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Standard XII

Chemistry

Molecular Orbitals of Carbon

If the nitrog...

Question

If the nitrogen atom had electronic configuration $1 S^{7}$ , it would have enrgy lower 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. Yet $1 s^{7}$ is not observed because it violates.

Heisenberg uncertainty principle

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Hund Rule

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Pauli exclusion principle

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Bohr postulate of stationary orbits

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Solution

The correct option is D Pauli exclusion principle
Pauli's exclusion principle states that the orbitals are filled in the increasing order of the energy shell e.g. ${1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6}$

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Similar questions

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. If the nitrogen atom had electronic configuration

1 s^{7}

, it would have energy lower 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. Yet

1 s^{7}

is not observed because it violates:

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 nitrogen atom had an electronic configuration of

1 s^{7}

, it would have energy lower than it’s normal ground state configuration of

1 s^{2} 2 s^{2} 2 p^{3} . Y e t, 1 s^{7}

is not observed as 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

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If the nitrogen atom had electronic configuration 1S7, it would have enrgy lower than that of the normal ground state configuration 1s2,2s2,2p3, because the electrons would be closer to the nucleus. Yet 1s7 is not observed because it violates.

The correct option is D Pauli exclusion principlePauli's exclusion principle states that the orbitals are filled in the increasing order of the energy shell e.g. 1s22s22p63s23p6

If the nitrogen atom had electronic configuration $1 S^{7}$ , it would have enrgy lower 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. Yet $1 s^{7}$ is not observed because it violates.

The correct option is D Pauli exclusion principle
Pauli's exclusion principle states that the orbitals are filled in the increasing order of the energy shell e.g. ${1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6}$