State the hybridisation of asterisked carbon in $\ce{CH3-CH=C^{✪}=CH2}$
I am not sure between $sp^2$ and $sp$ hybridization. Because of double bond I think it should be $sp^2$ but because of 2 $\pi$ bonds iI think $sp$.
So which one is correct?
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Sign up to join this communityState the hybridisation of asterisked carbon in $\ce{CH3-CH=C^{✪}=CH2}$
I am not sure between $sp^2$ and $sp$ hybridization. Because of double bond I think it should be $sp^2$ but because of 2 $\pi$ bonds iI think $sp$.
So which one is correct?
You must be clear that the hybridization is decided by the number of sigma electrons So for $\ce{CH4}$ the number of sigma electrons is 4 and so its hybridization is $sp^3$.
In your case: $\ce{CH3-CH=C^{✪}=CH2}$ the $*$ carbon is having 2 sigma and 2 pi bonds so its hybridization is $sp$.
Remember that possible hybridization for $\ce{C}$ are $sp^3$,$sp^2$ and $sp$.
As the asterisked carbon has two neighbors, the hybridization of this asterisked carbon is sp . i.e. the angle −CH=C✪=CH2 is 180 degrees.