Draw the Lewis structures for acetic acid and ammonia and show how they can hydrogen bond with one another.

To understand how acetic acid (CH₃COOH) and ammonia (NH₃) can form hydrogen bonds, we first need to draw their Lewis structures.

Lewis Structure of Acetic Acid (CH₃COOH)

Acetic acid consists of a methyl group (CH₃) attached to a carboxyl group (COOH). The Lewis structure can be represented as:

   H   O
   |  ||
 H-C--C  
       |  
       O-H
       

Here, the carbon atom in the carboxyl group is double-bonded to one oxygen (O) and single-bonded to another oxygen (O), which is also bonded to a hydrogen atom (H). The other carbon is single-bonded to three hydrogen atoms (H).

Lewis Structure of Ammonia (NH₃)

Ammonia consists of a nitrogen atom bonded to three hydrogen atoms. Its Lewis structure looks like this:

       H
       |
   H - N - H
       |
       H

The nitrogen atom has a lone pair of electrons, which plays a crucial role in hydrogen bonding.

Hydrogen Bonding Between Acetic Acid and Ammonia

Hydrogen bonds occur when a hydrogen atom is attracted to an electronegative atom, such as oxygen or nitrogen. In this case, the hydrogen bond can form between the hydrogen atom of the hydroxyl (O-H) group in acetic acid and the nitrogen atom in ammonia that has a lone pair.

The hydrogen bond can be illustrated as follows:

   H   O       H
   |  ||       |
 H-C--C  +   N-H
       |       |
       O-H     H

In this interaction, the lone pair on the nitrogen atom of ammonia attracts the hydrogen atom of the hydroxyl group from acetic acid, forming a hydrogen bond. This interaction is essential in various biological and chemical processes, contributing to the properties of substances like water and biological molecules.