Question

The number of angular and radial nodes in 3p orbital respectively are

• A. 3, 1
• B. 1, 1
• C. 2, 1
• D. 2, 3

Answer 1

The Correct Option is B

1. Recall the formulas for calculating the number of nodes:
Number of radial nodes = n - l - 1
Number of angular nodes = l
Total number of nodes = n - 1

where:
n is the principal quantum number
l is the azimuthal quantum number

2. Determine the quantum numbers for a 3p orbital:
For a 3p orbital:
n = 3
l = 1 (since p orbital corresponds to l = 1)

3. Calculate the number of radial and angular nodes:
Number of angular nodes = l = 1
Number of radial nodes = n - l - 1 = 3 - 1 - 1 = 1
The number of angular and radial nodes in a 3p orbital are 1 and 1 respectively.

Final Answer:
(B) 1, 1

Answer 2

The number of angular nodes (l) is equal to the value of the azimuthal quantum number (l), and the number of radial nodes is given by the formula:

Number of radial nodes = n - l - 1

For a 3p orbital, n = 3 (principal quantum number) and l = 1 (for p orbitals).

Thus, the number of angular nodes is:

Angular nodes = l = 1

The number of radial nodes is:

Radial nodes = n - l - 1 = 3 - 1 - 1 = 1

The correct answer is (B) : 1, 1.