Q11.15P - Chemistry: Molecular Nature Of Matter And Change

Question

Use partial orbital diagrams to show how the atomic orbitals of the central atom lead to hybrid orbitals in

(a)  ${\mathbf{GeCl}}_4$

(b)  ${\mathbf{BCl}}_3$

(c)  ${{\mathbf{CH}}_3}^{+}$

Step-by-Step Solution

Answer

The process of blending orbital to make new orbital with stable bonds is understood as hybridization. The amount of hybrid orbitals formed is up to the amount of atomic orbitals mixed.

 

The central atom

1. Germanium has ${\mathbf{sp}}^3$  hybridization
2. Boron has ${\mathbf{sp}}^2$   hybridization
3. Carbon has  ${\mathbf{sp}}^2$ hybridization

Step1: For GeCl 4

Three p and one s orbital of central atom forms tetrahedral geometry around germanium and formation of  ${\mathbf{sp}}^3$  hybrid orbital takes place.

 

 During the formation of bonds, each half-filled Germanium orbital gets the second electron from Chlorine atoms.

Step2: For BCl 3

Two p and one s orbital of central atom forms trigonal planar geometry around boron and formation of  ${\mathbf{sp}}^2$  hybrid orbital takes place.

 

During the formation of bonds, each half-filled Boron orbital gets the second electron from Chlorine atoms.

Step3: For CH 3 +

Two p and one s orbital of central atom forms trigonal planar geometry around boron and formation of  ${\mathbf{sp}}^2$ hybrid orbital takes place.

During the formation of bonds, each half-filled Carbon orbital gets the second electron from hydrogen atoms.