STATEMENT-1 : `I_(2)rarrIO_(3)^(-)+I^(-)`, is example of a disproportionation reaction.
STATEMENT-2 : Oxidation number of I can vary from `-1` to `+7`.

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 reaction involving iodine.

### Step 1: Analyze Statement 1
The reaction given is:
\[ I_2 \rightarrow IO_3^{-} + I^{-} \]

This reaction involves iodine (I) in its elemental form (I2) transforming into iodate (IO3-) and iodide (I-).

### Step 2: Determine the Oxidation States
- In \( I_2 \), the oxidation state of iodine is 0 (since it is in its elemental form).
- In \( IO_3^{-} \):
- Let the oxidation state of iodine be \( x \).
- The oxidation state of oxygen is -2.
- Therefore, for three oxygen atoms, the total contribution is \( -6 \).
- The overall charge of the ion is -1, leading to the equation:
\[ x - 6 = -1 \]
\[ x = +5 \]
- In \( I^{-} \), the oxidation state of iodine is -1.

### Step 3: Identify Oxidation and Reduction
- The oxidation state of iodine changes from 0 in \( I_2 \) to +5 in \( IO_3^{-} \) (oxidation).
- The oxidation state changes from 0 in \( I_2 \) to -1 in \( I^{-} \) (reduction).

Since iodine is both oxidized (to +5) and reduced (to -1) in this reaction, it is classified as a disproportionation reaction.

### Conclusion for Statement 1
Thus, Statement 1 is correct: the reaction is indeed an example of a disproportionation reaction.

### Step 4: Analyze Statement 2
Statement 2 claims that the oxidation number of iodine can vary from -1 to +7.

- Iodine can have an oxidation state of -1 when it gains an electron (as in \( I^{-} \)).
- It can also have oxidation states up to +7 in compounds such as \( IO_4^{-} \) (where it loses up to 7 electrons).

### Conclusion for Statement 2
Thus, Statement 2 is also correct: the oxidation number of iodine can vary from -1 to +7.

### Final Evaluation
Both statements are true, but Statement 2 does not explain Statement 1 directly. Therefore, the correct option is that both statements are true, but Statement 2 is not the correct explanation of Statement 1.

### Summary of Answers
- **Statement 1**: True (disproportionation reaction)
- **Statement 2**: True (oxidation states of iodine)