Select that pairs in which bond angle of first member is higher than second one.

Options

A. `BrO_3^(-), ClO_3^(-)`
B. `Asl_3, Sbl_3`
C. `SbBr_3, SbI_3`
D. `NF_3, NH_3`

Explanation

To solve the question of which pairs have a higher bond angle in the first member compared to the second member, we need to analyze each pair based on the factors that influence bond angles: the electronegativity of surrounding atoms and the size of the central atom.

### Step-by-Step Solution:

1. **Understanding Bond Angles**:
- Bond angles are influenced by the electronegativity of surrounding atoms and the size of the central atom.
- Higher electronegativity of surrounding atoms leads to smaller bond angles.
- Larger central atoms result in smaller bond angles due to increased repulsion between bonding pairs.

2. **Analyzing the First Pair: BrO3- and ClO3-**:
- Bromine (Br) is larger than chlorine (Cl).
- Since Br is larger, the bond angle in BrO3- will be smaller than in ClO3-.
- **Conclusion**: Bond angle of BrO3- < Bond angle of ClO3-.

3. **Analyzing the Second Pair: AsI3 and SbI3**:
- Arsenic (As) is smaller than antimony (Sb).
- Therefore, the bond angle in AsI3 will be larger than in SbI3.
- **Conclusion**: Bond angle of AsI3 > Bond angle of SbI3.

4. **Analyzing the Third Pair: SbBr3 and SbI3**:
- The central atom is the same (Sb), but the surrounding atoms differ (Br and I).
- Bromine is more electronegative than iodine, which means SbBr3 will have a smaller bond angle than SbI3.
- **Conclusion**: Bond angle of SbBr3 < Bond angle of SbI3.

5. **Analyzing the Fourth Pair: NF3 and NH3**:
- The central atom is nitrogen (N), but the surrounding atoms differ (F and H).
- Fluorine is more electronegative than hydrogen, leading to a smaller bond angle in NF3 compared to NH3.
- **Conclusion**: Bond angle of NF3 < Bond angle of NH3.

6. **Final Conclusion**:
- The only pair where the bond angle of the first member is higher than that of the second member is **AsI3 and SbI3**.
- Therefore, the correct answer is **Option 2**.