Consider the Lewis structure for acetic acid, which is known as vinegar:

(a) What are the approximate bond angles about each of the two carbon atoms, and what are the hybridizations of the orbitals on each of them?

Key Concepts

Hybridization

Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In the case of carbon atoms, sp, sp², and sp³ hybridizations correspond to different types of bonding and geometry. For example, sp hybridization involves the mixing of one s and one p orbital, resulting in two equivalent sp hybrid orbitals, which are oriented linearly at 180°.

Bond Angles

Bond angles are the angles formed between adjacent bonds in a molecule, which are influenced by the hybridization of the central atom. For sp hybridized carbon atoms, the bond angles are approximately 180°, while sp² hybridized carbons have bond angles of about 120°, and sp³ hybridized carbons have angles close to 109.5°. Understanding these angles helps predict molecular geometry.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons. They provide a visual representation of how atoms are connected and help in determining the hybridization and bond angles. In acetic acid, the Lewis structure reveals the arrangement of atoms and the types of bonds, which are essential for analyzing the molecular geometry.