Chemistry Midterm #6

Ionic compound

Ionic compound

compound that consists of a metal and nonmetal

Covalent Compound

Metallic Compound

Ionic Bond

bonds formed between metals that lose electrons to form an octet and nonmetals that gain electrons to form an octet; the electron is “transferred” from the metal to the nonmetal

Covalent Bond

bonds formed between two nonmetals: each donate one or more electrons to the shared bond

Non-polar covalent bond

a covalent bond in which there is a relatively equal sharing of the bonding electron pair

Polar covalent bond

a covalent bond in which there is an unequal sharing of the bonding electron pair

Coordinate covalent bond

a covalent bond in which the shared pair of electrons is donated by the same atom instead of each atom donating one

Metallic bonds

tightly packed metal cations in a sea of delocalized valence electrons

Breaking bonds

always endothermic

Forming Bonds

always exothermic

Bond Energy

the total energy required to break the bond between two covalently bonded atoms forming neutral atoms. This is the measure of the strength of a covalent bond and is always endothermic.

Lattice Energy

the energy required to separate one mole of a solid ionic compound into its gaseous ions; measure of the strength of an ionic bond

Heat of Vaporization

is a measure of the strength of a metal bond

Hybridization

the mixing of different types of atomic orbitals to produce a set of equivalent “hybrid” orbitals of equal but intermediate energy

Dipole-Dipole

polar-polar

Dipole-Induced Dipole

polar-nonpolar

London Dispersion Forces

nonpolar-nonpolar

Hydrogen Bonding

Intermolecular Forces

weak attractive forces that exist between molecules holding molecules together; collectively these are called Van der Waals Forces

Intramolecular Forces

strong attractive forces that exist between atoms within a molecule and holds the molecule together in a combined state