Assuming that the Pauli exclusion principle is non-existent, which of the following will be the most unacceptable configuration of Li in the ground state?

1 2

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Solution

The correct option is B
1

According to Pauli's exclusion principle, "No two electrons can have same set of four quantum numbers”.

This means,

"Only two electrons can exist in the same orbital and they will have opposite spin”.

But we are assuming that there is no such rule.

Therefore, all 3 electrons will try to go to lowest energy orbital, i.e., 1s

$\Rightarrow$ Li $\to$ 1 $s^{3}$

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Similar questions

Assuming that the Pauli exclusion principle is non-existent, which of the following will be the most acceptable configuration of Li in the ground state?

If carbon atom has electronic configuration 1 $s^{6}$ , it would have energy lower than that of the normal ground state configuration 1 $s^{2}$ 2 $s^{2}$ 2 $p^{2}$ . Yet 1 $s^{6}$ is not observed because it violates

Q. If the nitrogen atom had an electronic configuration of

1 s^{7}

it would have lower energy than that of the normal ground state configuration

1 s^{2}, 2 s^{2}, 2 p^{3}

because the electrons would be closer to the nucleus.

1 s^{7}

is not observed because it violates:

Q. Statement 1: Two electrons in the

2 s

subshell must have opposite spins.
Statement 2: The Pauli Exclusion Principle states that no two electrons in the same atom can have identical quantum numbers.

Q. Statement 1 : Two electrons in the 2s sub-shell must have opposite spins.
Statement 2 : The Pauli exclusion principle states that no two electrons in the same atom can have identical quantum numbers.

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