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(C) The four quantum numbers are defined as follows:$1$. Principal quantum number $(n)$: Determines the size and energy of the orbital.$2$. Azimuthal

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$m$ gives the energy of the electron in the orbital.

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(C) The four quantum numbers are defined as follows:$1$. Principal quantum number $(n)$: Determines the size and energy of the orbital.$2$. Azimuthal quantum number $(l)$: Determines the shape of the orbital.$3$. Magnetic quantum number $(m_l)$: Determines the orientation of the orbital in space.$4$. Spin quantum number $(s)$: Determines the direction of electron spin.Statement $C$ is false because the magnetic quantum number $(m_l)$ describes the orientation of the orbital,not the energy of the electron. The energy is primarily determined by $n$ (and $l$ in multi-electron atoms).

Column-$I$	Column-$II$
$A$. The orbital which has two angular nodes	$P$. $4d_{x^2-y^2}$
$B$. The $d$ orbital with zero nodal plane	$Q$. $3d_{z^2}$
$C$. The orbital with two radial nodes	$R$. $4f$
$D$. The orbital with three angular nodes	$S$. $3s$

Which of the following statements concerning the four quantum numbers is false?

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The orbital angular momentum for a $d$-electron is

Match the column:

Column-$I$ Column-$II$

$A$. The orbital which has two angular nodes $P$. $4d_{x^2-y^2}$

$B$. The $d$ orbital with zero nodal plane $Q$. $3d_{z^2}$

$C$. The orbital with two radial nodes $R$. $4f$

$D$. The orbital with three angular nodes $S$. $3s$

Correct match will be $:-$

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For a $d$-electron,the orbital angular momentum is:

Which of the following represents an excited state of an atom?

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