What is the hybridization of a Nitrogen atom if it forms two sigma and two pi bonds. The answer is sp3. Please explain?
What is the hybridization of a...
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I'm thinking it would have 1 single bond and 1 triple bond.
Single bond= 1 sigma bond
Double bond= 1 sigma and 1 pi bonds
Triple bond= 1 sigma and 2 pi bonds
If you have 2 sigmas and 2 pi bonds, you can only have 1 single and 1 triple and stay within the octet rule.
so I guess it should be sp hybridized.
Single bond= 1 sigma bond
Double bond= 1 sigma and 1 pi bonds
Triple bond= 1 sigma and 2 pi bonds
If you have 2 sigmas and 2 pi bonds, you can only have 1 single and 1 triple and stay within the octet rule.
so I guess it should be sp hybridized.
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You can't have pi bonds and still be sp3. Even if you had the single and triple bond, that's still an sp hybridization. sp3 is 4 sigma bonds, think of a carbon atom.
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An atom that has 2 sigma and 2 pi bonds can either have a triple bond and a single bond or two double bonds. In either case, it is sp hybridized.
Put in another way, for an atom to have two pi bonds, it needs 2 unhybridized p orbitals. Since there are three p orbitals, only 1 p is available to hybridize with s.
In any case, it is not sp3 hybridized.
Put in another way, for an atom to have two pi bonds, it needs 2 unhybridized p orbitals. Since there are three p orbitals, only 1 p is available to hybridize with s.
In any case, it is not sp3 hybridized.
Okay. I'm glad all these posts agree with what I was thinking. I came across that question in an exam (https://www.ada.org/oat/oat_sample_test.pdf , question 93, page 20) and was really confused because the answer really was sp3 and I was thinking it should be sp, so I thought I was missing some important piece of knowledge. Thanks.
