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Hybridization of C2and C3of H3C −− CH = C = CH −− CH3are
- a)Sp, Sp3
- b)Sp2, Sp2
- c)Sp2, Sp
- d)None of the above
Correct answer is option 'C'. Can you explain this answer?
Most Upvoted Answer
Hybridization ofC2andC3ofH3C−−CH=C=CH−−CH3area...
The first carbon atom forms four sigma bonds, three with Hydrogen and one with carbon. So, the carbon here is sp3 hybridised.The second carbon atom forms three sigma bonds and one pi bond. The three sigma bonds can be possible only when carbon is sp2 hybridised. The fourth electron forms a pi overlap with an electron from third carbon atom.
Carbon atom 3 forms two sigma bonds and is sp hybridised. The two p electrons form a pi bond with p electrons of the neighbouring carbon atoms.Carbon atom 4 is similar to carbon 2, forms 3 sigma bonds and is sp2 hybridised.
As the aldehyde formed has molar mass of 44u, so the aldehyde is acetaldehyde or ethanal. The alkene that gives rise to ethanal, is but-2-ene. Ozonolysis leads to breaking the alkene molecule into two molecules at the double bond. As only one product, ethanal is formed, two carbon atoms surround the two sides of the double bond.
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Community Answer
Hybridization ofC2andC3ofH3C−−CH=C=CH−−CH3area...
To determine the hybridization of carbon atoms C2 and C3 in H3C, we need to first draw the Lewis structure of the molecule.
H3C can be represented as:
H - C - C - H
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H
In this structure, carbon atom C2 is bonded to three hydrogen atoms and one carbon atom (C3), while carbon atom C3 is bonded to two hydrogen atoms and one carbon atom (C2).
Now, let's determine the hybridization of C2 and C3.
To do this, we count the number of regions of electron density around each carbon atom. This includes the number of bonded atoms and lone pairs.
For C2:
- C2 is bonded to three hydrogen atoms and one carbon atom (C3). This gives a total of 4 regions of electron density.
For C3:
- C3 is bonded to two hydrogen atoms and one carbon atom (C2). This also gives a total of 3 regions of electron density.
To determine the hybridization, we use the following guidelines:
- 2 regions of electron density: sp hybridization
- 3 regions of electron density: sp2 hybridization
- 4 regions of electron density: sp3 hybridization
Based on this, we can conclude that carbon atom C2 has sp3 hybridization (since it has 4 regions of electron density), and carbon atom C3 has sp2 hybridization (since it has 3 regions of electron density).
H3C can be represented as:
H - C - C - H
|
H
In this structure, carbon atom C2 is bonded to three hydrogen atoms and one carbon atom (C3), while carbon atom C3 is bonded to two hydrogen atoms and one carbon atom (C2).
Now, let's determine the hybridization of C2 and C3.
To do this, we count the number of regions of electron density around each carbon atom. This includes the number of bonded atoms and lone pairs.
For C2:
- C2 is bonded to three hydrogen atoms and one carbon atom (C3). This gives a total of 4 regions of electron density.
For C3:
- C3 is bonded to two hydrogen atoms and one carbon atom (C2). This also gives a total of 3 regions of electron density.
To determine the hybridization, we use the following guidelines:
- 2 regions of electron density: sp hybridization
- 3 regions of electron density: sp2 hybridization
- 4 regions of electron density: sp3 hybridization
Based on this, we can conclude that carbon atom C2 has sp3 hybridization (since it has 4 regions of electron density), and carbon atom C3 has sp2 hybridization (since it has 3 regions of electron density).
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