Q17P - 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) ${\mathbf{SeCI}}_{\mathbf{2}}$

(b) ${\mathbf{H}}_{\mathbf{3}}{\mathbf{O}}^{\mathbf{+}}$

(c) ${\mathbf{IF}}_{\mathbf{4}}^{\mathbf{-}}$

Step-by-Step Solution

Answer

The process of mixing orbital to form new orbital with stable bonds is known as hybridization. The number of hybrid orbitals formed is equal to the number of atomic orbitals mixed.

 

The central atom

      a. selenium has ${\mathbf{sp}}^{\mathbf{3}}$ hybridization

      b. oxygen has ${\mathbf{sp}}^{\mathbf{3}}$ hybridization

      c. iodine has ${\mathbf{sp}}^{\mathbf{3}}{\mathbf{d}}^{\mathbf{2}}$ hybridization

Step1:For SeCI 2

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

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

Step2:For H 3 O +

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

During the formation of bonds, each half-filled oxygen orbital gets the second electron from hydrogenatoms.

Step3: For IF 4 -

Two d,three p and one s orbital of central atom forms square planar geometry instead of octahedral because of lone pairs around iodine,and formation of ${\mathbf{sp}}^{\mathbf{3}}{\mathbf{d}}^{\mathbf{2}}$ hybrid orbital takes place

During the formation of bonds, each half-fillediodineorbital gets the second electron from fluorine atoms.