The chloride that CANNOt get hydrolysed is :

Options

A. `SnCl_4`
B. `C Cl_4`
C. `SiCl_4`
D. `PbCl_4`

Explanation

To determine which chloride cannot get hydrolyzed among the given options (SnCl4, CCl4, SiCl4, PbCl4), we will analyze the hydrolysis behavior of each compound.

### Step-by-Step Solution:

**Step 1: Identify the elements and their electronic configurations.**
- The elements in question are tin (Sn), carbon (C), silicon (Si), and lead (Pb), all of which belong to group 14 of the periodic table.
- The electronic configurations are as follows:
- Carbon (C): 1s² 2s² 2p²
- Silicon (Si): 1s² 2s² 2p⁶ 3s² 3p²
- Tin (Sn): [Kr] 5s² 4d¹⁰ 5p²
- Lead (Pb): [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²

**Step 2: Analyze the ability to hydrolyze.**
- Hydrolysis involves the reaction of a compound with water, leading to the formation of hydroxides or acids.
- For a compound to undergo hydrolysis, it typically requires vacant orbitals to accommodate the incoming water molecules.

**Step 3: Examine each chloride for hydrolysis.**
1. **SnCl4 (Tin(IV) chloride)**:
- Tin has vacant d-orbitals and can undergo hydrolysis to form Sn(OH)4.

2. **CCl4 (Carbon tetrachloride)**:
- Carbon does not have any vacant orbitals (it has a full valence shell), making it unable to accommodate water molecules for hydrolysis. Therefore, CCl4 does not hydrolyze.

3. **SiCl4 (Silicon tetrachloride)**:
- Silicon has vacant d-orbitals and can hydrolyze to form Si(OH)4 (silicic acid).

4. **PbCl4 (Lead(IV) chloride)**:
- Lead can also undergo hydrolysis due to its vacant orbitals, forming Pb(OH)4.

**Step 4: Conclusion**
- Among the options, CCl4 is the only chloride that cannot undergo hydrolysis due to the absence of vacant orbitals.

### Final Answer:
The chloride that cannot get hydrolyzed is **CCl4**.