Which of the following violates the Aufbau pr | vedclass

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(D) The Aufbau principle states that electrons fill lower energy orbitals first. According to Hund's rule,pairing of electrons in degenerate orbitals

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(D) The Aufbau principle states that electrons fill lower energy orbitals first. According to Hund's rule,pairing of electrons in degenerate orbitals (like $2p$) only occurs after each orbital is singly occupied. Option $A$ shows a correctly filled $2s$ and $2p$ orbital for Nitrogen $(1s^2 2s^2 2p^3)$. Option $B$ violates the Aufbau principle because the $2s$ orbital is not fully filled before electrons enter the $2p$ orbital. Option $C$ follows both rules for Carbon $(1s^2 2s^2 2p^2)$. Option $D$ violates Hund's rule because electrons are paired in the first $2p$ orbital before the second $2p$ orbital is singly occupied.

Laws	Statements
$(1)$ Hund's Rule	$(A)$ No two electrons in an atom can have the same set of all four quantum numbers.
$(2)$ Aufbau Principle	$(B)$ Half-filled and fully-filled orbitals have greater stability.
$(3)$ Pauli Exclusion Principle	$(C)$ Electrons prefer to remain unpaired in degenerate orbitals first.
$(4)$ Heisenberg's Uncertainty Principle	$(D)$ It is impossible to determine simultaneously the exact position and exact momentum of an electron.
	$(E)$ In the ground state of atoms,orbitals are filled in the order of increasing energy.

Column-$I$	Column-$II$
$(1)$ Photon	$(A)$ Value of $4$ for $N$ shell
$(2)$ Electron	$(B)$ Probability density
$(3)$ $\psi^2$	$(C)$ Always $+$ value
$(4)$ Principal quantum number $(n)$	$(D)$ Represents wavelength and momentum

Which of the following violates the Aufbau principle and Hund's rule?

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Match the following columns:

Column-$I$ Column-$II$

$(1)$ Photon $(A)$ Value of $4$ for $N$ shell

$(2)$ Electron $(B)$ Probability density

$(3)$ $\psi^2$ $(C)$ Always $+$ value

$(4)$ Principal quantum number $(n)$ $(D)$ Represents wavelength and momentum

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