Which statement is correct about bond angle of `NCl_(3),NF_(3)` and `NH_(3)`
Bond angle of `NCl_(3) gt NF_(3)`
Bond angle of `NCl_(3) lt NF_(3)`
Bond angle of `NH_(3) gt NF_(3)`
Bond angle of `NH_(3) lt NF_(3)` .

Options

A. I,II
B. I,III
C. I,II,III
D. I,II,IV

Explanation

To determine the correct statement about the bond angles of NCl₃, NF₃, and NH₃, we will analyze the bond angles based on the electronegativity of the surrounding atoms and the molecular geometry of each compound.

### Step-by-Step Solution:

1. **Understanding Bond Angles**:
- The bond angle in a molecule is influenced by the electronegativity of the surrounding atoms. Generally, as the electronegativity of the side atom increases, the bond angle decreases.

2. **Analyzing NH₃ (Ammonia)**:
- NH₃ has a trigonal pyramidal shape due to the presence of a lone pair of electrons on nitrogen.
- The bond angle in NH₃ is approximately 107°.

3. **Analyzing NF₃ (Nitrogen Trifluoride)**:
- NF₃ also has a trigonal pyramidal shape, similar to NH₃, but the electronegativity of fluorine is higher than that of hydrogen.
- This results in a smaller bond angle in NF₃ compared to NH₃. The bond angle in NF₃ is approximately 102°.

4. **Analyzing NCl₃ (Nitrogen Trichloride)**:
- NCl₃ has a similar trigonal pyramidal shape, but chlorine has a lower electronegativity compared to fluorine.
- Therefore, the bond angle in NCl₃ will be larger than that in NF₃. The bond angle in NCl₃ is approximately 107° to 110°.

5. **Comparing the Bond Angles**:
- From the analysis:
- NH₃ (107°) > NF₃ (102°)
- NCl₃ (107° to 110°) > NF₃ (102°)
- NCl₃ (107° to 110°) > NH₃ (107°)

6. **Conclusion**:
- The correct statements regarding the bond angles are:
- Bond angle of NCl₃ > NF₃
- Bond angle of NH₃ > NF₃
- Therefore, the correct answer is that the bond angle of NCl₃ is greater than that of NF₃.

### Final Answer:
The correct statement is: **Bond angle of NCl₃ > NF₃**.