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Molecular Orbitals of Carbon

Which out of ...

Question

Which out of the following configurations is INCORRECT?

1 s^{2}, 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{1} 2 p_{z}^{1}

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1 s^{2}

2 s^{2}

2 p_{x}^{1}

2 p_{y}^{1}

2 p_{z}^{o}

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1 s^{2}

2 s^{2}

2 p_{x}^{1}

2 p_{y}^{1}

2 p_{z}^{1}

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1 s^{2}

2 s^{2}

2 p^{6}

3 s^{2}

3 p^{6}

3 d^{5}, 4 s^{1}

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Solution

The correct option is A $1 s^{2}, 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{1} 2 p_{z}^{1}$
According to Hund's rule electrons are distributed among the orbitals of subshell in such a way as to give maximum number of unpaired electron with parallel spin, i.e. in a subshell pairing of electron will not start until and unless all the orbitals of that subshell will get one electron each with same spin.
Thus, $1 s^{2}, 2 s^{2}, 2 p_{x}^{2}, 2 p_{y}^{1} 2 p_{z}^{1}$ has the incorrect configuration among all.

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Similar questions

{1 s}^{2} {2 s}^{2} {2 p x}^{1} {2 p y}^{1} {2 p z}^{1}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {3 d}^{6} {4 s}^{1}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{1}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{5}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {4 s}^{1}

{(I E)}_{1}

{(I E)}_{4}

1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}

{1 s}^{2} {2 s}^{2} {2 p}^{6} {3 s}^{2} {3 p}^{6} {4 s}^{2}

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