Final answer:
Hydrogen bonds in water molecules lead to strong cohesive properties and a higher boiling point, contributing to water's life-sustaining abilities and stability of biological molecules like DNA and proteins.
Step-by-step explanation:
Hydrogen bonding in water molecules is a key factor in determining water's unique properties. These hydrogen bonds occur when there is an attraction between the slightly positive hydrogen atoms and the slightly negative oxygen atoms of adjacent water molecules. This bonding allows water to have a higher boiling point than most molecules of similar mass, meaning water remains a liquid at room temperature when other similar-sized molecules are gases.
The bent shape of the water molecule and the presence of two hydrogen atoms allow each water molecule to form hydrogen bonds with up to four neighbors, creating a strong network of interactions. These interactions are responsible for the strong cohesive properties of water, such as surface tension and water's ability to form droplets. These properties are essential for life, as they contribute to how water travels through plant tissues and regulates temperature in the environment.
Although individual hydrogen bonds are weak and can be easily broken, their collective strength is significant, and this is what gives water its life-sustaining properties. Hydrogen bonding also stabilizes biological molecules like proteins and DNA, making it fundamental to the structure and function of living organisms.