between NH3 and CCl4 which has greater bond angle?Explain in detail with explantation
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The bond angle of a molecule depends on several factors. We have to look at all the factors and then decide the result according to them.
The difference in bond angles in NF3NFX3 and NH3NHX3 is only determined by the electronegativity difference between the central atom and the bonded atom. As FFis more electronegative than HH, in NH3NHX3, bonding electron pair shifts more towards NN than they shift in NF3NFX3. So, the bond angle increases. There is no other effect at all in this case.
But in the case of NCl3NClX3, you can notice there is a lone pair on the central NN atom. Most importantly, there is an introduction of vacant low lying 3d3d orbital of ClCl where the lone pair of NN can delocalise. This effect is known as pπ−dπpπ−dπ backbonding. So, due to this backbonding, which is quite strong, the bond between NN and ClCladopts a significant double bond character.
Although the electronegativity difference is decreased in the case of NCl3NClX3 and bond pair is shifted away from central NN, this introduction of double-bond character increase the repulsion between the bond pairs even more, and that's why the bond angle increases.
So, in case of NF3NFX3 and NH3NHX3 there was no vacant and valence d orbitals either in FF or in HH. So, this backbonding doesn't occur there. But in NCl3NClX3, the case is different and more factors determine the bond angle. As the backbonding is much stronger, this effect overall dominates over the electronegativity factor and make the bond angle increase.
Experimental evidence of this double bond character: In NCl3NClX3, N−ClN−Cl bond length is 1.759 angstroms but N−ClN−Clsingle bond length is 1.91 angstroms. This indicates the presence of some partial double bond character which shrinks the bond length.
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The difference in bond angles in NF3NFX3 and NH3NHX3 is only determined by the electronegativity difference between the central atom and the bonded atom. As FFis more electronegative than HH, in NH3NHX3, bonding electron pair shifts more towards NN than they shift in NF3NFX3. So, the bond angle increases. There is no other effect at all in this case.
But in the case of NCl3NClX3, you can notice there is a lone pair on the central NN atom. Most importantly, there is an introduction of vacant low lying 3d3d orbital of ClCl where the lone pair of NN can delocalise. This effect is known as pπ−dπpπ−dπ backbonding. So, due to this backbonding, which is quite strong, the bond between NN and ClCladopts a significant double bond character.
Although the electronegativity difference is decreased in the case of NCl3NClX3 and bond pair is shifted away from central NN, this introduction of double-bond character increase the repulsion between the bond pairs even more, and that's why the bond angle increases.
So, in case of NF3NFX3 and NH3NHX3 there was no vacant and valence d orbitals either in FF or in HH. So, this backbonding doesn't occur there. But in NCl3NClX3, the case is different and more factors determine the bond angle. As the backbonding is much stronger, this effect overall dominates over the electronegativity factor and make the bond angle increase.
Experimental evidence of this double bond character: In NCl3NClX3, N−ClN−Cl bond length is 1.759 angstroms but N−ClN−Clsingle bond length is 1.91 angstroms. This indicates the presence of some partial double bond character which shrinks the bond length.
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