[Imo]

What is the hybridization of the carbon in a compound with C+ making 3 bonds? sp3 or sp2? why?
Of the C- is sp3, right?

[Nescafe]

What is the hybridization of the carbon in a compound with C+ making 3 bonds? sp3 or sp2? why?
Of the C- is sp3, right?

H3C(+) is sp2
H3C(-) is sp3

Cheers,

Nescafé.

[Imo]

Really? Hmm...I heard that exists exceptions but i did not understand when the teacher said...do you know anything about?

[Nescafe]

Really? Hmm...I heard that exists exceptions but i did not understand when the teacher said...do you know anything about?

From my understanding it's all about the number of electrons around the atom. I guess if lets say the negative charge was in resonance you could say its Sp2/Sp3 as the charge is delocalized, but I can't think of any particular "exceptions". If anyone else has anything to add please do so,

Cheers,

Nescafé.

[fledarmus]

This might help you - http://en.wikipedia.org/wiki/VSEPR_theory

A carbon atom with three single bonds and a -1 charge has picked up an extra electron - it has three bonding pairs of electrons and one non-bonding pair. Consequently, it will adopt a trigonal pyramidal shape, with sp³ hybridization.

A carbon atom with three single bonds and a +1 charge as lost an electron - it has three bonding pairs of electrons and no non-bonding pairs. Consequently, it will adopt a trigonal planar shape, with sp² hybridization.

[Imo]

Yes, my teacher make a problem that was a compound in resonance. We say that the carbon has the hybridization of the compound that is more stable? my teacher seems not accept two answers : sp2/sp3 , only one, sp2 or sp3...

[Nescafe]

Yes, my teacher make a problem that was a compound in resonance. We say that the carbon has the hybridization of the compound that is more stable? my teacher seems not accept two answers : sp2/sp3 , only one, sp2 or sp3...

I can't give you the answer you kind of answered it yourself. The more stable would mean what?

I'm guessing you are talking about a negative charge? I already gave you the Answer in my previous post.

Cheers,

Nescafé.