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(A) . Orbital angular momentum is determined by the azimuthal quantum number $(l)$, given by $\sqrt{l(l+1)} \frac{h}{2\pi}$. Thus, $A-q$.$B$. The Paul

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$A-q, B-s, C-p, q, r, D-p, q$

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(A) . Orbital angular momentum is determined by the azimuthal quantum number $(l)$, given by $\sqrt{l(l+1)} \frac{h}{2\pi}$. Thus, $A-q$.$B$. The Pauli exclusion principle applies to electrons, involving the spin quantum number $(s)$. Thus, $B-s$.$C$. The shape, size, and orientation of orbitals are determined by the principal $(n)$, azimuthal $(l)$, and magnetic $(m_l)$ quantum numbers. Thus, $C-p, q, r$.$D$. The probability density at the nucleus depends on the radial wave function, which is determined by $n$ and $l$. Thus, $D-p, q$.

Column $I$	Column $II$
$A$. Orbital angular momentum of the electron in a hydrogen-like atomic orbital	$p$. Principal quantum number
$B$. $A$ hydrogen-like one-electron wave function obeying Pauli principle	$q$. Azimuthal quantum number
$C$. Shape, size and orientation of hydrogen-like atomic orbitals	$r$. Magnetic quantum number
$D$. Probability density of electron at the nucleus in hydrogen-like atom	$s$. Electron spin quantum number

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