Food & Drink0 min ago
Bonding of Carbon
5 Answers
Can anyone explain the bonding and structure of carbon in benzene to me with reference to the electron orbitals and hybridisation?
Here's what I already know:
C<sup>12 electron configuration: 1s2, 2s2, 2p2
Excitation causes one of the 2s electrons to become a 2p electron.
Then 2 of the 2p electrons and one of the 2s electrons hybridise formind a 2 sp2 hybrid orbital. The C-C bonding in benzene in formed by the single overlap of the 2 sp2 orbitals on adjacent C atoms. The bond formed is 0.139nm long - in between the length of a single bond and a double bond. Is the C-H bond the same?
Each carbon has 1 valence electron (which occupies a P orbital) remaining. The Pi bond is formed by the double overlap of the P orbitals.
Have I got anything wrong or missed anything?
I'm an A Level student and I inquired about this - my teacher briefly explained and I wanted to see how much I remember and how much of it is right. I have an interview at Newcastle University for Medicine on Monday and I think I'll mention this if they ask whether I've encountered anything interesting in the subjects I'm studying.
Incidentally, how does the bonding in a saturated carbon compound differ?
Thanks in advance,
SarCaustic
Here's what I already know:
C<sup>12 electron configuration: 1s2, 2s2, 2p2
Excitation causes one of the 2s electrons to become a 2p electron.
Then 2 of the 2p electrons and one of the 2s electrons hybridise formind a 2 sp2 hybrid orbital. The C-C bonding in benzene in formed by the single overlap of the 2 sp2 orbitals on adjacent C atoms. The bond formed is 0.139nm long - in between the length of a single bond and a double bond. Is the C-H bond the same?
Each carbon has 1 valence electron (which occupies a P orbital) remaining. The Pi bond is formed by the double overlap of the P orbitals.
Have I got anything wrong or missed anything?
I'm an A Level student and I inquired about this - my teacher briefly explained and I wanted to see how much I remember and how much of it is right. I have an interview at Newcastle University for Medicine on Monday and I think I'll mention this if they ask whether I've encountered anything interesting in the subjects I'm studying.
Incidentally, how does the bonding in a saturated carbon compound differ?
Thanks in advance,
SarCaustic
Answers
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There must be some good sources of information on the internet, but basically you're correct. You should note that the C-H bond is a different length to the C-C (should be longer, but you can look it up).
In a saturated organic molecule you're only dealing with 2sp3 orbitals, arranged roughly tetrahedrally (depending on the other atoms involved.
In a saturated organic molecule you're only dealing with 2sp3 orbitals, arranged roughly tetrahedrally (depending on the other atoms involved.
It is not the electrons which hybridise but the atomic orbitals.
In benzene, sp2 hybridisation takes place producing 3 hybrid orbitals at 120 degrees to each other. These hybrid orbitals each containing one electron form 3 sigma bonds with two carbon atoms and one hydrogen atom.
That leaves one unhybridised p orbital, containing one electron, on each carbon atom. These overlap around the ring to form pi bonds.
In benzene the bond lengths are: C-C 140 pm and C-H 109 pm. (Values vary slighly depending on where you look them up).
In saturated compounds sp3 hybridisation takes place producing 4 identical orbitals in a tetrahedral arrangement. These form sigma bonds with other carbon atoms and hydrogen atoms. The bond length is 154 pm.
In benzene, sp2 hybridisation takes place producing 3 hybrid orbitals at 120 degrees to each other. These hybrid orbitals each containing one electron form 3 sigma bonds with two carbon atoms and one hydrogen atom.
That leaves one unhybridised p orbital, containing one electron, on each carbon atom. These overlap around the ring to form pi bonds.
In benzene the bond lengths are: C-C 140 pm and C-H 109 pm. (Values vary slighly depending on where you look them up).
In saturated compounds sp3 hybridisation takes place producing 4 identical orbitals in a tetrahedral arrangement. These form sigma bonds with other carbon atoms and hydrogen atoms. The bond length is 154 pm.
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