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Topic: Hybridization and bond length  (Read 1028 times)

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Offline Zookid239

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Hybridization and bond length
« on: January 12, 2023, 08:42:34 AM »
One molecule has HC triple bonded to a carbon that is single bonded on the other side to another carbon with 3 single bonds to 3 CH3 molecules. The second molecule has a carbon atom single bonded to 3 H atoms and another carbon atom which is single bonded to 3 CH3 molecules. Is the single bond between the C atom triple bonded to HC and the C atom single bonded to 3 CH3 molecules shorter and stronger than the single bond between the C bonded to two sp3 carbon atoms?

Offline Corribus

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Re: Hybridization and bond length
« Reply #1 on: January 12, 2023, 11:19:14 AM »
First, it would be helpful if you drew the molecule using SMILES, used an appropriate compound name, or uploaded a drawing. That way it is easy to know what molecule you are talking about.

Second, it is a forum policy that you have to show or describe your work to receive help.
What men are poets who can speak of Jupiter if he were like a man, but if he is an immense spinning sphere of methane and ammonia must be silent?  - Richard P. Feynman

Offline Vidya

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Re: Hybridization and bond length
« Reply #2 on: January 20, 2023, 07:08:56 AM »
One molecule has HC triple bonded to a carbon that is single bonded on the other side to another carbon with 3 single bonds to 3 CH3 molecules. The second molecule has a carbon atom single bonded to 3 H atoms and another carbon atom which is single bonded to 3 CH3 molecules. Is the single bond between the C atom triple bonded to HC and the C atom single bonded to 3 CH3 molecules shorter and stronger than the single bond between the C bonded to two sp3 carbon atoms?
Yes it is correct.
sp3 C  bonded to sp3 carbon is longer and weaker than sp carbon bonded to sp3 carbon.
Remember size of orbitals decreases in this order.- sp carbon < sp2 carbon < sp3 carbon

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