The strength of bonds formed by 2s - 2s, 2p - 2p and 2p - 2s overlap has the order:
The strength of bonds formed by 2s - 2s, 2p - 2p and 2p - 2s overlap has the order:
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The correct option is
C
p-p > s-p > s-s
As we know, a sigma bond is formed by head-on or end-to-end overlapping. Also, the directional character of the orbital is taken into account. Thus, the strength of a sigma bond is directly proportional to the extent of overlapping and the directional character.
Here we have two orbitals s and p. The ‘s’ orbital has a spherical symmetry hence it tends to have a uni-directional character. However, the ‘p’ orbital has a multi-directional character; it can align itself in the x, y, and z-axis. Thus, the overlapping between s and s orbital would cover less area and so its strength will be less.
On the other hand, the area for p and p orbital overlapping will be more which will eventually increase the strength of the bond.
Also, overlapping between p orbital and s orbital will be more than s-s overlap but less than p-p overlap.
So the increasing order of strength of Sigma bond will be:
s−s< s−p<p−p
During the axial overlap of p-p orbitals, the electron density increases around the axis, so the bond formed is the strongest. Therefore, the strongest bond formed is when p-p orbital overlap occurs.
The correct option is
C
p-p > s-p > s-s
As we know, a sigma bond is formed by head-on or end-to-end overlapping. Also, the directional character of the orbital is taken into account. Thus, the strength of a sigma bond is directly proportional to the extent of overlapping and the directional character.
Here we have two orbitals s and p. The ‘s’ orbital has a spherical symmetry hence it tends to have a uni-directional character. However, the ‘p’ orbital has a multi-directional character; it can align itself in the x, y, and z-axis. Thus, the overlapping between s and s orbital would cover less area and so its strength will be less.
On the other hand, the area for p and p orbital overlapping will be more which will eventually increase the strength of the bond.
Also, overlapping between p orbital and s orbital will be more than s-s overlap but less than p-p overlap.
So the increasing order of strength of Sigma bond will be:
s−s< s−p<p−p
During the axial overlap of p-p orbitals, the electron density increases around the axis, so the bond formed is the strongest. Therefore, the strongest bond formed is when p-p orbital overlap occurs.
