Chemical Bonding and Molecular Geometry

distance between the nuclei of the atoms forming a bond, usually expressed in picometers (pm) or angstroms (Å)

electron that is part of a covalent bond

chemical bond that forms when valence electrons are shared between atoms

molecule with partial positive and partial negative charges

attractive or repulsive force between two polar molecules resulting from partial positive and partial negative charges of the molecules

covalent bond in which two pairs of electrons are shared between two atoms

tendency of an atom to attract electrons toward itself when forming bonds

hypothetical charge assigned to an atom in a molecule with the assumption that bonding electrons are shared equally

atom, molecule, or ion with one or more unpaired electrons

weak intermolecular bond between a hydrogen atom of one molecule and a highly electronegative atom of a nearby molecule. The electronegative atom is usually fluorine, oxygen, or nitrogen.

having more than an octet of valence electrons

polarized bond induced by an electric field

dipole that forms because of a short-lived imbalance in charge distribution in an otherwise nonpolar atom or molecule

attractive or repulsive force between a molecule and a nearby molecule, atom, or ion

attractive or repulsive force between atoms that make up a molecule or between ions

electrostatic interaction between ions and polar ends of molecules with permanent dipoles

electrostatic force that holds cations and anions together

model that represents covalent bonds and nonbonding electrons with symbols, dots, and lines

interaction between induced, instantaneous dipoles in nonpolar molecules or atoms

valence electron pair that does not form a bond

three-dimensional shape of a molecule that takes into account bonding and nonbonding electron pairs and molecular rotations to minimize their interactions

covalent bond in which the nuclei of the bonded atoms exert equal or nearly equal force on the shared electrons

rule that states that atoms tend to share or donate electrons such that the valence shell contains eight electrons $(\text{octet}=ns+np=8)$

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.

ability for dipole moments to change because of the presence of an applied electric field

one of two or more Lewis structures with multiple equivalent representations

covalent bond in which one pair of electrons is shared between two atoms

covalent bond in which three pairs of electrons are shared between two atoms

electron in the outermost shell of an atom

dipole-dipole interaction, London dispersion force, or intermolecular force between permanent molecular dipoles