Among `LiCI,BeCI_(2)` and `C CI_(4)` the covalent bond character varies as .

Options

A. `BeCI_2 gt LiCI gt BCI_3 gt C C I_4`
B. `LiCI lt BeCI_2 lt BCI_3 lt C CI_4`
C. `LiCI gt BeCI_2 gt C C I_4 gt BCI_3`
D. `LiCl gt BeCl_2 gt BCl_3 gt C C I_4`.

Answer

To determine the order of covalent bond character among LiCl, BeCl₂, and CCl₄, we can follow these steps:

### Step 1: Identify the Cations and Anions
- The cations in the compounds are Li⁺ (from LiCl), Be²⁺ (from BeCl₂), and C⁴⁺ (from CCl₄).
- The anion in all cases is Cl⁻ (chloride ion).

### Step 2: Analyze the Size of Cations
- The size of the cations decreases as we move from Li⁺ to Be²⁺ to C⁴⁺:
- Li⁺ is larger than Be²⁺, which is larger than C⁴⁺.
- Smaller cations have a higher charge density, which increases their ability to polarize the electron cloud of the anion.

### Step 3: Consider the Polarization Power
- According to Fajans' rules, the covalent character of an ionic bond increases with:
- Smaller cation size (higher charge density).
- Larger anion size (greater polarizability).
- Since Cl⁻ is the same in all cases, we focus on the cation size.

### Step 4: Determine the Order of Covalent Character
- CCl₄ has the smallest cation (C⁴⁺), which will have the highest polarization power and thus the highest covalent character.
- BeCl₂ has a larger cation (Be²⁺) compared to C⁴⁺ but is smaller than Li⁺, giving it moderate covalent character.
- LiCl has the largest cation (Li⁺), resulting in the least covalent character.

### Conclusion
The order of covalent bond character from highest to lowest is:
**CCl₄ > BeCl₂ > LiCl**