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(A) Pauli's exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers,meaning an orbital can hold a ma

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(A) Pauli's exclusion principle states that no two electrons in an atom can have the same set of four quantum numbers,meaning an orbital can hold a maximum of two electrons with opposite spins. Hund's rule states that electron pairing in degenerate orbitals (like $p$-orbitals) does not occur until each orbital is singly occupied.In option $(A)$,the $2p_x$ orbital contains two electrons with parallel spins,which violates the Pauli exclusion principle. Furthermore,since the $2p_y$ orbital is empty while $2p_x$ is paired,it also violates Hund's rule regarding the order of filling.Therefore,option $(A)$ violates both principles.

In which of the following cases are both the Pauli exclusion principle and Hund's rule violated?

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