Chem unit 7 review

aqueous

Referring to a solution where water is the solvent.

electrolyte

A substance that dissociates into ions when dissolved in water and conducts electricity.

nonelectrolyte

A substance that does not dissociate into ions in solution and does not conduct electricity.

solute

The substance that is dissolved in a solution.

dissolving

The process by which a solute becomes incorporated into a solvent, forming a solution.

solvent

The substance that does the dissolving in a solution.

solution

A homogeneous mixture composed of two or more substances.

surface tension

The elastic-like force existing on the surface of a liquid, caused by intermolecular forces.

homogeneous

A mixture that is uniform in composition throughout.

heterogeneous

A mixture that consists of visibly different substances or phases.

concentration

The amount of solute in a given volume of solvent.

dilute solution

A solution that contains a small amount of solute relative to the solvent.

immiscible

Two liquids that do not mix or form a homogeneous solution.

solubility

The maximum amount of solute that can dissolve in a solvent at a given temperature.

miscible

Two substances that can mix together in any proportion to form a homogeneous solution.

molarity

A way to express concentration, defined as the number of moles of solute per liter of solution.

saturated

A solution that cannot dissolve any more solute at a given temperature.

unsaturated

A solution that can still dissolve more solute at a given temperature.

supersaturated

A solution that contains more dissolved solute than it can normally hold at a given temperature.

polar molecule

A molecule with an uneven distribution of charges, leading to partial positive and negative charges.

solvation

The process of surrounding solute particles with solvent particles during the dissolution process.

Hydrogen bonding

A strong type of dipole-dipole interaction between molecules that have hydrogen attached to an electronegative atom.

ionic compound

A compound made up of cations and anions held together by ionic bonds.

hydrophobic

Literally means 'afraid of water'; refers to molecules that do not readily interact with water.

intermolecular forces (IMFs)

Forces that hold molecules together in a substance.

hexagonal lattice

The unique structure formed by water molecules in ice, leading to lower density.

crystallization

The process by which solute particles form a solid structure from a supersaturated solution.

dissociation

The process in which an ionic compound separates into its individual ions.

ions

Charged particles that result from the dissociation of an electrolyte.

octet rule

A chemical rule that reflects the observation that atoms of main group elements tend to bond in such a way that they have eight electrons in their valence shell.

saturation point

The point at which a solvent can no longer dissolve additional solute.

solvent separated

When solvent molecules surround and separate solute particles.

water polarity

A characteristic of water, where one end is slightly positive and the other end is slightly negative, leading to strong intermolecular forces.

pH

A scale used to specify the acidity or basicity of an aqueous solution.

NaCl

Sodium chloride, a strong electrolyte consisting of sodium and chloride ions.

sugar

A non-electrolyte that dissolves in water but does not dissociate into ions.

solubility curve

A graph that shows the relationship between solubility and temperature for a solute.

saturation

The state of a solution when it has dissolved the maximum amount of solute at a specific temperature.

heat effect

The change in temperature of a solvent when solute is dissolved into it.

gas solution

A type of solution where gases, like O2 and CO2, are dissolved in another gas.

liquid solution

A solution where solids or gases are dissolved in a liquid, such as saltwater.

solid solution

A homogeneous mixture of two or more substances in solid form, like alloys.

solubility product constant

A constant relating the solubility of a sparingly soluble salt to the concentration of its ions.

kinetic theory

The theory that explains the behavior of gases in terms of particles in constant motion.

dynamic equilibrium

A state of balance in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction.