1. Periodic Table

2. Metals n Conductors n Lose electrons n Malleable and ductile

3. Nonmetals n Brittle n Gain electrons n Covalent bonds

4. Semi-metals or Metalloids

5. Alkali Metals

6. Alkaline Earth Metals

7. Halogens

8. Transition metals

9. Noble Gases

10. Inner Transition Metals

11. +1+2-2-3

12. Naming compounds n Two types n Ionic - metal and non metal or polyatomics. n Covalent- we will just learn the rules for 2 non-metals.

13. Ionic compounds n If the cation is monoatomic- Name the metal (cation) just write the name. n If the cation is polyatomic- name it. n If the anion is monoatomic- name it but change the ending to –ide. n If the anion is poly atomic- just name it n Practice.

14. Covalent compounds n Two words, with prefixes. n Prefixes tell you how many. n mono, di, tri, tetra, penta, hexa, septa, nona, deca n First element whole name with the appropriate prefix, except mono. n Second element, -ide ending with appropriate prefix. n Practice

15. Ionic Compounds n Have to know what ions they form n off table, polyatomic, or figure it out n CaS nK2SnK2SnK2SnK2S n AlPO 4 n K 2 SO 4 n FeS n CoI 3

16. Ionic Compounds n Fe 2 (C 2 O 4 ) n MgO n MnO n KMnO 4 n NH 4 NO 3 n Hg 2 Cl 2 n Cr 2 O 3

17. Ionic Compounds n KClO 4 n NaClO 3 n YBrO 2 n Cr(ClO) 6

18. n CO 2 n CO n CCl 4 nN2O4nN2O4nN2O4nN2O4 n XeF 6 nN4O4nN4O4nN4O4nN4O4 n P 2 O 10 Naming Covalent Compounds

19. Ionic Formulas n Sodium nitride n sodium- Na is always +1 n nitride - ide tells you it comes from the table n nitride is N -3

20. Ionic Formulas n Sodium nitride n sodium- Na is always +1 n Nitride - ide tells you it comes from the table n nitride is N -3 Na +1 N -3

21. Ionic Compounds n Sodium sulfite n calcium iodide n Lead (II) oxide n Lead (IV) oxide n Mercury (I) sulfide n Barium chromate n Aluminum hydrogen sulfate n Cerium (IV) nitrite

22. Covalent compounds n The name tells you how to write the formula n Sulfur dioxide n diflourine monoxide n nitrogen trichloride n diphosphorus pentoxide

23. Acids n Substances that produce H + ions when dissolved in water. n All acids begin with H. n Two types of acids: n Oxyacids n Non-oxyacids

24. Naming acids n If the formula has oxygen in it n write the name of the anion, but change –ate to -ic acid –ite to -ous acid n Watch out for sulfuric and sulfurous n H 2 CrO 4 n HMnO 4 n HNO 2

25. Naming acids n If the acid doesn’t have oxygen n add the prefix hydro- n change the suffix -ide to -ic acid n HCl nH2SnH2SnH2SnH2S n HCN

26. Formulas for acids n Backwards from names. n If it has hydro- in the name it has no oxygen n Anion ends in -ide n No hydro, anion ends in -ate or -ite n Write anion and add enough H to balance the charges.

27. Formulas for acids n hydrofluoric acid n dichromic acid n carbonic acid n hydrophosphoric acid n hypofluorous acid n perchloric acid n phosphorous acid

28. Hydrates n Some salts trap water crystals when they form crystals. n These are hydrates. n Both the name and the formula needs to indicate how many water molecules are trapped. n In the name we add the word hydrate with a prefix that tells us how many water molecules.

29. Hydrates n In the formula you put a dot and then write the number of molecules. Calcium chloride dihydrate = CaCl 2  2  Calcium chloride dihydrate = CaCl 2  2  Chromium (III) nitrate hexahydrate = Cr(NO 3 ) 3  6H 2 O Chromium (III) nitrate hexahydrate = Cr(NO 3 ) 3  6H 2 O