Oxidation		The representation of a compound by two or more basic structures in which the valence electrons are rearranged to give structures of similar probability
Valence Electrons		Used to describe the gain of electrons by a molecule, atom or ion.
Orbitals		These are chemical bonds that occur between molecules.
Covalent Crystal		Used to describe the loss of electrons by a molecule, atom or ion.
Polarity		Atom with most boding sites, usually in the middle of a structural formula.
Substitutional Alloy		It is a formula that shows how atoms in a compound are attached to one another.
Octet Rule		the ability of an atom to inductively pull electrons towards itself
Structural Formula		Same as Bohr Model this model shows the electrons fixed energy levels.
Lone Pair		These are chemical bonds that occur within a molecule.
Intramolecular Bond		The atom having a positive or negative charge.
Dipole-dipole Forces		A chemical bond between two atoms that is created by sharing two electrons. The difference in electronegativity is less than 1.7.
Non-polar Molecule		A bond that is a special type of a dipole-dipole bond, which exists between a highly electronegative atoms and hydrogen atoms.
Stereochemistry		Chemical compounds with an unequally distributed electrons, such as the water molecule. The opposite charges attract each other....
Interstitial Alloy		Model which states there is a state of lowest energy for the electron, that there is a maximum energy, beyond which the electron is no longer bound to the nucleus and that within these two energies the electron can only exist in certain energy levels.
Ion		Force of attraction between oppositely charged particles.
Central Atom		An _____ can contain two electrons with paired spins and is often associated with a specific region of an atom.
Ionic Crystal		Rules which is designed to show the shapes of individual molecules. The rule uses a Lewis structure, which shows all of the bonds within the molecule and the locations of lone pairs of electrons to predict the 3D shape of the molecule
Electronegativity		Pair of electrons in the valance shell, it is not bonding site.
VSEPR Rules		It is the same as Lewis Structural Diagrams. The chemical symbol for the atom is surrounded by a number of dots corresponding to the number of valence electrons.
Bonding Electrons		A type of intermolecular forces which occurs from the polarization of molecules, there are two types: dipole-dipole forces and London dispersion forces.
Reduction		A crystal consisting of ions bound together by their electronegativity.
London Dispersion Forces		A chemical bond formed by electronegativity attraction between oppositely charged ions
Metallic Bond		The electrons that are in the outer shell.
Resonance		A crystal with covalent bonds between all of the atoms in the crystal.
Covalent Bond		A chemical bond in which shared electrons move freely among the atoms.
Electron Dot Diagram		The study of the spatial arrangements of atoms in molecules and compounds.
Isotope		An atom has the same number of protons, but different numbers of neutrons.
Bohr Model		Two electrons that form a pair of electrons in the valance shell of two atoms, used to form a bond between them.
Ionic Bond		An atom or group of atoms that carries a positive or negative charge as a result of having lost or gained one or more electrons.
Van der Waals Forces		A rule which states that an element's valence shell is full and most stable when it contains eight electrons.
Energy Level Model		A form of Van der Waals force, the random movements of electrons create short intermediate states of charged atoms.
Intermolecular Bond		Same as the Electron Dot Diagram, which shows electrons in the valance shell.
Dipole		Non-polar molecule is when the electrons are distributed more symmetrically and does not have an abundance of charges at the opposite sides.
Lewis Formula		A metal atom replaces another similarly sized atom in the structure.
Polar Molecule		Two types of metal atom mixed together, one type of atom is significantly smaller than the other type of atom.
Hydrogen Bonding		There is an unequal sharing of electrons. _____ _____ is when the electrons are not distributed symmetrically and thus does have an abundance of charges at the opposite sides.