Consider the following hydrocarbon:
a. What is the hybridization at each carbon atom in the molecule?

Verified step by step guidance

1. Identify the type of bonds around each carbon atom. Single bonds indicate sp3 hybridization, double bonds indicate sp2 hybridization, and triple bonds indicate sp hybridization.
2. For each carbon atom, count the number of atoms it is directly bonded to and the number of pi bonds it forms.
3. Determine the hybridization based on the number of sigma bonds and lone pairs around each carbon.
4. Recall that sp3 hybridization occurs with four sigma bonds or lone pairs, sp2 with three, and sp with two.
5. Assign the appropriate hybridization to each carbon atom based on the analysis of its bonding and geometry.

Key Concepts

Hybridization

Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals are used to explain the geometry of molecular bonding. For example, sp3 hybridization involves one s and three p orbitals, resulting in a tetrahedral shape, while sp2 hybridization involves one s and two p orbitals, leading to a trigonal planar shape.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the hybridization of the orbitals. Understanding molecular geometry is crucial for predicting the shape and reactivity of the molecule.

Valence Bond Theory

Valence Bond Theory (VBT) explains how atoms in a molecule bond through the overlap of their atomic orbitals. According to VBT, the type of hybridization at each atom can be determined by the number of bonds and lone pairs present. This theory helps in understanding the bonding characteristics and the resulting molecular structure of hydrocarbons.