var nc = 39, fc = new Array(nc); fc[0] = {t:"Antibonding Orbital",d:"Term in MO theory describing regions of electron density in a molecule that destabilize the molecule because they do not increase the electron density between nuclear centers."}; fc[1] = {t:"Aromatic Compound",d:"A cyclic, planar compound with delocalized π (pi) electrons above and below the plane of the molecule."}; fc[2] = {t:"Bond Angle",d:"The angle (in degrees) defined by lines joining the centers of two atoms to a third atom to which they are chemically bonded."}; fc[3] = {t:"Bond Dipole",d:"Separation of electrical charge created when atoms with different electronegativities form a covalent bond."}; fc[4] = {t:"Bonding Orbital",d:"Term in MO theory describing regions of increased electron density between nuclear centers that serve to hold atoms together in molecules."}; fc[5] = {t:"Chirality",d:"Property of a molecule that is not superimposable on its mirror image."}; fc[6] = {t:"Delocalization",d:"(adjective: delocalized)
When electrons in alternating single and double bonds are spread over the three or more atoms in a molecule."}; fc[7] = {t:"Diamagnetic",d:"Describes a substance with no unpaired electrons that is weakly repelled by a magnetic field."}; fc[8] = {t:"Dipole Moment (μ)",d:"A measure of the degree to which a molecule aligns itself in an applied electric field; a quantitative expression of the polarity of a molecule."}; fc[9] = {t:"Electron-Pair Geometry",d:"The three-dimensional arrangement of bonding pairs and lone pairs of electrons about a central atom."}; fc[10] = {t:"Hybrid Atomic Orbital",d:"In valence bond theory one of a set of equivalent orbitals about an atom created when specific atomic orbitals are mixed."}; fc[11] = {t:"Hybridization",d:"In valence bond theory the mixing of atomic orbitals to generate new sets of orbitals that then are available to form covalent bonds with other atoms."}; fc[12] = {t:"Molecular Geometry",d:"The three-dimensional arrangement of the atoms in a molecule."}; fc[13] = {t:"Molecular Orbit (MO) Theory",d:"A bonding theory based on the mixing of atomic orbitals of similar shapes and energies to form molecular orbitals that belong to the molecule as a whole."}; fc[14] = {t:"Molecular Orbital",d:"A region of characteristic shape and energy where electrons in a molecule are located."}; fc[15] = {t:"Molecular Orbital Diagram",d:"In MO theory, an energy-level diagram showing the relative energies and electron occupancy of the molecular orbitals for a molecule."}; fc[16] = {t:"Molecular Recognition",d:"The process by which molecules interact with other molecules to produce a biological effect."}; fc[17] = {t:"Octahedral",d:"Molecular geometry about a central atom with a steric number of 6 and no lone pairs of electrons in which all six sites are equivalent."}; fc[18] = {t:"Overlap",d:"A term in valence bond theory describing bonds arising from two orbitals on different atoms that occupy the same region of space."}; fc[19] = {t:"Paramagnetic",d:"Describes a substance with unpaired electrons that is attracted to a magnetic field."}; fc[20] = {t:"Pi (π) Bond",d:"A covalent bond in which electron density is greatest on opposite sides of the bonding axis."}; fc[21] = {t:"Pi (π) Molecular Orbitals",d:"In MO theory, formed by the mixing of atomic orbitals oriented above and below, or in front of and behind the bonding axis."}; fc[22] = {t:"Seesaw",d:"Molecular geometry about a central atom with a steric number of 5 and one lone pair of electrons in an equatorial position."}; fc[23] = {t:"Sigma (σ) Bond",d:"A covalent bond in which the highest electron density lies between the two atoms along the bond axis."}; fc[24] = {t:"Sigma (σ) Molecular Orbital",d:"In MO theory, the lowest-energy orbital that forms when atomic orbitals mix; electrons in σ molecular orbitals form sigma (σ) bonds."}; fc[25] = {t:"sp Hybrid Orbitals",d:"Two hybrid orbitals on opposite sides of the hybridized atom formed by mixing one s and one p orbital."}; fc[26] = {t:"sp2 Hybrid Orbitals",d:"Three hybrid orbitals in a trigonal planar orientation formed by mixing of one s and two p orbitals."}; fc[27] = {t:"sp3 Hybrid Orbitals",d:"A set of four hybrid orbitals with a tetrahedral orientation produced by mixing one s and three p atomic orbitals."}; fc[28] = {t:"sp3d Hybrid Orbitals",d:"Five equivalent hybrid orbitals with lobes pointing toward the vertices of a trigonal bipyramid that form by mixing one s orbital, three p orbitals, and one d orbital from the same shell."}; fc[29] = {t:"sp3d2 Hybrid Orbitals",d:"Six equivalent hybrid orbitals that point toward the vertices of an octahedron form from mixing one s orbital, three p orbitals, and two d orbitals from the same shell."}; fc[30] = {t:"Square Planar",d:"Molecular geometry about a central atom with a steric number of 6 and two lone pairs of electrons that occupy axial sites; the atoms occupy four equatorial positions."}; fc[31] = {t:"Square Pyramidal",d:"Molecular geometry about a central atom with a steric number of 6 and one lone pair of electrons; as typically drawn, the atoms occupy four equatorial and one axial site."}; fc[32] = {t:"Steric Number (SN)",d:"The sum of the number of atoms bonded to a central atom plus the number of lone pairs of electrons on the central atom."}; fc[33] = {t:"Tetrahedral",d:"Molecular geometry about a central atom with a steric number of 4 and no lone pairs of electrons."}; fc[34] = {t:"Trigonal Bipyramidal",d:"Molecular geometry about a central atom with a steric number of 5 and no lone pairs of electrons in which three atoms occupy equatorial sites and two other atoms occupy axial sites above and below the equatorial plane."}; fc[35] = {t:"Trigonal Planar",d:"Molecular geometry about a central atom with a steric number of 3 and no lone pairs of electrons."}; fc[36] = {t:"T-shaped",d:"Molecular geometry about a central atom with a steric number of 5 and two lone pairs of electrons that occupy equatorial positions; the atoms occupy two axial sites and one equatorial site."}; fc[37] = {t:"Valence Bond Theory",d:"A quantum mechanics–based theory of bonding that assumes covalent bonds form when half-filled orbitals on different atoms overlap or occupy the same region in space."}; fc[38] = {t:"Valence-Shell Electron-Pair Repulsion Theory (VSEPR)",d:"A model predicting the arrangement of valence electron pairs around a central atom that minimizes their mutual repulsion to produce the lowest-energy orientations."};