Qrtr 4 final

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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¯ 4. Cr in Cr2O7 2¯ 5. Fe in Fe2O3 6. Pb in PbOH + 7. V in VO2 + 8. V in VO 2+ 9. Mn in MnO4¯ 10. Mn in MnO4 2¯ Notes:
7. Half Reactions A half-reaction is simply one which shows either reduction OR oxidation, but not both. Here is the example redox reaction used in a different file: Ag + + Cu → Ag + Cu 2+ It has BOTH a reduction and an oxidation in it. That is why we call it a redox reaction, from REDuction and OXidation. What you must be able to do is look at a redox reaction and separate out the two half-reactions in it. To do that, identify the atoms which get reduced and get oxidized. Here are the two half-reactions from the above example: Ag+ → Ag Cu → Cu 2+ The silver is being reduced, its oxidation number going from +1 to zero. The copper's oxidation number went from zero to +2, so it was oxidized in the reaction. In order to figure out the halfreactions, you MUST be able to calculate the oxidation number of an atom. Keep in mind that a half-reaction shows only one of the two behaviors we are studying. A single halfreaction will show ONLY reduction or ONLY oxidation, never both in the same equation. Also, notice that the reaction is read from left to right to determine if it is reduction or oxidation. If you read the reaction in the opposite direction (from right to left) it then becomes the other of our two choices (reduction or oxidation). For example, the silver half-reaction above is a reduction, but in the reverse direction it is an oxidation, going from zero on the right to +1 on the left. There will be times when you want to switch a half-reaction from one of the two types to the other. In that case, rewrite the entire equation and swap sides for everything involved. If I needed the silver half-reaction to be oxidation, I'd write Ag → Ag+ rather than just doing it mentally. The next step is that both half-reactions must be balanced. However, there is a twist. When you learned about balancing equation, you made equal the number of atoms of each element on each side of the arrow. That still applies, but there is one more thing: the total amount of charge on each side of the half-reaction MUST be the same. When you look at the two half-reactions above, you will see they are already balanced for atoms with one Ag on each side and one Cu on each side. So, all we need to do is balance the charge. To do this you add electrons to the more positive side. You add enough to make the total charge on each side become EQUAL. To the silver half-reaction, we add one electron: To the copper half-reaction, we add two electrons: Ag+ + e¯ ---> Ag Cu ---> Cu 2+ + 2e¯
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Alexandra’s Chemistry Notebook
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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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9 Print vs. print Online vs. online
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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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17 SCIENTIFIC NOTATION RULES How to
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19 Convert each number from Scienti
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21 Significant Figures Rules There
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23 How Many Significant Digits for
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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 35
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Electron Configuration Color the su
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Electron Configuration In order to
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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: The trans
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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 Planar Molecular Geometry
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Tetrahedral Orbital Equation Lone P
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Orbital Equation Lone Pairs Angle S
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T Shaped Orbital Equation Lone Pair
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Square Planar Orbital Equation Lone
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Name Formula Charge Dichromate Cr
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Chapter 23 Functional Groups The st
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31
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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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For these problems, you start of li
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Page 115 and 116: Name: Alexandra M Name: Alexa B Gra
Page 117 and 118: 2 * 3 = 3 * 2 solve for this side P
Page 119: 8 = 4 8 4 Must be constant volume!
Page 124 and 125: Combined Gas Law- The combined g
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Page 136 and 137: The Time-Temperature Graph We are g
Page 138 and 139: Step Two: solid ice melts Now, we c
Page 140 and 141: Step Four: liquid water boils Now,
Page 142 and 143: The following table summarizes the
Page 144 and 145: The Learning Goal for this section
Page 146 and 147: C 6 H 6 + Br 2
Page 148 and 149: 11 In which of the following reacti
Page 150 and 151: The Learning Goal for this section
Page 152 and 153: This would be a generic base: XOH -
Page 154 and 155: HCl + H2O ⇌ H3O + + Cl¯ HCl - th
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Page 158 and 159: 1. 2.82 2. 8.30 3. 0.00 4. 3.485 5.
Page 164 and 165: One point of concern: notice that e
Page 166 and 167: Reference Tables for Physical Setti
Page 168 and 169: 150. 140. Table G Solubility Curves
Page 170 and 171: Table I Heats of Reaction at 101.3
Page 172 and 173: Table O Symbols Used in Nuclear Che
Page 174 and 175: 0 6.941 +1 Li 3 2-1 Na 39.0983 K +1
Page 176 and 177: First Atomic Symbol Name Ionization
Page 178 and 179: Collier County CHEMISTRY EXAM FORMU
Page 180 and 181: CHEMISTRY EXAM FORMULA AND RESOURCE
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