Question

Two radial and two angular nodes are present in the orbital.

• A. $5\mathrm{d}$
• B. $4\mathrm{f}$
• C. $3\mathrm{p}$
• D. $4\mathrm{d}$

Answer 1

The correct option is A

$5\mathrm{d}$

Explanation for Correct option:

A. $5\mathrm{d}$

Radial nodes:

• Radial nodes are the areas of a spherical surface where there is no chance of locating an electron.
• Both the primary quantum number and the azimuthal quantum number values are relevant.
• Specific orbitals have more nodes with a rise in their principal quantum number.
• $\mathrm{Number}\mathrm{of}\mathrm{radial}\mathrm{nodes}=\mathrm{n}-\mathrm{l}-1$
• Here, the primary quantum number is represented by $\mathrm{n}$, and the azimuthal quantum number is represented by $\mathrm{l}$.

Angular nodes:

• The term "angular node" refers to the planes or planar regions surrounding the nucleus where there is no chance of discovering an electron.
• The value of the primary quantum number has no bearing on the value of the angular nodes.
• It is just reliant on the azimuthal quantum number's value.
• $\mathrm{Angular}\mathrm{node}=\mathrm{l}$

$\mathrm{Number}\mathrm{of}\mathrm{radial}\mathrm{nodes}=\mathrm{n}-\mathrm{l}-1$

Final Answer: Therefore, Option A is the correct option.