Chemistry Unit 5: Covalent Bonding

chemical bond

Any of several forces, especially the ionic bond, covalent bond, and metallic bond, by which atoms or ions are bound in a molecule or crystal.

tetrahedral

Bond Angle - 109.5°

trigonal planar

Bond Angle - 120°

linear

Bond Angle - 180°

T-shaped

Bond Angle - 90° and 180°

octahedral

Bond Angle - 90° and 180°

square planar

Bond Angle - 90° and 180°

square pyramidal

Bond Angle - 90° and 180°

trigonal bipyramidal

Bond Angle - 90°, 120° and 180°

See-saw

Bond Angle - 90°, 120⁰ and 180°

trigonal pyramidal

Bond Angle - Less than 109.5°

trigonal bent

Bond Angle - Less than 120°

valence electron

an electron that is found in the outermost shell of an atom and that determines the atom's chemical properties

resonance structure

any one of two or more possible configurations of the same compound that have identical geometry but different arrangements of electrons

covalent bond

a bond formed when atoms share (fight) one or more pairs of electrons

polar covalent bond

a covalent bond in which a shared pair of electrons is held more closely by one of the atoms

nonpolar covalent bond

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

single bond

a covalent bond in which two atoms share one pair of electrons

triple bond

a covalent bond in which two atoms share three pairs of electrons

double bond

a covalent bond in which two atoms share two pairs of electrons

dipole

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

unshared pair

a nonbonding pair of electrons in the valence shell of an atom; also called lone pair

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

VSEPR theory

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

bond length

the distance between two bonded atoms at their minimum potential energy; the average distance between the nuclei of two bonded atoms

bond energy

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

molecular orbital

the region of high probability that is occupied by an individual electron as it travels with a wavelike motion in the three-dimensional space around one of two or more associated nuclei