Honors Chemistry Unit 5 Test Review

Flashcards covering key vocabulary and definitions related to chemical bonding and compounds.

Covalent Bond

A bond formed when nonmetals or metalloids share electrons.

Molecular Compound

A compound composed of molecules that shows the kinds of atoms present and the number of each.

Diatomic Molecule

A molecule that contains two atoms, typically found together in nature.

Octet Rule

The principle that atoms tend to achieve a stable electron configuration by having eight valence electrons.

Unshared Electron Pairs

Electron pairs that are not involved in bonding but are part of the molecular orbitals.

Single Bond

A bond in which two electrons are shared between two atoms.

Double Bond

A bond where four electrons are shared between two atoms.

Triple Bond

A bond in which six electrons are shared between two atoms.

Coordinate Covalent Bond

A bond where one atom provides both bonding electrons.

Bond Dissociation Energy

The energy required to break a bond; the higher the energy, the stronger the bond.

Resonance Structures

Different ways of drawing the same molecule that show alternate bonding arrangements.

Sigma Bond

A bond formed through the direct overlap of atomic orbitals.

Pi Bond

A bond formed when orbitals overlap above and below the axis of the bonded atoms.

VSEPR Theory

A theory stating that the repulsion between electron pairs causes molecular shapes to adjust.

Polar Covalent Bond

A bond where electrons are unequally shared, creating slight charges.

Nonpolar Covalent Bond

A bond where electrons are equally shared between atoms.

Ionic Compound

A compound composed of positive and negative ions held together by electrostatic attraction.

Chemical Formula

An expression that indicates the number and type of atoms in the smallest representative unit of a substance.

Formula Unit

The lowest whole-number ratio of ions in an ionic compound.

Metallic Bond

A bond formed from the attraction between free-floating electrons and positive metal ions.

Alloy

A mixture of two or more elements, with at least one being a metal.

Properties of Ionic Compounds

Solid with high melting points, crystalline structure, and conduct electricity when melted or dissolved.

Valence Electrons

Electrons in the highest occupied energy level of an atom.

Hybridization

The blending of atomic orbitals to form new hybrid orbitals.

Examples of Diatomic Elements

H2, N2, O2, F2, Cl2, Br2, I2.