Question

oxygen is acting as an oxidizing agent in all of the following reactions excepta. \\(2 c(s) + o_2(g) \
ightarrow 2 co(g)\\)b. \\(s(s) + o_2(g) \
ightarrow so_2(g)\\)c. \\(2 f_2(g) + o_2(g) \
ightarrow 2 of_2(g)\\)d. \\(2 na(s) + o_2(g) \
ightarrow na_2o_2(s)\\)e. \\(2 mg(s) + o_2(g) \
ightarrow 2 mgo(s)\\)

Explanation:

To determine when oxygen is not an oxidizing agent, we analyze the oxidation state of oxygen in each reaction:

• Option A: In \(O_2\) (oxidation state = 0), in \(CO\), O has oxidation state -2. Oxygen is reduced (gains electrons), so it is an oxidizing agent.
• Option B: In \(O_2\) (0), in \(SO_2\), O has -2. Oxygen is reduced, so it is an oxidizing agent.
• Option C: In \(O_2\) (0), in \(OF_2\), O has +2 (since F is -1, and \(2\times(-1)+x = 0\) gives \(x = +2\)). Oxygen is oxidized (loses electrons), so it is a reducing agent, not an oxidizing agent.
• Option D: In \(O_2\) (0), in \(Na_2O_2\), O has -1. Oxygen is reduced, so it is an oxidizing agent.
• Option E: In \(O_2\) (0), in \(MgO\), O has -2. Oxygen is reduced, so it is an oxidizing agent.

Only in Option C, oxygen is oxidized (acts as a reducing agent), so it is not acting as an oxidizing agent here.

Answer:

C. \(2 F_2(g) + O_2(g)
ightarrow 2 OF_2(g)\)