The halides which can react with water or undergo hydrolysis are `PCl_(5), SiCl_(4), BCl_(3), C Cl_(4) and SF_(6)`

Options

A. `PCl_(5), SiCl_(4), BCl_(3), C Cl_(4) and SF_(6)`
B. `PCl_(5), SiCl_(4), BCl_(3) and C Cl_(4)`
C. `PCl_(5), SiCl_(4) and BCl_(3)`
D. `PCl_(5) and SiCl_(4)`

Answer

To determine which halides can react with water or undergo hydrolysis from the given options \(PCl_5\), \(SiCl_4\), \(BCl_3\), \(CCl_4\), and \(SF_6\), we need to analyze each compound based on their electronic configurations and the presence of vacant orbitals.

### Step-by-Step Solution:

1. **Analyze \(PCl_5\)**:
- Phosphorus (P) is in group 15 and has the electronic configuration \(1s^2 2s^2 2p^6 3s^2 3p^3\).
- It has vacant d-orbitals available for bonding.
- Therefore, \(PCl_5\) can undergo hydrolysis.

2. **Analyze \(SiCl_4\)**:
- Silicon (Si) is in group 14 with the electronic configuration \(1s^2 2s^2 2p^6 3s^2 3p^2\).
- Silicon can also utilize its empty d-orbitals for bonding.
- Thus, \(SiCl_4\) can undergo hydrolysis.

3. **Analyze \(BCl_3\)**:
- Boron (B) is in group 13 and has the electronic configuration \(1s^2 2s^2 2p^1\).
- Boron is electron-deficient and can accept a pair of electrons, allowing it to react with water.
- Therefore, \(BCl_3\) can undergo hydrolysis.

4. **Analyze \(CCl_4\)**:
- Carbon (C) is in group 14 with the electronic configuration \(1s^2 2s^2 2p^2\).
- Carbon does not have d-orbitals; hence, it cannot accommodate additional electrons for hydrolysis.
- Therefore, \(CCl_4\) does not undergo hydrolysis.

5. **Analyze \(SF_6\)**:
- Sulfur (S) is in group 16 with the electronic configuration \(1s^2 2s^2 2p^6 3s^2 3p^4\).
- Although sulfur has d-orbitals, the steric hindrance from the six fluorine atoms prevents water from attacking the sulfur atom.
- Therefore, \(SF_6\) does not undergo hydrolysis.

### Conclusion:
The halides that can react with water or undergo hydrolysis are \(PCl_5\), \(SiCl_4\), and \(BCl_3\). The correct answer is:

**Answer: \(PCl_5\), \(SiCl_4\), and \(BCl_3\)**