1. MORE IONIC COMPOUNDS

2. A solid compound that contains a metal with a non- metal (m-nm)(s) When the element is representative the valence of the element is determined by the group number. Some other metals have more than one valence! Example:Fe 2+ and Fe 3+ Example:Cu 1+ and Cu 2+ Find some other examples on your periodic table.

3. MULTI-VALENT METALS Multi-valent metals must be named precisely; Fe 2+ is Iron (II) Fe 3+ is Iron (III) Cu 1+ is Copper (I) Cu 2+ is Copper (II) The roman numeral indicates the valence of the metal. I IIIIIIVVVIVIIVIII

4. Multi-valent compounds Iron (II) chloride Fe 2+ Cl - FeCl 2(s) Manganese (IV) Oxide Mn +4 O 2- Mn 2 O 4 (s) MnO 2 (s)

5. Write the following formulas; Iron (III) oxide Copper (II) chloride Titanium (IV) sulfide Vanadium (V) oxide Manganese (IV) phosphide Cobalt (II) bromide Fe 2 O 3(s) CuCl 2(s) TiS 2(s) V 2 O 5(s) Mn 3 P 4(s) CoBr 2(s)

6. Complete Page 195 #1  9

7. Answers 1. a) They are equal and opposite so that the compound has an overall neutral charge. b)Al 2 O 3 -overall charge is 2(+3) + 3(-2) =0

8. 2.Mg donates 2e-’s to two fluorine atoms to make two fluoride ions. Mg 2+, F -, F - MgF 2 (s) 3.LiF(s) CaBr 2 (s) Na 3 N(s) AlN(s)

9. 4. lithium fluoride Calcium bromide Sodium nitride Aluminum nitride 5.NaI(s) BeF 2 (s) MgO(s) Al 2 S 3 (s)

10. 7.CuBr(s) CuBr 2 (s) FeS(s) FeS(s) 8 Tin (II) chloride Tin (IV) chloride Lead (II) bromide Lead (II) bromide

11. 9. Fe 2 O 3(s) CaF 2 (s) Cu 2 S(s) Cu 2 S(s) Iron (III) oxide Calcium fluoride Copper (I) sulfide

12. Another type of ionic compound! Ionic compounds are composed of ; Metal with a non-metal Multi-valent metal with a non-metal Metal with a polyatomic ion!

13. WHAT IS A POLYATOMIC ION? Are groups of atoms that tend to stay together and carry an overall ionic charge. Example: the hydroxide ion OH - is an ion which is made of an oxygen atom with a hydrogen atom and one extra electron.

14. Other Examples: CO 3 2- Carbonate NO 3 1- Nitrate NO 2 1- Nitrite SO 4 2- Sulfate SO 3 2- Sulfite Note: SPELLING IS IMPORTANT!!! Use your periodic table for reference!

15. WRITING FORMULAS FOR POLYATOMIC COMPOUNDS Example: What is the formula for the ionic compound formed by sodium and sulfate ion?

16. STEPS 1 ) Write the symbols of the metal and of the polyatomic group Na SO 4 2) Write the ionic charges Na +1 SO 4 -2 3) Choose the number of ions to balance the charge Na +1 Na +1 SO 4 -2 4) Write the formula using subscripts. Na 2 SO 4 You could use the criss-cross rule if you wanted to.

17. Example: What is the formula for the ionic compound formed between magnesium and hydroxide. Mg 2+ OH 1- Mg 1 OH 2 More than one polyatomic ions requires brackets!! Mg(OH) 2(s)

18. What is the formula for lead (IV) carbonate? 1) Pb CO 3 2) Pb +4 CO 3 -2 3) criss-cross rule 4) Pb 2 (CO 3 ) 4 5)Pb(CO 3 ) 2(s) *reduce and give the state!

19. Ammonium is a positive polyatomic ion that sometimes replaces the metal in an ionic compound. Ammonium is NH 4 + Ammonium chloride is NH 4 + Cl - NH 4 Cl

20. Complete: Ammonium hydroxide Ammonium phosphate Ammonium sulfate NH 4 OH(s) (NH 4 ) 3 PO 4 (s) (NH 4 ) 2 SO 4 (s)

21. Naming Ionic Compounds What is the name of Ca(NO 3 ) 2 ? Go through the steps backwards. Solution: Calcium Nitrate

22. What is Na 3 PO 4 (s)? What is NH 4 Br(s)? What is Fe(OH) 2 (s)? What is Fe(OH) 3 (s)? Sodium phosphate Ammonium bromide Iron (II) hydroxide Iron (III) hydroxide

23. HOMEWORK PAGE 198; 3, 4, 6, 7

24. SOLUTIONS 3a) Na 3 PO 4(s) 3b) CaSO 4(s) 3c) KClO 3(s) 3d) Al(OH) 3(s) 3e) Be(N0 3 ) 2(s) 3f) Mg(HCO 3 ) 2(s) 3g) NiCO 3(s) 4a) Potassium Carbonate 4b) Sodium Sulfate 4c) Aluminum bicarbonate 4d) Silver Nitrate

25. 6 NH 4 NO 3 NH 4 + is a polyatomic ion and must be written as a unit. NO 3 - is a polyatomic ion and must be written as a unit. 7a)NH 4 Cl(s) Ammonium chloride 7b) (NH 4 ) 2 SO 4 (s) Ammonium sulfate