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Ag+ + Cu ---> Ag + Cu2+ I have deliberately not balanced it and I have also written it in net ionic form. I have found that kids studying redox get confused by net ionic form and how to change a full equation into net ionic form. Redox equations need to be balanced but, except for the simplest ones, it cannot be done by inspection (also called trial and error). I take that back, complex ones can be done by trial and error. It typically takes quite a bit of work, especially when compared to how long it takes when the proper technique is used. There is a technique used to balance redox reactions. It is called "balancing by half-reactions." The basic plan will be to split the full equation into two simpler parts (called half-reactions), balance them following several standard steps, then recombine the balanced half-reactions into the final answer. This is another technique called the "ion-electron method." I plan to ignore it. Notes: Positive Ion + Electron = Neutral Ion Negative Ion - Electron = Neutral Ion 5. Some Definitions Positive Ion + Electron(s) = Negative Ion Negative Ion - Electron (s) = Positive Ion Oxidizing Agent - that substance which oxidizes somebody else. It is reduced in the process. Reducing Agent - that substance which reduces somebody else. It is oxidized in the process. It helps me to remember these definitions by the opposite nature of what happens. By that, I mean the oxidizing agent gets reduced and the reducing agent gets oxidized. 6. Rules for Assigning Oxidation Numbers The Oxidation Number of an element corresponds to the number of electrons, e - , that an atom loses, gains, or appears to use when joining with other atoms in compounds. In determining the Oxidation Number of an atom, there are seven guidelines to follow: 1. The Oxidation Number of an individual atom is 0. This includes diatomic elements such as O2 or others like P4 and S8 2. The total Oxidation Number of all atoms in: a neutral species is 0 and in an ion is equal to the ion charge. 3. Group 1 metals have an Oxidation Number of +1 and Group 2 an Oxidation Number of +2 4. The Oxidation Number of fluorine is -1 in compounds 5. Hydrogen generally has an Oxidation Number of +1 in compounds, except hydrides 6. Oxygen generally has an Oxidation Number of -2 in compounds, except peroxides 7. In binary metal compounds, Group 17 elements have an Oxidation Number of -1, Group 16 of - 2, and Group 15 of -3. Note: The sum of the Oxidation Number s is equal to zero for neutral compounds and equal to the charge for polyatomic ion species. Now, some examples: 1. What is the oxidation number of Cl in HCl? Since H = +1, the Cl must be -1 (minus one). 161
2. What is the oxidation number of Na in Na2O? Since O = -2, the two Na must each be +1. 3. What is the oxidation number of Cl in ClO¯? The O is -2, but since a -1 must be left over, then the Cl is +1. 4. What is the oxidation number for each element in KMnO4? K = +1 because KCl exists. We know the Cl = -1 because HCl exists. O = -2 by definition Mn = +7. There are 4 oxygens for a total of -8, K is +1, so Mn must be the rest. 5. What is the oxidation number of S in SO4 2¯ O = -2. There are four oxygens for -8 total. Since -2 must be left over, the S must = +6. Please note that, if there is no charge indicated on a formula, the total charge is taken to be zero. Practice Problems Find oxidation numbers 1. N in NO3¯ 2. C in CO3 2¯ 3. Cr in CrO4 2¯ +5 +4 +6 4. Cr in Cr2O7 2¯ 5. Fe in Fe2O3 6. Pb in PbOH + +6 +3 +4 7. V in VO2 + 8. V in VO 2+ +5 4+ 9. Mn in MnO4¯ +7 10. Mn in MnO4 2¯ +6 Notes: O = 2- (unless w/ F [2+] or in a peroxide [1-]) H = 1+ (unless with metal, then it is 1-) Any uncombined element = 0 Monatomic ion = charge of ion Polyatomic ion = sum of oxidation #'s must equal charge Neutral compound = sum of oxidation #'s must equal 0 Group 1 = oxidation # is 1+ Group 2 = oxidation # is 2+ Al = oxidation # is 3+ Fluorine (F) = in a compound, oxidation # is always 1- Note: Most electronegative atom's oxidation # is the charge it would have if it were an ion. 162
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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
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Electrovalence Don't get worried ab
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Summary Atoms are essentially the b
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Electron Configuration Color the su
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Electron Configuration In order to
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Calcium (Ca) Nickel (Ni) Carbon (C)
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Research the Scientist and summariz
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Using Wikipedia, define the 8 categ
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Ionization Energy Define Ionization
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Ion Size Define Ion Size: Ion size
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Chapter 7 Ionic and Metallic Bondin
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10. Name __________________________
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The Nucleus A typical model of the
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Gamma Radiation After a decay react
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This analysis shows that sodium has
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Metals, with only a few electrons i
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POLAR BONDING results when two diff
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Step 6 Put the atoms in the structu
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Trigonal Planal Molecular Geometry
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Tetrahedral Molecular Geometry Orbi
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Bent Molecular Geometry Orbital Equ
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T-Shaped Molecular Geometry Orbital
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Square Planar Molecular Geometry Or
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sp 3 d 2 AX6 None 90 Octahedral sp
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Chapter 9 Unit 4 Chemical Names and
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Learning Goals: Describe the proper
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Unit 5 Chapter 10 Chemical Quantiti
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www.youtube.com/watch?v=AsqEkF7hcII
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Categories of Reactions All chemica
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List what type the following reacti
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How to Balance Chemical Equations A
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Step 5 Balance the hydrogen atoms n
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6) ___ Mn(NO2)2 + ___ BeCl2 ___ Be
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The Learning Goal for this assignme
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Stoichiometry and Balanced Equation
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Step 1: 200g C3H8 is equal to 4.54
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Stoichiometry and balanced equation
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%yield = 6.1 tons × 100 = 64% 9.6t
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Use the space provided to write out
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Unit 6 Chapter 13 States of Matter
Page 113 and 114: The Learning Goal for this assignme
Page 115 and 116: uniform internal structure, and amo
Page 117 and 118: Volume Pressure Temperature is Aver
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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
Page 137 and 138: The Time-Temperature Graph We are g
Page 139 and 140: Step Two: solid ice melts Now, we c
Page 141 and 142: Step Four: liquid water boils Now,
Page 143 and 144: The following table summarizes the
Page 145 and 146: The Learning Goal for this section
Page 147 and 148: B. decreasing the concentration of
Page 149 and 150: everse reaction rate as well. 11. I
Page 151 and 152: Unit 8 Chapter 19 Acid and Bases Th
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Page 155 and 156: This would be a generic base: XOH -
Page 157 and 158: HCl + H2O ⇌ H3O + + Cl¯ HCl - th
Page 159 and 160: Several categories of substances ca
Page 161 and 162: 1. 2.82 2. 8.30 3. 0.00 4. 3.485 5.
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Page 170 and 171: Table E Selected Polyatomic Ions Fo
Page 172 and 173: Table H Vapor Pressure of Four Liqu
Page 174 and 175: Table K Common Acids Table N Select
Page 176 and 177: Table R Organic Functional Groups C
Page 178 and 179: Table S Properties of Selected Elem
Page 180 and 181: Table T Important Formulas and Equa
Page 182 and 183: CHEMISTRY EXAM FORMULA AND RESOURCE
Page 184: Activity Series of Metals Name Symb
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