Question

The number of angular and radial nodes present in '4d' orbitals are respectively:

• A. 2, 1
• B. 4, 3
• C. 2, 2
• D. 3, 2
• E. 4, 2

Hint:

The number of angular nodes in an orbital is equal to the value of \( l \), while the number of radial nodes is given by the formula \( n - l - 1 \), where \( n \) is the principal quantum number.

Answer 1

The Correct Option is A

The number of angular nodes and radial nodes in an orbital can be determined by the following formulas:

1. Angular nodes: The number of angular nodes is equal to \( l \), where \( l \) is the azimuthal quantum number. For a 'd' orbital, \( l = 2 \).
Therefore, the number of angular nodes is:

\[ \text{Angular nodes} = l = 2 \] 2. Radial nodes: The number of radial nodes is given by the formula:

\[ \text{Radial nodes} = n - l - 1 \] where \( n \) is the principal quantum number. For the '4d' orbital, \( n = 4 \) and \( l = 2 \). So, the number of radial nodes is:

\[ \text{Radial nodes} = 4 - 2 - 1 = 1 \] 
Thus, the number of angular nodes is 2, and the number of radial nodes is 1.

Therefore, the correct answer is:

\[ \boxed{\text{A) 2, 1}} \]