The greater the extent of overlapping, the higher the probability of recognize the valence electron in in between the nuclei and hence the bond will be stronger & shorter.
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In MOT, this can be explained using Overlap Integral. This is exactly how Atkins depicts it :
In an easy terms, after developing a sigma-bond (a pre-requisite because that pi-bonds), the 2 atoms get locked along the inter-nuclear axis. As a result, the orbitals obtainable for pi-bonding deserve to only partly overlap, thus creating a weaker bond.
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As stated previously, it is due to the head-on overlap that sigma bonds and also the lateral overlap that pi-bonds.
The smaller sized overlap of pi bonds likewise explains why dual and triple bonds usually exist only for second row facets (C,N,O especially) and not for greater row elements. A C=C bond has a length of 133 pm. A Si-Si bond length is at about 186 pm, thus the donation of the pi-integral overlap is nearly negligible.
The inability of Silicium to kind strong pi bond is also one of the price why life on earth is carbon based and also not silicium based, due to the fact that the richness of organic tasiilaq.net is in part due to the capacity of carbon to form strong dual and triple bonds.
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answer Jun 19 "14 in ~ 3:49
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Pi bond involve party overlap if sigma bond entails head top top or axial overlap. Axial overlaps have greater degree of overlapping than sideways overlap.
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Unsaturated compounds (due to the presence of a double bond) are much more reactive than saturated compounds, due to the fact that the electron density at the internuclear axis is zero in a pi bond (in contrast to the sigma bond).
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