Chemistry Test Review 11/11

Ionic bond

A bond formed by the transfer of electrons between atoms, resulting in electrostatic attraction.

Covalent bond

A bond formed by the sharing of electron pairs between atoms.

Metallic bond

A bond characterized by delocalized electrons shared among a lattice of metal atoms.

Electronegativity difference

The difference in electronegativity between two atoms that helps determine the type of bond formed.

Polar covalent bond

A type of covalent bond where electrons are shared unequally between atoms with different electronegativities.

Nonpolar covalent bond

A bond where electrons are shared equally due to similar electronegativities of the bonded atoms.

High melting point

A property often associated with ionic and metallic bonds due to strong interactions.

Conductivity in solution

The ability of a substance to conduct electrical current when dissolved in water, typically seen in ionic compounds.

Solubility

The ability of a substance to dissolve in a solvent, varying by bond type.

True octet

Refers to an atom having eight electrons in its valence shell, contributing to stability.

Lewis Structure

A diagram that shows the bonding between atoms and the lone pairs of electrons.

Electron domain

Regions around a central atom where electrons are likely to be found, influencing molecular geometry.

VSEPR theory

Valence Shell Electron Pair Repulsion theory, which predicts the geometry of molecules based on electron pair repulsion.