Final Chemistry Notebook

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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: when your losing electrons your gaining oxidation numbers . Reduction is gaining elcectrons.If somrething is reeducing itself its going from a higher oxidation number to a lower. Reducing oxidation agent. 5. Some Definitions 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). 165
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 +5 6 1. N in NO3¯ +4 2. C in CO3 2¯ -6 3. Cr in CrO4 2¯ 4. Cr in Cr2O7 2¯ N=+5 c=+4 +6 -8 Cr= +6 +6 -14 Cr=+6 5. Fe in Fe2O3 6. Pb in PbOH + +5 +6 -2 -4 7. V in VO2 + -6 +1 8. V in VO 2+ 9. Mn in MnO4¯ Fe=+3 Pb=+2 V=+5 v=+4 mn=+7 10. Mn in MnO4 2¯ mn=+6 Notes: Oxidation and reduction reactions are reactions that in which electrons are lost by an atom or ion in one reactant and also gained by an atom in another reactant. Even though electrons are gained and lost in these reactions, the balanced equation for a redox reaction does not show the electrons that are being transferred because they are being cancled out to become stable. In order to tell whether a redox reaction has occurred or if it has not , we need a way to keep track of electrons. The best way to do so is by assigning oxidation numbers to the atoms or ions involved in a chemical reaction and seeing if the reaction is oxidation or reduction by identifying if the reaction is increasinf or decreasing. If its increasing its oxidation . While if its losing or decreasing its Reduction 166
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. Chemistry Honors Notebook 2017-20
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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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7
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Print vs. print Online vs. online P
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11 To use the Stair-Step method, fi
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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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25 The following rule applies for m
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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 Atoms are the most importan
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Research the Scientist and summariz
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39 Electron Configuration Color the
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Electron Configuration In order to
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Ca= Calcium Ni=nickel C=carbon Xe=x
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10. Name __________________________
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Using Wikipedia, define the 8 categ
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Define Ionization Energy: Ionizatio
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51 Define Ion Size: Ion Size Ion si
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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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Nuclear Fission The word fusion mea
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Students will be able to predict sh
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electrons in the outer energy level
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Non-metals, which lack only one or
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AlCl3+ HgI2 But remember to look ba
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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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Orbitals Equation Lone Pairs Angle
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Carbon dioxide Chemical Name CO 2 C
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Hydronium Chemical Name H 3 O + Che
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Sulfur hexafluoride Chemical Name S
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Bent: They look, well, bent. Bond a
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4. the chlorine atom in hydrochlori
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Chapter 23 Functional Groups The st
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anched chains: Hexane - a 6-carbon
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Isomers Because carbon can bond in
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Chapter 12 Stoichiometry The studen
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Other atomic weights are listed on
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Find Molecular Mass 1- 10 1. NaBr N
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Right side: 1 carbon, 2 hydrogen an
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Add a coefficient of 5 to the oxyge
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1) 2 NaNO3 + PbO Pb(NO3)2 + Na2O 2
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4) Double displacement: This is whe
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Decomposition ab=>A+B Determine the
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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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Page 138 and 139: STP-Standard Temperature And Pressu
Page 140 and 141: Chapter 14 The Behavior of Gases Th
Page 142 and 143: CORNELL NOTES Learning Goal: Differ
Page 144 and 145: Questions/Main Ideas NOTES 13.4 cha
Page 146 and 147: It is important that you realize th
Page 148 and 149: 127 3. The pressure of nitrogen gas
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Page 152 and 153: dissolved in water. All electrolyte
Page 154 and 155: Create and interpret potential ener
Page 156 and 157: Structure effects: determines what
Page 158 and 159: Specific Heat Here is the definitio
Page 160 and 161: Step One: solid ice rises in temper
Page 162 and 163: Step Three: liquid water rises in t
Page 164 and 165: Step Five: steam rises in temperatu
Page 166 and 167: then it is exothermic, meaning the
Page 168 and 169: Define the types of reactions. Give
Page 170 and 171: 1. If this compound was at room tem
Page 172 and 173: 1. In what part of the curve would
Page 174 and 175: Reduction Oxidation reduction react
Page 176 and 177: So far, the properties have an obvi
Page 178 and 179: The acid base theory of Brønsted a
Page 180 and 181: IV. Problems with the Theory This t
Page 182 and 183: Let's discuss significant figures a
Page 184 and 185: On your calculator you would input
Page 188 and 189: 7. Half Reactions A half-reaction i
Page 190: Notice that each separate substance
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