The chloride that Cannot get hydrolysed is:
Central atom has no vacant orbital.
Hydrolysis of chlorides occurs when a chloride compound reacts with water, typically forming hydrochloric acid and the corresponding hydroxide or oxide. This happens when the central atom has vacant d-orbitals or can expand its octet, allowing nucleophilic attack by water molecules.
Let's analyze each option:
SnCl4: Tin(IV) chloride. Tin has vacant d-orbitals and can expand its octet. It hydrolyzes vigorously:
PbCl4: Lead(IV) chloride. Lead also has the ability to expand its octet. It is unstable and hydrolyzes easily:
CCl4: Carbon tetrachloride. Carbon, being a second-period element, has no low-lying d-orbitals available to accept a lone pair from a water molecule in a nucleophilic attack. Its octet is complete and cannot be expanded. Therefore, it does not undergo hydrolysis under normal conditions. This is a key exception.
SiCl4: Silicon tetrachloride. Silicon has vacant 3d orbitals, which it can use to expand its octet. It hydrolyzes rapidly:
Final Answer: CCl4 (Carbon tetrachloride) is the chloride that cannot get hydrolyzed.
The tendency of a covalent chloride to hydrolyze depends primarily on the availability of vacant orbitals on the central atom. If the central atom can accept a lone pair from a water molecule (acting as a Lewis acid), hydrolysis occurs. Elements like Si, Ge, Sn, and P have accessible d-orbitals and their chlorides hydrolyze. Carbon, in the second period, has no available d-orbitals, making CCl4 resistant to hydrolysis.
The general reaction for the hydrolysis of a tetrachloride is: (where M is an element like Si, Sn, etc.)
This reaction is not possible for carbon due to the absence of d-orbitals and the high stability of the C-Cl bond.
The total number of carboxylic acid groups in the product P is
