Question

Identify the structure of ${\mathrm{SnCl}}_2$

Answer 1

Tin chloride:

1. Tin chloride is a crystalline substance having the chemical formula Tin (II) chloride in its solid-state. It has a crystalline white appearance and has no odor.
2. We need to know the Steric number to figure out how to hybridization of tin chloride.
3. Electronic configuration of Tin with atomic number$=50$ is$1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^{2}4{\mathrm{p}}^{6}4{\mathrm{d}}^{10}5{\mathrm{s}}^{2}5{\mathrm{p}}^2$, therefore, valence electrons$=4$in which $2$ are electron lone pairs of electrons.
4. Electronic configuration of chlorine$=1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^5$ therefore valence electron$=7$.
5. Steric number$=3$ two bond pair of tin and chlorine along with one lone pair of electrons.
6. Three tin atomic orbitals hybridize to form three degenerate hybrid orbits${\mathrm{SnCl}}_2$. One s-orbital and two p-orbital make up the three atomic orbitals. As a result, the hybridization will be${\mathrm{sp}}^2$, and the structure will be bent, resulting in angular geometry due to the presence of lone pairs.

Therefore, the structure of ${\mathrm{SnCl}}_2$ is trigonal pyramidal or V-shape or bent due to the presence of lone pair.