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Moles

Represented by 6.02x10^23 entities, used to count atoms or molecules

Atomic mass

Mass of an atom, sum of protons and neutrons

Valence electrons

Electrons in the outermost shell, determine chemical properties

Anion

Negatively charged ion

Cation

Positively charged ion

Ionic bonds

Formed by attraction between oppositely charged ions

Covalent bonds

Sharing of electron pairs between atoms

Polar molecules

Unequal sharing of electrons

Nonpolar molecules

Equal sharing of electrons

Intermolecular forces

Forces between molecules

London dispersion forces (LDFs)

Weakest forces, present in all molecules

Dipole-dipole forces

Moderate strength forces in polar molecules

Hydrogen bonding

Strongest intermolecular force involving F, O, N

Gas laws

PV=nRT, ideal gas behavior at high temp and low pressure

Molarity

Concentration in moles per liter

Net ionic equation

Shows only the species involved in a reaction

Reaction rate

Determined by collision frequency and energy

Activation energy

Energy required to start a reaction

Enthalpy

Heat content of a system at constant pressure

Equilibrium

Forward and reverse reaction rates are equal

Le Chatelier's Principle

System shifts to counteract changes

pH

Negative logarithm of hydrogen ion concentration

Buffers

Resist changes in pH, weak acid and conjugate base

Entropy

Measure of disorder in a system

Gibbs free energy

Thermodynamic favorability of a reaction

Galvanic cells

Produce electrical energy from redox reactions

Nernst equation

Calculates cell potential under nonstandard conditions

Current (I)

Flow of electric charge, measured in amperes