Standard free energy (G°) The Gibbs free energy for a reaction under standard conditions. See Gibbs free energy.
Standard hydrogen electrode (SHE) The electrode defined as having a potential of zero under standard conditions. All redox potentials are measured relative to the standard hydrogen electrode at 25°C and with 1.0 M of each ion in solution.
Standard potential The voltage associated with a half-reaction of a specific redox reaction. Generally tabulated as a reduction potential, compared to the SHE.
Standard temperature and pressure (STP) Defined as 0°C (273 K) and 1 atm. Used for measuring gas volume and density.
State The set of defined macroscopic properties of a system that must be specified in order to reproduce the system exactly. Sometimes also used as a synonym for phase.
State function A function that depends on the state of a system but not on the path used to arrive at that state.
Strong acid An acid that undergoes complete dissociation in an aqueous solution (e.g., HCl).
Strong base A base that undergoes complete dissociation in an aqueous solution (e.g., KOH).
Sublimation A change of phase from solid to gas without passing through the liquid phase.
Subshell The division of electron shells or energy levels defined by a particular value of the azimuthal quantum number (e.g., s, p, d, and f subshells). Composed of orbitals. Also called sublevels.
Surroundings All matter and energy in the universe not included in the particular system under consideration.
System The matter and energy under consideration.
Temperature A measure of the average energy of motion of the particles in a system. Compare heat.
Third law of thermodynamics The law stating that the entropy of a perfect crystal at absolute zero is zero.
Titrant A solution of known concentration that is slowly added to a solution containing an unknown amount of a second species to determine its concentration.
Titration, acid-base A method used to determine the concentration of an unknown solution.
Titration curve A plot of the pH of a solution versus the volume of acid or base added in an acid-base titration.
Torr A pressure unit equal to 1 mm Hg; 760 torr = 1 atm.
Transition metal Any of the elements in the B groups of the periodic table, all of which have partially filled d sublevels.
Triple point The pressure and temperature at which the solid, liquid, and vapor phases of a particular substance coexist in equilibrium. See phase equilibrium.
Unit cell A three-dimensional representation of the repeating units in a crystalline solid.
Unsaturated solution A solution into which more solute may be dissolved.
Valence electron An electron in the highest occupied energy level of an atom, whose tendency to be held or lost determines the chemical properties of the atom.
van der Waals equation One of several real gas laws, or “equations of state.” It corrects for attractive and repulsive forces assumed to be negligible in the Ideal Gas law.
van der Waals forces The weak forces that contribute to intermolecular bonding, including hydrogen bonding, dipole–dipole interactions, and dispersion forces. See intermolecular forces.
Vapor pressure The pressure exerted by a vapor when it is in equilibrium with the liquid or solid phase of the same substance. The partial pressure of the substance in the atmosphere above the liquid or solid.
Vapor pressure depression The decrease in the vapor pressure of a liquid caused by the presence of dissolved solute; a colligative property. See Raoult’s law.
Voltaic cell See galvanic cell.
Water dissociation constant (Kw) The equilibrium constant of the water dissociation reaction at a given temperature; 1.00 × 10-14 at 25°C.
Weak acid An acid that undergoes partial dissociation in an aqueous solution (e.g., CH3COOH).
Weak base A base that undergoes partial dissociation in an aqueous solution (e.g., NH4OH).
Yield The amount of product obtained from a reaction.
Nuclear charge (Z) Equivalent to atomic number.
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