Question

The hybridization of \[PC{{l}_{5}}\] molecule is:
(a)- \[s{{p}^{3}}\]
(b)- \[s{{p}^{2}}{{d}^{2}}\]
(c)- \[s{{p}^{3}}d\]
(d)- \[s{{p}^{2}}\]

Answer 1

Hint: When one s, three p and one d-atomic orbitals mix, it forms five \[s{{p}^{3}}d\] hybrid orbitals of equal energy called \[s{{p}^{3}}d\] hybridization.
When one s, three p and two d orbitals mix, it forms six identical hybrid orbitals called \[s{{p}^{3}}{{d}^{2}}\] hybridization.
Similarly, on mixing one s and three p orbitals, three identical hybrid orbitals are formed called \[s{{p}^{3}}\] hybridization.


Complete step by step solution:
The electronic configuration of phosphorus and chlorine is \[[Ne]\,3{{s}^{2}}3{{p}^{3}}\] and \[[Ne]\,3{{s}^{2}}3{{p}^{5}}\]respectively. We can see that the number of valence electrons in the phosphorus atom is 5, here in \[PC{{l}_{5}}\], according to VSEPR theory it will form a single bond with each of the chlorine atoms i.e. Phosphorus atom needs five orbitals to form the five P-Cl bonds.

It has two electrons in its 3s orbital and three in 3p orbitals in the valence shell, so it must use one of its 3d to form the fifth bond, So, one electron from 3s gets excited to the d orbital and they form five hybrid orbitals.

Therefore, the hybridization of \[PC{{l}_{5}}\] id \[s{{p}^{3}}d\].Hence, the correct option is (c).

Additional Information:
Phosphorus pentachloride is a greenish-yellow solid, having a trigonal bipyramid structure. It is readily soluble in water.

Note: Hybridization of a molecule can also be calculated by a formula:
Hybridization = \[\dfrac{1}{2}(V+M-C+A)\]
where, V = valence electrons,
M = monovalent atom linked to central atom,
C = charge on cation,
A = charge on anion.
After getting the numerical value,
2 = \[sp\]
3 = \[s{{p}^{2}}\]
4 = \[s{{p}^{3}}\]
5 = \[s{{p}^{3}}d\]
6 = \[s{{p}^{3}}{{d}^{2}}\]