Question

The number of angular nodes for $4d$ orbital is

• A. $1$
• B. $2$
• C. $3$
• D. 4

Answer 1

The correct option is B

$2$

Explanation for correct option

(B) $2$

Step 1. The formula of angular node

$\text{Angular node}=l$

Here, $l$ is the azimuthal quantum number.

Step 2. Angular nodes for $4d$ orbital

• The value of $l$ for $4d$ orbital is $2$.
• Hence, the number of angular nodes for $4d$ orbital is $2$.

Explanation for incorrect option

The number of angular nodes for $4d$ orbital is $2$. Hence, the options (A), (C), and (D) are incorrect.

Hence, option (B) is correct. The number of angular nodes for $4d$ orbital is $2$.