1. Unit 1
Chapters 1, 2, and 3
Labs for this unit should include: Vernier labs 1 and 2, and possibly the carbonate mixture inquiry lab.

2. What Is Chemistry?
Chemistry is the study of matter and how it changes.
Elements:
Atoms:
Molecules and Compounds:

3. States of Matter
Solid:
Liquid:
Gas:

4. Matter

5. Pure Substnaces
Pure substance:
Mixture:
Heterogeneous:
Homogeneous:

6. Properties of Matter
Physical Properties:
Chemical Properties:

7. Intensive Properties:
Extensive Properties:

8. Atomic Theory Subatomic Particles: Electrostatic Forces:
Stress the importance of electrostatic forces.

9. Radioactivity
Radio activity: Spontaneous emission of radiation.

10. The Nuclear Atom Nucleus: Electronic Charge: Atomic Mass:
Give charge of electron and proton

11. Atomic Size:
Talk about angstorms and how they relate to meters.

12. Isotopes Isotope: Average Atomic Mass:
show example from chapter notes of average atomic mass of C. Cover mass spectroscopy in advanced lab skills. Show example of average atomic mass problem page 47

13. Naturally occurring chlorine is 75
Naturally occurring chlorine is % 35Cl, which has an atomic mass of amu, and % 37Cl, which has an atomicmass of amu. Calculate the average atomic mass of chlorine.
sample exercise 2.4 p 47

14. The Periodic Table How it’s arranged:
go over basic sections of the periodic table.

15. Law of Definite Proportions

16. The Law of Multiple Proportions

17. Ions and Ionic Compounds
Cation:
Anion:

18. Common Ions and their charges
Group 1: H+, Li+, Na+
Group 2: Be2+, Mg2+, Ca2+
Group 15: N3-, P3-, As3-
Group 16: O2-, S2-, Se2-
Group 17: F-, Cl-, Br-
Transition elements can usually have more than one charge. Example Fe2+ and Fe3+

19. Transition Metal Ions
Most transition metals can have a few different charges.
Example:
Fe2+, Fe3+
Fe2O3
FeO

20. Polyatomic Ions Ammonium: NH4+ Nitrite: NO2- Nitrate: NO3-
Hydroxide: OH-
Hypochlorite: ClO-

21. Chlorite: ClO2-
Chlorate: ClO3-
Perchlorate: ClO4-
Carbonate: CO32-
Sulfite: SO32-
Sulfate: SO42-
Peroxide: O22-
Phosphate: PO43-

22. Naming Ionic Compounds

23. Practice NH4Cl Fe(NO3)3 TiBr3 Pb(SO4)2 Chromium (VI) Phosphate
Tin (II) Nitrate
Cobalt (III) Oxide
Chromium (III) Hydroxide

24. Chromium (III) Sulfite
Barium Carbonate
Aluminum Hydroxide
Copper (I) Sulfide
Lead (II) Phosphate
Zinc (II) Iodide
Chromium (III) Sulfite
NH4Br
NaClO3
Fe2S3
AgNO3
CuF2
Ni(ClO)3
Ru3(PO4)4

25. Naming Molecular Compounds

26. Practice
Naming practice worksheets

27. The Mole

28. Molar Mass

29. Percent Mass
Show empirical formula example, molecular formula example and give out formula packet

30. Hydrates
good time to do vernier lab 2.

31. Empirical And Molecular Formula

32. Chemical Reactions Chemical Equations:
Highlight the difference between coefficients and subscripts. Give out a balancing worksheet

33. C6H12O6(s) + 6 O2(g)  6 CO2(g) + 6 H2O(l)
Stoichiometry
How many grams of water are produced in the combustion of 1.00 g of glucose?
C6H12O6(s) + 6 O2(g)  6 CO2(g) + 6 H2O(l)
Have a bunch of stoichiometry practice ready!

34. Limiting Reactants
Use bread and cheese example.

35. Consider the reaction that occurs in a fuel cell:
2 H2(g) + O2(g)  2 H2O(g)
Suppose the fuel cell is set up with 150 g of hydrogen and 1500 g of oxygen. How many grams of water can be formed?

36. Theoretical Yield and Percent Yield
show 3.14 on page 105

37. 6 C6H12(l) + 5 O2(g)  2 H2C6H8O4(l) + 2 H2O(g)
Adipic acid (H2C6H8O4) is used to produce nylon. The acid is made commercially by a controlled reaction between cyclohexane (C6H12) and O2:
6 C6H12(l) + 5 O2(g)  2 H2C6H8O4(l) + 2 H2O(g)
a.) Assume that you carry out this reaction starting with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yeild of adipic acid?
b.) If you obtain 33.5 g of adipic acid from your reaction, what is the percent yeild?

38. Example AP Questions
Complete combustion of a sample of a hydrocarbon in excess oxygen produces equimolar quantities of carbon dioxide and water. Which of the following could be the molecular formula of the compound?
C2H2
C2H6
C4H8
C6H6

39. The mass percent of carbon in pure glucose, C6H12O6, is 40. 0%
The mass percent of carbon in pure glucose, C6H12O6, is 40.0%. A chemist analyzes an impure sample of glucose and determines that the mass percent of carbon is 38.2 %. Which of the following impurities could account for the low mass percent of carbon in the sample?
Water, H2O
Ribose, C5H10O5
Fructose, C6H12O6. An isomer of glucose
Sucrose, C12H22O11

40. How many protons, neutrons, and electrons are in a 5626Fe atom?
Protons Neutrons Electrons

41. Atoms of Mg combine with atoms of F to from a compound
Atoms of Mg combine with atoms of F to from a compound. Atoms of which of the following elements combine with atoms of F in the same ratio? Li Ba Al Cl Ne

42. C3H8(g) + 5 O2(g)  3 CO3(g) + 4 H2O(l)
In the reaction represented above, what is the total number of moles of reactants consumed when 1.00 mole of CO2(g) is produced?
0.33 mol
1.33 mol
1.50 mol
2.00 mol
6.00 mol

43. LiHCO3(aq) + H2SO4(aq)  Li2SO4(aq) + H2O(l) + CO2(g)
When the equation above is balanced and the coefficients are reduced to lowest whole-number terms, what is the coefficient of H2O 1 2 3 4 5

44. When a 3. 22 g sample of an unknown hydrate of sodium sulfate, Na2SO4
When a 3.22 g sample of an unknown hydrate of sodium sulfate, Na2SO4 * x H2O(s) is heated, H2O (molar mass 18) is driven off. The mass of the anhydrous Na2SO4(s) (molar mass 142 g) that remains is 1.42 g. The value of x in the hydrate is
0.013
1.8
6.0
10.0
20.0

45. What is the empirical formula of an oxide of chromium that is 48 percent oxygen by mass?
CrO
CrO2
CrO3
Cr2O
Cr2O3