The correct statement`(s) is//are`

Options

A. `BeCl_(2)` is a covalent compound
B. `BeCl_(2)` can form dimer
C. `BeCl_(2)` is an electron-deficient molecule
D. The hybrid state of `Be` in `BeCl_(2)` is `sp^(2)`

Explanation

To determine the correct statements regarding beryllium chloride (BeCl2), we will analyze each statement one by one.

### Step-by-Step Solution:

1. **Statement 1: BeCl2 is a covalent compound.**
- **Analysis:** Beryllium chloride (BeCl2) is indeed a covalent compound. Beryllium is a small atom, and as we move down the group in alkaline earth metals, the ionic character of compounds increases while the covalent character decreases. Since BeCl2 has a significant covalent character, this statement is correct.

2. **Statement 2: BeCl2 can form a dimer.**
- **Analysis:** BeCl2 exists in a dimeric form in the vapor phase. The dimer can be represented as (Cl-Be-Cl)2, where two beryllium atoms are coordinated by chlorine atoms. This statement is also correct.

3. **Statement 3: BeCl2 is an electron deficient molecule.**
- **Analysis:** BeCl2 is indeed electron deficient because beryllium has only four valence electrons and can accept only two pairs of electrons from neighboring chlorine atoms to complete its octet. This leads to the formation of a polymeric structure, confirming that this statement is correct.

4. **Statement 4: The hybrid state of Be in BeCl2 is sp2.**
- **Analysis:** This statement is incorrect. The hybridization of beryllium in BeCl2 is sp, not sp2. In BeCl2, beryllium forms two bonds with chlorine atoms, leading to a linear structure, which corresponds to sp hybridization.

### Conclusion:
The correct statements are:
- Statement 1: BeCl2 is a covalent compound. (Correct)
- Statement 2: BeCl2 can form a dimer. (Correct)
- Statement 3: BeCl2 is an electron deficient molecule. (Correct)
- Statement 4: The hybrid state of Be in BeCl2 is sp2. (Incorrect)

Thus, the correct statements are 1, 2, and 3.

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