Thermodynamics

Ionization Energy

The energy required to remove an electron from an atom.

Electron Configuration

The distribution of electrons in an atom's orbitals.

Cations

Positively charged ions formed by the loss of electrons.

Anions

Negatively charged ions formed by the gain of electrons.

Isotopes

Atoms with the same number of protons but different numbers of neutrons.

Photoelectron Spectroscopy (PES)

A technique that measures the binding energies of electrons in an atom.

Bond Polarity

The distribution of electrical charge over the atoms in a bond.

Exothermic Reaction

A reaction that releases energy, resulting in a negative ΔH.

Le Chatelier's Principle

A principle stating that a system at equilibrium will shift to counteract changes.

pH Scale

A scale that measures the acidity or basicity of a solution.

Empirical Formula

The simplest whole number ratio of atoms in a compound.

Molecular Formula

The actual number of atoms of each element in a molecule.

Gas Laws Relationships

Describes the relationship between pressure, volume, and temperature of gases.

Thermodynamic Favorability

Determines if a reaction is spontaneous based on changes in enthalpy and entropy.

Half-Life

The time required for half of a substance to decay or react.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals.

Strong Acids

Acids that completely dissociate in solution, e.g., HCl, HNO₃.

Strong Bases

Bases that completely dissociate in solution, e.g., NaOH, KOH.

Collision Theory

A theory that states for a reaction to occur, particles must collide with sufficient energy.

Equilibrium Constant (K)

A value that expresses the ratio of products to reactants at equilibrium.