Science Exam Review

Alkali Metals

Most reactive elements with 1 valence electron

Alkaline Earth Metals

Less reactive elements with 2 valence electrons

Halogen Gases

Very reactive elements with 7 valence electrons

Noble Gases

Non-reactive elements with a full valence shell (8)

Ionic Compound

Compound formed by the transfer of electrons from a metal to a non-metal

Molecular Compound

Compound formed by the sharing of valence electrons between non-metals

Balancing equations

Process of adjusting coefficients to ensure the same number of atoms on both sides of an equation

Acids

Substances with a pH below 7, sour taste, and corrosive to metals

Bases

Substances with a pH above 7, bitter taste, and corrosive but not to metals, slippery

Neutralization

Reaction between an acid and a base resulting in the formation of salt and water

Synthesis

Reaction where two elements combine to form a compound (A + B → AB)

Decomposition

Reaction where a compound breaks down into smaller elements (AB → A + B)

Combustion

Reaction where a hydrocarbon combines with oxygen to produce carbon dioxide and water

Single Displacement

Reaction where an element replaces another element in a compound (AB + C → CB + A)

Double Displacement

Reaction where two compounds combine and the metals switch places (AB + CD → CB + AD)

Incandescent

Type of light emitted when a metal heats up and glows

Fluorescent

Type of light emitted when a substance is exposed to radiation

Phosphorescent

Type of light emitted when a substance absorbs light and releases it over time

Chemiluminescent

Type of light emitted during a chemical reaction

Triboluminescence

Type of light emitted when friction is applied to certain materials

Bioluminescence

Ability of organisms to produce their own light

Electric Discharge

Light produced when an electric current passes through a gas