What is the hybridization of both carbons in:
C=CH2 ?
Are you sure you have typed this correctly? H2C=CH2 I might believe but not C=CH2.
Well, H2C=c=Ch2 is the original question, but for part B) I'm supposed to depict the hybrid orbital formation using the orbital diagrams for the central carbon and one of the terminal carbon atoms in the molecule.
Both C atoms are sp2.
Just remember, sp3 is C(4 bond) like CH4
sp2 = C(3 bonds) like H2C=
sp = C(2 bonds) like HCtriplebond
To determine the hybridization of the carbons in C=CH2, we need to follow a few steps.
Step 1: Determine the number of sigma bonds around each carbon.
In the given molecule, there are two carbons, labeled as C1 and C2. Counting the number of sigma bonds around each carbon:
- C1: It is directly connected to two other atoms (one hydrogen and one carbon), so it forms two sigma bonds.
- C2: It is directly connected to three other atoms (two hydrogens and one carbon), so it forms three sigma bonds.
Step 2: Determine the number of lone pairs on each carbon.
In the given molecule, there are no lone pairs on either carbon.
Step 3: Calculate the hybridization.
The hybridization of an atom is determined by adding the number of sigma bonds and the number of lone pairs and using it to identify the appropriate hybridization state.
In the case of C1:
Number of sigma bonds: 2
Number of lone pairs: 0
2 + 0 = 2
Based on the sum, C1 is sp hybridized.
In the case of C2:
Number of sigma bonds: 3
Number of lone pairs: 0
3 + 0 = 3
Based on the sum, C2 is sp2 hybridized.
Therefore, the hybridization of C1 is sp and the hybridization of C2 is sp2.