1. Naming Compounds PSc.2.2.3

2. Naming Ionic Binary Compounds Metal -- Nonmetal NaClSodium Chloride KBrPotassium Bromide Calcium Oxide CaO First element – No change in name. Second element – Change ending to –IDE.

3. Naming Ionic Binary Compounds Metal -- Nonmetal KClPotassium Chloride LiBrLithium Bromide Calcium Chloride CaCl 2 First element : No change in name. Second element : Change ending to – IDE.

4. Naming Ionic Binary Compounds you try LiFLithium Fluoride BaOBarium Oxide Calcium Sulfide CaS First element : No change in name Second element : Change ending to – IDE.

5. Naming Covalent Compounds Nonmetal -- Nonmetal COCarbon Oxide We need to differentiate between the two CO 2 One oxygen Two oxygens

6. Naming Covalent Compounds Nonmetal -- Nonmetal NONitrogen Oxide We need to differentiate between the two NO 2 One oxygen Two oxygens

7. Naming Covalent Compounds COCarbon Oxide To differentiate the two we use Prefixes; Mono1Tetra4 Di2Penta5 Tri3Hexa6 CO 2 One oxygen Two oxygen

8. Naming Covalent Compounds CO Carbon monoxide CO 2 One oxygen Two oxygens Carbon dioxide

9. Naming Covalent Compounds NO Nitrogen monoxide NO 2 One oxygen Two oxygensNitrogen dioxide N2O3N2O3 Dinitrogen trioxide Two nitrogens Three oxygens

10. Naming covalent compounds using prefixes CO Carbon mono-oxide BH 3 Boron tri-hydride SiO 2 PO 5 Phosphorous penta-oxide Carbon tetra-fluoride Silicon di-oxide CF 4 SF 6 Sulfur hexa-fluoride

11. Naming Compounds formed between metals of ambiguous oxidation state and nonmetals. Metals in Group 3 to Group 14 can have different oxidation states Distinguish the different oxidation state using roman numerals Arabic numbers and Roman numerals 1(I)6(VI) 2(II)7(IIV) 3(III)8(VIII) 4(IV)9(IX) 5(V)10(X)

12. Naming Compounds with Metal -- Nonmetal TiCl 2 Titanium (II) Chloride TiCl 4 Titanium (IV) Chloride SnCl 2 Tin (II) Chloride SnCl 4 Tin (IV) Chloride PbOLead (II) Oxide PbO 2 Lead (IV) Oxide First element – No change, add ( I ) or ( II ). Second element – Change ending to –IDE.

13. Naming ionic and covalent compounds NONitrogen monoxide (Covalent) AlH 3 Aluminum hydride (Ionic) BaCl 2 N2O5N2O5 Dinitrogen pentoxide(Covalent) Tin (IV) chloride(Ionic) Barium chloride (Ionic) SnCl 4 PbO 2 Lead (VI) oxide (Ionic)

14. Charge of positive Ions To determine the charge of an ion use the periodic table Group 1 elements form ions with a +1 charge Group 2 elements form ions with a +2 charge Group3 and Group13 elements mostly form ions with a +3 charge Group 4 and 14 elements form ions with a +4 charge This rule applies for the most common ions. Elements can form less common ions, these have different charges.

15. Charge of negative Ions To determine the charge of an ion use the periodic table Group 17 elements form ions with a -1 charge Group 16 elements form ions with a -2 charge Group 15 elements form ions with a -3 charge This rule applies for the most common ions. Elements can form less common ions, These have different charges.

16. Polyatomic ions Memorize these Acetate ( C 2 H 3 O 2 ) -1 or (Ac) - Ammonium (NH 4 ) +1 Hydroxide (OH) -1 Carbonate (CO 3 ) -2 Hydrogen Carbonate (HCO 3 ) -1 Nitrate (NO 3 ) -1 Nitrite (NO 2 ) -1 Sulfate (SO 4 ) -2 Sulfite (SO 3 ) -2 Phosphate (PO 4 ) -3 Phosphite (PO 3 ) -3

17. Ionic compounds Lead (II) Acetate Pb( C 2 H 3 O 2 ) 2 Tin (IV) chloride SnCl 4 Ammonium hydroxide (NH 4 ) (OH) Lead (IV) nitrate Pb (NO 3 ) 4 Potassium Hydroxide K(OH) Aluminum oxide Al 2 O 3 Magnesium Carbonate Mg(CO 3 ) Sodium Hydrogen Carbonate NaHCO 3 Calcium Nitrate Ca(NO 3 ) 2 Potassium Nitrite K(NO 2 ) Lead (II) Sulfate Pb (SO 4 ) Magnesium Sulfite Mg(SO 3 ) Calcium Phosphate Ca 3 (PO 4 ) 2 Potassium Phosphite K 3 (PO 3 )