(A) : lodine is the only halogen that is naturally available in positive oxidation states
(R): Iodine is slightly electropositive among halogens .

Options

A. Both A & R are true, R is the correct explanation of A
B. Both A & R are true, R is not correct explanation of A
C. A is true, R is false
D. A is false, R is true

Answer

To analyze the statements given in the question, we will break down each part step by step.

### Step 1: Understand the statement (A)
**Statement (A)**: "Iodine is the only halogen that is naturally available in positive oxidation states."

- **Explanation**: Halogens typically exhibit negative oxidation states, particularly in their most common forms (like -1 in halides). However, iodine can exist in positive oxidation states such as +1, +3, +5, and +7 in various compounds (e.g., iodates, iodine pentafluoride).
- **Conclusion**: This statement is **true**.

### Step 2: Understand the statement (R)
**Statement (R)**: "Iodine is slightly electropositive among halogens."

- **Explanation**: Electropositivity refers to the tendency of an atom to lose electrons and form positive ions. Among the halogens, as we move down the group from fluorine to iodine, the size of the atoms increases, and the electronegativity decreases. Iodine, being larger and having a lower electronegativity compared to other halogens, exhibits some metallic character, which contributes to its slight electropositivity.
- **Conclusion**: This statement is also **true**.

### Step 3: Determine the relationship between (A) and (R)
- Since both statements (A) and (R) are true, we need to check if (R) provides a correct explanation for (A).
- The explanation provided in (R) about iodine's larger atomic size and its metallic character helps to justify why iodine can exist in positive oxidation states.

### Final Conclusion
- Both statements (A) and (R) are true, and (R) is the correct explanation of (A).

### Answer
The correct option is: **Both A and R are true, and R is the correct explanation of A.**

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