which of the folowing is the strongest oxidizing agent?

Options

A. `N_(2)O`
B. NO
C. `NO_(2)`
D. `N_(2)O_(5)`

Answer

To determine which of the following compounds is the strongest oxidizing agent among N2O, NO, NO2, and N2O5, we will analyze the oxidation states of nitrogen in each compound and their implications for oxidizing and reducing behavior.

### Step-by-Step Solution:

**Step 1: Calculate the oxidation state of nitrogen in each compound.**

1. **For N2O:**
- The equation is: \(2N + (-2) = 0\)
- Solving gives: \(2N = +2\) → \(N = +1\)

2. **For NO:**
- The equation is: \(N + (-2) = 0\)
- Solving gives: \(N = +2\)

3. **For NO2:**
- The equation is: \(N + 2(-2) = 0\)
- Solving gives: \(N = +4\)

4. **For N2O5:**
- The equation is: \(2N + 5(-2) = 0\)
- Solving gives: \(2N = +10\) → \(N = +5\)

**Step 2: Summarize the oxidation states of nitrogen.**
- N2O: +1
- NO: +2
- NO2: +4
- N2O5: +5

**Step 3: Identify the maximum and minimum oxidation states of nitrogen.**
- The maximum oxidation state of nitrogen is +5 (in N2O5).
- The minimum oxidation state of nitrogen is -3 (not present in the given compounds).

**Step 4: Determine the oxidizing and reducing behavior of each compound.**
- A compound with a higher oxidation state can act as a stronger oxidizing agent because it can accept electrons and be reduced.
- N2O5 (with nitrogen in the +5 oxidation state) cannot be oxidized further, meaning it can only act as an oxidizing agent.
- The other compounds (N2O, NO, NO2) have lower oxidation states and can act as both oxidizing and reducing agents.

**Step 5: Conclusion.**
- Since N2O5 has the highest oxidation state of nitrogen (+5) and can only act as an oxidizing agent, it is the strongest oxidizing agent among the given options.

### Final Answer:
**N2O5 is the strongest oxidizing agent.**

---