Assetion : The green manganate is paramagnetic but the pruple permanganate is diamagnetic in nature.
Reason : `MnO_(4)^(2-)` contains on upaired electron while in `MnO_(4)^(-)` all electrons are paried.

Options

A. Statement-1 is true , Statement-2 is true and Statement-2 is correct explanation for Statement-1
B. Statement-1 is true, Statement-2 is True and Statement-2 is Not correct explanation for statement-1
C. Statement-1 is true, Statement-2 is False
D. Statement-1 is False, Statement-2 is True

Explanation

To solve the assertion and reason question regarding the paramagnetic nature of manganate and the diamagnetic nature of permanganate, we can break it down into the following steps:

### Step 1: Analyze the Assertion
The assertion states that "The green manganate is paramagnetic but the purple permanganate is diamagnetic in nature."

**Explanation**:
- Manganate ion (MnO₄²⁻) appears green and is paramagnetic, meaning it has unpaired electrons.
- Permanganate ion (MnO₄⁻) appears purple and is diamagnetic, meaning all its electrons are paired.

### Step 2: Analyze the Reason
The reason provided is "MnO₄²⁻ contains one unpaired electron while in MnO₄⁻ all electrons are paired."

**Explanation**:
- For MnO₄⁻ (permanganate), manganese is in the +7 oxidation state. The electronic configuration of manganese in this state is [Ar] 3d⁰, which means there are no unpaired electrons.
- For MnO₄²⁻ (manganate), manganese is in the +6 oxidation state. The electronic configuration in this state is [Ar] 3d¹, which means there is one unpaired electron.

### Step 3: Conclusion
Both the assertion and reason are true, and the reason correctly explains the assertion.

### Final Answer:
- The assertion is true.
- The reason is true and provides a correct explanation for the assertion.