1. Chemical Names & Formulas Chapter 9

2. Warm Up Take 7 min to finish Homework

3. Go Over ChemQuest 21 Skill Practice 19-21 More Ionic Bonding Practice

4. Time to Review Ionic Bonding IB QUIZ NEXT CLASS This should go quick. All of this has been taught. Some of these slides you have already seen

5. Ionic Bonding: Between Metals and Nonmetals

6. Monatomic Ions Ions consisting of one atom Determined by using the periodic table

7. Transition Metals - the charge must be provided Ex.) Fe(III) has a +3 charge Fe(II) has a +2 charge  Reference Table 9.2, p.255 for trans. metal names and charges  Stock Name vs. Classical Name  Ex) Copper(I) ion (stock name) and Cuprous ion (classical name)

9. Polyatomic Ions Tightly bound group of atoms that behave as a unit and carry a charge Treated the same as monatomic ions when writing chemical formulas and naming (also called tertiary compounds) Ex.) (PO 4 ) 3- (CO 3 ) 2- Phosphate Carbonate

10. Polyatomic Ions

11. Types of Compounds Ionic – Metal & Non-Metal Molecular – 2 Non-Metals

12. Ionic Compounds Ionic bond forms between ions (atoms w/ a charge b/c they have extra or missing e - ) –Represented by chemical formulas (or formula units) Ex) NaCl –Typically solids at room temperature Occurs between oppositely charged ions (“opposites attract”) Include a cation & an anion Cation = + charges Anion = - charges

13. In an ionic compound, the atoms combine in ratios to balance the charges (neutral compound) Ex.) How many Mg will react w/ S? Mg 2+ + S 2-  MgS

14. Criss-Cross Method An easier way to determine the subscripts Use it if it makes sense to you. Otherwise, continue balancing the charges

15. Criss-Cross Method: How many B will react w/ S? B 3+ & S 2- B 3+ S 2- + B2S3B2S3 Notice: when you write the formula the cation (metal) goes 1st 32

16. Examples: What is the formula when Al and F combine? Al 3+ & F 1- Al 3+ F 1- + AlF 3 31

17. Examples: Lithium and Bromine LiBr Calcium and Sulfur CaS Zn (II) and Phosphorus Zn 3 P 2 Sodium and Phosphate Na 3 PO 4

18. Naming Ionic Compounds Binary compounds - composed of 2 elements 1 st write the name of the cation 2 nd write the name of the anion Replace the ending with “-ide”

19. Examples: Al 2 O 3 Aluminum Oxide Sodium Chloride Calcium Oxide Iron(II) Sulfide Copper(II) Bromide NaCl CaO FeS CuBr 2

20. Naming Ionic Compounds with Polyatomic Ions composed of 3 or more different elements 1 st write the name of the cation 2 nd write the name of the polyatomic ion

21. Examples: Al(NO 3 ) 3 Copper(I) Phosphate Aluminum Nitrate Na(OH) Sodium Hydroxide Ca(SO 4 ) Fe(CrO 4 ) Cu 3 (PO 4 ) Calcium Sulfate Iron(II) Chromate

22. Naming Race Worksheet Second Page (Front/Back) of packet Work with ONE partner OR by yourself Do all 45 Get answers checked by me First group done:

23. Naming Acids Use the template below to name acids: Anion ending ExampleAcid nameExample - ideHCl Chloride Hydro( )-ic acid Hydrochloric acid - iteH 2 SO 3 Sulfite ( ) – ous acid Sulfurous acid - ateHNO 3 Nitrate ( ) – ic acidNitric acid

24. Properties of IB Properties - Electrically neutral compounds - High boiling/melting point (BP/MP) - Form crystal solids which are brittle - Dissolve in Water - Conduct electricity in molten or dissolved state

25. Ionic Compounds Dissociate into ions when they dissolve So, –NaCl Na + + Cl - –AlCl 3 Al +3 + 3Cl - Note: The number of each ion becomes a coefficient (3Cl - ) Ions have a charge, so the charge MUST be written

26. Write the equation when the following ionic compounds dissolve in water MgO Na 3 P Fe 2 O 3 Mg(NO 3 ) 2 FeSO 4

27. Work on Ionic Bonding Practice First Page (Front/Back) of Packet

28. STOP Complete any unfinished worksheets

29. Molecular Compounds Compounds composed of molecules (usually 2 or more non-metals) –Represented by molecular formulas Ex) H 2 O –Typically exist as gasses or liquids at room temperature Diatomic molecules – H 2, N 2, O 2, F 2, Cl 2, Br 2, I 2

30. Naming Molecular Compounds Binary molecular compounds - composed of 2 non-metals – Use prefixes to distinguish between different compounds (Table 6.5, p.159) – Atom which is furthest to the left is written first

31. PrefixNumber Mono-1 Di-2 Tri-3 Tetra-4 Penta-5 Hexa-6 Hepta-7 Octa-8 Nona-9 Deca-10

32. Examples: SO 3 Trisulfur Octiodide Sulfur trioxide CO Carbon Monoxide OF 6 P 2 Br 4 S3I8S3I8 Oxygen Hexafluoride Diphosphorus tetrabromide

33. Examples Name the following acids –HBr –HNO 2 –H 2 SO 4 Write the formula for the following acids –Hydrofluoric acid –Phosphorous acid

34. The Law of Definite Proportions the masses of the elements are always in the same proportions in any sample of a chemical compound 8:116:1

35. The Law of Multiple Proportions Comparison of the ratios of one element in 2 different compounds containing that particular element

36. Example: A sample of water contains 16 g of oxygen, whereas a sample of hydrogen peroxide contains 32 g of oxygen. What is the ratio of oxygen in the two compounds?