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1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2) 6 AgI + Fe2(CO3)3 2 FeI3 + 3 Ag2CO3 3) C2H4O2 + 2 O2 2 CO2 + 2 H2O 4) ZnSO4 + Li2CO3 ZnCO3 + Li2SO4 5) V2O5 + 5 CaS 5 CaO + V2S5 6) Mn(NO2)2 + BeCl2 Be(NO2)2 + MnCl2 7) 3 AgBr + GaPO4 Ag3PO4 + GaBr3 8) 3 H2SO4 + 2 B(OH)3 B2(SO4)3 + 6 H2O 9) S8 + 8 O2 8 SO2 10) Fe + 2 AgNO3 Fe(NO3)2 + 2 Ag Additional Notes: -When you take inventory, make sure everything that is the same is on the same line -if you have an isolated element, leave it to the end -you may need to use the least common multiple if the product and reactant cannot be the same without it -if you are unable to multiply it by a whole number, then use a fraction and then multiply it so that it becomes a whole number and change the coefficients -the number of atoms that are present in the reactants has to balance the number of atoms that are present in the products. Steps: 1. Write down the equations and underneath of the reactants write the elements and how many there are. Repeat that on the products side 2. look at the different amount of elemnets on each side and then place the number in the equation that will make both sides equal 3. repeat for the elements until each element is the same on both the product and reactant side 4. rewrite the correct equation - coefficient and subscripts are multiplied to find the amount of a certain element 101
The Learning Goal for this assignment is: Characterize types of chemical reactions, for example: redox, acid-base, synthesis, and single and double replacement reactions. Categories of Reactions All chemical reactions can be placed into one of six categories. Here they are, in no particular order: 1) Synthesis: A synthesis reaction is when two or more simple compounds combine to form a more complicated one. These reactions come in the general form of: One example of a synthesis reaction is the combination of iron and sulfur to form iron (II) sulfide: 8 Fe + S8 ---> 8 FeS If two elements or very simple molecules combine with each other, it’s probably a synthesis reaction. The products will probably be predictable using the octet rule to find charges. 2) Decomposition: A decomposition reaction is the opposite of a synthesis reaction - a complex molecule breaks down to make simpler ones. These reactions come in the general form: One example of a decomposition reaction is the electrolysis of water to make oxygen and hydrogen gas: 2 H2O ---> 2 H2 + O2 If one compound has an arrow coming off of it, it’s probably a decomposition reaction. The products will either be a couple of very simple molecules, or some elements, or both. 3) Single displacement: This is when one element trades places with another element in a compound. These reactions come in the general form of: A will either be a positive metal or a negative nonmetal depending on which letter it is replacing One example of a single displacement reaction is when magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas: or Positive letter comes first Mg + 2 H2O ---> Mg(OH)2 + H2 If a pure element reacts with another compound (usually, but not always, ionic), it’s probably a single displacement reaction. The products will be the compounds formed when the pure element switches places with another element in the other compound. Important note: these reactions will only occur if the pure element on the reactant side of the equation is higher on the activity series than the element it replaces. 102
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Powered by TCPDF (www.tcpdf.org) Ed
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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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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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Print vs. print Online vs. online P
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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 6 The Periodic Table The st
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Atoms Are Building Blocks Atoms are
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Electrovalence Don't get worried ab
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Summary 35
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Research the Scientist and summariz
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Electron Configuration Color the su
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Electron Configuration In order to
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10. Name __________________________
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Using Wikipedia, define the 8 categ
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Ionization Energy Define Ionization
Page 71 and 72: Ion Size Define Ion Size: the size
Page 73 and 74: The Nucleus A typical model of the
Page 75 and 76: Gamma Radiation After a decay react
Page 77 and 78: Nuclear Fission The word fusion mea
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Page 81 and 82: This analysis shows that sodium has
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Page 85 and 86: 1 2 3 4 5 6 Name of Cation Calcium
Page 87 and 88: POLAR BONDING results when two diff
Page 89 and 90: Step 6 Put the atoms in the structu
Page 91: Orbitals Equation Lone Pairs Angle
Page 94 and 95: Carbon Dioxide Chemical Name CO2 Ch
Page 96 and 97: Hydronium Chemical Name H3O+ Chemic
Page 98 and 99: Sulfur Hexaflouride Chemical Name S
Page 100 and 101: Bent: They look, well, bent. Bond a
Page 102 and 103: 4. the chlorine atom in hydrochlori
Page 104 and 105: Chapter 23 Functional Groups The st
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Page 108 and 109: anched chains: Hexane - a 6-carbon
Page 110 and 111: Isomers Because carbon can bond in
Page 112 and 113: Chapter 12 Stoichiometry The studen
Page 114 and 115: Other atomic weights are listed on
Page 116 and 117: Find Molecular Mass 1- 10 1. NaBr N
Page 118 and 119: Step 3 Always leave hydrogen and ox
Page 120 and 121: 1) ___ 2 NaNO3 + ___ 1 PbO ___ 1 P
Page 124 and 125: 4) Double displacement: This is whe
Page 126 and 127: Determine the Type of Reaction for
Page 128 and 129: Volume to Volume Conversions: the a
Page 130 and 131: we can determine that 2 moles of HC
Page 132 and 133: 111 When there is no limiting reage
Page 134 and 135: Example 7 How much 5M stock solutio
Page 136 and 137: Theoretical and Actual Yields Key T
Page 138 and 139: Review Purposes To get an over
Page 140 and 141: Chapter 14 The Behavior of Gases Th
Page 142 and 143: The learning goal for this assignme
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Page 148 and 149: 3. The pressure of nitrogen gas in
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Page 152 and 153: Hydrates the water contained in a c
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Page 158 and 159: Specific Heat Here is the definitio
Page 160 and 161: 139 Step One: solid ice rises in te
Page 162 and 163: 141 Step Three: liquid water rises
Page 164 and 165: Step Five: steam rises in temperatu
Page 166 and 167: 145 then it is exothermic, meaning
Page 168 and 169: 147 Define the types of reactions.
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151 1. In what part of the curve wo
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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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