Question

why 2p&3d orbitals does not have any node?

Answer 1

The azimuthal quantum number â„“ determines the number of angular nodes in an orbital. A radial node is a circular ring that occurs as the principle quantum number increases.
Number of radial nodes = (n - l - 1)
Total number of nodes = n - 1

For 3d orbital: n = 3 and l = 2

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

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

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