In the hydrocarbon

(a) What is the hybridization at each carbon atom in the molecule?

Verified step by step guidance

1. Identify the number of regions of electron density (bonds and lone pairs) around each carbon atom.
2. Determine the hybridization based on the number of regions of electron density: 2 regions = sp, 3 regions = sp2, 4 regions = sp3.
3. For Carbon 1: It has 3 regions of electron density (1 double bond and 2 single bonds), so it is sp2 hybridized.
4. For Carbon 2: It has 3 regions of electron density (1 double bond and 2 single bonds), so it is sp2 hybridized.
5. For Carbon 3: It has 4 regions of electron density (4 single bonds), so it is sp3 hybridized.

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 form covalent bonds in molecules. The type of hybridization (sp, sp2, sp3, etc.) depends on the number of bonds and lone pairs around the central atom, influencing the geometry and bond angles of the molecule.

Carbon Atom Hybridization

In organic chemistry, carbon atoms can undergo different types of hybridization based on their bonding. For example, sp hybridization occurs when a carbon atom forms two double bonds or one triple bond, resulting in a linear geometry. In contrast, sp2 hybridization is seen in carbon atoms with one double bond and two single bonds, leading to a trigonal planar shape, while sp3 hybridization involves four single bonds, resulting in a tetrahedral geometry.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the hybridization of the central atom and the presence of lone pairs. Understanding molecular geometry is crucial for predicting the shape and reactivity of molecules, as it influences properties such as polarity, phase of matter, and biological activity.