Question

Match the orbital overlap figures shown in column I with the description given in column II and select the correct answer using the codes given below

• A. A-4, B-3, C-2, D-1
• B. A-1, B-2, C-3, D-4
• C. A-2, B-3, C-1, D-4
• D. A-4, B-1, C-2, D-3

Answer 1

The correct option is C A-2, B-3, C-1, D-4

First we need to know which is a p-orbital and which is a d-orbital.

If you don't already know, the one shaped like a dumbbell will be our p-orbital and one shaped like a double dumbbell will be our d-orbital.

The question of whether it is a σ bond or a π bond can be answered by looking at the orientation of the bonding. σ bonds are formed when orbitals overlap end to end and π bonds form when orbitals overlap sideways or laterally.

In this question, if you observe you will see that half of a particular orbital is coloured brown whereas the other half isn't coloured. This is a representation of the phase of the orbital.

Whenever the orbitals in the same phase, i.e. the same colour, overlap they are said to be bonding. If they are out of phase, i.e opposite coloured, they are said to be antibonding.

With this information it should be very straightforward for you to figure out the answer.