1. REVIEW of IONS OBJECTIVE: When atoms give away electrons

2. IONS ION What is it? An atom that LOST/GAINED electron(s)

3. IONS Goal is to get to the NEAREST Noble Gas RULES 1.If you go LEFT, you become POSITIVE. 2.If you go RIGHT, you become NEGATIVE

4. IONS Ions that LOSE electrons have a POSTIVE charge called cations pronounced “cat – ions”

5. IONS All metals become CATIONS

6. IONS USE HALF SHEET FOR TRANSITION METALS

7. IONS Ions that GAINS electrons have a NEGATIVE charge called anions pronounced “an – ions”

8. IONS Ex: CN - NH 4 + CO 3 2- Because these ions are made from two or more atoms, they are called polyatomic ions Some ions are made from two or more atoms

9. IONS -ite has less oxygen than –ate Memorize? Kind of

10. IONS Summary & Review 1.What is an ion? 2.What are the two types of ions? 3.Which ions gains electrons: cations or anions? 4.Predict the charge of each atom if it were to become an ion: Ca, Cl, Cu, F, Fe, Li, Na, N, O

11. Ionic Compounds OBJECTIVE: Joining Cations + Anions to make compounds

12. Ionic Compounds Na + + Cl -  NaCl cation anionionic compound forumula NaCl joined by IONIC BOND IONIC BOND = giving away/gaining electrons

13. Ionic Compounds Li + + Cl -  K + + Cl -  Ca 2+ + Cl -  Li + + O 2-  Ca 2+ + O 2-  LiCl KCl CaCl 2 Li 2 O CaO Charges must cancel and = 0

14. Ionic Compounds Cu + + CH 3 COO -  NH 4 + + Cr 2 O 7 -  Mg 2+ + OH -  CuCH 3 COO NH 4 Cr 2 O 7 Mg ( OH ) 2 Parenthesis for POLYATOMIC

15. Ionic Compounds Write formula for ionic compounds 1. Al 3+ + O 2-  2. Fe 2+ + Cl -  3. Na + + HCO 3 -  4. Na + + NO 2 -  5. Ca 2+ + PO 4 3-  6. H + + SO 4 2-  7. Mg 2+ + OH -  8. Fe 3+ + Cl -  9. NH 4 + + PO 4 3- 

16. 1. Naming Ionic Compounds Write from 1 to 5 in Roman Numerals I II

17. 1. Naming Ionic Compounds OBJECTIVE: Learn how to name compounds like NaHCO 3

18. 1. Naming Ionic Compounds First Name + Last Name = Full Name only TRANSITION METALS have roman numerals

19. Cations with Roman Numerals in BOLD

20. 1. Naming Ionic Compounds 1. Start with CATION, always 2. Name the anion using the suffix “ IDE ”. If anion is polyatomic…

21. 1. Naming Ionic Compounds “uncross” numbers to figure our roman numeral for cation FeCl 3 Cr 2 O 3 Cu 2 OMn 3 N 2 Mn(NO 2 ) 3 Mn(NO 3 ) 3 Mn(NO 3 ) 2 If no numbers then 1. Figure out charge of anion FeOCrO MnOCoN CrPO 4 ZnCrO 7 CuSO 4 CuNO 3

22. 1. Naming Ionic Compounds 1. Start with CATION, always 2. If cation is Transition Metal check table for roman numerals 3. Name the anion using the suffix “ IDE ”. If anion is polyatomic… 4. That’s it!

23. 1. Naming Ionic Compounds Writing formulas from names of ionic compounds 1. Write anion and charge. 2. Write cation and charge. 3. Cross charges and write formula. -ATE-ITE half sheet

24. Naming Ionic Compounds 1. Sodium Chloride 2. Lithium Fluoride 3. Iron(II) Chloride 4. Sodium Nitrate 5. Magnesium Hydroxide 6. Sodium Acetate 7. Ammonium Chloride 8. Hydrogen Peroxide 9. Sodium Carbonate 10. Ammonium Phosphate

25. 1. Naming Ionic Compounds SUMMARY & REVIEW Formula to Name 1. Start with cation 2. When to use roman numerals? 3. Then add…to anion 4. What about polyatomic ions? Name to Formula 1. Start with anion – LAST NAME 2. What if anion ends in ATE or ITE? 3. Write symbol for cation – FIRST NAME 4. Roman numerals?

26. 4. Lewis Dot Structures

27. 7. Lewis Structures 1. Write elements 2. Count total number of valence e 3. LEAST electronegative is in the center (usually CARBON) 4. Draw bond 5. Then draw dots until you run out 6. Make double/triple bonds if necessary

28. 7. Lewis Dot Structures Exceptions to the Octet Rule 1.Less than 8 2.More than 8 3.Polyatomic Ions

29. 7. Lewis Dot Structures Exceptions to the Octet Rule 1.Less than 8 Group 1 & Beryllium and Boron BeCl 2 BCl 3

30. 4. Lewis Dot Structures Exceptions to the Octet Rule 2. More than 8 Phosphorus,Sulfur and Xenon PCl 5 SF 6 XeF 4

31. 4. Lewis Dot Structures Exceptions to the Octet Rule 3. Polyatomic Ions CationsAnions SUBTRACT electrons ADD electrons add brackets [ ]