Covalent Bonding

ionic bond

Formed when one or more electrons are transferred from one atom to another

polyatomic ion

A charged group of covalently bonded atoms

valence electrons

Electrons on the outermost energy level of an atom

VESPR theory

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

Linear shaped molecule

2 atoms around the central atom, 180 degrees

Bent shaped molecule

-105 degrees

-2 binding and 1 or 2 lone pairs

trigonal planar

3 bonds, 0 lone pairs, 120 degrees

trigonal pyramidal

3 bonds, 1 lone pair

Tetrahedral shaped molecule

4 atoms around a central atom

Electronegativity

the ability of an atom to attract electrons when the atom is in a compound

polar covalent bond

A covalent bond in which electrons are not shared equally

non polar covalent bond

equal sharing of electrons

intermolecular forces

attractive forces between molecules

octet rule

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons

octet rule exceptions

Hydrogen (2e-) and Boron (6e-)

lone pair electrons

Electrons that are paired up in an orbital and are not part of a covalent bond

dipole-dipole interactions

attractive forces that act between polar molecules

hydrogen bond

Attraction between a slightly positive hydrogen atom and a slightly negative atom (O, N, F)

dispersion forces

the weakest of all molecular interactions, are caused by the motion of electrons

ion-dipole forces

attractive forces between an ion and a polar molecule