2. IonicCovalent Starts with a metalStarts with a nonmetal Transfer of electronsShares electrons Formula unitMolecules Strong bondWeak bond Hi melting/boiling pointsLo melting/boiling points Hard, brittle solidsSoft solids or gases Good conductorsPoor conductors Crystal structuresVSEPR shapes Cations (+) and anions (-)Polar or nonpolar bonds

3.  Roman numeral = charge  Metals always (+)  Written 1 st  Nonmetals (-) in ionic bonding  Exception NH 4 1+ (ammonium ion)

4.  ide = original element (nonmetal)  ate and ite = polyatomic ions  2 exceptions: CN 1- (cyanide) and OH 1- (hydroxide) Don’t confuse valence # with charge. Valence # is the number of electrons in the outer shell Charge is the transfer of electrons

5.  Hydro --- ic acid  Hydro --- ic becomes ide = original element (nonmetal)  ous acid  ous becomes ite polyatomic ion  ic acid  ic beomes ate polyatomic ion

6.  Hydrosulfuric acid  H 2 S  Sulfurous acid  H 2 SO 3  H 3 P  Hydrophosphoric acid  H 3 PO 4  Phosphoric acid

7.  Disulfur hexafluoride  S 2 F 6  Carbon monoxide  CO  P 3 O  Triphosphorus monoxide  C 3 Cl 8  Tricarbon octachloride

8.  Magnesium sulfide  MgS  Iron (III) sulfate  Fe 2 (SO 4 ) 3  Na 2 O  Sodium oxide  Cu(NO 3 ) 2  Copper (II) nitrate