Question

The number of angular nodes and radial nodes in $3s$ orbital are

• A. 0 and 2, respectively
• B. 1 and 0, respectively
• C. 3 and 0, respectively
• D. 0 and 1, respectively

Answer 1

The Correct Option is A

To determine the number of angular and radial nodes in the $3s$ orbital, we need to use the following concepts:

1. Principal Quantum Number (n): This number indicates the main energy level occupied by the electron. For the $3s$ orbital, the principal quantum number is 3.
2. Azimuthal Quantum Number (l): This quantum number defines the shape of the orbital. For s orbitals, the azimuthal quantum number l is 0.

Using these quantum numbers, we calculate the nodes:

1. Angular Nodes: The formula to calculate angular nodes is:
   l
   For a 3s orbital, since l = 0, there are 0 angular nodes.
2. Radial Nodes: The formula to calculate radial nodes is:
   n - l - 1
   Substituting the values for the 3s orbital:
   3 - 0 - 1 = 2
   Therefore, there are 2 radial nodes.

In conclusion, the 3s orbital has 0 angular nodes and 2 radial nodes.

The correct answer is: 0 and 2, respectively.