In a multi-electron atom,which of the followi | vedclass

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(D) In a multi-electron atom,the energy of an orbital depends on both the principal quantum number $(n)$ and the azimuthal quantum number $(l)$.
Orbit

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$4$ and $5$

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(D) In a multi-electron atom,the energy of an orbital depends on both the principal quantum number $(n)$ and the azimuthal quantum number $(l)$.
Orbitals with the same $n$ and $l$ values are degenerate (have the same energy) in the absence of external fields.
Comparing the given sets:
$1. n=1, l=0$ $(1s)$
$2. n=2, l=0$ $(2s)$
$3. n=2, l=1$ $(2p)$
$4. n=3, l=2$ $(3d)$
$5. n=3, l=2$ $(3d)$
Since $4$ and $5$ have the same $n=3$ and $l=2$,they represent the same subshell $(3d)$ and thus have the same energy.

In a multi-electron atom,which of the following orbitals described by the three quantum numbers will have the same energy in the absence of magnetic and electric fields?
$1. n = 1, l = 0, m = 0$
$2. n = 2, l = 0, m = 0$
$3. n = 2, l = 1, m = 1$
$4. n = 3, l = 2, m = 0$
$5. n = 3, l = 2, m = 0$

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In a multi-electron atom,which of the following orbitals described by the three quantum numbers will have the same energy in the absence of magnetic and electric fields? $1. n = 1, l = 0, m = 0$ $2. n = 2, l = 0, m = 0$ $3. n = 2, l = 1, m = 1$ $4. n = 3, l = 2, m = 0$ $5. n = 3, l = 2, m = 0$