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covalent bond bond formed when 2 or more valence electrons are attached by the positively charged nuclei of 2 atoms and are thus shared between both atoms.
molecular orbital a region where an electron is most likely to exist as it travels in 3-dimensional space around 2 nuclei.
bond length the distance between 2 bonded atoms their minimum potential energy, the average distance between 2 bonded atoms.
bond energy energy required to break a chemical bond between 2 atoms and separate them.
nonpolar covalent bond an attraction between 2 atoms in which bonding electrons are shared equally between the atoms.
polar covalent bond an attraction between 2 atoms in which bonding electrons are localized on the more electronegative atom.
dipole a molecule in which one end has a partial positive charge and the other end has a partial negative charge.
valence electron electron in the outermost energy level of an atom, where it can participate in bonding.
lewis structure a stucture in which atomic symbols represent nuclei and inner-shell electrons, and dots are used to represent valence electrons.
unshared pairs a pair of valence electrons not involved in bonding to another atom.
single bond covalent bond in which one pair of electrons is shared betweeen atoms.
VSEPR theory a simple model that predicts the general shape of a molecule based on the repulsion between both bonding and non-bonding electrons
intermolecular forces an attraction that exists between molecules.
hydrogen bond form of dipole attraction in which a hydrogen atom bonded to a strongly electronegative atom is attracted to another electron rich atom.
london force an attraction between atoms and molecules caused by the formation of instantaneous dipoles in the atoms and molecules.
reasonance structure possible lewis dot structure of a molecule for which more than one lewis structure can be written.
Created by: ashley28