Viviana's Chemistry Notebook

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The Learning Goal for this assignment is: Notes Section: Question Sig Figs Question Add & Subtract Question Multiple & Divide 1 4 1 55.36 1 20,000 2 4 2 84.2 2 94 3 3 3 115.4 3 300 4 3 4 0.8 4 7 5 4 5 245.53 5 62 6 3 6 34.5 6 0.005 7 3 7 74.0 7 4,000 8 2 8 53.287 8 3,900,000 9 2 9 54.876 9 2 10 2 10 40.19 10 30,000,000 11 3 11 7.7 11 1,200 12 2 12 67.170 12 0.2 13 3 13 81.0 13 0.87 14 4 14 73.290 14 0.049 15 4 15 29.789 15 2,000 16 3 16 39.53 16 0.5 17 4 17 70.58 17 1.9 18 2 18 86.6 18 0.05 19 2 19 64.990 19 230 20 1 20 36.0 20 460,000
Significant Figures Rules There are three rules on determining how many significant figures are in a number: 1. Non-zero digits are always significant. 2. Any zeros between two significant digits are significant. 3. A final zero or trailing zeros in the DECIMAL PORTION ONLY are significant. Please remember that, in science, all numbers are based upon measurements (except for a very few that are defined). Since all measurements are uncertain, we must only use those numbers that are meaningful. Not all of the digits have meaning (significance) and, therefore, should not be written down. In science, only the numbers that have significance (derived from measurement) are written. Rule 1: Non-zero digits are always significant. If you measure something and the device you use (ruler, thermometer, triple-beam, balance, etc.) returns a number to you, then you have made a measurement decision and that ACT of measuring gives significance to that particular numeral (or digit) in the overall value you obtain. Hence a number like 46.78 would have four significant figures and 3.94 would have three. Rule 2: Any zeros between two significant digits are significant. Suppose you had a number like 409. By the first rule, the 4 and the 9 are significant. However, to make a measurement decision on the 4 (in the hundred's place) and the 9 (in the one's place), you HAD to have made a decision on the ten's place. The measurement scale for this number would have hundreds, tens, and ones marked. Like the following example: These are sometimes called "captured zeros." If a number has a decimal at the end (after the one’s place) then all digits (numbers) are significant and will be counted. In the following example the zeros are significant digits and highlighted in blue. 960. 70050.
Page 1 and 2: Viviana’s Chemistry Notebook
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: Chapter 1 Unit 1 Introduction to Ch
Page 12 and 13: Chapter 1 Benchmark: Determine appr
Page 14 and 15: 2. One cereal bar has a mass of 37
Page 16 and 17: 1. How many meters are in one kilom
Page 18 and 19: The Learning Goal for this assignme
Page 20 and 21: RULE #3: To add/subtract in scienti
Page 24 and 25: Rule 3: A final zero or trailing ze
Page 26 and 27: For addition and subtraction, look
Page 28 and 29: Dimensional Analysis This is a way
Page 30 and 31: Chapter 4 Unit 2 Atomic Structure T
Page 32 and 33: The Learning Goal for this assignme
Page 34 and 35: Looking at Ions We haven’t talked
Page 36 and 37: Neutron Madness We have already lea
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: The size
Page 53 and 54: Chapter 7 Ionic and Metallic Bondin
Page 55 and 56: 10. Name __________________________
Page 57 and 58: The Nucleus A typical model of the
Page 59 and 60: Gamma Radiation After a decay react
Page 61 and 62: This analysis shows that sodium has
Page 63 and 64: Metals, with only a few electrons i
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
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Bent Molecular Geometry Orbital Equ
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T- shaped Molecular Geometry Orbita
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Square Planar Molecular Geometry Or
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Name Formula Charge Dichromate Cr
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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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4) Double displacement: This is whe
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Determine the Type of Reaction for
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Step 3 Always leave hydrogen and ox
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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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Mole to mass: 1. Determine how many
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Chapter 14 The Behavior of Gases Th
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4) A Model of Liquids - The kinetic
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Name: Viviana Jimenez Name: Leeza L
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3 x 2 2 x 3 Notes: - The mass is th
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Notes: - As we increase the tempera
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KHDBDCM 1) 1 atmosphere = 760 torrs
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1) 108 kPa / 41 C = x / 22 C - turn
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Ideal Gas Law A physical law descri
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Electrolytes and Nonelectrolytes -
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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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Question 2: By adding a catalyst to
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It is not A, C, or D because it doe
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Question 13: The answer is C becaus
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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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Ag+ + Cu ---> Ag + Cu2+ I have deli
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7. Half Reactions A half-reaction i
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Notice that each separate substance
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Table E Selected Polyatomic Ions Fo
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Table H Vapor Pressure of Four Liqu
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Table K Common Acids Table N Select
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Table R Organic Functional Groups C
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Table S Properties of Selected Elem
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Table T Important Formulas and Equa
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CHEMISTRY EXAM FORMULA AND RESOURCE
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Activity Series of Metals Name Symb
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