"Noting that the bond angle of an sp3 hybridized atom is 109.58 and that of an sp2 hybridized atom is 1208, do you expect the bond angle between two hybrid orbitals to increase or decrease as the s-character of the hybrids is increased?"
The answer key says that the bond angle increases as the s-character increases. Can someone explain why this is?
Thanks!
Textbook 2F.15: s-character and bond angle
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Re: Textbook 2F.15: s-character and bond angle
In this case the s-character increases as the p-character decreases, so increasing s-character would cause regions of electron density to decrease. Because an sp2 orbital has less regions of e- density than an sp3 orbital, the bond angles increase. Hope that helps!
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Re: Textbook 2F.15: s-character and bond angle
would an explanation be that s orbital is lower energy than p orbital so if s character of the hybrids increased then the energy would decrease meaning a decrease of electron density or the space the electron occupies has decreased causing an increase in bond angles?
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Re: Textbook 2F.15: s-character and bond angle
Does s & p character just mean how many s & p orbitals there are? like p character would be increasing from sp to sp2?
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