STATEMENT-1 : `MnO_(2)` can act as an oxidizing agent as well as reducing agent.
STATEMENT-2 : Oxidation state of `MnO_(2)` lies between highest and lowest oxidation state.

Options

A. If both the statement are TRUE and STATEMENT -2 is the correct explanation of STATEMENT-1
B. If both the statement are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT- is 1 TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To solve the question, we need to analyze both statements regarding the compound MnO₂ and determine their validity.

### Step 1: Determine the oxidation state of manganese in MnO₂.
- The oxidation state of oxygen (O) is -2. In MnO₂, there are two oxygen atoms.
- Therefore, the total contribution of oxygen to the oxidation state is:
\[ 2 \times (-2) = -4 \]
- Let the oxidation state of manganese (Mn) be \( x \). The overall charge of the compound is neutral (0), so we can set up the equation:
\[ x + (-4) = 0 \]
\[ x = +4 \]
- Thus, the oxidation state of manganese in MnO₂ is +4.

### Step 2: Identify the highest and lowest oxidation states of manganese.
- The highest oxidation state of manganese is +7 (as seen in MnO₄⁻).
- The lowest oxidation state of manganese is 0 (as seen in elemental manganese).

### Step 3: Analyze the range of oxidation states.
- The oxidation state of manganese in MnO₂ (+4) lies between the highest (+7) and lowest (0) oxidation states.
- Therefore, the oxidation state of MnO₂ indeed lies between the highest and lowest oxidation states of manganese.

### Step 4: Determine the behavior of MnO₂ as an oxidizing and reducing agent.
- When manganese is in its highest oxidation state (+7), it can act as an oxidizing agent because it can accept electrons and reduce itself to a lower oxidation state.
- Conversely, when manganese is in its lowest oxidation state (0), it can act as a reducing agent because it can donate electrons and oxidize itself to a higher oxidation state.
- Since MnO₂ has an oxidation state of +4, it can act as both an oxidizing agent (by reducing from +4 to +7) and a reducing agent (by oxidizing from +4 to 0).

### Conclusion:
- **Statement 1**: MnO₂ can act as an oxidizing agent as well as a reducing agent. (True)
- **Statement 2**: The oxidation state of MnO₂ lies between the highest and lowest oxidation states. (True)

Therefore, both statements are true, and Statement 2 provides the correct explanation for Statement 1.

### Final Answer:
Both statements are true, and Statement 2 is the correct explanation for Statement 1.

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