The bond angles in `NH_(3), NF_(3) and NCl_(3)` are in the order:

Options

A. `NCl_(3) gt NH_(3) gt NF_(3)`
B. `NH_(3)gt NCl_(3) gt NF_(3)`
C. `NH_(3)gt NH_(3)gt NCl_(3)`
D. `NF_(3) gt NCl_(3) gt NH_(3)`

Answer

To determine the bond angles in NH₃ (ammonia), NF₃ (nitrogen trifluoride), and NCl₃ (nitrogen trichloride), we can analyze the molecular geometry and the effects of lone pairs and electronegativity using VSEPR (Valence Shell Electron Pair Repulsion) theory and N-B-E-P-R (Non-Bonded Electron Pair Repulsion) theory.

### Step-by-Step Solution:

1. **Identify the Molecular Geometry**:
- All three compounds (NH₃, NF₃, NCl₃) have a trigonal pyramidal shape due to the presence of one lone pair of electrons on the nitrogen atom.

2. **Consider the Effect of Lone Pairs**:
- In NH₃, the lone pair exerts repulsion on the bonding pairs, which slightly decreases the bond angle from the ideal tetrahedral angle (109.5°).
- In NF₃, the lone pair also repels the bonding pairs, but the electronegativity of fluorine pulls the bonding pairs closer to the nitrogen, which can lead to a smaller bond angle compared to NH₃.
- In NCl₃, the larger size of chlorine atoms compared to hydrogen and fluorine results in less repulsion from the lone pair, which can lead to a larger bond angle.

3. **Analyze Electronegativity**:
- Fluorine is more electronegative than hydrogen, which means that in NF₃, the bond angles will be smaller due to the stronger pull of the fluorine atoms on the bonding electrons.
- Chlorine is less electronegative than fluorine, which means that in NCl₃, the bond angles will be larger compared to NF₃.

4. **Compare the Bond Angles**:
- The bond angles can be expected to follow this trend based on the above analysis:
- NCl₃ > NH₃ > NF₃
- Therefore, the bond angles in the order are:
- NCl₃ (largest) > NH₃ (intermediate) > NF₃ (smallest).

### Conclusion:
The bond angles in NH₃, NF₃, and NCl₃ are in the order: **NCl₃ > NH₃ > NF₃**.