2. Read the notes in the powerpoint and do the Practice problems on a separate sheet of paper to be handed in next class.

3. Different Rules for Naming Different Compounds Ionic: metal donates e - to non-metal – Simple Binary Ionic – Multivalent – Polyatomic Covalent: 2 nonmetals share e -

4. 1. Simple Ionic Compounds (1 st element) + (space) + (2 nd element with the ending changed to “-ide”) E.g. NaCl = sodium chloride KI = potassium iodide

5. Name  Chemical Formula How do we know what the subscripts are from the name? Look at the oxidation states (charge) of the ion on the periodic table, then criss cross E.g. magnesium iodide Mg is +2 and I is -1  Mg 2+ + I -  Mg 1 I 2  MgI 2

6. Practice #1 - Simple Ionic Compounds Write the name: 1)AgI 2) CaCl 2 3)NaH 4)K 2 O Write the formula: 5) Hydrogen iodide 6) Hydrogen 7) Magnesium nitride 8) Cesium phosphide

7. 2. Ionic Compounds with Multivalent Metals “Multi” = many, “valent” = combining power Multivalent: metals with many charges – E.g. Fe can be Fe 2+ or Fe 3+ Use Roman numerals in brackets after the multivalent ion E.g. FeCl 3 = iron(III) chloride, Vs. FeCl 2 = iron (II) chloride

8. Roman Numerals Roman NumeralHindu-Arabic Numeral (nulla)0 I1 II2 III3 IV4 V5 VI6 VII7 VIII8 IX9 X10 XI11

9. Name the following: Cr 2 O 3 Cr 2+ O 2- CrO chromium (II) oxide ✖ Cr 3+ O 2- Cr 2 O 3 chromium (III) oxide ✔

10. Write the name: 1)CuI 2) PbCl 2 3) SnClO 2 Write the formula: 4) Copper(II) sulfate 5) Lead(IV) sulfide 6) Mercury(II) bromide Practice #2 - Multivalent Ionic Compounds

11. Naming Ionic Compounds with Polyatomic Ions “Poly” = many Polyatomic ion = ion with more than 1 atom E.g. OH -, SO 4 2-, NH 4 + Use formula sheet to find their names and charges

12. (1 st element) + (polyatomic ion) – E.g. NaOH = sodium hydroxide (polyatomic ion) + (2 nd element with “-ide”) – E.g. NH 4 Cl = ammonium chloride

13. The atoms of polyatomic ions are covalently bonded together and don’t separate Their charges are applied to the entire ion as a whole E.g. K + + SO 4 2-  K 2 (SO 4 ) 1  K 2 SO 4

14. Naming Polyatomic Ionic Compounds Write the name: 1)NaOH 2) CaCO 3 3) NH 4 Cl 4) HCN Write the formula: 5) Aluminum Permanganate 6) Sodium sulfide 7) Sodium nitrate 8) Barium dichromate Practice #3 - Ionic Compounds with Polyatomic Ions

15. Naming Covalent Compounds All you do is add a prefix or two…

16. Naming Covalent Compounds

17. Covalent Compounds Formula  Name (Prefix + 1 st element) + (space) + (prefix + 2 nd element with the ending changed to “-ide”) “Mono” prefix is not needed for 1 st element CO 2 = carbon dioxide not monocarbon dioxide H 2 O = dihydrogen monoxide

18. Covalent Compounds Name  Formula Find out the number of atoms of an element by looking at its prefix Dihydrogen monoxide = 2(hydrogen)+1(oxide) = H 2 O 1 = H 2 O Carbon monoxide = carbon + 1(oxide) = CO

19. Write the name: 1)PCl 3 2) NO 2 3)ICl 3 4)N 2 O 4 Write the formula: 5) dichlorine monoxide 6) silicon monocarbide 7) nitrogen triiodide 8)carbon tetraiodide Practice #4 – Covalent Compounds