Question

Define the term Hybridization.Using the concept of Hybridization explain the shapes of CH2 and PCL5 molecules.

Answer 1

it is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory. Hybrid orbitals are very useful in the explanation of molecular geometry and atomic bonding properties .
What is the hybridization of PCL5?

erefore the hybridisation number of PCl5 is 5 and it has a hybridisation state of sp3f
In PCl5 one s ,3 p and one d orbital are involved in hybridisation.

Hybridisation of a molecule can be calculated by using the formula:

H = 0.5 × (V + M - C + A)

where, H → Hybridisation; V → Number of Valence Electrons of Free Central Atom; M → Number of Monovalent atoms linked to the central atom; C → Charge on Cation; A → Charge of Anion

After getting a numerical value, you can use the following list for finding out the hybridisation of the required molecule:

2 → sp Hybridisation

3 → sp2 Hybridisation

4 → sp3 Hybridisation

5 → sp3d Hybridisation

6 → sp3d2 Hybridisation

So, for PCl5, where P is the central atom and Cl is the Monovalent atom linked to P,

H = 0.5 × (5 + 5 – 0 + 0) = 0.5 × 10 = 5

So, from the above list, we can deduce that the hybridisation of PCl5 is sp3d.

Hope this helps!

Answer 2

Hybridization:

• Hybridization is defined as the mixing of the atomic orbitals belonging to the same atom but having slightly different energies so that redistribution of energy takes place between them, resulting in the formation of new orbitals of equal energies and identical shapes.
• Hybridisation of a molecule can be calculated by using the formula:

                              H = 0.5 × (V + M - C + A)

steps involved for getting hybridization:

1. STEP-1: Write the Lewis structure
2. STEP-2: Calculate the number of sigma (σ) bonds
3. STEP-3: Calculate the number of lone pairs(V-B-C/2).
4. STEP-4: Calculate the steric number
5. STEP-5: Assign hybridization and shape of the molecule.

A)Hybridization in CH4:

• In ethene CH2=CH2, carbon atom is attached to 3 atoms(1C, 2H) through 3 sigma bonds and 1 π bond.
• steric number of each carbon is 3.
• as the double bond-single bond repulsion is greater than single bond-single bond, it gives 120° planar shape.
• the hybridization of the CH2=CH2 molecule is SP2.

B)Hybridization in  PCL5:

• The phosphorus has atomic number 15 and valence electrons that are present are 5.
• These five electrons present, will make bonds with five Cl that are there in PCl5(There is no lone pair present).  
• The Hybridization of PCl5   will be Sp3d
• as z is equal to five and the corresponding geometry will be trigonal bipyramidal.
• There will be two types of bonds that will be formed in PCl5   that are equatorial bonds and axial bonds.