Chapter 3 practice test review lecture

Descriptive

Referring to language or information that describes characteristics or qualities.

Compound

A substance formed when two or more elements are chemically bonded together.

Molecular Compound

A chemical compound whose smallest units are molecules, which consists of nonmetals.

Ionic Compound

A compound formed from the electrostatic attraction between oppositely charged ions, typically composed of metals and nonmetals.

Empirical Formula

A formula that shows the simplest whole-number ratio of atoms in a compound.

Molar Mass

The mass of one mole of a substance, expressed in grams per mole (g/mol).

Oxoacid

An acid that contains one or more oxygen atoms and hydrogen, and can donate protons (H+ ions).

Diatomic Molecule

A molecule consisting of two atoms, which can be of the same or different chemical elements.

Polyatomic Ion

An ion composed of two or more atoms covalently bonded that functions as a single ion.

Hydrate

A compound that contains water molecules in its structure.

Avogadro's Number

The number of particles (atoms, molecules, etc.) in one mole of a substance, approximately 6.022 x 10^23.

Mass Percent

The mass of a particular component divided by the total mass of the compound, multiplied by 100.

Transition Metal

Elements that have partially filled d orbitals and are found in groups 3 to 12 of the periodic table.

Subscript

A number written below and to the right of a chemical symbol in a formula to indicate the number of atoms of that element in a molecule.

Crisscross Method

A technique used to determine the chemical formula of an ionic compound by swapping the charges between the ions.

Coefficient

A number placed in front of a chemical formula in a reaction to balance the number of atoms of each element.