Final Answer:
The Lewis structure of acetic acid (CH₃COOH) consists of a central carbon atom bonded to two oxygen atoms (carbonyl group), one oxygen atom through a single bond (hydroxyl group), and three hydrogen atoms. The appropriate set hybridization states for the three central atoms are sp² for the carbon in the carbonyl group, sp³ for the carbon in the hydroxyl group, and sp³ for the oxygen in the hydroxyl group.
Step-by-step explanation:
In the Lewis structure of acetic acid (CH₃COOH), the central carbon atom forms three sigma bonds with two oxygen atoms in the carbonyl group and one oxygen atom in the hydroxyl group. The carbon in the carbonyl group exhibits sp² hybridization since it forms a sigma bond with each of the three surrounding atoms. The carbon in the hydroxyl group forms sigma bonds with three atoms, including one oxygen and two hydrogen atoms, resulting in sp³ hybridization.
Additionally, the oxygen atom in the hydroxyl group forms a sigma bond with the carbon atom in the hydroxyl group and also has two lone pairs of electrons. The oxygen atom adopts sp³ hybridization to accommodate the sigma bond and the lone pairs of electrons. Therefore, the appropriate set hybridization states for the three central atoms in acetic acid are sp² for the carbon in the carbonyl group, sp³ for the carbon in the hydroxyl group, and sp³ for the oxygen in the hydroxyl group.
In summary, understanding the hybridization states of atoms in acetic acid is essential for describing its molecular geometry and predicting its reactivity in chemical reactions. The hybridization states provide insights into the arrangement of orbitals and the overall structure of the molecule.