1. Ionic compounds form when metals react with nonmetals, resulting in the transfer of electrons and formation of cations and anions bonded ionically. 2. Ionic compounds have high melting points and boiling points due to the strong electrostatic forces between cations and anions in the crystalline lattice structure. 3. Metallic bonds form when metal cations attract delocalized electrons in the "sea of electrons" that moves throughout the entire metallic crystal. This produces metallic properties like conductivity and ductility.

1. Chapter 8 Ionic Compounds

14. Ionic Bonds: One Big Greedy Thief Dog!

21. Naming Ionic Compounds (continued) * Polyatomic ions each have specific names which should be memorized so they can be recognized on sight. (At this point, if you are asked to name any compound that contains more than two elements, it will contain at least one polyatomic ion.) A few of the more common polyatomic ions Formula Name C 2 H 3 O 2 1- acetate CO 3 2- carbonate HCO 3 1- bicarbonate NH 4 1 + ammonium Formula Name NO 3 1- nitrate OH 1- hydroxide PO 4 3- phosphate SO 4 2- sulfate

22. Naming Ionic Compounds: Examples Na 2 SO 4 sodium sulfate Fe(NO 3 ) 2 iron (II) nitrate AlCl 3 aluminum chloride PbI 4 lead (IV) iodide (NH 4 ) 3 PO 4 ammonium phosphate Mg 3 N 2 magnesium nitride AgC 2 H 3 O 2 silver acetate C 2 H 3 O 2 1- acetate CO 3 2- carbonate HCO 3 1- bicarbonate NH 4 1+ ammonium NO 3 1- nitrate OH 1- hydroxide PO 4 3- phosphate SO 4 2- sulfate * Groups I & II, Al, Zn, Cd, and Ag need no Roman numeral.