in your experiment to help you decide how
to plot a graph after you have completed the practical work.
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Next you will practice writing a method. This is essentially like a recipe for
cooking – it is an instruction list on how to carry out the experiment.
To write a good method you need to remember to do some key things….
A method should start with an equipment list.
The method should be written impersonally – this means do not say things
like ‘I will collect the equipment…’ or ‘We will heat the beaker of water…’
Instead say it like this ‘The equipment will be gathered’ or ‘The water in
the beaker will be heated’.
A method should always be written in the future tense ‘This will happen’
and That will happen’ – never ‘This happened’.
Be thorough – include every step in the procedure.
Activity…
Write a method for either experiment 1 or 2 on the previous page.
At this stage you would normally actually carry out the practical work.
Your teacher will help you do this and you can collect the results.
However as you learned earlier you really should prepare for this by
designing a results table beforehand.
Activity…
Design a results table to record results for either experiment 1 or 2 on the
previous page.
The next step is to plot a graph to display your results.
You will need to decide which variables to put on the axes.
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Nearly done now… you now need to evaluate your results and use them and your
graph to draw valid conclusions. You practiced this earlier so hopefully you can
now do this for your own experimental results.
Finally you need to evaluate how reliable your results are. You can do this by
looking at your graph to spot anomalies and how close your averages are to each
of the actual results.
You should also evaluate your method now to identify any things you could
improve on if you were to repeat this experiment.
Finally you should use the check list below to ensure you have written up the
experiment properly…
Title
Aim
Equipment List
Risk Assessment
Variables
Fair Test
Method
Results Table
Graph(s)
Discussion of results and Conclusion
Evaluation of results and method
At GCSE level you will have to write experiments up like you have just
done.
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Topic 7 – Careers in Science
Welcome to your last topic in Year 10 Key Stage 3 Science – Careers in Science.
You have done some work on this at the end of each topic in Years 8, 9 and 10
but now you will have a closer look at what opportunities are out there for you if
you study science at GCSE and A-level.
By the end of this chapter you should be able to..
Understand the importance of science as a subject
Understand the topics covered in GCSE and BTEC science and
how they are assessed
Be aware of how science goes well with certain other subjects
Be aware of the range of interesting careers which are
directly related to science
Know of the skills that are developed in Science that are
useful for any career
Know about some of the university courses and career
pathways that St. Mary’s College pupils have followed
Activity 1
Copy out and answer these questions…
What did you want to do as an adult when you were in Year 8? Do you
still have the same ambition? If not, what do you want to do as an adult
now? Do you know what qualifications and skills are needed for this job?
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St. Mary’s College Science Department
Year 10 Science
Why should you study science?
Next year you will be studying science as it is compulsory for all pupils at St.
Mary’s College. This is because we recognise how important it is to have some
knowledge of science.
Science is vital for various reasons…
Health:– scientists make all the medicines, imaging devices and
treatments which keep us healthy and help us fight disease. Nurses and
doctors look after us when we are unwell -they have also studied science.
Communication & Leisure:– scientists invented Television, radio, mobile
phones, i-pads, the internet. Touch screen technology
Food:– scientists help grow our food and figure out ways to grow more
and healthier food, they help us make food last longer and they even
invented the microwave oven to help us cook our food faster!
The survival of our planet:– scientists are currently working on ways to
remove Carbon Dioxide from the atmosphere to help stop our planet from
warming up which could avoid floods and other extreme weather
conditions
To put it simply science is our future!
There are more job opportunities in the areas of Science and STEM
thatn any other area.
(Remember: STEM = Science, Technology, Engineering and Maths)
Science helps us understand the world we live in. and it helps us
understand and solve the big problems like Global warming, Energy for the
world, what is our place in the Universe, disease and cures etc.
Activity 2
Research one of the Big questions in science – how to meet the world;s
energy needs; how to slow or stop global warming; how to meet the
world’s food needs; how to prevent disease (or another big question)
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St. Mary’s College Science Department
Year 10 Science
Science…
Helps develop skills such as team work, time management
and presentation
Helps you understand your own body
Helps you develop skills such as interpreting graphs which
are also useful in Maths
Combines well with lots o other subjects such as
Geography, Technology, Maths, Engineering, ICT and even
P.E.
Covers a very wide range of topics
Provides an opportunity for carrying out practical work
and field work
Activity 3
For each of the skills listed above, give one example of something you
have learned in science this year which you think helps develop the skill.
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St. Mary’s College Science Department
Year 10 Science
What does GCSE science involve?
St. Mary’s College offers two different science course in Key Stage 4…
1. Level 2 BTEC Science or
2. Double Award CCEA Science
Both these courses are Double Award.
This means that, if you pass them, you actually get 2 GCSEs or the equivalent of
2 GCSEs.
The only group of girls who don’t do Double Award Science are the Gold Pathway
group who do the Single BTEC – so it is equivalent to 1 GCSE.
More detail on each of the courses is given below…
1. Level 2 BTEC Science
This course is actually 2 separate courses. In year 11 you will do a course
called Level 2 BTEC First Award in principles of Applied Science. This is
worth 1 GCSE.
In year 12 you will then do another course called Level 2 BTEC First award in
Application of Science which is worth a second GCSE.
If you pass both courses you will have the equivalent of 2 GCSEs.
These can be used, just like normal GCSEs to apply for university.
Many of our Level 2 BTEC pupils have gone to university to study courses like
Nursing, Pyschology, Child Care, Helath Science and many other courses.
It is possible to pass one of the courses but not the other.
This would just mean that you get 1 GCSE instead of 2.
(Remember: to get back into 6 th Form at St. Mary’s College, you normally need 5
GCSEs or equivalent)
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St. Mary’s College Science Department
Year 10 Science
The big advantage for some pupils of doing BTEC science is that most of the
course is assessed by portfolio rather than by exams.
In fact 75% of each of the 2 courses is assessed by your portfolio work which
you do every day in class. Only 25% is assessed by exams.
This means that it is possible to PASS the BTEC courses even if you FAIL the
exams.
Below are outlines of the 2 BTEC courses…
Level 2 BTEC First Award in Principles of Applied Science (done in Year 11)
Number / Name of Unit Type of assessment How much is
it worth?
1. Principles of Science By exam (1 hour long –
normally done in
March)
2. Chemistry and our Earth By portfolio (like
coursework)
3. Energy and our Universe By portfolio (like
coursework)
4. Biology and our Environment By portfolio (like
coursework)
25% of the
total marks
25% of the
total marks
25% of the
total marks
25% of the
total marks
Level 2 BTEC First Award in Application of Science (done in Year 12)
Number / Name of Unit Type of assessment How much is
it worth?
5. Applications of Chemical
Substances
6. Applications of Physical
Science
7. Health Applications of Life
Science
By portfolio (like
coursework)
By portfolio (like
coursework)
By portfolio (like
coursework)
8. Scientific Skills By exam (1 hour long,
normally done in
March)
25% of the
total marks
25% of the
total marks
25% of the
total marks
25% of the
total marks
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St. Mary’s College Science Department
Year 10 Science
The other option is the Double Award CCEA GCSE.
This course is a Double Award course – you can’t finish after one year and get 1
GCSE!
However you can get a mixed grade – for example: you could get a CD which
means you have one GCSE at grade C and another GCSE at grade D.
An outline of this Double Award CCEA course is given below…
In Year 11…
Number / Name of Unit Type of assessment How much is
it worth?
Biology Unit 1:
Living Processes and Diversity
Chemistry Unit 1:
Structures, trends and Chemical
reactions
Physics Unit 1:Force and Motion,
Energy, Moments and Radioactivity
By exam
By exam
By exam
11% of your
total DA GCSE
11% of your
total DA GCSE
11% of your
total DA GCSE
In Year 12…
Number / Name of Unit Type of assessment How much is
it worth?
Biology Unit 2: Body Systems, By exam
Genetics, Micro-organisms and
health
Chemistry Unit 2: Further By exam
Chemical reactions and Organic
Chemistry
Physics Unit 2: Waves, Sound and By exam
Light, Electricity and the earth
and Universe
Practical Skills By carrying out 3
practical experiments
(one each for Biology,
Chemistry and Physics)
and then doing a short
exam about them.
14% of your
total DA GCSE
14% of your
total DA GCSE
14% of your
total DA GCSE
25% of your
total DA GCSE
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St. Mary’s College Science Department
Year 10 Science
The grade boundaries for the exams for CCEA are as follows…
A* = 90% or above
A = 80% - 89%
B = 70% - 79%
C = 60% - 69%
D = 50% - 59%
E = 40% - 49%
U = Below 40%
The exams in year 11 are marked out of 70 so you normally need to get around
42 out of 70 to get a grade C.
In year 12 the exams are marked out of 90 so you normally need around 54
marks out of 90 to get a grade C.
Activity 4
Listen to a talk by Year 12 students – one who does BTEC science and one
who does CCEA science.
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St. Mary’s College Science Department
Year 10 Science
What are the results like for GCSE and BTEC science?
The science results in St. Mary’s College are normally very good and well above
the average for similar schools.
Last year the results were as follows…
CCEA Double Award Science
% of pupils achieving grade C
or higher in St. Mary’s
College
90%
(100% achieved at least one
GCSE grade C or higher)
Average for similar schools
in N. Ireland
74%
Level 2 BTEC Science
% of pupils achieving grade C
or higher in St. Mary’s
College
98.4% N/A
Average for similar schools
in N. Ireland
Only 2 pupils last year did not achieve at least one GCSE or equivalent in
Science and both of them had an attendance of less than 70%.
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St. Mary’s College Science Department
Year 10 Science
Jobs in Science
The following jobs which are all related to science are currently listed as High
Demand by the government.
This measn we don’t have enough people to do these jobs and if you decided to
do one of these, you have a great chance of finding a good job.
Why not do some of your own research on one or more of these jobs to find out
more about them…
Astronomer
Aviation Inspector
Chemical Technician
Chemistry Teacher
Climate Change Analyst
Electrician
Environmental Scientist
Food Science Technician
Forensic Science Technician
Geo-scientist
Hydologist
Meterologist
Nuclear Monitoring Technician
Nurse
Physics Teacher
Radiographer
Soil Scientist
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St. Mary’s College Science Department
Year 10 Science
Did you know?
Read the following quotes by some people you might have heard of and how
important they think science is…
“Science is the key to
our future, and if you
don’t believe in science,
then you’re holding
everybody back.”
Bill Nye (TV presenter)
Any spare time I
have, I bury my
head in a science
book. It is how you
understand the
word.
Ann Hathaway
(actress)
Life is not easy for any of us. But so
what? We must have perseverance
and above all confidence in ourselves.
We must believe that we are gifted
for something and that this thing
must be science.
Marie Curie (scientist)
Activity 5
Research one job in science that sounds interesting to you.
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St. Mary’s College Science Department
Year 10 Science
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St. Mary’s College Science Department
Year 10 Science
I have not failed. I have successfully discovered 10,000 things that do not work!
Thomas Edison
Somewhere, something
incredible is waiting to be
known
If at first you don’t succeed, try
two more times so that your failure
is reliable.
The 3 stages of scientific research…
1. It’s completely impossible.
2. It is possible but it’s not worth
doing.
3. I said it was a good idea all along.
Unlike protons, I don’t deal with
negativity.
Nothing travels faster than light…
except Year 10 St. Mary’s College
girls at 3.10pm on a Friday afternoon!
Being a scientist is like doing a jig-saw
in a snow-storm at night with some
pieces missing and no idea what the
finished picture looks like!
When you are with a lovely person an hour is like a second and when you
are standing on burning coal a second is like an hour – that is relativity!
Albert Einstein
Teamwork is essential when
carrying out science
experiments – that way you
always have someone else to
blame.
If an experiment works, something
has definitely gone wrong!
Does a radioactive cat have 18 halflives?
If we are all made of atoms, then a
scientist studying atomic physics is
basically a group of atoms studying
themselves!
The optimist sees the glass half
full. The pessimist sees the glass
half empty. The chemist sees the
glass completely full, half with
liquid and half with air.
Let us now pause for a moment of science.
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