oxygen is acting as an oxidizing agent in all of the following reactions except\na.\n2 c(s) + o_2(g) → 2…

oxygen is acting as an oxidizing agent in all of the following reactions except\na.\n2 c(s) + o_2(g) → 2 co(g)\nb.\ns(s) + o_2(g) → so_2(g)\nc.\n2 f_2(g) + o_2(g) → 2 of_2(g)\nd.\n2 na(s) + o_2(g) → na_2o_2(s)\ne.\n2 mg(s) + o_2(g) → 2 mgo(s)

oxygen is acting as an oxidizing agent in all of the following reactions except\na.\n2 c(s) + o_2(g) → 2 co(g)\nb.\ns(s) + o_2(g) → so_2(g)\nc.\n2 f_2(g) + o_2(g) → 2 of_2(g)\nd.\n2 na(s) + o_2(g) → na_2o_2(s)\ne.\n2 mg(s) + o_2(g) → 2 mgo(s)

Answer

Explanation:

Step 1: Define oxidizing agent

An oxidizing agent is a substance that gains electrons (is reduced) in a chemical reaction, causing another substance to be oxidized.

Step 2: Analyze oxidation states in A, B, D, E

In reactions A, B, D, and E, oxygen starts with an oxidation state of $0$ in $O_2$ and ends with a negative oxidation state ($-2$ in $CO$, $SO_2$, $MgO$; $-1$ in $Na_2O_2$). Since oxygen's oxidation state decreases, it is reduced and acts as an oxidizing agent.

Step 3: Analyze oxidation state in C

In reaction $2 F_2(g) + O_2(g) \rightarrow 2 OF_2(g)$, fluorine is more electronegative than oxygen. Fluorine takes an oxidation state of $-1$, forcing oxygen to have an oxidation state of $+2$. Since oxygen's oxidation state increases from $0$ to $+2$, oxygen is oxidized, meaning it acts as a reducing agent, not an oxidizing agent.

Answer:

C. $2 F_2(g) + O_2(g) \rightarrow 2 OF_2(g)$