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

2. Definitions n An IONIC COMPOUND consists of a metal cation bonded to a nonmetal anion. Electrostatic attraction holds them together. n A COVALENT COMPOUND consists of two nonmetal atoms sharing valence electrons. n A BINARY compound is one that is made of just two elements.

3. 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”

4. 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

5. Examples: Type I Binary Ionic Compounds Write the formulas: Di-potassium oxide zinc chloride silver sulfide Write the names: K 3 N AgI ZnBr 2

6. 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)

7. Examples: Type II Binary Ionic Compounds Write the formulas: iron (II) oxide copper (II) chloride tin (IV) sulfide cobalt (III) selenide Write the names: Fe 2 O 3 Pb 3 P 2 CuBr FeCl 3

8. 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 -

9. 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

10. 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: perchorateClO 4 - sulfateSO 4 2- chlorateClO 3 - sulfiteSO 3 2- chloriteClO 2 - hypochloriteClO - nitrateNO 3 - nitriteNO 2 -

11. n If an 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 net charge: examples: Sulfide:S 2- hydrogen sulfide:HS - (bisulfide) 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 -

12. More Formulas with Complex Ions a) Sodium bicarbonateNaHCO 3 b) Nickel (II) hydrogen sulfideNi(HS) 2 c) Aluminum perchlorateAl(ClO 4 ) 3 d) Barium dihydrogen phosphateBa(H 2 PO 4 ) 2

13. 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

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

15. 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. 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!

16. 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

17. 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

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 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 chlorous acidHClO 2 Can you propose a rule for naming oxy-acids with complex ions ending in “ite”?