AP Chemistry Review Flashcards

Flashcards covering key concepts from AP Chemistry lecture notes, focusing on vocabulary and definitions.

The soluble component that goes through the filter paper during a filtering process.

Filtrate

A process that separates mixtures based on differences in boiling point.

Distillation

H₂, N₂, Cl₂, Br₂, I₂, F₂ These elements exist as two atoms bonded together in their elemental form. When in a compound, their number of atoms can vary.

Diatomic elements

Mass per unit volume (mass/volume).

Density

The simplest whole number ratio of atoms in a compound.

Empirical Formula

A whole number multiple of the empirical formula, representing the actual number of atoms of each element in a molecule.

Molecular Formula

The reactant that determines the amount of product formed in a reaction.

Limiting Reactant

The net positive charge experienced by an electron in a multi-electron atom.

Zeff (Effective Nuclear Charge)

A technique used to determine the ionization energies of electrons in atoms or molecules.

PES (Photoelectron Spectroscopy)

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

Isotopes

A chemical bond formed by the sharing of electrons between two nonmetals.

Covalent Bond

A chemical bond formed through the transfer of electrons between a metal and a nonmetal.

Ionic Bond

A measure of the ability of an atom in a chemical compound to attract electrons.

Electronegativity

A chemical process that involves rapid oxidation producing heat and light, typically involving a hydrocarbon and oxygen to produce CO2 and H₂O.

Combustion Reaction

The energy required to separate one mole of an ionic compound into its gaseous ions.

Lattice Energy

The charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between atoms, used to determine the most stable Lewis structure.

Formal Charge

A separation technique based on differences in polarity or other physical properties of the components in a mixture.

Chromatography

Attractive forces between molecules (London Dispersion, Dipole-Dipole, Hydrogen Bonding, Ion-Dipole).

Intermolecular Forces (IMFs)

Weak, short-range intermolecular forces arising from temporary dipoles in nonpolar molecules; present in all molecules.

London Dispersion Forces (LD Forces)

Attractive forces between polar molecules due to the attraction of positive and negative ends.

Dipole-Dipole Forces

A strong type of dipole-dipole attraction between a hydrogen atom bonded to a highly electronegative atom (N, O, F) and another electronegative atom.

Hydrogen Bonding

The pressure exerted by a vapor in equilibrium with its liquid or solid phase.

Vapor Pressure

The tendency of a substance to vaporize.

Volatility

An alloy formed when small atoms fit into the spaces between larger atoms in a metallic crystal.

Interstitial Alloy

An alloy formed when atoms of similar size are substituted for each other in a crystal lattice.

Substitutional Alloy

A hypothetical gas that perfectly obeys the ideal gas law.

Ideal Gas

The point in a titration where the number of moles of titrant added is stoichiometrically equivalent to the number of moles of analyte in the sample.

Equivalence Point

An acid that completely ionizes in solution.

Strong Acid

A base that completely dissociates in solution.

Strong Base

A number assigned to an element in a chemical combination that represents the number of electrons lost or gained.

Oxidation Number

The minimum energy required for a chemical reaction to occur.

Activation Energy

A substance that speeds up a reaction without being consumed in the process by lowering the activation energy.

Catalyst

The step-by-step sequence of elementary reactions by which overall chemical change occurs.

Reaction Mechanism

A species that is produced in one step of a reaction mechanism and consumed in a subsequent step.

Intermediate

A reaction that releases heat (negative ΔH).

Exothermic Reaction

A reaction that absorbs heat (positive ΔH).

Endothermic Reaction

The state where the rate of forward and reverse reactions are equal, and the net change in concentrations of reactants and products is zero.

Equilibrium

If a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress.

Le Chatelier's Principle

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

Buffer

A reaction that has a negative change in Gibbs Free Energy (ΔG < 0), indicating spontaneity.

Thermodynamically Favorable Reaction

A connection containing an electrolyte which allows ion flow between half cells to maintain charge neutrality (cations flow to cathode, anions to the anode).

Salt Bridge

A cell that uses electricity to drive non-spontaneous reactions

Electrolytic Cell