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

Heisenberg's Uncertainty principle

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Hund's rule

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Pauli exclusion principle

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Aufbau Principle

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Solution

The correct options are
C
Pauli exclusion principle

D
Aufbau Principle

Pauli Exclusion principle can be stated as: "only two electrons may exist in the same orbital and these electron must have opposite spin.

Now, we can conclude that in s orbital only 2 electrons can be filled.

So 1 $s^{6}$ configuration violates Pauli Exclusion principle.

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Similar questions

Q. If carbon has electronic configuration

1 s^{6}

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

1 s^{2} 2 s^{2} 2 p^{2}

, because the electrons would be closer to the nucleus. Yet

1 s^{6}

is not observed, since it violates

Q. If the nitrogen atom had an electronic configuration of

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

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Q. The principles that gives the correct explanation why ground state electronic configuration of

S i

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Q. If carbon has electronic configuration

1 s^{6}

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

1 s^{2} 2 s^{2} 2 p^{2}

, because the electrons would be closer to the nucleus. Yet

1 s^{6}

is not observed, since it violates

Nitrogen has the electronic configuration $1 s^{2}, 2 s^{2} 2 p_{x}^{1} 2 p_{y}^{1} 2 p_{z}^{1}$ and not $1 s^{2}, 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{1} 2 p_{z}^{0}$ which is determined by

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If carbon atom has electronic configuration 1s6, it would have energy lower than that of the normal ground state configuration 1s2 2s2 2p2. Yet 1s6 is not observed because it violates

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