Chemistry 6A Midterm Exam 1 Review

Flashcards covering important chemistry concepts and definitions to help with Midterm Exam 1 preparation.

SI Base Units

The six standard units used in the International System of Units.

Diatomic Molecules

Molecules that consist of two atoms, which can be of the same or different chemical elements.

Avogadro’s Constant

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

Empirical Formula

The simplest positive integer ratio of atoms in a compound.

Molecular Formula

The chemical formula that shows the actual number of each type of atom in a molecule.

Molarity

A measure of concentration in chemistry, defined as the number of moles of solute per liter of solution.

Stoichiometric Coefficients

Numbers that appear in front of compounds in a balanced chemical equation to indicate the ratio of each substance involved.

Electrolytes

Substances that dissociate into ions in solution and can conduct electricity.

Strong Electrolyte

A substance that completely dissociates into ions in solution.

Weak Electrolyte

A substance that only partially dissociates into ions in solution.

Balanced Chemical Equation

A chemical equation that has the same number of each type of atom on both sides of the equation.

Significant Figures

Digits in a number that contribute to its precision, including all non-zero digits, zeroes between significant digits, and trailing zeroes in the decimal portion.

Dimensional Analysis

A mathematical technique used to convert between units by using conversion factors.

Chemical Formula

A representation of a substance using symbols for its constituent elements and numbers to indicate the ratio of atoms.

Ionic Compound

A compound formed by the electrostatic attraction between positive and negative ions.

Precipitation Reaction

A reaction in which an insoluble substance is formed from mixing two soluble substances.