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Chapter 6 Vocabulary

Chemical Bond a mutual electrical attraction between the nuclei and valence electrons of different atoms that bind atoms together
Covalent Bonding results from sharing of electron pairs between two atoms
Ionic Bonding chemical bonding that results from the electrical attraction between large number of cations and anions
Non-polar 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
Polar uneven distribution of charge
Polar-Covalent Bond a covalent bond in which the bonded atoms have an unequal attractions for the shared electrons
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 Formula indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
Diatomic Model a molecule containing only tow atoms
Double Bond a covalent bond produced by the sharing of two pairs of electrons between two atoms
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 system's element
Lewis Structure formulas 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
Lone Pair(Unshared Pair) a pair of electrons that is not involved in bonding and that belongs exclusively to one atom
Molecular Compound a chemical compound whose simplest units are molecules
Molecular Formula shows the types and numbers of atoms combined in a single molecule of molecular compound
Molecule a neutral group of atoms that are held together by covalent bonds
Multiple bond double and triple bonds
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
Resonance refers to bonding 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 indicates the kind, number, arrangement, and bonds but not the unshared pairs of atoms in a molecule
Triple Bond a covalent bond produced by the sharing of three pairs of electrons between two atoms
Formula Unit the simplest collection of atoms where an ionic compound's formula can be established
Ionic Compound composed of positive and negative ions that are combined so that the numbers of negative and positive charges are equal
Lattice Energy the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
Polyatomic Ion a charged group of covalently bonded atoms
Created by: DaniRaine