Term
|
Definition
| forces that strongly attach atoms or ions |
|
|
Term
|
Definition
| electrostatic forces that exist between ions of opposite charge . may be formed by the transfer of electrons from one atom to another |
|
|
Term
|
Definition
| results from the sharing of electrons between 2 atoms. usually b/w 2 nonmetallic elements |
|
|
Term
|
Definition
| found in metals like copper, iron, and aluminum. each atom is bonded to several neighboring atoms. the bonding electrons are free to move throughout the 3D structure of the metal |
|
|
Term
|
Definition
| consists of the chemical symbol for the element plus a dot for each valence electron |
|
|
Term
|
Definition
| atoms try to get 8 valence electrons |
|
|
Term
|
Definition
| energy require to completely separate a mole of a solid ionic compound into its gaseous ions |
|
|
Term
|
Definition
| useful thermochemical cycle in which we use Hess' Law to calculate the lattice energy as the sum of several steps in formation of an ionic compound |
|
|
Term
|
Definition
| ions possess the same number of electron |
|
|
Term
|
Definition
| show electron pair shared b/w atoms as a line, and unshared electron pairs as dots |
|
|
Term
|
Definition
| useful in describing the sharing of electrons b/w atoms |
|
|
Term
|
Definition
| numerical measure of the ability of an atom, i a molecule, to compete with other atoms for the electrons shared between them |
|
|
Term
|
Definition
| what is produced when 2 electrical charges of equal magnitude but opposite sis are seperated by a distance |
|
|
Term
|
Definition
| quantitative measure of the magnitude of a dipole measured in debyes (D) |
|
|
Term
|
Definition
| charge an atom in a molecule would have if all atoms had the same elctronegativity |
|
|
Term
|
Definition
| equivalent Lewis structures |
|
|
Term
|
Definition
| enthalpy change for the breaking of a particular bond in a mole of a gaseous substance |
|
|
Term
|
Definition
| distance b/w the nuclei of the atoms involved in a bond |
|
|
