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. 2C1₂(g) + Sn(s) - SnCl (s) redox reaction? O yes reducing 0 agent: oxidizing agent: 0 redox reaction? no X Do S

In the following reaction, what species is the reducing agent?: Ca + Br2 --> CaBr2 Са Br2 This not an oxidation-reduction reaction

y If an ion consists of a single atom, what is the value of the oxidation number of the atom? O smaller than the charge of the ion о O zero equal to the charge of the ion bigger than the charge of the ion -- Fo Search FB & C F9 F10 Ra D F11 ) F12 G Del

Assign oxidation states to all of the species in the following redox reaction. For the reactants, also identify electron loss or gain, the species oxidized, the species reduced, the oxidizing agent and the reducing agent. Oxidation state Electron gain/loss Oxidized or reduced Reducing or oxidizing agent Mg(s) ♥ ↑ ↑ ♥ + Hg²+ (aq) ♥ ↑ ↑ ♥ Mg2+ (aq) + Hg(1) ◊ Total number of electrons transferred from the reducing agent to the oxidizing agent for the equation given is:

Equation Number Balanced Equation 1 2 ZnS(s) + 3 O,(g) 2 ZnO(s) + 2 S0,(g) Ag*(aq) + Br¯(aq) 10 H*(aq) + SO (aq) + 8 I¬(aq) → AgBr(s) 3 4 L, (s) + H, S(g) + 4 H, O(1) Classify each reactant in the chemical equations as an oxidizing agent, a reducing agent, or neither. Oxidizing agent Reducing agent Neither Answer Bank SO Ag* Br ZnS H+

3 N2O4 (g) + 2 Al (s) → 6 NO2–(aq) + 2 Al3+(aq)In the reaction above what substance is being reduced?     Al (s)     Al3+(aq)     N2O4 (g)     NO2–(aq)