(FINAL) Chemistry Notebook 2016-17

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The Learning Goal for this assignment is: The students will learn what makes up atoms and how are atoms of one element different from atoms of another element. Notes Section Smaller Than Atoms? -Atoms make up all matter -Subatomic particles include the electron, proton, and neutron -Protons and neutrons mak up the nucleus, and electrons float around the nucleus in orbitals -Electrons are negative (-), protons are poitive (+), and neutrons have no charge (0) -If there are more or less electrons than protons, that atom is an ion. Looking at Ions -Normal atoms have a neutral charge -Atoms want full valence shells, so they will lose or gain electrons to complete them, making an ion -Positive ions are called cations and negative ions are anions -Once atoms have full valence shells, they'll have a positive or negative charge, and will bond with atoms of the opposite charge -There are covalent and ionic bonds -Ionic bonds are groups of charged electrons held together by electrical froces, but are easily broken by outside electrical forces, and very weak in water. Atomic Mass -An isotope is an atom with an extra or missing neutron -Electrons have a barely noticable mass compared to protons and neutrons -Atomic mass is the average mass of the element, including the average of all the isotopes http://www.learner.org/interactives/periodic/basics_interactive.html 30
Atoms Are Building Blocks Atoms are the basis of chemistry. They are the basis for everything in the Universe. You should start by remembering that matter is composed of atoms. Atoms and the study of atoms are a world unto themselves. We're going to cover basics like atomic structure and bonding between atoms. Smaller Than Atoms? Are there pieces of matter that are smaller than atoms? Sure there are. You'll soon be learning that atoms are composed of pieces like electrons, protons, and neutrons. But guess what? There are even smaller particles moving around in atoms. These super-small particles can be found inside the protons and neutrons. Scientists have many names for those pieces, but you may have heard of nucleons and quarks. Nuclear chemists and physicists work together at particle accelerators to discover the presence of these tiny, tiny, tiny pieces of matter. Even though super-tiny atomic particles exist, you only need to remember the three basic parts of an atom: electrons, protons, and neutrons. What are electrons, protons, and neutrons? A picture works best to show off the idea. You have a basic atom. There are three types of pieces in that atom: electrons, protons, and neutrons. That's all you have to remember. Three things! As you know, there are almost 120 known elements in the periodic table. Chemists and physicists haven't stopped there. They are trying to make new ones in labs every day. The thing that makes each of those elements different is the number of electrons, protons, and neutrons. The protons and neutrons are always in the center of the atom. Scientists call the center region of the atom the nucleus. The nucleus in a cell is a thing. The nucleus in an atom is a place where you find protons and neutrons. The electrons are always found whizzing around the center in areas called shells or orbitals. You can also see that each piece has either a "+", "-", or a "0." That symbol refers to the charge of the particle. Have you ever heard about getting a shock from a socket, static electricity, or lightning? Those are all different types of electric charges. Those charges are also found in tiny particles of matter. The electron always has a "-", or negative, charge. The proton always has a "+", or positive, charge. If the charge of an entire atom is "0", or neutral, there are equal numbers of positive and negative pieces. Neutral means there are equal numbers of electrons and protons. The third particle is the neutron. It has a neutral charge, also known as a charge of zero. All atoms have equal numbers of protons and electrons so that they are neutral. If there are more positive protons or negative electrons in an atom, you have a special atom called an ion.
Page 1 and 2: 2016-17 CHEMISTRY NOTEBOOK - LEONAR
Page 3 and 4: Unit 1 Measurement Lab Separation o
Page 5 and 6: Unit 5 (28 days) Chapter 10 Chemica
Page 7 and 8: 30. Always lubricate glassware (tub
Page 10 and 11: 8 Chapter 1 Unit 1 Introduction to
Page 13 and 14: To use the Stair-Step method, find
Page 15 and 16: Using SI Units Match the terms in C
Page 17 and 18: Standards of Measurement Fill in th
Page 19 and 20: SCIENTIFIC NOTATION RULES How to Wr
Page 21 and 22: Convert each number from Scientific
Page 23 and 24: Significant Figures Rules There are
Page 25 and 26: How Many Significant Digits for Eac
Page 27 and 28: The following rule applies for mult
Page 29 and 30: 1qt=32 oz 1gal = 4qts 1.00 qt = 946
Page 31: Chapter 5 Electrons in Atoms The st
Page 35 and 36: Electrovalence Don't get worried ab
Page 37 and 38: Summary Atoms make up all matter, a
Page 39 and 40: Electron Configuration Color the su
Page 41 and 42: Electron Configuration In order to
Page 43 and 44: Calcium [Ca] Nickel [Ni] Carbon [C]
Page 45 and 46: Research the Scientist and summariz
Page 47 and 48: Using Wikipedia, define the 8 categ
Page 49 and 50: Ionization Energy Define Ionization
Page 51 and 52: Ion Size Define Ion Size: Explanati
Page 53 and 54: 51 Chapter 7 Ionic and Metallic Bon
Page 55 and 56: 53 10. Name _______________________
Page 57 and 58: The Nucleus A typical model of the
Page 59 and 60: 57 Gamma Radiation After a decay re
Page 61 and 62: This analysis shows that sodium has
Page 63 and 64: 61 Metals, with only a few electron
Page 65 and 66: POLAR BONDING results when two diff
Page 67 and 68: Step 6 Put the atoms in the structu
Page 69 and 70: Trigonal Planar Molecular Geometry
Page 71 and 72: Tetrahedral Molecular Geometry Orbi
Page 73 and 74: 71 Bent Molecular Geometry Orbital
Page 75 and 76: 73 T-Shaped Molecular Geometry Orbi
Page 77 and 78: 75 Square Planar Molecular Geometry
Page 79 and 80: Name Formula Charge Dichromate Cr
Page 81 and 82: Chapter 23 Functional Groups The st
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81
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Chapter 12 Stoichiometry The studen
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www.youtube.com/watch?v=BTRm8PwcZ3U
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87 4) Double displacement: This is
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89 Determine the Type of Reaction f
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91 Step 3 Always leave hydrogen and
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1) ___ 2 NaNO3 + ___ PbO ___ Pb(NO
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1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2
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we can determine that 2 moles of HC
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When there is no limiting reagent b
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Example 7 How much 5M stock solutio
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Theoretical and Actual Yields Key T
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Review Purposes To get an over
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Moles to Mass: (*in a balanced equa
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Chapter 14 The Behavior of Gases Th
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Connection: This is why when liquid
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Name: Leonardo Gutierrez Name: Joel
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As pressure increases, volume must
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Constant Volume and Mass Pressure i
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119
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121
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Ideal Gas Law: To figure out how ma
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collide into it. This process of th
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Create and interpret potential ener
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Part 1: Mass Percent Mass percent (
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Glossary Concentration: Amount of d
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Specific Heat Here is the definitio
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Step One: solid ice rises in temper
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Step Three: liquid water rises in t
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Step Five: steam rises in temperatu
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then it is exothermic, meaning the
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*Catalysts increase the rate of rea
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9 H2O2, hydrogen peroxide, naturall
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* When a decrease in pressure happe
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Reduction Oxidation reduction react
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So far, the properties have an obvi
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The acid base theory of Brønsted a
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IV. Problems with the Theory This t
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Let's discuss significant figures a
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On your calculator you would input
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Reference Tables for Physical Setti
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150. 140. Table G Solubility Curves
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Table I Heats of Reaction at 101.3
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Table O Symbols Used in Nuclear Che
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0 6.941 +1 Li 3 2-1 Na 39.0983 K +1
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First Atomic Symbol Name Ionization
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Collier County CHEMISTRY EXAM FORMU
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CHEMISTRY EXAM FORMULA AND RESOURCE
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(FINAL) Chemistry Notebook 2016-17

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