chem bonding

Unit 10: Chemical Bonding Chapter 9 Vocabulary Bond length (p295) distance between the centers of two bonded atoms in a molecule Born-Haber cycle (p291) cycle that relates lattice energies of ionic compounds to ionization energies, electron affinities, and other atomic and molecular properties Coordinate covalent bond (p308) bond in which the pair of electrons is supplied by one of the two bonded atoms Coulomb's law (p291) The potential energy between two ions is directly proportional to the product of their charges and inversely proportional to the distance between them. Covalent bond (p294) bond in which two electrons are shared by two atoms Covalent compound (p294) compound containing only covalent bonds Double bond (p295) covalent bond in which two atoms share two pairs of electrons Electronegativity (p296) ability of an atom to attract electrons toward itself in a chemical bond Formal charge (p302) electrical charge difference between the number of valence electrons in an isolated atom and the number of electrons assigned to that atom in a Lewis structure Ionic bond (p289) electrostatic force that holds ions together in an ionic compound Lattice energy (p291) energy required to completely separate one mole of a solid ionic compound into gaseous ions Lewis dot symbol (p288) symbol of an element with dots to represent the valence electrons the atom possesses Lewis structure (p294) representation of covalent bonding using Lewis symbols. Shared electron pairs are shown either as lines or pairs of dots between two atoms, and lone pairs are shown as pairs of dots on individual atoms Lone pair (p294) valence electrons that are not involved in covalent bond formation Multiple bond (p295) bonds formed when two atoms share two or more pairs of electrons Octet rule (p294) an atom other than hydrogen tends to form bonds until it is surrounded by eight valence electrons Polar covalent bond (p296) electrons spend more time in the region of one atom of the covalent bond vs the other Resonance (p305) use of two or more Lewis structures to represent a particular molecule or ion Resonance structure (p305) one of two or more alternative Lewis structures for a single molecule that cannot be described fully with a single Lewis structure Single bond (p295) two atoms held together by one electron pair are joined by a single bond Triple bond (p295) covalent bond in which two atoms share three pairs of electrons Chapter 10 Vocabulary Antibonding molecular orbital (p352) molecular orbital that is of higher energy and lower stability than the atomic orbitals from which it was formed Bonding molecular orbital (p352) molecular orbital that is of lower energy and greater stability than the atomic orbitals from which it was formed Dipole moment (μ) (p334) product of the charge and the distance between the charges in the molecule Homonuclear diatomic molecule (p356) diatomic molecule containing atoms of the same element Hybrid orbital (p340) atomic orbitals obtained when two or more nonequivalent orbitals of the same atom combine before covalent bond formation Hybridization (p340) process of mixing the atomic orbitals in an atom (usually the central atom) to generate a new set of atomic orbitals before covalent bond formation Molecular orbital (p351) orbital that results from the interaction of atomic orbitals of the bonding atoms Nonpolar molecule (p335) molecule that does not possess a dipole moment Pi bond (π bond) (p348) covalent bond formed by sideways overlapping orbitals; its electron density is concentrated above and below the plane of the nuclei of the bonding atoms Pi molecular orbital (p353) molecular orbital in which the electron density is concentrated above and below the line joining the two nuclei of the bonding atoms Polar molecule (p335) molecule that possesses a dipole moment Sigma bond (o bond) (p348) covalent bond formed by orbitals overlapping end-to-end; its electron density is concentrated between the nuclei of the bonding atoms Sigma molecular orbital (p352) molecular orbital in which the electron density is concentrated around a line between the two nuclei of the bonding atoms Valence shell (p324) outermost electron-occupied shell of an atom, which holds the electrons that are usually involved in bonding Valence-shell electron-pair repulsion (VSEPR) model (p324) A model that accounts for the geometrical arrangements of shared and unshared electron pairs around a central atom in terms in terms of the repulsive forces of electron pairs