1. Chemical Nomenclature 1. Binary Ionic Compounds - Type I 2. Binary Ionic Compounds - Type II 3. Ionic Compounds & Polyatomic (Complex) Ions 4. Oxy-Acids 5. Hydrated Ionic Compounds 6. Binary Acids 7. Binary Covalent Compounds

2. Type I Binary Ionic Compounds n The metal cations in these compounds have only ONE possible charge. Na + Zn 2+ Al 3+ Ca 2+ sodiumzinc aluminumcalcium The charges are memorized or predicted using a periodic table! n The cations are bonded to nonmetal anions: O 2 - N 3 - F - Br - oxide nitride fluoride bromide Notice that simple anions are always named with the suffix “ide”

3. n In an ionic compound, the charges of the cations and anions must always cancel out. n Subscripts are used if more than one atom is needed to cancel the charges: sodium chloride: Na + and Cl -  NaCl lithium oxide: Li + and O 2-  Li 2 O aluminum bromide: Al 3+ and Br -  AlBr 3 zinc nitride: Zn 2+ and N 3-  Zn 3 N 2 potassium iodide: K + and I -  KI silver phosphide: Ag + and P 3-  Ag 3 P

4. Examples: Type I Binary Ionic Compounds Write the formulas: potassium oxide zinc chloride silver sulfide aluminum nitride gallium oxide calcium iodide Write the names: K 3 N AgI ZnBr 2 Al 2 O 3 Ba 3 P 2 LiH

5. Type II Binary Ionic Compounds n These are ionic compounds where the metal cation can form TWO different charges. Fe 2 + iron (II) Fe 3 + iron (III) Ni 2 + nickel (II) Ni 3 + nickel (III) Co 2 + cobalt (II) Co 3 + cobalt (III) Cu + copper (I) Cu 2 + copper (II) Au + gold (I) Au 3 + gold (III) Sn 2 + tin (II) Sn 4 + tin (IV) An older system uses suffixes and Latin names, - ous for the lower charge, - ic for the higher charge: Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic

6. Examples: Type II Binary Ionic Compounds Write the formulas: iron (II) oxide copper (II) chloride tin (IV) sulfide cupric nitride nickel (III) oxide ferrous iodide cobalt (III) selenide Write the names: Fe 2 O 3 SnS NiBr 2 CuS Pb 3 P 2 CuBr FeCl 3

7. Examples: Type II Binary Ionic Compounds Write the formulas: iron (II) oxide FeO copper (II) chloride CuCl 2 tin (IV) sulfide SnS 2 cupric nitride Cu 3 N 2 nickel (III) oxide Ni 2 O 3 ferrous iodide FeI 2 cobalt (III) selenide Co 2 Se 3

8. n Write the names: n Fe2O3 Iron (III) oxide Ferric oxide n SnS Tin(II)sulphide stannous sulfide n NiBr2 Nickle (II) bromide n CuS Copper (II) Sulfide Cupric sulphide n Pb3P2 L n CuBr n FeCl

9. Polyatomic (Complex) Ions n All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons. n A molecule is a particle that forms when two or more atoms bond together. n A complex ion is a charged molecule. Complex ions may be cations or anions. examples: nitrate: NO 3 - sulfate: SO 4 2 - hydroxide: OH -

10. Writing formulas with Complex Ions a) Ammonium chloride b) Silver sulfate c) Aluminum hydroxide d) Calcium phosphate e) Iron (III) nitrate f) Copper(II) permanganate g) Ammonium dichromate h) Zinc acetate

11. Writing formulas with Complex Ions a) Ammonium chlorideNH 4 Cl b) Silver sulfateAg 2 SO 4 c) Aluminum hydroxideAl(OH) 3 d) Calcium phosphateCa 3 (PO 4 ) 2 e) Iron (III) nitrateFe(NO 3 ) 3 f) Copper(II) permanganateCu(MnO 4 ) 2 g) Ammonium dichromate(NH 4 ) 2 Cr 2 O 7 h) Zinc acetateZn(CH 3 COO) 2

12. Things to Notice n Most complex ions are anions. Ammonium, NH 4 +, is the most common complex cation. n Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms: perchlorateClO 4 - sulfateSO 4 2- chlorateClO 3 - sulfiteSO 3 2- chloriteClO 2 - hypochloriteClO - nitrateNO 3 - nitriteNO 2 -

13. More Formulas with Complex Ions a) Sodium carbonate b) Nickel (II) sulfite c) Aluminum chlorate d) Barium phosphite e) Iron (III) sulfite f) Cupric sulfate g) Zinc periodate

14. More Formulas with Complex Ions a) Sodium carbonateNa 2 CO 3 b) Nickel (II) sulfiteNiSO 3 c) Aluminum chlorateAl(ClO 3 ) 3 d) Barium phosphiteBa 3 (PO 3 ) 2 e) Iron (III) sulfiteFe 2 (SO 3 ) 3 f) Cupric sulfateCuSO 4 copper (II) Sulphate Cuprous sulphate Cu 2 SO 4 copper (I)Sulphate g) Zinc periodateZn(IO 4 ) 2

15. Hydrated Ionic Compounds n A HYDRATE is an salt that has water molecules trapped within its crystals. n Every hydrate has a certain number of water molecules associated with each formula unit of the ionic compound. The number of water molecules is indicated by using prefixes. monohexa dihepta triocta tetranona pentadeca CuSO 4 · 5 H 2 O copper (II) sulfate pentahydrate MgCO 3 ·10 H 2 O magnesium carbonate decahydrate

16. Examples of hydrates: n Write the formulas: copper(II) fluoride tetrahydrate calcium nitrate trihydrate n Write the names: MgSO 4 · 7 H 2 O FeCl 2 · H 2 O CuF 2 ·4 H 2 O Ca(NO 3 ) 2 ·3 H 2 O magnesium sulfate heptahydrate iron (II) chloride monohydrate

17. Examples of hydrates: n Write the formulas: copper(II) fluoride tetrahydrate calcium nitrate trihydrate n Write the names: MgSO 4 · 7 H 2 O FeCl 2 · H 2 O

18. Oxy-Acids n An acid can also be made of a hydrogen ion bonded to a complex ion. Complex ions whose names end in “ate”: NO 3 - SO 4 2- CO 3 2- PO 4 3- nitric acid: HNO 3 sulfuric acid: H 2 SO 4 carbonic acid:H 2 CO 3 phosphoric acid:H 3 PO 4 Chloric acidHClO 3 Can you propose a rule for naming oxy-acids with complex ions ending in “ate”?

19. More Oxy-Acids n Complex ions ending in “ite”: NO 2 - SO 3 2- ClO - ClO 2 - nitrous acid:HNO 2 sulfurous acid:H 2 SO 3 hypochlorous acid:HClO ( from hypochlorite ion) chlorous acidHClO 2 Can you propose a rule for naming oxy-acids with complex ions ending in “ite”?

20. Acids n Nitric Acid n Nitrous acid n Hyposulphurous acid n Perchloric acid

21. Acids n Nitric Acid HNO 3 Nitrous acid HNO 2 n Hyposulphurous acid H 2 SO 2 n Perchloric acid HClO 4

22. n Acid Salts Acid Salt ions can be formed if an oxy ion carries a charge like “-2” or “- 3”, a series of related ions can be formed by adding hydrogen cations (H + ) while still leaving a remainder net charge: examples: Sulfate:SO 4 2- hydrogen sulfate:HSO 4 - (bisulfate) Carbonate:CO 3 2- hydrogen carbonate:HCO 3 - (bicarbonate) Phosphate:PO 4 3- hydrogen phosphate:HPO 4 2- dihydrogen phosphate:H 2 PO 4 -

23. More Formulas with Complex Ions a) Sodium hydrogen carbonate b) Nickel (II) hydrogen sulfate c) Aluminum perchlorate d) Barium dihydrogen phosphate e) Iron (III) sulfite f) Cuprous Hydrogen hyposulphite g) Zinc periodate

24. More Formulas with Complex Ions a) Sodium bicarbonateNaHCO 3 b) Nickel (II) hydrogen sulfateNi(HSO 4 ) 2 c) Aluminum perchlorateAl(ClO 4 ) 3 d) Barium dihydrogen phosphateBa(H 2 PO 4 ) 2 e) Iron (III) sulfiteFe 2 (SO 3 ) 3 f) Cuprous hydrogen hyposulphite CuHSO 2 g) Zinc periodateZn(IO 4 ) 2

25. Binary Acids n A simple definition of an “acid” is a substance which produces H+ ions in water. n Most acids have hydrogen ions in their formulas. n A binary acid composed of a hydrogen cation bonded to one other element: HCl HBr H 2 S hydrochloric acidhydrobromic acidhydrosulfuric acid Binary acids are always named: hydro____ic acid

26. Binary Covalent Compounds n Covalent compounds are made of two NONMETAL elements sharing valence electrons. n There are no ions involved!! n Because there are no charges to help us write the formulas of covalent compounds, prefixes are used to indicate the number of each atom present in the formula. Brandon is awesome. CO 2 is named “carbon dioxide” CO is named “carbon monoxide” N 2 O is named “dinitrogen monoxide” SO 3 is named “sulfur trioxide” The prefix, “mono” is never used for the first element in the formula!

27. Examples of Covalent Naming n Write the names: SO 2 P 4 O 10 n Write the formulas: phosphorus pentachloride dinitrogen trioxide

28. Examples of Covalent Naming n Write the names: SO 2 sulfur dioxide P 4 O 10 tetraphosphorus decoxide n Write the formulas: phosphorus pentachloridePCl 5 dinitrogen trioxideN 2 O 3