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 (oxidation state decreases), so it acts as an oxidizing agent.
• Option B: In \(O_2\) (0), in \(SO_2\), O is -2. Oxygen is reduced, so it is an oxidizing agent.
• Option C: In \(O_2\) (0), in \(OF_2\), O has an oxidation state of +2 (since F is -1, and \(2\times(-1)+x = 0\) gives \(x = +2\)). Here, oxygen's oxidation state increases (from 0 to +2), so it is oxidized. Thus, \(O_2\) is acting as a reducing agent, not an oxidizing agent.
• Option D: In \(O_2\) (0), in \(Na_2O_2\), O has an oxidation state of -1. Oxygen is reduced, so it is an oxidizing agent.
• Option E: In \(O_2\) (0), in \(MgO\), O is -2. Oxygen is reduced, so it is an oxidizing agent.

Answer:

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