13 September 2011

1. 13 September 2011 • Objective: You will be able to: • review chapter 2 concepts • Homework Quiz: • Give the number of protons and electrons in the ion Mg2+ • Name the compound BaCl2 • Write the formula for iodine heptachloride

2. Agenda • Homework Quiz • Ch. 1 #105 • Chapter 2 Review • Problems in Chapter 2? Homework: Chapter 1 Problem Set: Thurs.

3. Announcement • Do I have your signed syllabus page yet? • You really want to be a TA for chemistry…

4. Chapter 2 Review: Atoms, Molecules, Ions

5. Atoms, Molecules and Ions • Review your notes from 2.1 – 2.5

6. Ionization • A review of how to determine which ion an atom makes

7. Valence Shell • Valence Shell: The most outer energy level. • 1s22s22p63s23p3 1s 2s 2p 3s 3p

8. Stability 1s 2s 2p 3s 3p 1s 2s 2p 3s 3p

9. Valence Electrons: Label on your PTE 1 8 2 3 4 5 6 7

10. Group 1 s p s p New valence shell

11. Ions • Ion: An atom that has lost or gained one or more electrons • Cation: An atom that has lost an electron • Positive Charge • Anion: An atom that has gained an electron • Negative Charge

12. Octet Rule • Octet Rule: All atoms lose and gain electrons to form a full valence shell • H, He = 2 • All other elements = 8

13. Ions formed by group - Add to your PTE 1+ 1 8 2 2+ 3+ 3 4 5 3- 6 2- 7 1- Gain e- Lose e- Anions Cations

14. Set up a table:

15. Set up a table:

16. Number of Valence Electrons Li Be B F O N Cl P K Ca Al Se Br Kr

17. Anion or Cation? • Cation is positive because it has LOST electrons. • It is a positive thing to have a cat, and it would be sad if you lost your cat. • Anion is negative because it has GAINED electrons • Mnemonic?

18. Symbols for Ions • Element SymbolCharge • Li+ • Cl- • Al3+ • Number, then + or – • No need to write a “1” • 1 is often invisible in chemistry

19. Names for Ions • Cations: Same name as the element • Li+: lithium ion • Sr2+: strontium ion

20. Naming Ions • Anions: Ending changes to “-ide” • N3-: nitride ion • O2-: oxide ion • F-: fluoride ion • S2-: sulfide ion • Cl-: chloride ion • Br-: bromide ion • I-: iodide ion

21. Polyatomic Ions NH4+ ammonium CO32- carbonate HCO3- hydrogen carbonate ClO3- chlorate CrO42- chromate Cr2O72- dichromate CN- cyanide PO43- phosphate HPO42- hydrogen phosphate H2PO4-dihydrogen phosphate

22. More Polyatomic Ions SO32- sulfite SO42- sulfate HSO4- hydrogen sulfate OH- hydroxide NO3- nitrate NO2- nitrite MnO4- permanganate O22- peroxide

23. 14 September 2011 • Objective: You will be able to: • Name ionic and covalent compounds • Homework Quiz: • Write the formulas for: • iron (III) chloride • ammonium sulfate • dihydrogen monoxide

24. Agenda • Homework Quiz • Questions about ch. 1 problem set? • Chapter 2 review Homework: Ch. 1 problem set due tomorrow

25. Formulas of Ionic Compounds • Formed by electrostatic attraction between cations and anions. • Examples: • potassium bromide • zinc iodide • aluminum oxide • magnesium nitrate • iron (II) chloride (p. 54 for charges of transition metals)

26. Practice • rubidium sulfate • barium hydride • manganese (IV) oxide • ammonium carbonate

27. Names of Ionic Compounds • Examples • KBr • CuCl • FeCl3 • Cu(NO3)2 • KH2PO4 • NH4ClO3

28. Practice • MgBr2 • Li2SO3 • PbO • FeCO3

29. Molecular Compounds • Prefix system • 1 mono (**only used for second element in compound) • 2 di • 3 tri • 4 tetra • 5 penta • 6 hexa • 7 hepta • 8 octa • 9nona • 10 deca

30. Naming Molecular Compounds • Examples • CO • CO2 • N2O4

31. Practice Naming Molecular Compounds • SiCl4 • P4O10

32. Writing Formulas for Molecular Compounds • Examples • nitrogen dioxide • dihydrogen monoxide

33. Practice Writing Formulas for Molecular Compounds • nitrogen trihydride (a.k.a. ammonia) • carbon tetrachloride (a.k.a. freon) • carbon disulfide • disiliconhexabromide

34. Naming Acids • Acid: any substance that yields hydrogen ions (H+) when dissolved in water • If the anion ends in “-ide”, the acid is a “hydro –ic” acid HF hydrofluoric acid HCl hydrochloric acid HBrhydrobromic acid HI hydriodic acid HCN hydrocyanic acid H2S hydrosulfuric acid

35. Oxoacids • Contain hydrogen, oxygen and another element. • Used as reference acids to name other acids H2CO3 carbonic acid HClO3chloric acid HNO3 nitric acid H3PO4 phosphoric acid H2SO4 sulfuric acid

36. More oxoacids • Often, two or more oxoacids have the name central atom but a different number of O atoms • Adding one O atom to an “-ic” acid = “per… -ic” acid • Removing one O atom from an “-ic” acid = “-ous” acid • Removing two O atoms from an “-ic” acid = “hypo…-ous” acid

37. Oxyacid examples • HClO3chloric acid • Add an oxygen: HClO4 • perchloric acid • Remove an oxygen: HClO2 • chlorous acid • Remove two oxygens: HClO • hypochlorous acid

38. Oxyacid Problems • Name the following oxyacids • HNO2 • H2SO3 • H2CO4 • H2SO2

39. Naming Bases • A base yields hydroxide (OH-) ions when dissolved in water • NaOH sodium hydroxide • Ba(OH)2 barium hydroxide (Some bases don’t contain OH-, but more on that later.)

40. Hydrates • Hydrates are compounds with a specific number of water molecules attached to them • Example: CuSO4·5H2O • copper (II) sulfate pentahydrate • BaCl2·2H2O • barium chloride dihydrate

41. 15 Sept. 2011 • Objective: You will be able to: • Practice identifying subatomic particles, isotopes, determining ionization, naming and writing formulas for compounds. • design a procedure to determine the formula of a hydrate.

42. Agenda • Questions about chapter 2 summer assignment? • Chapter 2 problem set • Design an procedure! Homework: Chapter 2 problem set: Tues. Ch. 1-2 quiz Tues.

43. Your challenge! • Copper (II) sulfate hydrate • Hydrate: a compound with water “tagged on to” the crystal structure. • Determine the number of molecules of water of hydration per formula unit of copper (II) sulfate.

44. Your procedure… • A complete list of steps which include • specific quantities • names of equipment you’ll need to use • some way to determine when your procedure is “finished” • Directions and equations for any calculations you’ll need to make Due: Monday!

45. Homework • Quiz on ch. 1-2 Tuesday • Lab procedure: Monday

46. 19 September 2011 • Take out your lab notebook and turn to your procedure • Objective: You will be able to: • carry our your procedure and collect data to determine the number of molecules of water of hydration of copper (II) sulfate hydrate.

47. Agenda • Procedure discussion • Carry out your procedure • Make calculations Homework: Quiz on ch. 1-2 tomorrow Chapter 2 problem set: Tues. Complete calculations (including name of hydrate): Thurs.

48. Safety • Wear goggles until all your equipment has been cleaned and returned. • A hot crucible looks just like a cold crucible! Always use crucible tongs. • Work efficiently but carefully.

49. Technical notes • Heat the crucible uncovered or with the cover tilted to allow water vapor to escape. • Cool the crucible with the cover on. • Cool the crucible in the desiccator for very best results. • Never mass a hot or warm crucible. • Oil from your fingers will stick to the crucible and effect your data.

50. Work Ethic • Work quickly. If you have “down time,” think: “What can I do now to save time later?” • Set up data tables and calculations while you wait.