Chapter 7: Chemical Bonding and Molecular StructureKey Termsaxial positionlocation in a trigonal bipyramidal geometry in which there is another atom at a 180° angle andthe equatorial positions are at a 90° anglebond angleangle between any two covalent bonds that share a common atombond dipole momentseparation of charge in a bond that depends on the difference in electronegativity and the bonddistance represented by partial charges or a vectorbond distance(also, bond length) distance between the nuclei of two bonded atomsbond energy(also, bond dissociation energy) energy required to break a covalent bond in a gaseoussubstancebond lengthdistance between the nuclei of two bonded atoms at which the lowest potential energy isachievedBorn-Haber cyclethermochemical cycle relating the various energetic steps involved in the formation of an ionicsolid from the relevant elementscovalent bondbond formed when electrons are shared between atomsdipole momentproperty of a molecule that describes the separation of charge determined by the sum of theindividual bond moments based on the molecular structuredouble bondcovalent bond in which two pairs of electrons are shared between two atomselectron-pair geometryarrangement around a central atom of all regions of electron density (bonds, lone pairs, orunpaired electrons)electronegativitytendency of an atom to attract electrons in a bond to itselfequatorial positionone of the three positions in a trigonal bipyramidal geometry with 120° angles between them;the axial positions are located at a 90° angleformal chargecharge that would result on an atom by taking the number of valence electrons on the neutralatom and subtracting the nonbonding electrons and the number of bonds (one-half of thebonding electrons)free radical
molecule that contains an odd number of electronshypervalent moleculemolecule containing at least one main group element that has more than eight electrons in itsvalence shellinert pair effecttendency of heavy atoms to form ions in which their valenceselectrons are not lostionic bondstrong electrostatic force of attraction between cations and anions in an ionic compoundlattice energy (ΔHlattice)energy required to separate one mole of an ionic solid into its component gaseous ionsLewis structurediagram showing lone pairs and bonding pairs of electrons in a molecule or an ionLewis symbolsymbol for an element or monatomic ion that uses a dot to represent each valence electron inthe element or ionlinearshape in which two outside groups are placed on opposite sides of a central atomlone pairtwo (a pair of) valence electrons that are not used to form a covalent bondmolecular structurearrangement of atoms in a molecule or ionmolecular structurestructure that includes only the placement of the atoms in the moleculeoctahedralshape in which six outside groups are placed around a central atom such that athree-dimensional shape is generated with four groups forming a square and the other twoforming the apex of two pyramids, one above and one below the square planeoctet ruleguideline that states main group atoms will form structures in which eight valence electronsinteract with each nucleus, counting bonding electrons as interacting with both atoms connectedby the bondpolar covalent bondcovalent bond between atoms of different electronegativities; a covalent bond with a positive
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