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Cation

A positively charged ion formed by losing one or more electrons.

Anion

A negatively charged ion formed by gaining one or more electrons.

Ionic Bonding

An attraction between cations and anions through electrostatic forces.

Giant Ionic Lattices

Regular arrangements of alternating cations and anions in three dimensions.

Covalent Bonding

A type of bonding that occurs when two atoms share pairs of electrons.

Coordinate Bonding

A type of covalent bond where one atom donates both electrons.

Giant Covalent Structures

Large networks of atoms bonded by covalent bonds, exhibiting high melting and boiling points.

VSEPR Theory

A theory explaining the 3D arrangement of atoms in a molecule to minimize electron pair repulsion.

Bond Polarity

The distribution of electrical charge over bonded atoms; significant differences in electronegativity create polar bonds.

Chromatography

A technique used to separate mixtures based on differences in movement through a medium.

Intermolecular Forces

Forces between molecules that affect properties like boiling and melting points.

Dipole-Dipole Interactions

Attractions between polar molecules due to differences in electronegativity.

London Dispersion Forces

Weak attractions that occur between all molecules due to temporary shifts in electron density.

Metallic Bonding

Bonding that occurs when metal atoms share their valence electrons in a delocalized manner.

Alloy

A mixture of two or more elements, at least one of which is a metal, designed for specific properties.