The number of radial and angular nodes in 4d | vedclass

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

Question

(A) For a $4d$ orbital,the principal quantum number $n = 4$ and the azimuthal quantum number $l = 2$.The number of radial nodes is calculated using th

Vedclass · Accepted Answer

$1$ and $2$

Vedclass · Answer

(A) For a $4d$ orbital,the principal quantum number $n = 4$ and the azimuthal quantum number $l = 2$.The number of radial nodes is calculated using the formula: $	ext{Radial nodes} = n - l - 1$.Substituting the values: $	ext{Radial nodes} = 4 - 2 - 1 = 1$.The number of angular nodes is equal to the azimuthal quantum number $l$.Therefore,$	ext{Angular nodes} = l = 2$.Thus,the number of radial and angular nodes are $1$ and $2$,respectively.

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

Similar Questions

Maximum number of electrons theoretically possible for an orbit with principal quantum number $n=6$ in an atom is

The energy of a $2p$ orbital in a multi-electron atom is

How many electrons can be fit into the orbitals that comprise the $3^{rd}$ quantum shell $(n = 3)$?

If the magnetic quantum number of a given orbital is represented by $-3$,then what will be the minimum possible value of its principal quantum number $(n)$?

The electronic configuration $1s^2, 2s^2 2p^5, 3s^1$ represents:

Vedclass Test Series

Exam Paper Generator

Online Exam Module