Historic Chem Lock-in

chemical formula

an expression that shows the elements in a
compound and the relative proportions of those elements.

Stoichiometry

The study of quantitative relations between amounts of reactants and products.

Stoichiometric Factor

A mole‑ratio factor relating moles of one compound to moles of another in a chemical equation.

Limiting Reagent

The reactant present in limited supply that determines the maximum product formed.

Excess Reagent

The reactant present in excess supply that remains after the reaction

Theoretical Yield

Maximum amount of product that can be produced from the limiting reagent.

Actual Yield

Experimentally measured amount of product obtained.

Percent Yield

Ratio of actual yield to theoretical yield × 100%.

Molarity (M)

Number of moles of solute per liter of solution.

Mole (mol) –

Amount of substance containing 6.022×10²³ entities (Avogadro’s number)

Molecular Mass 

Sum of atomic masses (amu) in a molecule.

Molar Mass –

Mass of 1 mole of a substance in grams.

Formula Mass –

Sum of atomic masses of all atoms in a compound’s formula.

Percent Composition by Mass –

Percent by mass of each element in a compound

Chemical Formula –

Expression showing elements in a compound and their proportions.

Empirical Formula –

Simplest whole‑number ratio of atoms in a compound.

Molecular Formula –

Actual number of atoms in a molecule

Chemical Equation –

Symbolic representation of a chemical reaction

Oxidation‑Reduction (Redox) Reaction –

Reaction involving electron transfer.

Oxidized Element

– Loses electrons.

Reduced Element –

Gains electrons.

combination run

Decomposition Rxn

Single displacement Rxn 

Double displacement

Precipitate

insoluble solid that separates from solution

Combustion

a fast reaction of a compound with molecular oxygen

Pressure

force per unit area

Partial pressure of a gas

the pressure exerted by a specific gas in a gas mixture at the temperature and volume of the mixture

Boyles Law

the pressure exerted by a fixed quantity of a gas at constant temperature is inversely proportional to its volume.

Charles’s Law

the volume occupied by a fixed quantity of a gas at constant pressure is directly proportional to its Kelvin temperature

Ideal gas law (IGL)

the product of the pressure times volume of a gas is directly proportional to the product of the number of moles
of the gas times its absolute temperature. The constant of proportionality is known as the gas constant R = 0.08206 L∙ atm/mol ∙ K

Dalton’s law of partial pressures

the total pressure of a mixture of gases is equal to the sum of the partial pressure of each gas in
the mixture