1. Chapter 4

2. Binary compounds-contain 2 elements 1) metal w/ charge and non-metal (Type I) 2) Transition metal and non-metal (Type II) 3) two non-metals (Type III)

3.  (Type I) Cation- 1 st – same name as element Anion- 2 nd - root + ide Examples  NaI  CaO

4.  1) write element symbol and charge  2) net charges must equal zero  3) add subscripts if charges don’t add up to zero  Barium sulfide  Magnesium phosphide

5.  How to write formula from name  1) write element symbol and charge  2) net charges must equal zero  3) add subscripts if charges don’t add up to zero  Lead (II) oxide  Iron (III) sulfide  Roman numeral= charge of transition metal

6. Write name from formula Need to figure out the charge Include roman numeral in name  FeCl 2 (__x 1) + (-1 x 2)= 0 Fe +2 Iron (II) chloride  ic- higher charge Fe +3 Ferric  ous- lower charge Fe +2 Ferrous  Example 4.2, 4.3

7.  1) name the first element by its element name  2) second element is named as though it were an anion (ide ending)  3) prefixes are used to denote the number of atoms (Table 4.3 pg 95)  4) mono is never used for the first element  Example 4.4, 4.5

8.  Example 4.6

9.  Polyatomic ion- charged entities composed of several atoms bound together  Oxyanions- SO 3 and SO 4 ite ate  hypo-less than  per- more than  ClO- hypochlorite  ClO 2 – chlorite  ClO 3 – chlorate  ClO 4 - perchlorate

10.  Must know - name of polyatomic ion - charge of polyatomic ion - recognize polyatomic ion  NH 4 C 2 H 3 O 2  FeSO 4  Example 4.7  more than one polyatomic ion or polyatomic ions with a subscript require parentheses  (NH 4 ) 2 SO 4  Fe 3 (PO 4 ) 2

11.  Polyatomic ions names do not change  Ammonium nitrate  Calcium hydroxide  Lead (II) sulfate

12.  Acids- when dissolved in H 2 O, they produce H + ions  Sour taste Naming  1) if the anion does not contain O 2 then use hydro prefix, element root + ic (ex: HCl)  2) if O 2 is in the anion, then look at the ending of the polyatomic ion (HNO 3 and HNO 2 ) ite- ous  acid ending ate- ic

13.  Calcium hydroxide Ca(OH) 2  Iron (II) oxide FeO Example 4.9

14. 1. HF 9. Chlorous Acid 10. HClO 3 2. HBr 11. HClO 4 3. H 3 PO 4 12. carbonic acid 4. HNO 2 13. HC 2 H 3 O 2 5. Nitric acid 14. HClO 6. H 2 SO 3 15. HI 7. H 2 SO 4

15. 1. Hydrofluoric Acid 9. HClO 2 2. HCl 10. Chloric Acid 3. Hydrobromic Acid 11. Perchloric Acid 4. Phosphoric Acid 12. H 2 CO 3 5. Nitrous Acid 13. Acetic Acid 6. HNO 3 14. Hypochlorous Acid 7. Sulfurous Acid 15. Hydroiodic Acid 8. Sulfuric Acid