1. Warm up 10-13-14 1.Covalent bonds are between _____ and _____ elements 2.Ionic bonds are between _____ and _____ elements 3.Identify if these compounds are ionic or covalent: FeS, CO 2, Cl 2 and AlBr 3 Agenda -Turn in HW online bonds -Take quiz -Notes Chp 6-2 Lewis dot -Lab chemical bonds Homework Oct 24 – Online HW (57Qs)

2. Review For the Quiz Chapter 5 – Ions (positive and negative charge) - Bonds (3 types)

3. Formulas and Names of Ionic and Covalent Compounds Chp 5-3 and 6-2

4. Nomenclature: Naming of compounds Must determine which bond made up the compound -Ionic bond has metal elements -Covalent bond has no metal elements

5. Naming Covalent (Molecular) Compounds 1. Use a prefix to indicate the amount of each element in the compound 2. Never use mono– on the first element name. 3. Give the last element an –ide ending.

6. Naming Covalent (Molecular) Compounds Mono– 1 Di– 2 Tri– 3 Tetra– 4 Penta– 5 Hexa– 6 Hepta– 7 Octa– 8 Nona– 9 Deca– 10 Prefixes

7. Examples CO 2 B 2 H 4 Dinitrogen trioxide

8. Naming Covalent Compounds Practice Chemical Formula Name 1. CO 2. P 2 S 5 3. SiO 2 4. SCl 4 5.Trinitrogen pentabromide 6.Dinitrogen trioxide Why incorrect?Monosulfur dioxide

9. Naming Ionic Compounds 1. Ending element change to –ide. (no prefixes) 2. Make sure all the charge cancel each other out 3. If there is a transition metal you indicate the charge with a roman numeral after the name of the metal. 4. If it is a polyatomic ion, you simply use the name as it is. (no –ide)

10. Examples 1.CaCl 2 2.MgI 2 3.Potassium Sulfide 4.Beryllium Fluoride 5.Iron (II) Nitride 6.FeCl 2

11. Naming Ionic Compounds Practice 1. ______________ AlCl 3 2. ______________ Na 2 S 3.Lithium Bromide_____ 4.Calcium Fluoride_____ 5.Aluminum Oxide_____ 6.____________CuCl 2 7.Iron (III) Phosphide____ Writing Chemical Formula for Ionic Compounds -Write the symbol and charge -Cation goes in front -Make sure all the charges Cancel each other out Transition metal

12. Naming Ionic Compounds - Polyatomic Ions (NH 4 ) + Ammonium(NH 3 ) Ammonia (OH) - Hydroxide (CO 3 ) -2 Carbonate (NO 3 ) - Nitrate(NO 2 ) - Nitrite (SO 4 ) -2 Sulfate(SO 3 ) -2 Sulfite (PO 4 ) -3 Phosphate(PO 3 ) -3 Phosphite (Cr 2 O 7 ) -2 Dichromate

13. Naming Polyatomic Ions 1.______________Li 2 SO 4 2.______________ Sr(NO 3 ) 2 3.Potassium Phosphate_____ 4.Ammonium Oxide_____ 5.______________NaOH 6.______________ Ca(NO 2 ) 2 7.Calcium Carbonate______ 8.Ammonium Sulfide_____

14. More Examples Mixture of covalent, ionic and polyatomic nomenclature.

15. SrS Strontium Sulfide

16. GaCl 3 Gallium Chloride

17. Ammonium NH 4 +

18. Calcium Oxide CaO

19. Sulfate SO 4 2-

20. Phosphate PO 4 3-

21. Strontium Nitride Sr 3 N 2

22. Li 3 N Lithium Nitride

23. Hydroxide OH -

24. Beryllium Carbonate BeCO 3

25. BeSe Beryllium Selenide

26. Mg(NO 3 ) 2 Magnesium Nitrate

27. KBr Potassium Bromide

28. AlPO 4 Aluminum Phosphate

29. Magnesium Arsenide Mg 3 As 2

30. NaOH Sodium Hydroxide

31. Potassium Sulfate K 2 SO 4

32. Ba 2 P 3 Barium Phosphide

33. Rubidium Phosphide Rb 3 P

34. Potassium Chloride KCl

35. Sodium Oxide Na 2 O

36. Rb 2 O Rubidium Oxide

37. Bond Identification lab Objectives: Classify compounds as having ionic or covalent bond based on its physical property: solubility, conductivity and melting point Procedure: 1.Obtain the chemicals (half of a well) 2.Set up the apparatus and label your aluminum foil using a pencil 3.Put the chemicals on top of the aluminum foil and apply heat to it 4.Record the order that each compound melt 5.Dissolve the chemicals in water and ethanol