The number of radial node/s for 3 p orbital is :

Solution

Chemistry ma’am · 3 steps

Radial nodes are n - l - 1: for 3p, put in n = 3 and l = 1 and you are done.

1. Two kinds of node. An orbital has n - 1 nodes in total. Of these, l are angular nodes (planes or cones), and the rest are radial nodes (spherical shells where the probability is zero).

   Radial nodes = n - l - 1

2. Read off values. For a 3p orbital, n = 3. A p orbital always has l = 1. So radial nodes = 3 - 1 - 1 = 1, and the one angular node is the nodal plane every p orbital has.
3. So. The 3p orbital has 1 radial node, option (c).

The idea to keep. Total nodes = n - 1, angular nodes = l, radial nodes = n - l - 1. Always split the total this way before you answer.

Answer from the NTA final answer key. Solution by PrepWiser.