Bond dissociation energy
the energy required to break the bond between two covalently bonded atoms
Bonding orbital
A molecular orbital that can be occupied by two electrons of a covalent bond.
Covalent bond
A bond formed by the sharing of electrons between atoms.
Coordinate covalent bond
A covalent bond in which one atom contributesboth bonding electrons.
Diatomic molecule
A molecule consisiting of two atoms.
Dipole interactions
Intermolecular forces resulting from attraction of oppositely charged regions of polar molecules.
Dipole
A molecule that has two poles, or regions with opposite charges.
VSEPR theory
Valence shell electron pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible.
Van der Waals Forces
The two weakest intermolecular attractions- dispersion interactions and dipole forces.
Unshared pair
A pair of valence electrons that is not shared between atoms.
Triple covalent bond
A covalent bond in which three pairs of electrons are shared by two atoms.
Tetrahedral angle
A bond angle of 109.5 degrees that results when a central atom forms four bonds directed toward the center of a regular tetrahedron.
Structural formula
A chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion, each dash between a pair of atoms idicates a pair of shared electrons.
Single covalent bond
A bond formed when two atoms share a pair of electrons
Sigma bond
A bond formed when two atomic orbitals combine for form a molecular orbital that is symmetrical around the axis connectiong the two atomic nuclei.
Resonance structure
one of the two or more equally valid electron dot structures of a molecule or polyatomic ion
Polyatomic ion
A tightly bound group of atoms that behaves as a unit and has a positive or negative charge
Dispersion forces
Attraction between molecules caused by the electrons motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules.
Double covalent bond
A bond in which two atoms share two pairs of electrons.
Hybridization
The mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals.
Hydrogen bonds
Attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared election pair of another electronegative atom.
Molecular compound
A compound that is composed of molecules.
Molecular formula
A chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound
Molecular orbital
An orbital that applies to the entire molecule
Molecule
a neutral group of atoms joined together by covalent bonds
Polar bond
A molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive.
Network solids
A solid in which all of the atoms are covalently bonded to each other
Nonpolar covalent bond
A covalent bond in which the electrons are shared equally by the two atoms
Pi bond
A covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms
Polar molecule
A molecule in which one side of the molecule is slightly negative and the opposite side is lsightly positive.
Polar covalent bond
A covalent bond between atoms in which the electronsa are shared unequally