Chemistry and Water
Water is literally life-changing! Its polarity and hydrogen bonding give it special properties that make life possible. Water molecules stick to each other (cohesion), creating surface tension that lets insects walk on water and keeps oceans together. They also stick to other surfaces (adhesion), allowing capillary action that pulls water up plant roots.
Water's high specific heat means it resists temperature change, which helps moderate air temperatures and stabilizes oceans. Its high heat of vaporization enables cooling through evaporation (think sweating), while its heat of fusion stabilizes aquatic environments. As the "universal solvent," water dissolves minerals, flushes toxins, and transports nutrients to cells.
The macromolecules that make up living things contain primarily carbon, hydrogen, oxygen, and nitrogen, with phosphorus and sometimes sulfur. These elements form different types of bonds that determine molecular structure: covalent bonds (shared electrons), ionic bonds (between charged ions), and hydrogen bonds (between partial charges).
Quick Tip: Remember that water's polarity is the key to understanding all its life-supporting properties. The slightly positive hydrogen atoms and slightly negative oxygen create the hydrogen bonds that give water its unique characteristics!
Carbon is especially important in biology because it has four valence electrons, allowing it to form complex molecules. It moves through the environment as CO₂ and is used by organisms to build new molecules for storage and cell formation.
Isomers - molecules with the same formula but different structures - are biologically crucial. Structural isomers have different covalent bond arrangements, geometric isomers differ in arrangement around double bonds (cis or trans), and enantiomers are mirror images that can have dramatically different biological effects.