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

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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 $2$

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(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.

Set	$(n, l, m_l)$
$A$	$(3, 3, -3)$
$B$	$(3, 2, -2)$
$C$	$(2, 1, +1)$
$D$	$(2, 2, +2)$

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

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