The orbital diagram in which both the Pauli's | vedclass

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(C) $Pauli's$ exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers. This means an orbital can hol

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(C) $Pauli's$ exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers. This means an orbital can hold a maximum of two electrons with opposite spins. $Hund's$ rule of maximum multiplicity states that electron pairing in $p, d,$ and $f$ orbitals cannot occur until each orbital of a given subshell contains one electron each (singly occupied). In option $C$,the first orbital of the $p$-subshell contains two electrons with the same spin,which violates $Pauli's$ exclusion principle. Furthermore,the second orbital is empty while the first is paired,which violates $Hund's$ rule.

List-$I$ (Quantum Number)	List-$II$ (Information provided)
$A$. $m_l$	$I$. Shape of orbital
$B$. $m_s$	$II$. Size of orbital
$C$. $l$	$III$. Orientation of orbital
$D$. $n$	$IV$. Orientation of spin of electron

The orbital diagram in which both the Pauli's exclusion principle and Hund's rule are violated is

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