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17 terms

Ch. 6 Vocab #2

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Single Bond
a covalent bond in which one pair of electrons is shared between two atoms
Structural Formula
Indicates the kind, number, arrangement and bonds but not the unshared pairs of the atoms in a molecule
Triple Bond
a covalent bond in which two atoms share three pairs of electrons
Hybridization
the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies
Formula Unit
the simplest collection of atoms from which an ionic compound's formula can be established
Ionic Compound
composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
Lattice Energy
the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
Polyatomic Ion
a charged group of covalently bonded atoms
Ductility
the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire
Malleability
the ability of a substance to be hammered or beaten into thin sheets
Dipole
created by equal but opposite charges that are separated by a short distance
Hybrid Orbitals
orbitals of equal energy produced by the combination of two or more orbitals on the same atom
Hydrogen Bonding
the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
Intermolecular Forces
forces of attraction between molecules
London Dispersion Forces
the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Molecular Polarity
the uneven distribution of molecular charge
VSEPR Theory
states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible