chem 111

Significant Figures

The number of digits in a measurement that are known with certainty plus one estimated digit.

Metric Conversions

The process of converting measurements from one metric unit to another, such as centimeters to meters.

Density

Mass per unit volume, typically expressed in g/mL or kg/m³.

Polyatomic Ions

Ions composed of two or more atoms, which are covalently bonded, that have a net charge.

Scientific Notation

A method of expressing numbers as a product of a coefficient and a power of ten.

Empirical Formula

The simplest whole number ratio of elements in a compound.

Isotopes

Atoms of the same element that have different numbers of neutrons.

Molar Mass

The mass of one mole of a substance, typically expressed in g/mol.

Stoichiometry

The calculation of reactants and products in chemical reactions based on the balanced equation.

Limiting Reactant

The reactant in a chemical reaction that is consumed first, limiting the amount of product formed.

Balanced Equation

An equation that has the same number of each type of atom on both sides, representing the conservation of mass.

Acid-Base Reaction

A chemical reaction that occurs between an acid and a base, typically resulting in the formation of water and a salt.

Periodic Table

A chart that organizes elements based on their atomic number and properties.

Oxidation Numbers

A concept that represents the degree of oxidation (loss of electrons) of an atom in a compound.

Net Ionic Equation

An equation that shows only the species that actually participate in a reaction, omitting spectator ions.

Gas Laws

Mathematical relationships that describe the behavior of gases in terms of pressure, volume, and temperature.

Percent Composition

The percentage by mass of each element in a compound.

Avogadro’s Number

The number of atoms, molecules, or particles in one mole of a substance, approximately 6.022 x 10²³.

Conversion Factor

A numeric factor used to convert between different units of measurement.

Dilution

The process of reducing the concentration of a solute in a solution, usually by adding more solvent.

Strong Acids

Acids that completely dissociate in solution, releasing H⁺ ions.

Energy Levels

Regions around the nucleus of an atom where electrons are likely to be found.

Hydrocarbon

An organic compound consisting entirely of hydrogen and carbon.

Saturation Point

The point at which a solution can no longer dissolve any more solute.

Chemical Properties

Properties that describe the ability of a substance to undergo changes and form new substances.

Ionic Compounds

Compounds formed from the electrostatic attraction between positively and negatively charged ions.

Covalent Compounds

Compounds formed by the sharing of electrons between non-metal atoms.

Mixtures

Physical combinations of two or more substances that retain their individual properties.