Chemistry Chapter 3: The Chemistry of Water

In a water molecule, the shared electrons spend more time near the oxygen atom, creating a slightly negative charge on the oxygen and a slightly positive charge on the hydrogens. This uneven charge distribution makes water polar, allowing it to form hydrogen bonds with other water molecules.

A type of weak bond that occurs between a slightly positive hydrogen atom of one molecule and a slightly negative atom of another molecule, typically oxygen or nitrogen. It's a crucial force in water molecules.

The ability of water molecules to stick together due to hydrogen bonds. This leads to surface tension and plays a role in the transport of water in plants.

The attraction between water molecules and other substances due to polarity. It helps water to climb up plant stems against gravity.

A property of water that allows it to resist breaking or stretching due to strong cohesive forces between its molecules, making it act like a thin, invisible film.

Water's ability to absorb and release heat energy with minimal temperature change. This helps moderate temperature fluctuations in the environment.

When water freezes, it expands due to the formation of a crystalline structure. This helps insulate aquatic life and prevents lakes from freezing solid.

Water's ability to dissolve many substances due to its polarity. This helps transport nutrients and remove waste in living organisms.

The amount of heat required to raise the temperature of 1 gram of water by 1 degree Celsius.

The energy associated with the random movement of atoms or molecules within a substance.

The amount of heat energy that must be absorbed or released to change the temperature of 1 gram of a substance by 1 degree Celsius.

Hydrogen bonds between water molecules require a significant amount of energy to break, resulting in water's high specific heat.

Water's high specific heat helps moderate temperature fluctuations, preventing extreme changes in temperature.

The transformation of a substance from a liquid to a gas.

The amount of heat required to convert 1 gram of a liquid into a gas.

The cooling effect that occurs when a liquid evaporates, taking heat away from the remaining liquid or surrounding environment.

Water's unusual property where ice floats on liquid water due to a less dense crystalline structure.

A measure of how much mass is contained in a given volume. Density explains why ice floats on water.

A solution is a homogeneous mixture of substances. The solvent is the dissolving agent, and the solute is what gets dissolved. Water is the universal solvent.

The uneven distribution of electrons in a water molecule creates a slightly negative charge on the oxygen and a slightly positive charge on the hydrogens. This makes water a polar molecule.

Water's ability to dissolve many substances due to its polarity. Essential for life's processes.

Substances attracted to water, like sugar. They contain polar regions.

Substances repelled by water, like oil. They primarily contain nonpolar regions.

A weak bond formed between hydrogen atoms and a highly electronegative atom like oxygen. Crucial for water's properties.

The sum of the atomic masses of all atoms in a molecule.

A unit used to measure the amount of a substance, containing 6.02 x 10^23 molecules.

The concentration of a solute in a solution, expressed as moles of solute per liter of solution.

A substance that increases the H+ concentration of a solution, also known as a 'proton donor.'

A substance that can accept H+ ions in a solution, also known as a 'proton acceptor.'

The negative logarithm of the H+ concentration in a solution, measured on a scale from 0 to 14.

A state where the rate of a forward reaction equals the rate of the reverse reaction, in this case, the continuous dissociation and reformation of water molecules.

The process of water molecules splitting into hydrogen ions (H+) and hydroxide ions (OH-), which occurs at the same rate as their reformation.