1. Nomenclature Chapter 5

2. Good News and Bad News Good News: No calculations! Bad News: Memorization!

3. Common Names Sugar of lead Lead acetate Blue vitriol copper(II) sulfate pentahydrate, CuSO 4 ·5 H 2 O. Quicklime CaO Epsom salts MgSO4·7H2O Milk of magnesia Mg(OH) 2 Gypsum CaSO 4 Laughing gas N 2 O

4. Naming Compounds Binary Compounds Metal with a nonmetal Two nonmetals

5. Binary Ionic Compounds Contains a metal ion and a nonmetal ion Cations are positive (metals) and written 1st Anions are negative (usually nonmetals) and written 2 nd Table 5.1 (need to know) Notice that Hydrogen can be a cation or an anion! Anions change ending to ide

6. Type I Compounds Metal can form only one ion Metals are from groups 1 and 2 only Easiest to name Three simple rules

7. Rules for Type I Compounds 1. The cation is always names first and the anion is named second. 2. To name the cation, use the element name. 3. Anions have the ending changed to ide.

8. Examples NaCl Sodium Chloride KI Potassium Iodide CaS Calcium Sulfide CsBr Cesium Bromide MgO Magnesium Oxide

9. Your Turn Cs 2 O BeF Al 2 O 3 AgCl

10. Type II Ionic Compounds Contains a cation that can have more than one charge Almost always a transition metal Examples: Copper can be 2+ or 1+ Iron can be 2+ or 3+ Tin can be 2+ or 4+ See table 5.2 P133

11. Rules for naming type II 1. Name the metal as an element followed by the charge in Roman Numerals in parenthesis. 2. Name the anion as usual. How do you find the charge? MnO 2

12. Examples Fe 2 O 3 Iron (III) oxide HgO Mercury (II) oxide PbCl 2 Lead (II) chloride CuCl 2 Copper (II) chloride

13. Your Turn SnCl 2 PbF 2 Co 2 O 3 CuO

14. Type III Binary Compounds 1. The first element is named using the full element name 2. The second element is named as an anion 3. Prefixes are used to denote the numbers of atoms of each type present. See table 5.3 on P 137 4. The prefix mono is never used for naming the first element.

15. Examples BF 3 Boron Trifluoride N2O3N2O3 Dinitrogen trioxide NO Nitrogen monoxide CO Carbon monoxide CO 2 Carbon dioxide

16. Your Turn NO 2 P 4 O 6 SF 6 N 2 O 3

17. Naming Binary Compounds Binary Compound? Metal Present? Does the Metal form more than one cation? Type I Type II Roman Numerals Yes Type III Prefixes Yes No

18. Polyatomic Ions Ions with more than one atom type Can be cations or anoins See table 5.4 p 142

19. Oxyanions Contain an element combined with oxygen in different proportions Example: NO 2 and NO 3 Use ite and ate respectively

20. Worst Case Scenario ClO - ClO 2 - ClO 3 - ClO 4 - Hypochlorite Chlorite Chlorate Perchlorate

21. Examples Na 2 CO 3 CsClO 3 CuNO 3 FePO 4

22. Your Turn BaSO 3 NaClO 4 KMnO 4 Na 3 PO 4

23. Naming Acids When dissolved in water produce a H+ Common acids: Citric Acid Vinegar contains acetic acid

24. Rules for Naming Does it contain oxygen? 1. If it does not contain oxygen, add the prefix hydro and the suffix acid to the element. 2. If it contains oxygen,you add the suffix ic or ous and acid. Ate goes to ic Ite goes to ous

25. Examples HCl HCN H 2 S H 2 SO 4 H 2 SO 3

26. Your Turn HClO 4 H 3 PO 4 HNO 3 HNO 2

27. Last Slide! You need to know tables 5.5 and 5.6 All the variations of halogen acids (not just chlorine (F, Br and I) Key terms