Question

The number of radial nodes of 3s and 2p orbitals are....

Answer 1

For a given orbital with principal quantum number, n and azimuthal quantum number, l

Number of radial nodes = (n - l - 1)

Solution:

For 3s orbital: n = 3 and l = 0

Therefore, number of radial nodes = 3 - 0 - 1 = 2

For 2p orbital: n = 2 and l = 1

Therefore, number of radial nodes = 2 - 1 - 1 = 0

Answer 2

Hi friend,
number of radial nodes for an orbital=n-l-1
for 3s n=3 l=0 so number of radial nodes will be 3-1=2
for 2p orbital n=2 and p=1 so radial nodes= 2-1-1=0.