Which is an oxidising as well as a reducing agent in the following?

Options

A. `Na_(2)O_(2)`
B. `Na_(2)O`
C. `SnCl_(4)`
D. `NaNO_(2)`

Answer

To determine which compound acts as both an oxidizing and a reducing agent among the given options, we need to analyze the oxidation states of the elements in each compound.

### Step-by-Step Solution:

1. **Identify the Compounds**: The compounds given are:
- Na2O2 (Sodium peroxide)
- Na2O (Sodium oxide)
- SnCl4 (Tin(IV) chloride)
- NaNO2 (Sodium nitrite)

2. **Analyze Na2O2**:
- Sodium (Na) has an oxidation state of +1.
- Oxygen (O) in peroxides has an oxidation state of -1.
- The oxidation state of Na2O2 can be calculated as follows:
\[ 2x + 2(-1) = 0 \implies 2x - 2 = 0 \implies 2x = 2 \implies x = +1 \]
- Since Na cannot increase its oxidation state beyond +1, Na2O2 cannot act as both an oxidizing and reducing agent.

3. **Analyze Na2O**:
- Sodium (Na) has an oxidation state of +1.
- Oxygen (O) has an oxidation state of -2.
- The calculation is:
\[ 2x + (-2) = 0 \implies 2x - 2 = 0 \implies 2x = 2 \implies x = +1 \]
- Similar to Na2O2, Na2O cannot act as both an oxidizing and reducing agent.

4. **Analyze SnCl4**:
- Tin (Sn) has an oxidation state of +4.
- Chlorine (Cl) has an oxidation state of -1.
- The calculation is:
\[ x + 4(-1) = 0 \implies x - 4 = 0 \implies x = +4 \]
- SnCl4 can act as an oxidizing agent because it can accept electrons, but it cannot act as a reducing agent.

5. **Analyze NaNO2**:
- Sodium (Na) has an oxidation state of +1.
- Nitrogen (N) in NaNO2 has an oxidation state of +3.
- Oxygen (O) has an oxidation state of -2.
- The calculation is:
\[ +1 + x + 2(-2) = 0 \implies 1 + x - 4 = 0 \implies x - 3 = 0 \implies x = +3 \]
- Since nitrogen is in an intermediate oxidation state (+3), NaNO2 can act as both an oxidizing agent (by accepting electrons) and a reducing agent (by donating electrons).

6. **Conclusion**:
- Among the given options, NaNO2 is the compound that acts as both an oxidizing and a reducing agent.

### Final Answer:
NaNO2 (Sodium nitrite) acts as both an oxidizing and a reducing agent.