1. Water's Properties & the Chemistry of Life
Life depends on water's unique properties, nearly all of which emerge from its polarity and its capacity to form hydrogen bonds with other water molecules and with other polar or charged substances.
Water is a polar molecule (bent shape, unequal electron sharing between O and H) that forms hydrogen bonds; these bonds explain water's high specific heat (resists temperature change, buffers organisms and climate), high heat of vaporization (evaporative cooling), cohesion (surface tension, capillary action) and adhesion (water climbs against gravity in plant xylem), and lower density as a solid than a liquid (ice floats, insulating aquatic ecosystems). Water is the ``universal solvent'' for polar and ionic solutes because of hydration shells. $pH = -$; buffers resist pH change by absorbing or releasing H$^+$.
Cohesion (water molecules bonding to EACH OTHER, producing surface tension) vs.\ adhesion (water molecules bonding to OTHER polar surfaces, producing capillary action in xylem).
Students attribute water's high specific heat to a strong covalent O--H bond breaking; the property comes from the energy needed to break HYDROGEN BONDS between separate water molecules, not the covalent bonds within one molecule.
Polar + H-bonds $arrow$ high specific heat, cohesion/adhesion, universal solvent, ice floats.