Question

In the reaction \[SnC{{l}_{2}}+2C{{l}^{-}}\to SnC{{l}_{4}}\], Lewis acid is
A. $SnC{{l}_{2}}$
B. $C{{l}^{-}}$
C. $SnC{{l}_{4}}$
D. None of these

Answer 1

Hint: According to the Lewis concept, the substance which is going to accept the electrons in a chemical reaction is called Lewis acid and the chemical which is going to donate the electrons in a chemical reaction then the chemical is called Lewis base.

Complete answer:
- In the question it is asked to find the chemical which is going to act as a Lewis acid in the given chemical reaction.
- The given chemical reaction is as follows.
\[SnC{{l}_{2}}+2C{{l}^{-}}\to SnC{{l}_{4}}\]
- We have to find the oxidation number of the tin before and after the chemical reaction to find the Lewis acid in the given chemical reaction.
- In the chemical reaction the chemical tin in $SnC{{l}_{2}}$ has an oxidation of ‘-2’, after the reaction with two chloride atoms the product is $SnC{{l}_{4}}$ .
- The oxidation state of tin in $SnC{{l}_{4}}$ is ‘-4’.
- Means the oxidation number of tin is going to decrease 2 times (-2).
- So, we can say that the tin chloride $SnC{{l}_{2}}$ is going to accept the electrons in the given chemical reaction.
- Therefore, the Lewis acid is $SnC{{l}_{2}}$ .

So, the correct option is A.

Note:
The correct way to identify the Lewis acid and Lewis base in the chemical reaction is to check the oxidation state of every chemical before and after the chemical reaction. By finding the change in the oxidation state of the chemical we can say which is Lewis acid and which is Lewis base.