AP Chem Review

A collection of flashcards covering key terms and definitions related to chemical principles, atomic structure, chemical reactions, and thermodynamics.

Atomic Structure

The arrangement and organization of subatomic particles, including protons, neutrons, and electrons, within an atom.

Isotopes

Atoms of an element that have the same number of protons but different numbers of neutrons.

Avogadro’s number

6.022 x 10^23, the number of atoms, ions, or molecules in one mole of a substance.

Molarity (M)

A measure of concentration representing the number of moles of solute per liter of solution.

Electron Configuration

The distribution of electrons in an atom's orbitals, usually described using the spdf notation.

Periodic Trends

The predictable patterns in the properties of elements as one moves across or down the periodic table.

Ionization Energy

The energy required to remove an electron from an atom in its gaseous state.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Covalent Bond

A chemical bond formed when two atoms share electrons.

Ionic Bond

A type of chemical bond that occurs when electrons are transferred from one atom to another, forming oppositely charged ions.

Hydrogen Bond

A weak attraction between a hydrogen atom, which is covalently bonded to an electronegative atom, and another electronegative atom.

London Dispersion Forces

Weak intermolecular forces that result from temporary shifts in electron density in molecules.

Le Chatelier’s Principle

A principle stating that if a dynamic equilibrium is disturbed, the position of equilibrium shifts to counteract the change.

Equilibrium Constant (K)

A number that expresses the relationship between the concentrations of reactants and products at equilibrium.

pH

A scale used to specify the acidity or basicity of an aqueous solution, calculated as the negative logarithm of the hydrogen ion concentration.

Buffer Solution

A solution that resists changes in pH when small amounts of acid or base are added.

Gibbs Free Energy (ΔG)

A thermodynamic potential that measures the useful work obtainable from a system at constant temperature and pressure.

Redox Reaction

A type of reaction that involves the transfer of electrons between two species.

Catalyst

A substance that increases the rate of a chemical reaction without undergoing permanent chemical change itself.

Activation Energy (Ea)

The minimum energy required for a chemical reaction to occur.