molecular orbital that induces a low electron density between two or more atoms. It is at a higher energy state than the atomic orbitals it is formed from.
molecular orbital that has a high electron density between two or more atoms due to the overlap of multiple atomic orbitals
vector quantity that defines the extent of the charge on either side of a polar covalent bond, with the direction that points from the positive side of the bond toward the negative side
shape description for all electron pairs (bonding and nonbonding) about a central atom
molecule consisting of two atoms of the same element, bound together by one or more covalent bonds
according to valence bond theory, an electron orbital that forms when two atomic orbitals combine to form a covalent bond
mathematical function that gives the probability of locating an electron in a localized volume of space
theory that atomic electron orbitals in covalent bonds are replaced by electron orbitals that belong to the entire molecule
region in which an electron has a high probability of being located. Orbitals are described by the quantum numbers s, p, d, and f, which differ from each other by their shapes.
covalent bond in which the electron density is more localized on one end of the bond. One end is slightly positive, and one end is slightly negative.
theory that the electrons in a covalent bond remain centralized around their original nuclei, and their atomic orbitals overlap
covalent bond theory that uses the repulsive forces between single electrons and pairs of electrons about the central atom to predict their relative positions around the atomic nuclei