First, assign oxidation numbers for each atom in the balanced chemical equation below. You'll find it easiest to fill the blanks in left to right since once there is an oxidation number typed in the blank it will be much closer to appearing over the appropriate elemental symbol. Blank 1 Blank 2Blank 3 12Blank 13 Blank 4Blank 5Blank 6 Blank 14Blank 15Blank 16 KMnO4(aq) + KCIO₂(aq) + H₂O(l) → 4 MnO₂(s) + 3 KCIO4(aq) + 4 KOH(aq) Now, identify each of the following • What underwent reduction? Blank 17 Blank 7Blank 8 • What gained electrons? Blank 18 • What got oxidized? Blank 19 • What is the oxidizing agent? Blank 20 • What is the reducer? Blank 21 What lost electrons? Blank 22 Blank 9Blank 10 Blank 11Blank

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Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. S₂ (s) + 4Pb (s) 4PbS₂ (s) 70₂(g) + 2CH₂CH₂(g) → 4CO₂(g) + 611₂0 (g) 3 HSO (aq) + OH¯(aq) → SO² (aq) + H₂0 (1) redox reaction? yes reducing agent: oxidizing 0 agent: redox reaction? yes reducing agent: oxidizing agent: 0 redox reaction? yes reducing agent: oxidizing □ agent: no no no X Ś

Specify which of the following are oxidation-reduction reactions, and if it is, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. If it is not, select No and leave the following boxes blank. Express your answers as chemical formulas. Omit states-of-matter. a. CH4 (9) + H2 O(g) → CO(9) + 3H2 (9) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes v b. 2AGNO3 (ag) + Zn(s) → Zn(NO3)2 (aq) + 2Ag(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced No v