Considering $x -$ axis as the internuclear axis, the overlap of which of the following orbitals will not form a sigma bond and why?
(a) $1 s$ and $2 s$
(b) $1 s$ and $2 p_{x}$
(c) $2 p_{y}$ and $2 p_{y}$
(d) $1 s$ and $2 s$

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Solution

The combination $c$ will not result in the formation of sigma bond as it will result in sideways overlap.
This will result in the formation of $π$ bond. In the options $a, b$ and $d$ , sigma bond will be formed.

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Similar questions

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.

Q. The electronic configuration

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

is of:

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 relative energies of molecular orbitals are found to be in increasing order as follows-

σ (1 s) < σ^{*} (1 s) < σ (2 s) < σ^{*} (2 s) < [π (2 p_{y}) π (2 p_{z})] < σ (2 p_{x}) < [π^{*} (2 p_{y}) π^{*} (2 p_{z})] < σ^{*} (2 p_{x})

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

1 s^{2}

(ii)

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

(iii)

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

(iv)

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

The tendency to form bond is greatest in:

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Considering x−axis as the internuclear axis, the overlap of which of the following orbitals will not form a sigma bond and why? (a) 1s and 2s (b) 1s and 2px (c) 2py and 2py (d) 1s and 2s

The combination c will not result in the formation of sigma bond as it will result in sideways overlap. This will result in the formation of π bond. In the options a,b and d, sigma bond will be formed.

Considering $x -$ axis as the internuclear axis, the overlap of which of the following orbitals will not form a sigma bond and why?
(a) $1 s$ and $2 s$
(b) $1 s$ and $2 p_{x}$
(c) $2 p_{y}$ and $2 p_{y}$
(d) $1 s$ and $2 s$

The combination $c$ will not result in the formation of sigma bond as it will result in sideways overlap.
This will result in the formation of $π$ bond. In the options $a, b$ and $d$ , sigma bond will be formed.