With respect to hypochlorite, chlorate and perchlorate ions, choose the correct statement(s).

Options

A. The hypochlorite ion is the strongest conjugate base.
B. The molecular shape of only chlorate ion is influenced by the lone pair of electrons of Cl.
C. The hypochlorite and chlorate ions disproportionate to give rise to identical set of ions.
D. The hypochlorite ion oxidises the sulfite ion.

Explanation

To solve the question regarding the hypochlorite, chlorate, and perchlorate ions, we will analyze each statement one by one.

### Step-by-Step Solution:

1. **Identify the Ions and Their Structures:**
- Hypochlorite ion: \( \text{ClO}^- \)
- Chlorate ion: \( \text{ClO}_3^- \)
- Perchlorate ion: \( \text{ClO}_4^- \)

2. **Evaluate the First Statement:**
- The hypochlorite ion is the strongest conjugate base.
- **Analysis:** The strength of a conjugate base is inversely related to the strength of its corresponding acid. Hypochlorous acid (\( \text{HClO} \)) is a weak acid, making hypochlorite (\( \text{ClO}^- \)) a relatively strong conjugate base compared to chlorate and perchlorate ions.
- **Conclusion:** This statement is **correct**.

3. **Evaluate the Second Statement:**
- The molecular shape of only chlorate ion is influenced by the lone pair of electrons on Cl.
- **Analysis:**
- Chlorate (\( \text{ClO}_3^- \)) has one lone pair on the chlorine atom, which affects its shape (trigonal pyramidal).
- Hypochlorite (\( \text{ClO}^- \)) has three lone pairs and perchlorate (\( \text{ClO}_4^- \)) has no lone pairs, which gives it a tetrahedral shape.
- **Conclusion:** The statement is **correct** as the shape of chlorate is influenced by its lone pair.

4. **Evaluate the Third Statement:**
- The hypochlorite and chlorate ions disproportionate to give rise to identical sets of ions.
- **Analysis:**
- Disproportionation of hypochlorite:
\[ \text{ClO}^- \rightarrow \text{Cl}^- + \text{ClO}_3^- \]
- Disproportionation of chlorate:
\[ \text{ClO}_3^- \rightarrow \text{Cl}^- + \text{ClO}_4^- \]
- The products are not identical; they differ in the products formed.
- **Conclusion:** This statement is **incorrect**.

5. **Evaluate the Fourth Statement:**
- The hypochlorite ion oxidizes the sulphite ion.
- **Analysis:** Hypochlorite (\( \text{ClO}^- \)) is a strong oxidizing agent and can oxidize sulphite (\( \text{SO}_3^{2-} \)) to sulfate (\( \text{SO}_4^{2-} \)).
- **Conclusion:** This statement is **correct**.

### Final Conclusion:
The correct statements are:
- A: The hypochlorite ion is the strongest conjugate base.
- B: The molecular shape of chlorate ion is influenced by the lone pair of electrons on Cl.
- D: The hypochlorite ion oxidizes the sulphite ion.

Thus, the correct options are A, B, and D.