Dear Future AP Chemistry Student

Dear Future AP Chemistry Student,

I am excited to see that you have signed up for AP Chemistry next year. It is a challenging course that will improve your analytical and problem solving skills. Most students who take the class leave with an enthusiasm for science, and many go on to major in chemistry or chemical engineering in college.

To improve your readiness for the course, you are expected to complete a summer assignment on the first three chapters of our textbook. This involves memorizing a list of common ions, writing names and formulas confidently, using significant figures and solving stoichiometry problems systematically. Students should complete the summer assignment in small segments throughout the summer, rather than all at once soon before school begins. On the first day of school, the packets will be collected, reviewed, and graded by me.

I have included a packet of the material containing the practice problems you are expected to solve. It is expected that you come to class next fall with the majority of this material already mastered, needing only light review and clarification. Please see me if you wish to check out a textbook.

Contents of the Review Packet:

List of common ions to memorize
A sample quiz on names and formulas
Significant Figures Review
“Mole Level” Calculations
2009-10 Unit One Test

Please do not hesitate to stop by my room, B217, if you have any questions or need any additional materials to help in your preparation.

Sincerely,

Mr. McDonald

List of Common Ions to Know

The following ions must be memorized.

Ammonium, NH4+

Hydronium, H3O+

Mercury(I), Hg22+

Mercury(II), Hg2+

Zinc, Zn2+

Silver, Ag+

Nitrite, NO2-

Nitrate, NO3-

Acetate, C2H3O2-

Carbonate, CO32-

Sulfite, SO32-

Sulfate, SO42-

Phosphite, PO33-

Phosphate, PO43-

Hypochlorite, ClO-

Chlorite, ClO2-

Chlorate, ClO3-

Perchlorate, ClO4-

Hydroxide, OH-

Chromate, CrO42-

Dichromate, Cr2O72-

Cyanide, CN-

Fluoride, F-

Chloride, Cl-

Bromide, Br-

Iodide, I-

Thiosulfate, S2O32-

Permanganate, MnO4-

AP Chemistry – Formulas and Nomenclature Quiz

Write either the name or formula (whichever is not given) for each chemical. All twenty of these chemicals appeared in the 2002 AP exam.

1)Carbon dioxide______

2)PbSO4______

3)Iron(III) chloride______

4)CaSO4______

5)CO______

6)S2-______

7)H2SO3______

8)NH4+______

9)Hydrofluoric acid______

10) Sodium sulfate______

11) KNO3______

12) Ce2(SO4)3______

13) Dinitrogen tetroxide______

14) ClO2-______

15) Zinc nitrate______

16) Na3PO4______

17) (NH4)2SO4______

18) SO2______

19) Acetic Acid______

20) HBr______

(The next 20 questions are from the retake of this quiz.)

21)Carbon tetrachloride______

22)CaSO3______

23)Cobalt (III) chloride______

24)AlPO4______

25)CO32-______

26)Na2S______

27)H2CO3______

28)NH3______

29)Sulfurous acid______

30) Sodium Nitrate______

31) FeCO3______

32) Fe2(SO4)3______

33) Dinitrogen pentoxide______

34) ClO3-______

35) Zinc acetate______

36) K3PO3______

37) NH4NO3______

38) SO3______

39) Acetate______

40) H3PO4______

Significant Figures (“Sigfigs”)

Counting Significant figures

number has a decimal pointnumber has no decimal point

count significant figures count significant figures

from the leftfrom the right

◊ all nonzero digits are significant.

◊ only count zeros after a nonzero digit.

Measurement / Sig Figs? / Measure. / Sig Figs? / Measure. / Sig Figs? / Measure. / Sig Figs?
20.1 g / 345.6 cm / 0.9 ml / 0.12 ms
10005 g / 0.99 m / 8.7 ml / 509 s
0.0043 kg / 300.2 cm / 0.500 cm3 / 710 s
0.0500 kg / 95.0 m / 21.0 cm3 / 8.820 min

Doing math with sig figs:

When adding and subtraction, your answer should match the number in the calculation with the fewest number of decimal points.
When multiplying and dividing, your answer should match the number in the calculation with the least number of significant figures.

Try these examples:

1) 892.993 g + 32.8 g =

2) 286.3 m – 234.1 m =

3) 300.22 ml + 23.774620 ml =

4) 79.93 m – 27.0000005 m =

5) 88.3 s + 2.9 s =

6) 342.5 m x 21.24 m =

7) 178.22 g/185 L =

8) 1030 cm x 0.23100 cm x 21 cm =

9) 34.00 cm2 / 2.51345 cm =

10) 89.02 m3 / 10.4 m2 =

Mole Level Calculations

Note: Please show your use of dimensional analysis for each problem.

Mole Level 1

Use the relationship 1 mole = 6.022 x 1023 particles to solve these problems.

34 mol Li = ______atoms Li

2.5 mol S = ______atoms S

18.066 x 1023 atoms Fe = ______mol Fe

67 x 1023 molecules NaCl = ______mol NaCl

0.25 mol O2 = ______molecules O2

39 x 1021 molecules H2O = ______mol H2O

2.4 x -3 mol SO2 = ______molecules SO2

Mole Level 2

Atomic masses indicate the mass of 1 mole of an element in grams.

Example: the mass of 1 mole of carbon atoms is 12.00 g.

450 g Rb = ______mol Rb

10 g Cl = ______mol Cl

1.5 mol He = ______g He

11 mol Ag = ______g Ag

45 g C = ______mol C

0.34 mol C = ______g C

Mole Level 3

Now convert from atoms to moles to grams and in reverse, too.

12.044 x 1023 atoms Hg = ______g Hg

12.044 x 1023 atoms Ba = ______g Ba

238 g Cu = ______atoms Cu

10.5 g N = ______atoms N

534 g Xe = ______atoms Xe

1.5 x 1024atoms F = ______g F

Mole Level 4

Determine the molecular mass of any molecule by adding atomic masses.

1 mol H2O = ______g H2O

1 mol CaCl2 = ______g CaCl2

1 mol Li3N = ______g Li3N

1 mol Ni(NO3)2 = ______g Ni(NO3)2

1 mol Ca(NO3)2 = ______g Ca(NO3)2

1 mol Ba3(PO4)2 = ______g Ba3(PO4)2

Mole Level 5

Practice manipulating molecular masses

2 mol CaCl2 = ______g CaCl2

870 g Li3N = ______mol Li3N

14 mol O2 = ______g O2

28.5 x 1023 molecules H2O = ______g H2O

100.32 g CH4 = ______molecules CH4

Mole Bonus Level 6 – You Made It!!!

Now, we mix them up.

1599.4 g Sm = ______atoms Sm

41.99 x 1023 molecules H2SO4 = ______g H2SO4

33.55 x 1023 atoms Sr = ______g Sr

25.99 x 1023 molecules NaCl = ______g NaCl

19.8 mol Si = ______atoms Si

212.5 g MgCO3 = ______mol MgCO3

455.7 g Na2O = ______mol Na2O

7.34 x 1025 molecules N2O5 = ______mol N2O5

AP Chemistry 2009-10 Unit One Test

Use the following choices for questions 1-3.

a.Dalton

b.Thomson

c.Rutherford

d.Democritus

e.Chadwick

1. Proposed the existence of a nucleus.

2. Made important discoveries about the negative particles of cathode rays; created the “Plum Pudding” model of the atom.

3. First to come up with the idea of the atom, though he had no proof

4. The correct chemical name of Pb3(PO4)2 is

(A) lead(III) phosphide

(B) lead(II) phosphite

(D) lead(II) phosphate

(E) lead(III) phosphate

5. In which of the following compounds is the mass ratio of sodium to oxygen closest to 0.958 to 1.00 ?

(A) NaClO
(B) NaClO2
(C) NaClO3
(D) Na2CO3
(E) Na2O

6. The molar mass of nitrogen pentoxide is:

(A) 30.01 g/mol

(B) 14.01 g/mol

(D) 150.05 g/mol

(E) 94.01 g/mol

7. In the compound iron(II) oxide, what is the cation?

(A) Fe+3

(B) Fe+2

(D) O-3

(E) Fe-2

8. Which of the choices is NOT part of Dalton’s atomic theory?

(A) Each element is made up of atoms.

(B) Atoms are made of protons, neutrons, and electrons.

(D) Chemical compounds form when atoms of different elements combine with each other.

(E) A given compound always has the same relative numbers and types of atoms.

9. What can be said is true about the people taking these measurements?

Trial length of rod
112.34 cm
212.39 cm
312.33 cm

(A) These people take very accurate measurements

(B) These people take very precise measurements.

(D) These people take very precise, but not very accurate measurements.

(E) These people take very accurate AND very precise measurements.

10. The correct chemical name of HNO2 is

(A) hydrogen nitrate

(B) hydrogen nitrite

(D) nitrous acid

(E) nitric acid

11. In lab, Allison measured the mass of her solid to be 5.50 g. She then measured 25.67 mL of water in a graduated cylinder. After putting her solid in the cylinder, the new volume was 38.22 mL. What is the density of her solid?

(A) 12.55 g/mL

(B) 0.44 g/mL

(D) 2.28 g/mL

(E) 2.3 g/mL

12. According to the reaction represented below, how many moles of O2 are required to produce 2 moles of H2O?

__C6H12 + ___O2 __CO2 + __H2O

(A) 2 moles

(B) 5/2 moles

(D) 7/2 moles

(E) 4 moles

13. The correct chemical name of Ni2CO3 is

(A) nickel (II) carbonate

(B) nickel(II) chlorate

(D) nickel (I) carbonate

(E) dinickel monocarbon trioxide

14. When a 1.00-gram sample of limestone was dissolved in acid, 0.38 grams of CO2 was generated. If the rock contained no carbonate other than CaCO3, what was the percent of CaCO3 by mass in the limestone?

(A) 17%
(B) 51%
(C) 64%
(D) 86%
(E) 100%

15. Which of the following best explains what isotopes are?

(A) Two atoms of different elements with the same mass number
(B) Two atoms of the same element with the same mass number
(C) Two atoms of different elements with different mass numbers
(D) Two atoms of the same element with different mass numbers
(E) Two atoms of the same element with different atomic numbers

16. If elemental carbon combusts completely to form carbon dioxide, then how many grams of carbon dioxide are formed if 35 grams of oxygen gas react?

(A) 0.55 g

(B) 1.1 g
(C) 2.2 g
(D) 48 g
(E) 96 g

17. In the compound CaCl2∙2H2O, what percentage of the compound is water?

(A) 13%
(B) 25%
(C) 40%
(D) 67%
(E) 75%

18. Which of the following contains the fewest number of oxygen atoms per molecule?

(A) acetate

(B) carbonate

(D) sulfite

(E) chlorate

19. Which of the following compounds has the greatest number of particles per formula unit?

(A) sodium nitrite

(B) aluminum chloride

(D) potassium nitrate

(E) calcium carbonate

20. You have a sample of silver chloride. Which of the following would have the greatest value?

(A) the number of atoms

(B) the number of formula units

(D) the number of moles

(E) the number of grams