STATEMENT-1 : Common oxidation states of iron and +2 and +3 in its compound .
and
STATEMENT-2: Iron can have only +2 and +3 oxidation states in its compounds .

Options

A. Statement-1 is True , Statement-2 is True , Statement-2 is a correct explanation for Statement-1
B. Statement-1 is True , Statement-2 is True , Statement-2 is NOT a correct explanation for Statement-1
C. Statement-1 is True , Statement-2 is False
D. Statement-1 is False , Statement-2 is True

Answer

To solve the question, we need to analyze both statements regarding the oxidation states of iron (Fe).

### Step-by-Step Solution:

**Step 1: Analyze Statement 1**
- **Statement 1**: Common oxidation states of iron are +2 and +3 in its compounds.
- Iron (Fe) has an atomic number of 26, which gives it the electronic configuration of [Ar] 3d^6 4s^2.
- In its compounds, iron commonly exhibits oxidation states of +2 and +3.
- In the +2 oxidation state (Fe^2+), iron loses the two 4s electrons: 3d^6 (4s^0).
- In the +3 oxidation state (Fe^3+), iron loses the two 4s electrons and one 3d electron: 3d^5 (4s^0).
- **Conclusion**: Statement 1 is true.

**Step 2: Analyze Statement 2**
- **Statement 2**: Iron can have only +2 and +3 oxidation states in its compounds.
- While +2 and +3 are the most common oxidation states of iron, it can exhibit other oxidation states as well.
- For example, in potassium ferrate (K2FeO4), iron has an oxidation state of +6.
- To determine this, we can set up the equation:
- Let the oxidation state of iron be x.
- The compound has 4 oxygen atoms (each with a -2 charge), contributing a total of -8.
- The two potassium ions (K^+) each contribute +1, totaling +2.
- Thus, we have:
\[ x + (-8) + 2 = 0 \implies x - 6 = 0 \implies x = +6 \]
- **Conclusion**: Statement 2 is false because iron can have oxidation states beyond +2 and +3.

**Final Conclusion**:
- Statement 1 is true, and Statement 2 is false. Therefore, the correct option is that Statement 1 is true and Statement 2 is false.