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 p s p

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

9. Valence Electrons: Label on your PTE1 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 PTE1+ 1 8 2 2+ 3+ 3 4 3- 5 6 2- 1- 7
Gain e-
Lose e-
Anions
Cations

14. Set up a table: Element # Valence E- Loses or Gains E-?
Cation or Anion?
Charge of Ion
Symbol of Ion
Name of Ion
Set up a table:

15. Set up a table: Element # Valence E- Loses or Gains E-?
Cation or Anion?
Charge of Ion
Symbol of Ion
Name of Ion
Set up a table:

16. Number of Valence ElectronsLi 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 1 mono (**only used for second 2 di 3 tri 4 tetra
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
disilicon hexabromide

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
HBr hydrobromic 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
HClO3 chloric 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 HClO3 chloric 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.

51. This period Carry out your procedure and collect data.
Begin calculations as soon as you can!
Percent of water in the hydrate by mass.
Mole ratio of anhydrous CuSO4 to H2O in your sample.
Work to show how you got your number of molecules of water of hydration.
Name of the hydrate

52. Homework Quiz on ch. 1-2 tomorrow Chapter 2 problem set: Tues.
Complete calculations (including name of hydrate): Thurs.