`C Cl_(4)` does not show hydrolysis but `SiCl_(4)` is readily hydrolysed because:

Options

A. Carbon cannot expand its octet but silicon can expand its octet .
B. Ionistatione nthalpy of carbon si hgithe thabn silicon
C. elecitrongatiivutty of carnon si higher than that of silicon
D. Caron forms double and tripple bnons .

Answer

To understand why \( CCl_4 \) does not undergo hydrolysis while \( SiCl_4 \) readily hydrolyzes, we can analyze the electronic structure and bonding characteristics of carbon and silicon.

### Step-by-Step Solution:

1. **Understanding Hydrolysis**: Hydrolysis is a chemical reaction involving the reaction of a compound with water. For a compound to hydrolyze, it typically needs to be able to form new bonds with water molecules.

2. **Examining \( CCl_4 \)**:
- \( CCl_4 \) (carbon tetrachloride) consists of a carbon atom bonded to four chlorine atoms.
- Carbon has four valence electrons and forms four covalent bonds with chlorine.
- Importantly, carbon does not have any vacant d orbitals. This means that it cannot expand its octet beyond four bonds.

3. **Examining \( SiCl_4 \)**:
- \( SiCl_4 \) (silicon tetrachloride) consists of a silicon atom bonded to four chlorine atoms.
- Silicon, like carbon, also has four valence electrons and forms four covalent bonds with chlorine.
- However, silicon has vacant d orbitals available. This allows silicon to expand its octet and form additional bonds with water molecules during hydrolysis.

4. **Conclusion**:
- The inability of carbon in \( CCl_4 \) to expand its octet means it cannot form new bonds with water, thus it does not undergo hydrolysis.
- In contrast, silicon in \( SiCl_4 \) can utilize its vacant d orbitals to form additional bonds with water, leading to hydrolysis.

### Final Answer:
\( CCl_4 \) does not show hydrolysis because carbon cannot expand its octet (due to the absence of vacant d orbitals), while \( SiCl_4 \) can hydrolyze because silicon can expand its octet using its vacant d orbitals.

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