Question

explain electronic configuration of he and n according to pauli and hunds principle​

Answer 1

Pauli's Principle:

This principle states that two electrons cannot have all the same Quantum numbers.

Hund's Principle:

This principle states that electrons will first occupy the orbitals singly and then undergo pairing.

Following these principles:

Helium has atomic number 2. Hence these two electrons occupy the 1s orbital in pair.

$\{He \}_{2} = \: \{ \uparrow \downarrow \} \\ \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: 1 {s}^{2}$

Nitrogen has atomic number 7.

$\{N \}_{7} = \: \{ \uparrow \downarrow \} \: \: \{ \uparrow \downarrow \} \: \: \{ \uparrow \uparrow \uparrow \}\\ \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: 1 {s}^{2} \: \: \: 2 {s}^{2} \: \: \: \: \: 2 {p}^{3}$

Hence , first two electrons occupy the 1s orbital, second to electron occupy the 2s orbital. And last three electron occupy the 2p orbital without pairing.

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Answer 2

Answer:this your answer.

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