Activation Energy: Minimum energy needs to be added to a system in order for the chemical reaction to occur

Alpha Particle: He2+

2 protons, mass number = 4, 2+ charge Highly ionizing particle; Low energy

Anion: Negatively charge ion

Arrhenius Acid: Donates a H+

ion

Arrhenius Base: Donates a OHion

Atom: Smallest constituent unit of ordinary matter that has the properties of a chemical element

Atomic Mass: Average of all naturally occurring isotopes

Atomic Number: Number of protons; defines the atom

Beta Particle: -1 proton, mass number =0; medium ionizing ability, 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: Means of measuring the heat gained/ lost by a system during a chemical reaction

Catalyst: Lowers the activation energy. Not a reactant. Not a 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 the sharing of electrons between atoms.

Deposition: Phase change from a gas to a solid

Dipole-Dipole: Permanent IMF present in polar molecules

Direct Relationship: Relationship between two variables where when one changes, the other changes in the

same manner

Dissociate: To break into ions

Dissolve: To break into smaller pieces

Distillation: Process of separating liquids based on differences in boiling temperatures

Double Bond: Two shared pairs of electrons

Electrolyte: Dissociates into charge particles which are capable of conducting electricity

Electrolytic Cell: Redox reaction that is spontaneous

Electronegativity: The ability of an atom to attract electrons from another atom. Quantity that can’t be

measured. ****** Fluorine is most electronegative element.

Electron Affinity: Energy released when an atom gains an electron. Actual quantity that can be measured.

*****Chlorine has highest electron affinity.

Electron: Negatively charged particle. Charge = -1, Mass ~ 0amu. Located in the orbitals surrounding the

nucleus

Empirical Formula: Lowest whole number ratio of atoms in a compound

Molecular Formula: The true formula representing the actual number of each atom present in the substance.

Endothermic: Energy is gained by the system

Evaporation: Process of removing water from an aqueous solution. Solute is left behind

Exothermic: Energy is released by the system

Filtrate: Liquid that passes through the 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, high energy

Halogen: Elements in group 17. Form halides as ions

Hydrogen Bonding: Strong dipole-dipole that results when H is bonded to F, O, or N (Special dipole that exists

in only selective polar molecules)

Indirect relationship: Relationship between two variables where when one changes, the other changes in the

opposite manner

Insoluble: Does not dissolve in water

Intermediate: Species produced in one step and consumed in another step

Intermolecular Forces, IMF: Attractive forces between molecules

Ion: Charge particle

Ionic Bond: Bond formed by the transfer of 1 or more 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 is a measure of KE

**** Gotta know it like you know your name....Can’t survive AP CHEM without knowing it......Limiting

Reactant: Reactant to runs out first thus limiting the amount of product that can be formed

London Dispersion Forces: Temporary IMF caused by the movement of electrons. Present in all nonpolar and

polar substances. Most prominent in Nonpolar molecules.

Lone Pair: Unbonded electrons

Mass Number: Mass of all protons and neutrons

Melting: Phase change from a solid to a liquid

Molar Mass: grams per 1 mol

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. No charge. Mass = 1amu, Located in the nucleus

Noble Gas: Group 18 on the PT. Each has 8 valence electrons. Nonreactive

Orbital: Regions of probability where electrons are located. Each orbital can contain up to 2 electrons

Oxidation Number: A charge assigned to an atom that represents that charge it would have if it contained and

ionic bond. Oxidation numbers are written as charge value, +4, -6, +2

Oxidation: Process of losing electrons which increases the oxidation number

Percent Error: Absolute value (Theoretical – Experimental) / Theoretical) x 100%

Percent Yield: (Quantity produced / Theoretical Amount) x 100%

Precipitate: Solid matter that forms from the reaction of two aqueous solutions

Principle Energy Level: n= 1 means first energy level. Energy levels contain sublevels

Proton: Positively charged particle. Charge = +1, Mass = 1amu, Located in the nucleus

Reduction: Process of gaining electrons which reduces the oxidation number

** Your new best friend:::: Significant Figures: Those digits that carry meaning contributing to its precision

Single Bond: One shared pair of electrons

Soluble: Dissolves in water

Solute: The species that gets dissolved to form a solution

Solution: Solute and solvent

Solvent: The species that does the dissolving to form a solution

Sources of Error: These are errors that you make in the lab which result in either increased or decreased yields.

These do not include Human Error, Calculations, Massing.....

Specific Heat: Energy required to raise 1 gram of a substance 1C

Strong Acid: Dissociates 100%

Strong Base: Dissociates 100%

Sublevel: s, p, d, and f. defines the shape

Sublimation: Phase change from a solid to a gas

Surroundings: This refers to everything outside of the system

System: This refers to the reaction

Triple Bond: Three shared pairs of electrons

Valence electrons: Outer electrons which are available for bonding

Weak Acid: Dissociate very little. Remains mostly in its molecular form

Weak Base: Dissociates very little. Remains mostly in its molecular form