Final answer:
When ammonia (NH₃) is dissolved in water, the hydrogen bonds between NH₃ molecules persist, although they are generally weaker compared to the more predominant hydrogen bonds established between NH₃ and water molecules. The introduction of water, with its highly polar nature and ability to engage in extensive hydrogen bonding, influences the intermolecular forces, leading to a dynamic equilibrium between NH₃-NH₃ and NH₃-water hydrogen bonding interactions in the solution.
Step-by-step explanation:
Yes, even when ammonia (NH₃) is dissolved in water and forms hydrogen bonds with water molecules, NH₃-NH₃ hydrogen bonds still exist to some extent. However, the strength of NH₃-NH₃ hydrogen bonding is weaker compared to the hydrogen bonds formed between NH₃ and water molecules.
In a pure liquid or gaseous state, ammonia molecules can form hydrogen bonds with each other due to the presence of the lone pair of electrons on the nitrogen atom. When dissolved in water, ammonia molecules can interact with water molecules through hydrogen bonding, where the hydrogen atoms of water molecules interact with the lone pair of electrons on the nitrogen atom of NH₃.
The interaction between NH₃ molecules in water is a dynamic process. While NH₃-NH₃ hydrogen bonds are still present, they are often disrupted and replaced by stronger NH₃-water hydrogen bonds. Water molecules are highly polar and form extensive hydrogen bonding networks, so the NH₃ molecules tend to interact more favorably with water molecules.
In summary, NH₃-NH₃ hydrogen bonds still exist to some extent in an NH₃ solution in water, but the dominant interactions involve hydrogen bonding between NH₃ and water molecules.