var nc = 23, fc = new Array(nc); fc[0] = {t:"Allotropes",d:"Different molecular forms of the same element, such as oxygen (O2) and ozone (O3)."}; fc[1] = {t:"Bond Energy",d:"The energy needed to break 1 mole of a particular covalent bond in a molecule or polyatomic ion in the gas phase."}; fc[2] = {t:"Bond Length",d:"The distance between the nuclear centers of two atoms joined together in a bond."}; fc[3] = {t:"Bond Order",d:"The number of bonds between atoms: 1 for a single bond, 2 for a double bond, and 3 for a triple bond."}; fc[4] = {t:"Bond Polarity",d:"A measure of the extent to which bonding electrons are unequally shared due to differences in electronegativity of the bonded atoms."}; fc[5] = {t:"Bonding Capacity",d:"The number of covalent bonds an atom forms to have an octet of electrons in its valence shell."}; fc[6] = {t:"Bonding Pair",d:"A pair of electrons shared between two atoms."}; fc[7] = {t:"Double Bond",d:"Results when two atoms share two pairs of electrons."}; fc[8] = {t:"Electronegativity",d:"A relative measure of the ability of an atom in a bond to attract electrons to itself."}; fc[9] = {t:"Formal Charge (FC)",d:"Value calculated for an atom in a molecule or polyatomic ion by determining the difference between the number of valence electrons in the free atom and the sum of lone-pair electrons plus half of the electrons in the atom’s bonding pairs."}; fc[10] = {t:"Free Radical",d:"An odd-electron molecule with an unpaired electron in its Lewis structure."}; fc[11] = {t:"Ionic Bond",d:"Results from the electrostatic attraction of a cation for an anion."}; fc[12] = {t:"Lewis Structure",d:"A two-dimensional representation of the bonds and lone pairs of valence electrons in a molecule or polyatomic ion."}; fc[13] = {t:"Lewis Symbol",d:"(also called Lewis dot symbol)
The chemical symbol for an atom surrounded by one or more dots representing the valence electrons."}; fc[14] = {t:"Lone Pair",d:"A pair of electrons that is not shared."}; fc[15] = {t:"Metallic Bond",d:"Consists of the nuclei of metal atoms surrounded by a “sea” of shared electrons."}; fc[16] = {t:"Nonpolar Covalent Bond",d:"A bond characterized by an even distribution of charge; electrons in the bonds are shared equally by the two atoms; pure covalent bonds give rise to nonpolar diatomic molecules."}; fc[17] = {t:"Octet Rule",d:"Atoms of main group elements make bonds by gaining, losing, or sharing electrons to achieve a valence shell containing 8 electrons, or four electron pairs."}; fc[18] = {t:"Polar Covalent Bond",d:"Results from unequal sharing of bonding pairs of electrons between atoms."}; fc[19] = {t:"Resonance",d:"Characteristic of electron distributions when two or more equivalent Lewis structures can be drawn for one compound."}; fc[20] = {t:"Resonance Structure",d:"One of two or more Lewis structures with the same arrangement of atoms but different arrangements of bonding pairs of electrons."}; fc[21] = {t:"Single Bond",d:"Results when two atoms share one pair of electrons."}; fc[22] = {t:"Triple Bond",d:"Results when two atoms share three pairs of electrons."};