The number of radial nodes and angular nodes | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) For any orbital,the number of angular nodes is equal to the azimuthal quantum number $(l)$.For a $4f$-orbital,the principal quantum number $n = 4$

Vedclass · Accepted Answer

$0, 3$

Vedclass · Answer

(A) For any orbital,the number of angular nodes is equal to the azimuthal quantum number $(l)$.For a $4f$-orbital,the principal quantum number $n = 4$ and the azimuthal quantum number $l = 3$.Angular nodes $= l = 3$.The number of radial nodes is given by the formula: $	ext{Radial nodes} = n - l - 1$.Substituting the values: $	ext{Radial nodes} = 4 - 3 - 1 = 0$.Therefore,the number of radial nodes is $0$ and the number of angular nodes is $3$.

The number of radial nodes and angular nodes of a $4f$-orbital are respectively:

Similar Questions

Explain $d$ orbital.

In an atom,the total number of electrons having quantum numbers $n=4, |m_{l}|=1$ and $m_{s}=-\frac{1}{2}$ is:

Which of the following orbitals has two angular nodes?

The number of angular and radial nodes of $4d$ orbital respectively are

The total maximum number of electrons possible in $3d$,$6d$,$5s$,and $4f$ orbitals with $m_l$ (magnetic quantum number) value $-2$ is

Vedclass Test Series

Exam Paper Generator

Online Exam Module