Question

The most commonly used reducing agent is:
A. $\mathrm{Al} \mathrm{C}_{3}$
B. $\mathrm{Pb} \mathrm{C}_{2}$
C. $\mathrm{Sn} \mathrm{C}_{4}$
D. $\mathrm{Sn} \mathrm{C}_{2}$

Answer 1

We know that the reduction of a compound in a redox reaction takes place due to the presence of a reducing agent. It is also known that the reducing agent is the one which itself gets oxidized and has the tendency to reduce other elements in a reaction.

Complete step by step answer:
We know that the chemical symbol of tin is $\mathrm{Sn}$ and it belongs to the $14^{\text {th }}$ group of the periodic table. Therefore, it’s the stable oxidation state is +4. However, the oxidation state of $\mathrm{Sn}$ is +2 in $\mathrm{Sn} \mathrm{C}_{2}$ . Thus, the oxidation of $\mathrm{Sn} \mathrm{C}_{2}$ to $\mathrm{Sn} \mathrm{C}_{4}$ takes place very easily so that $\mathrm{Sn}$ comes in its stable state. The chemical reaction representing the oxidation of $\mathrm{Sn} \mathrm{C}_{2}$ is shown below.
$\mathrm{SnCl}_{2}+2 \mathrm{Cl}^{-} \rightarrow \mathrm{SnCl}_{4}+2 \mathrm{e}^{-}$
Hence, we can say that, $\mathrm{Sn} \mathrm{C}_{2}$ acts as a good reducing agent and is also used commonly in various chemical reactions. Thus, the correct option is D.

Therefore, the correct option is option (D).

Note:
As we know, metals are electropositive in nature, that is they have the tendency to lose electrons. This property of metals makes the metal salts a good reducing agent which gets oxidized themselves and helps in the reducing the other elements. We can say that all the metals tend to be present in their stable oxidation state in their compounds.