1. Binary Ionic Compounds a) Writing Names MgF 2 K3PK3P AlBr 3

2. b) Writing Formulas sodium oxide strontium nitride calcium sulfide

3. Multivalent Metals SymbolAbbreviation of Latin Name Pb plumb Feferr Cu cupr Sn stann Au aur Hg mercur Ninickel Co cobalt

4. Binary Ionic Compounds with Multivalent Metals a) Writing Formulas iron (III) chloride gold (I) sulfide plumbic oxide cuprous nitride

5. b) Writing Names SnO NiBr 2 AuP

6. Polyatomic Ions Ion Name NO 3 - CO 3 2- ClO 3 - SO 4 2- HCO 3 - OH - PO 4 3- NH 4 + nitrate bicarbonate chlorate hydroxide sulfate carbonate phosphate ammonium

7. Prefix and/or Suffix # of O’s Added or Subtracted Example Polyatomic Ionic Compounds - ATE 0NO 3 – PER - ATE+ 1 NO 4 - - ITE (nitrate) (pernitrate) - 1 NO 2 - (nitrite) HYPO - ITE - 2 NO - (hyponitrite)

8. a) Writing Names Na 2 SO 4 Ca 3 (PO 4 ) 2 Ba(ClO 4 ) 2 Fe(NO) 2 CuCO 3

9. b) Writing Formulas potassium phosphate mercuric chlorite lead (II) persulfate aluminum hypocarbonite

10. Binary Covalent Compounds a) Writing Names Formula Prefix Method Stock System As 2 S 5 SO 3 CS 2

11. b) Writing Formulas carbon monoxide antimony trichloride diphosphorus pentoxide nitrogen (III) oxide

12. Binary Acids a) Writing Names HCl (aq) HBr (aq) H 2 S (aq)

13. b) Writing Formulas hydrofluoric acid hydroiodic acid

14. Oxyacids Prefix and/or Suffix # of O’s Added or Subtracted Example - IC 0 CO 3 2- PER - IC + 1 CO 4 2- - OUS - 1CO 2 2- HYPO - OUS- 2 CO 2- (carbonic) (percarbonic) (carbonous) (hypocarbonous)

15. a) Writing Names H 2 SO 4 (aq) HNO 2 (aq) HClO 4 (aq) H 3 PO 2 (aq)

16. b) Writing Formulas sulfurous acid carbonic acid phosphorous acid perchloric acid