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Activation Energy
Minimum energy needed to be added to a system for a chemical reaction to occur.
Alpha Particle
He2+; 2 protons, mass number = 4, 2+ charge; highly ionizing particle with low energy.
Anion
Negatively charged ion.
Arrhenius Acid
Donates a H+ ion.
Arrhenius Base
Donates a OH- ion.
Atom
Smallest unit of ordinary matter with the properties of a chemical element.
Atomic Mass
Average of all naturally occurring isotopes.
Atomic Number
Number of protons that defines the atom.
Beta Particle
-1 proton, mass number = 0; medium ionizing ability and medium energy.
Boiling
Phase change from a liquid to a gas.
Bronsted-Lowry Acid
Donates a proton (H+).
Bronsted-Lowry Base
Accepts a proton (H+).
Calorimetry
Method for measuring heat gained/lost by a system during a chemical reaction.
Catalyst
Lowers activation energy; not a reactant or product.
Cation
Positively charged ion.
Chemical Equilibrium
Rate of the forward reaction equals the rate of the reverse reaction.
Condensation
Phase change from a gas to a liquid.
Covalent Bond
Bond formed by sharing electrons between atoms.
Deposition
Phase change from a gas to a solid.
Dipole-Dipole
Permanent intermolecular force present in polar molecules.
Direct Relationship
Relationship where one variable changes in the same manner as another.
Dissociate
To break into ions.
Dissolve
To break into smaller pieces.
Distillation
Process of separating liquids based on boiling temperature differences.
Double Bond
Two shared pairs of electrons.
Electrolyte
Dissociates into charged particles capable of conducting electricity.
Electrolytic Cell
Redox reaction that is spontaneous.
Electronegativity
Ability of an atom to attract electrons; fluorine is the most electronegative element.
Electron Affinity
Energy released when an atom gains an electron; chlorine has the highest electron affinity.
Electron
Negatively charged particle with a charge of -1, mass ~ 0 amu, located in orbitals around the nucleus.
Empirical Formula
Lowest whole number ratio of atoms in a compound.
Molecular Formula
True formula representing the actual number of each atom in a substance.
Endothermic
Energy is gained by the system.
Evaporation
Process of removing water from an aqueous solution, leaving the solute behind.
Exothermic
Energy is released by the system.
Filtrate
Liquid that passes through filter paper.
Filtration
Process of separating a precipitate from its aqueous solution.
Formula Unit
Ionically bonded atoms.
Freezing
Phase change from a liquid to a solid.
Galvanic / Voltaic Cell
Redox reaction that is spontaneous.
Gamma Ray
0 protons, mass number = 0; low ionizing ability and high energy.
Halogen
Elements in group 17 that form halides as ions.
Hydrogen Bonding
Strong dipole-dipole interaction when H is bonded to F, O, or N.
Indirect Relationship
Relationship where one variable changes in the opposite manner to another.
Insoluble
Does not dissolve in water.
Intermediate
Species produced in one step and consumed in another.
Intermolecular Forces (IMF)
Attractive forces between molecules.
Ion
Charged particle.
Ionic Bond
Bond formed by transferring electrons from the least electronegative atom to the more electronegative atom.
Ionization Energy
Energy required to remove the outer electron.
Kinetic Energy
Energy of motion; temperature measures kinetic energy.
Limiting Reactant
Reactant that runs out first, limiting product formation.
London Dispersion Forces
Temporary IMF caused by electron movement; present in all substances.
Lone Pair
Unbonded electrons.
Mass Number
Total mass of protons and neutrons.
Melting
Phase change from a solid to a liquid.
Molar Mass
Grams per 1 mole.
Molarity
Moles of solute per liter of solution.
Molecular Formula
Actual number of moles of each atom in a compound.
Molecule
Covalently bonded atoms.
Neutron
Neutral particle with no charge, mass = 1 amu, located in the nucleus.
Note 
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