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Chapter 12 Stoichiometry The students will learn how balanced chemical equations are used in stoichiometric calculations and how to calculate amounts of reactants and products in a chemical equation. Apply the mole concept and the law of conservation of mass to calculate quantities of chemicals participating in reactions. Students will be able to use a balanced equation to determine mole ratios. Students will be able to apply law of conservation of mass to chemical equations. Students will be able to calculate empirical and molecular formulas. Students will be able to calculate the % composition of a compound. Students will be able to calculate theoretical yield. Students will be able to calculate % error. Students will be able to calculate molar mass. Students will be able to perform stoichiometric calculations, including limiting reagents. mole Avogadro’ s number molar mass gram formula mass 83
www.youtube.com/watch?v=AsqEkF7hcII www.youtube.com/watch?v=tEn0N4R2dqA www.youtube.com/watch?v=Pft2CASl0M0 www.youtube.com/watch?v=rwhJklbK8R0 The Mole What is a mole? A mole is a quantity of atoms represented by the number 23 6.02 x 10 also known as Avogadro's number. 12 A mole is equivalent to number of C atoms in 12g of Carbon A mole of an element contains its number of AMUs represented in grams. 12 12 (i.e. 1 mole of C = 12g of C) Coefficients in chemical equations/reactions represents the number of moles of a molecule. The mole is a bridge between the number of particles and the mass of something A mole ratio is the coefficient (or the number of moles) of a molecule to other molecules in an equation (i.e. Cu + 2AgNO = 2Ag + Cu(NO ) Ratio: 1 Cu/2AgNO etc.) 3 3 2 3 84
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Chemistry Notebook By: Joel J
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Unit 1 Measurement Lab Separation o
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Unit 5 (28 days) Chapter 10 Chemica
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30. Always lubricate glassware (tub
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Chapter 1 Unit 1 Introduction to Ch
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To use the Stair-Step method, find
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Using SI Units Match the terms in C
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Standards of Measurement Fill in th
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SCIENTIFIC NOTATION RULES How to Wr
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Convert each number from Scientific
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Significant Figures Rules There are
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How Many Significant Digits for Eac
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The following rule applies for mult
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1qt=32 oz 1gal = 4qts 1.00 qt = 946
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Chapter 5 Electrons in Atoms The st
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Atoms Are Building Blocks Atoms are
Page 35 and 36: Electrovalence Don't get worried ab
Page 37 and 38: Summary Atoms are essentially the b
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: Ion 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 Planal Molecular Geometry
Page 71 and 72: Tetrahedral Molecular Geometry Orbi
Page 73 and 74: Bent Molecular Geometry Orbital Equ
Page 75 and 76: T-Shaped Molecular Geometry Orbital
Page 77 and 78: Square Planar Molecular Geometry Or
Page 79 and 80: sp 3 d 2 AX6 None 90 Octahedral sp
Page 81 and 82: Chapter 9 Unit 4 Chemical Names and
Page 83 and 84: Learning Goals: Describe the proper
Page 85: Unit 5 Chapter 10 Chemical Quantiti
Page 89 and 90: Categories of Reactions All chemica
Page 91 and 92: List what type the following reacti
Page 93 and 94: How to Balance Chemical Equations A
Page 95 and 96: Step 5 Balance the hydrogen atoms n
Page 97 and 98: 6) ___ Mn(NO2)2 + ___ BeCl2 ___ Be
Page 99 and 100: The Learning Goal for this assignme
Page 101 and 102: Stoichiometry and Balanced Equation
Page 103 and 104: Step 1: 200g C3H8 is equal to 4.54
Page 105 and 106: Stoichiometry and balanced equation
Page 107 and 108: %yield = 6.1 tons × 100 = 64% 9.6t
Page 109 and 110: Use the space provided to write out
Page 111 and 112: Unit 6 Chapter 13 States of Matter
Page 115 and 116: uniform internal structure, and amo
Page 117 and 118: Volume Pressure Temperature is Aver
Page 119 and 120: Volume and temperature (in Kelvins)
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Page 123 and 124: 120
Page 125 and 126: Combined Gas Law: This gas law comb
Page 129 and 130: Unit 7 Chapter 16 Solutions The stu
Page 133 and 134: Part 5: Molarity Molarity (M) is th
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The Time-Temperature Graph We are g
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Step Two: solid ice melts Now, we c
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Step Four: liquid water boils Now,
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The following table summarizes the
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The Learning Goal for this section
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B. decreasing the concentration of
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everse reaction rate as well. 11. I
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Unit 8 Chapter 19 Acid and Bases Th
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The Learning Goal for this section
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This would be a generic base: XOH -
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HCl + H2O ⇌ H3O + + Cl¯ HCl - th
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Several categories of substances ca
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1. 2.82 2. 8.30 3. 0.00 4. 3.485 5.
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The Learning Goal for this assignme
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2. What is the oxidation number of
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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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