- Joined
- Sep 5, 2008
- Messages
- 511
- Reaction score
- 1
Molecular orbitals in hydrocarbons are formed
between the 1s atomic orbital of hydrogen and the sp,
sp2, or sp3 hybrid atomic orbitals of carbon. Which
choice correctly lists the energy level of the C-H
bonds, from lowest to highest?
A. C6H6, HC≡CH, CH4
B. H2C=CH2, CH4, C6H6
C. C6H6, CH4, H2C=CH2
D. HC≡CH, C6H6, CH4
Here they are asking for the strength of C-H and not C-C, but since we are just talking about hybridized molecular orbitals, won't the trend go CH4< C6H6<HC≡CH
C-C is longer bond, less strength and is easy to break
Kaplan says that the more S character, the less energy, which seems counter-intuitive since EK says as bond length increases, the bond strength and energy both decrease. I know that triple bonds are stronger than single bonds and are at a higher energy level. Can someone plzz explain!!
between the 1s atomic orbital of hydrogen and the sp,
sp2, or sp3 hybrid atomic orbitals of carbon. Which
choice correctly lists the energy level of the C-H
bonds, from lowest to highest?
A. C6H6, HC≡CH, CH4
B. H2C=CH2, CH4, C6H6
C. C6H6, CH4, H2C=CH2
D. HC≡CH, C6H6, CH4
Here they are asking for the strength of C-H and not C-C, but since we are just talking about hybridized molecular orbitals, won't the trend go CH4< C6H6<HC≡CH
C-C is longer bond, less strength and is easy to break
Kaplan says that the more S character, the less energy, which seems counter-intuitive since EK says as bond length increases, the bond strength and energy both decrease. I know that triple bonds are stronger than single bonds and are at a higher energy level. Can someone plzz explain!!