| A | B |
|---|
| bond energy | the energy required to break a chemical bond and form neutral isolated atoms |
| bond length | the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms |
| chemical bond | a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together |
| chemical formula | a formula that indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts |
| covalent bonding | a chemical bond resulting from the sharing of an electron pair between two atoms |
| diatomic molecule | a molecule containing only two atoms |
| dipole | equal but opposite charges that are separated by a short distance |
| dipole-dipole force | a force of attraction between polar molecules |
| double bond | a covalent bond produced by the sharing of two pairs of electrons between two atoms |
| ductility | the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire |
| electron-dot notation | an electron-configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol |
| formula unit | the simplest collection of atoms from which an ionic compound’s formula can be established |
| hybrid orbitals | orbitals of equal energy produced by the combination of two or more orbitals on the same atom |
| hybridization | the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies |
| hydrogen bonding | the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule |
| intermolecular force | the force of attraction between molecules |
| ionic bonding | the chemical bond resulting from electrical attraction between large numbers of cations and anions |
| ionic compound | a compound composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal |
| lattice energy | the energy released when one mole of an ionic crystalline compound is formed from gaseous ions |
| Lewis structure | a formula in which atomic symbols represent nuclei and innershell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons |
| London dispersion force | an intermolecular attraction resulting from the constant motion of electrons and the creation of instantaneous dipoles |
| lone pair | a pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
| malleability | the ability of a substance to be hammered or beaten into thin sheets |
| metallic bonding | chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons |
| molecular compound | a chemical compound whose simplest units are molecules |
| molecular formula | a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound |
| molecular polarity | the uneven distribution of molecular charge |
| molecule | a neutral group of atoms that are held together by covalent bonds |
| multiple bond | a double or triple bond |
| nonpolar-covalent bond | a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge |
| octet rule | chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level |
| polar | having an uneven distribution of charge |
| polar-covalent bond | a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons |
| polyatomic ion | a charged group of covalently bonded atoms |
| resonance | the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
| single bond | a covalent bond produced by the sharing of one pair of electrons between two atoms |
| structural formula | a formula that indicates the kind, number, arrangement, and bonds but not the unshared electron pairs of the atoms in a molecule |
| triple bond | a covalent bond produced by the sharing of three pairs of electrons between two atoms |
| unshared pair | a pair of electrons that is not involved in bonding and that belongs exclusively to one atom |
| VSEPR theory | repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible |
| binary compound | a compound composed of two different elements |
| empirical formula | the symbols for the elements combined in a compound with subscripts showing the smallest whole-number mole ratio of the different atoms in the compound |
| formula mass | the sum of the average atomic masses of all the atoms represented in the formula of any molecule, formula unit, or ion |
| monatomic ion | an ion formed from a single atom |
| nomenclature | a naming system |
| oxidation number | a number assigned to an atom in a molecular compound or molecular ion that indicates the general distribution of electrons among the bonded atoms |
| oxidation state | a number assigned to an atom in a molecular compound or ion that indicates the general distribution of electrons among the bonded atoms |
| oxyanion | a polyatomic ion that contains oxygen |
| percentage composition | the percentage by mass of each element in a compound |
| salt | an ionic compound composed of a cation and the anion from an acid |
