(A) The quantum numbers $n = 4$,$l = 2$,and $m = -2$ uniquely define a single orbital ($4d_{xy}$ or similar depending on convention).According to the

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(A) The quantum numbers $n = 4$,$l = 2$,and $m = -2$ uniquely define a single orbital ($4d_{xy}$ or similar depending on convention).According to the Pauli Exclusion Principle,any single orbital can accommodate a maximum of $2$ electrons with opposite spins ($m_s = +1/2$ and $m_s = -1/2$).

Class 11 Chemistry Structure of Atom Quantum number, Electronic configuration and Shape of orbitals

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What will be the maximum number of electrons in any atom having quantum numbers $n = 4, l = 2, m = -2$?

A
$2$
B
$10$
C
$1$
D
$6$

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Structure of Atom

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Quantum number, Electronic configuration and Shape of orbitals

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Which of the following orbitals will have zero probability of finding the electron in the $yz$ plane?

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The ground state term symbol for an electronic state is governed by

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What will be the maximum number of electrons in any atom having quantum numbers $n = 4, l = 2, m = -2$?

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Which of the following is not paramagnetic?

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