Question

oxygen is acting as an oxidizing agent in all of the following reactions except
a.
$2 c(s) + o_2(g) \
ightarrow 2 co(g)$

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 \( \ce{O2} \) (oxidation state 0) to \( \ce{CO} \) (O is -2), oxygen gains electrons (reduced), so it is an oxidizing agent.
• Option B: In \( \ce{O2} \) (0) to \( \ce{SO2} \) (O is -2), oxygen gains electrons (reduced), so it is an oxidizing agent.
• Option C: In \( \ce{O2} \) (0) to \( \ce{OF2} \) (O is +2), oxygen loses electrons (oxidized), so it is a reducing agent (not an oxidizing agent).
• Option D: In \( \ce{O2} \) (0) to \( \ce{Na2O2} \) (O is -1), oxygen gains electrons (reduced), so it is an oxidizing agent.
• Option E: In \( \ce{O2} \) (0) to \( \ce{MgO} \) (O is -2), oxygen gains electrons (reduced), so it is an oxidizing agent.

Answer:

C. \( \ce{2 F2(g) + O2(g) → 2 OF2(g)} \)