Among `LiCl,BeCl_(2), BCl_3` and `C Cl_(4)` the covalent bond character varies as .

Options

A. (a) `LiCl lt BCl_3 lt BeCl_2lt C Cl_4`
B. (b) `LiCl gt BeCl_2 lt BCl_3 lt C Cl_4`
C. (c) `LiCl lt BeCl_2 lt BCl_3 lt C Cl_4`
D. (d) `LiCl gt BeCl_2 gt BCl_3 gt C Cl_4`

Explanation

To determine the order of covalent bond character among LiCl, BeCl₂, BCl₃, and CCl₄, we need to analyze the electronegativity differences between the elements involved in these compounds. The covalent bond character is inversely related to the ionic character, which is influenced by the electronegativity difference between the bonded atoms.

### Step-by-Step Solution:

1. **Identify the Elements and Their Electronegativity:**
- Lithium (Li), Beryllium (Be), Boron (B), and Carbon (C) are all in the second period of the periodic table.
- The electronegativities of these elements are approximately:
- Li: 1.0
- Be: 1.5
- B: 2.0
- C: 2.5
- Chlorine (Cl) has an electronegativity of about 3.0.

2. **Calculate the Electronegativity Differences:**
- For LiCl: |1.0 - 3.0| = 2.0
- For BeCl₂: |1.5 - 3.0| = 1.5
- For BCl₃: |2.0 - 3.0| = 1.0
- For CCl₄: |2.5 - 3.0| = 0.5

3. **Analyze the Electronegativity Differences:**
- The larger the electronegativity difference, the more ionic character the bond has, and consequently, the less covalent character it exhibits.
- Therefore, the order of ionic character (and thus the inverse order of covalent character) is:
- LiCl > BeCl₂ > BCl₃ > CCl₄

4. **Establish the Order of Covalent Character:**
- Since covalent character increases as the electronegativity difference decreases, we have:
- CCl₄ > BCl₃ > BeCl₂ > LiCl

5. **Final Order of Covalent Bond Character:**
- The correct order of covalent bond character is:
- LiCl < BeCl₂ < BCl₃ < CCl₄

### Conclusion:
The order of covalent bond character among the compounds is:
**LiCl < BeCl₂ < BCl₃ < CCl₄**