Bonding Vocab Terms + Definitions

Valence Electron

s and/or p electrons in the highest energy level which are available for bonding

Single Bond

Bond formed from the sharing of 2 e- (sigma bond)

Double Bond

Bond formed from the sharing of 4 e- (one sigma bond, one pi bond)

Triple Bond

Bond formed from the sharing of 6 e- (one sigma bond and two pi bonds)

Ionic Bond

Bond formed between two atoms when the least electronegative atom gives 1 or more e- to the more electronegative atom

Covalent Bond

Bond formed between two atoms when 2 or more e- are shared between them

Lewis Dot Structure (LDS)

A diagram that shows the arrangement of valence e- around the atoms in a molecule

VSEPR Theory

Valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible

Hybridization

The mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals

Polar Bond

A covalent bond between atoms in which the electrons are shared unequally; the more electronegative atom pulls the shared pair closer to its nucleus

Polar Molecule

Molecule with an unequal distribution of charge, resulting in the molecule having a positive end and a negative end (Dipole Moment)

Electronegativity

A measure of the ability of an atom in a chemical compound to attract shared e- towards its nucleus

Formal Charge

The charge assigned to an atom in a molecule or polyatomic ion derived from a specific set of rules; FC = #valence e- minus (1/2 shared e- + # lone pair e-)

Bond Angle

The angle between any two covalent bonds that share a common atom

Sigma Bond

A single covalent bond that is formed when an electron pair is shared by the direct overlap of bonding orbitals; between two nuclei

Pi Bond

A bond that is formed when parallel orbitals overlap to share electrons; delocalized e-

Core Electrons

The electrons in the inner complete energy levels of an atom; these electrons are not involved in forming bonds

Dipole Moment

A property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative charge

Metallic Bonding

A bond formed by the attraction between positively charged metal ions and the delocalized electrons around them; Sea of e-

Network Covalent Bonding

A type of chemical bonding characterized by the sharing of valence electrons throughout the entire solid sample

Delocalized electrons

Electrons in a molecule, ion or metal that are not associated with a specific bond

Coulomb’s Law

Electric force of attraction between charged objects depends on the distance between the objects and the magnitude of the charges. F=Q1Q2/r² where Q1 = cation charge , Q2 = Anion Charge , r=radius between nuclei

Bond Length

The distance between two bonded atoms at their minimum potential energy, that is, the average distance between the nuclei of two bonded atoms

Bond Strength

Energy required to break a bond; endothermic process

Enthalpy

The heat content of a system at constant pressure, DeltaH

Interstitial alloy

Alloy of different size metallic/metalloid atoms; one atom fits between the others

Substitutional Alloy

Some of the host metal atoms are replaced by other metal atoms of similar sizes

Resonance Structure

One of the two or more equally valid LDS of a molecule or polyatomic ion; none are correct

Octet Rule

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons; H is an exception

Bond Energy

The amount of energy that will break a bond between two atoms

Lone Pair

A pair of electrons that is not involved in bonding and that belongs exclusively to one atom

Malleable

Capable of being shaped

Ductile

A term used to describe a material that can be pulled out into a long wire