Which of the following statements is CORRECT | vedclass

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(D) Statement $(I)$ is $CORRECT$ according to Hund's Rule of Maximum Multiplicity,which states that for a given electron configuration,the term with t

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$I, II$ and $III$

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(D) Statement $(I)$ is $CORRECT$ according to Hund's Rule of Maximum Multiplicity,which states that for a given electron configuration,the term with the maximum multiplicity has the lowest energy.Statement $(II)$ is $CORRECT$ because the Pauli Exclusion Principle only states that no two electrons in an atom can have the same set of four quantum numbers. If two electrons are in different orbitals within the same shell,they can have the same spin.Statement $(III)$ is $CORRECT$ because $He$ has a valence configuration of $1s^2$,while other noble gases like $Ne, Ar, Kr, Xe$ have $ns^2 np^6$ configurations.Therefore,all three statements are correct.

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.

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Which of the following statements is $CORRECT$ :$(I)$ Where orbitals are available in degenerate sets,maximum spin multiplicity is observed.$(II)$ Where two electrons occupy the same shell,they may have same spins.$(III)$ All noble gases do not have the same valence shell electronic configuration.