The species, having bonds angle of `120^(@)` is

Options

A. `PH_(3)`
B. `ClF_(3)`
C. `NCl_(3)`
D. `BCl_(3)`

Explanation

To determine the species that has bond angles of 120 degrees, we can analyze the molecular geometry of the given options based on the number of lone pairs and bond pairs. Here’s a step-by-step solution:

### Step 1: Analyze the Given Options
We need to look at each of the provided species and determine their molecular geometry and bond angles.

### Step 2: Evaluate Phosphine (PH₃)
- Phosphorus (P) has 5 valence electrons.
- In PH₃, phosphorus forms 3 bonds with hydrogen atoms and has 1 lone pair.
- The molecular geometry is tetrahedral due to the presence of the lone pair, but the bond angle is approximately 93.5 degrees, which is less than 120 degrees.

**Hint:** Remember that lone pairs can compress bond angles.

### Step 3: Evaluate Chlorine Trifluoride (ClF₃)
- Chlorine (Cl) has 7 valence electrons.
- In ClF₃, chlorine forms 3 bonds with fluorine atoms and has 2 lone pairs.
- The molecular geometry is T-shaped, and the bond angles between the fluorine atoms are approximately 90 degrees.

**Hint:** Consider how lone pairs affect the shape and angles.

### Step 4: Evaluate Chlorine Trichloride (Cl₃)
- Nitrogen (N) has 5 valence electrons.
- In Cl₃, nitrogen forms 3 bonds with chlorine atoms and has no lone pairs.
- The geometry is tetrahedral, but the bond angle is around 104 degrees due to the larger size of chlorine atoms.

**Hint:** Check if the central atom has lone pairs or not.

### Step 5: Evaluate Boron Trichloride (BCl₃)
- Boron (B) has 3 valence electrons.
- In BCl₃, boron forms 3 bonds with chlorine atoms and has no lone pairs.
- The molecular geometry is trigonal planar, and the bond angles are exactly 120 degrees.

**Hint:** Look for species with no lone pairs and three bond pairs for 120-degree angles.

### Conclusion:
The species that has bond angles of 120 degrees is **Boron Trichloride (BCl₃)**.

### Summary of Steps:
1. Analyze each species for valence electrons and bonding.
2. Determine the number of lone pairs and bond pairs.
3. Identify the molecular geometry and corresponding bond angles.
4. Conclude that BCl₃ has bond angles of 120 degrees.