BONDS

Bond energy

The energy required to break the bonds in 1 mol of a chemical compound.

Chemical bond

The attractive force that holds atoms or ions together.

Chemical formula

A combination of chemical symbols and numbers to represent a substance.

Covalent bond

A bond formed when atoms share one or more pairs of electrons.

Dipole

A molecule or a part of a molecule that contains both positively and negatively charged regions.

Ductility

The ability of a substance to be hammered thin or drawn out into a wire.

Electron dot notation

An electron configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element's symbol.

Formula unit

The collection of atoms corresponding to an ionic compound's formula such that the molar mass of the compound is the same as the mass of 1 mol of formula units.

Hybrid orbitals

Orbitals that have the properties to explain the geometry of chemical bonds between atoms.

Hybridization

The mixing of two or more atomic orbitals of the same atom to produce new orbitals; hybridization represents the mixing of higher- and lower-energy orbitals to form orbitals of intermediate energy.

Hydrogen bond

The intermolecular force occurring when a hydrogen atom that is bonded to a highly electronegative atom of one molecule is attracted to two unshared electrons of another molecule.

Ionic bond

A force that attracts electrons from one atom to another, which transforms a neutral atom into an ion.

Ionic compound

A compound composed of ions bound together by electrostatic attraction.

Lattice energy

The energy associated with constructing a crystal lattice relative to the energy of all constituent atoms separated by infinite distances.

Lewis structure

A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.

London dispersion force

The intermolecular attraction resulting from the uneven distribution of electrons and the creation of temporary dipoles.

Malleability

The ability of a substance to be hammered or beaten into a sheet.

Metallic bond

A bond formed by the attraction between positively charged metal ions and the electrons around them.

Molecular compound

A chemical compound whose simplest units are molecules.

Molecular formula

A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms.

Molecule

A group of atoms that are held together by chemical forces; a molecule is the smallest unit of matter that can exist by itself and retain all of a substance's chemical properties.

Multiple bond

A bond in which the atoms share more than one pair of electrons, such as a double bond or a triple bond.

Non polar covalent bond

A covalent bond in which the bonding electrons are equally attracted to both bonded atoms.

Polar

Describes a molecule in which the positive and negative charges are separated.

Polar covalent bond

A covalent bond in which a pair of electrons shared by two atoms is held more closely by one atom.

Polyatomic ion

An ion made of two or more atoms.

Resonance

The bonding in molecules or ions that cannot be correctly represented by a single Lewis structure.

Single bond

A covalent bond in which two atoms share one pair of electrons.

Structural formula

A formula that indicates the location of the atoms, groups, or ions relative to one another in a molecule and that indicates the number and location of chemical bonds.

VSEPR theory

A theory that predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other.