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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