Home > Flashcards > Chemistry > Chapter 6 - Chemical Bonding

Details Title: Chapter 6 - Chemical Bonding Description: Vocabulary/Key Terms Total Flash Cards: 40 Created: 03/16/2004 05:51:04	To study from this set of flash cards, or to create your own your own study flash cards, register HERE. If you are already a registered user, CLICK HERE.
Cards Term chemical bond Definition a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together Term ionic bonding Definition the chemical bond resulting from electrical attraction between large numbers of cations and anions Term covalent bonding Definition a chemical bond resulting from the sharing of an electron pair between two atoms Term nonpolar-covalent bond Definition a covalent bond in which the bonding electrons are shared equally by the bonded atoms, resulting in a balance of electrical charge Term polar Definition having an uneven distribution of charge Term polar-covalent bond Definition a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons Term molecule Definition a neutral group of atoms that are held together by covalent bonds Term molecular compound Definition a chemical compound whose simplest units are molecules Term chemical formula Definition a formula that indicates the relative numbers of atoms of each kind in a chemical compund by using atomic symbols and numerical subscripts Term molecular formula Definition a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound Term diatomic molecule Definition a molecule containing only two atoms Term bond length Definition the distance between two bonded atoms at their minimum potential energy, that is, the average distance between two bonded atoms Term bond energy Definition the energy required to break a chemical bond and form neutral isolated atoms Term octet rule Definition 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 Term electron-dot notation Definition 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 Term unshared pair Definition a pair of electrons that is not involved in bonding and that belongs exclusively to one atom Term lone pair Definition a pair of electrons that is not involved in bonding and that belongs exclusively to one atom Term Lewis structure Definition a formula in which atomic symbols represent nuclei and inner-shell 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 Term structural formula Definition a formula that indicates the kind, number, arrangement, and bonds but not the unshared electron pairs of the atoms in a molecule Term single bond Definition a covalent bond produced by the sharing of one pair of electrons between two atoms Term double bond Definition a covalent bond produced by the sharing of two pairs of electrons between two atoms Term triple bond Definition a covalent bond produced by the sharing of three pairs of electrons between two atoms Term multiple bond Definition a double or triple bond Term resonance Definition the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure Term ionic compound Definition a compound composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal Term formula unit Definition the simplest collection of atoms from which an ionic compound's formula can be established Term lattice energy Definition the energy released when one mole of an ionic crystalline compound is formed from gaseous ions Term polyatomic ion Definition a charged group of covalently bonded atoms Term metallic bonding Definition chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons Term malleability Definition the ability of a substance to be hammered or beaten into thin sheets Term ductility Definition the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire Term molecular polarity Definition the uneven distribution of molecular charge Term VSEPR theory Definition repulsion between the sets of valence-level electrons surrounding an atom causes these sets to oriented as far apart as possible Term hybridization Definition the mixing of two or more atomic oribitals of similar energies on the same atom to produce new orbitals of equal energies Term hybrid orbitals Definition orbitals of equal energy produced by the combination of two or more orbitals on the same atom Term intermolecular forces Definition the force of attraction between molecules Term dipole Definition equal but opposite charges that are separated by a short distance Term dipole-dipole force Definition a force of attraction between polar molecules Term hydrogen bonding Definition 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 Term London dispersion force Definition an intermolecular attraction resulting from the constant motion of electrons and the creation of instantaneous dipoles