Quantcast

Bootcamp GC question

This forum made possible through the generous support of SDN members, donors, and sponsors. Thank you.

helloboys

Full Member
5+ Year Member
Joined
May 18, 2016
Messages
278
Reaction score
188

Members don't see this ad.
How would the bond energy and bond length of a carbon-carbon bond in C2H6 compare to C2H4?

Answer: The bond energy for C2H4 would be greater, but the bond length would be shorter.

I understand that bond length would be shorter because single vs double bond. But wouldn't the bond energy for C2H4 be less than C2H6 because C2H4 has a double bound, and therefore more stable, which means it will have less energy?
 

themuffinman11

Full Member
5+ Year Member
Joined
Feb 14, 2017
Messages
167
Reaction score
130
A C=C bond has a smaller bond length, meaning it will take more energy to break that carbon-carbon double bond. I think you are getting bond energy mixed up with like the energy that a molecule exists in because in that case we think of a more stable molecule existing at a lower energy state (ex. cyclohexane conformations or newman projections)
 
Top