Determine the incorrect order of bond angle ?

Options

A. `NH_(3)ltNF_(3)ltNCl_(3)`
B. `OF_(2)ltOH_(2)ltOCl_(2)`
C. `SF_(2)ltSCl_(2)ltSBr_(2)ltSI_(2)`
D. `ClO_(2)^(-1)ltOCl_(2)`

Answer

To determine the incorrect order of bond angles among the given compounds, we need to analyze the molecular geometry and the effects of lone pairs and electronegativity on bond angles.

### Step-by-Step Solution:

1. **Identify the Compounds**: The first option consists of three compounds: NH3 (ammonia), NF3 (nitrogen trifluoride), and NCl3 (nitrogen trichloride).

2. **Analyze NH3**:
- NH3 has a trigonal pyramidal shape due to one lone pair on nitrogen.
- The bond angle is approximately 107 degrees. The presence of hydrogen, which is less electronegative, allows for greater electron density around nitrogen, leading to increased repulsion between the bonding pairs.

3. **Analyze NF3**:
- NF3 also has a trigonal pyramidal shape with one lone pair on nitrogen.
- However, fluorine is highly electronegative, pulling electron density away from nitrogen. This results in a smaller bond angle compared to NH3, approximately 102 degrees.

4. **Analyze NCl3**:
- NCl3 has a similar trigonal pyramidal shape with one lone pair on nitrogen.
- Chlorine is bulkier than fluorine but less electronegative, which means the bond angle is larger than that of NF3 but smaller than NH3. The bond angle is approximately 107 degrees.

5. **Order the Bond Angles**:
- From the analysis, we can order the bond angles as follows:
- NH3 > NCl3 > NF3
- Therefore, the statement given in the question (NCl3 > NF3 > NH3) is incorrect.

6. **Conclusion**: The incorrect order of bond angles is found in the first option regarding NH3, NF3, and NCl3.