What types of hybridization of carbon are in the compound ethene CH2CH2?
Question 2 options:
a) sp3
b) sp2
c) sp
d) answers b & c are possible
e) more information is required to answer this question.
is it b)?
Yes, the correct answer is b) sp2. In the compound ethene (CH2CH2), each carbon atom is bonded to three other atoms, resulting in a trigonal planar geometry. This indicates sp2 hybridization, where the carbon atom forms three sigma bonds with neighboring atoms using three of its available orbitals. The remaining p orbital is unhybridized and forms a pi bond with the neighboring carbon atom.
Yes, the correct answer is b) sp2.
Yes, the correct answer is b) sp2.
To determine the types of hybridization present in the compound ethene (CH2CH2), we need to consider the bonding and the number of sigma (σ) bonds surrounding the carbon atoms.
In ethene, each carbon atom is bonded to three other atoms - two hydrogens and one other carbon atom. Therefore, we have a total of four σ bonds around each carbon atom.
The hybridization of an atom is determined by counting the total number of bonded atoms and lone pairs around it. The number of hybrid orbitals formed is equal to the sum of the sigma bonds and lone pairs. Let's analyze the carbon atom in ethene:
Each carbon is bonded to three other atoms (two hydrogens and one carbon), meaning it has three sigma (σ) bonds. Additionally, there are no lone pairs of electrons on the carbon atom.
The relationship between the number of sigma bonds and the type of hybridization is as follows:
- sp3 hybridization: four sigma bonds (tetrahedral arrangement)
- sp2 hybridization: three sigma bonds (trigonal planar arrangement)
- sp hybridization: two sigma bonds (linear arrangement)
Since each carbon in ethene has three sigma bonds, it undergoes sp2 hybridization. Therefore, option b) sp2 is the correct answer.