Question

Number of radial and angular nodes in 3p orbitals respectively are

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

Answer 1

The correct option is A

$1,1$

Step 1: Formula for radial and angular nodes

1. Number of radial nodes= $\mathrm{n}-\mathrm{l}-1$, where n= principal quantum number, l= azimuthal quantum number
2. Number of angular nodes=l where l= azimuthal quantum number

Step 2: Calculation of number of radial and angular nodes in $3\mathrm{p}$ orbital

1. In $3\mathrm{p}$ orbital the value of n is 3 and l=1 because of p orbital where the value of l=1
2. Putting the values in the above formula we get Radial nodes= $3-1-1$=$1$
3. Angular nodes=l=1

Therefore, the number of radial and angular nodes is 1,1. Hence option (A) is correct.