Western Governors University (WGU) BIO1010 C190 Introduction to Biology Practice Exam

Hydrogen bonds are especially significant in water due to the unique polar nature of water molecules. Each water molecule consists of one oxygen atom covalently bonded to two hydrogen atoms, giving it a partial negative charge near the oxygen atom and a partial positive charge near the hydrogen atoms. This polarity allows water molecules to attract each other through hydrogen bonds, which occur between the positively charged hydrogen of one molecule and the negatively charged oxygen of another.

These hydrogen bonds lead to water's high surface tension, its ability to dissolve many substances, and its unique thermal properties. For example, water's high specific heat capacity means it can absorb a lot of heat without a significant change in temperature, which is critical for regulating climate and supporting living organisms. The hydrogen bonding in water also contributes to its solid state (ice) being less dense than its liquid state, allowing ice to float, which is vital for aquatic ecosystems.

In contrast, the other substances listed do not exhibit significant hydrogen bonding. Oxygen gas is nonpolar, carbon dioxide has a linear structure and is also nonpolar, while amino acids can form hydrogen bonds but are more complex and varied in their bonding capabilities. Thus, the emphasis on water illustrates the crucial role hydrogen bonds play in many of its unique properties vital