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Overlaps Taking All Together

Considering x...

Question

Considering x-axis as the internuclear axis which out of the following will not form a sigma bond and why? (a) 1s and 1s (b) 1s and 2p_x (c) 2p_y and 2p_y (d) 1s and 2s.

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Solution

2p_y and 2p_y orbitals will not a form a sigma bond. Taking x-axis as the internuclear axis, 2p_y and 2p_y orbitals will undergo lateral overlapping, thereby forming a pi (π) bond.

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x -

axis as the internuclear axis, the overlap of which of the following orbitals will not form a sigma bond and why?

1 s

2 s

1 s

2 p_{x}

2 p_{y}

2 p_{y}

1 s

2 s

Q. Electronic configuration

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

corresponds to :

Q. The electronic configuration

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

Q. Considering x-axis as the internuclear axis, which out of the following will not form a sigma bond.

Q. The electronic structure of four element a, b, c and d are
(i)

1 s^{2}

1 s^{2}, 2 s^{2}

1 s^{2}, 2 s^{2} 2 p^{5}

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

The tendency to form bond is greatest in:

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