Question

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

• A. 2, 0
• B. 0, 2
• C. 1, 2
• D. 2, 1

Answer 1

Answer: (A)

2, 0

For a given orbital with principal quantum number n and the azimuthal quantum number $l$, the number of radial nodes $=n-l-1$.
For $3s=3-0-1=2$ is the number of radial node
For $2p=2-1-1=0$ is the number of radial node