Download 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, NO2Nitrate, NO3Acetate, C2H3O2Carbonate, CO32Sulfite, SO32Sulfate, SO42Phosphite, PO33Phosphate, PO43Hypochlorite, ClOChlorite, ClO2Chlorate, ClO3Perchlorate, ClO4Hydroxide, OHChromate, CrO42Dichromate, Cr2O72Cyanide, CNFluoride, FChloride, ClBromide, BrIodide, IThiosulfate, S2O32Permanganate, 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) S27) H2SO3
8) NH4+
9) Hydrofluoric acid
10) Sodium sulfate
11) KNO3
12) Ce2(SO4)3
13) Dinitrogen tetroxide
14) ClO215) Zinc nitrate
16) Na3PO4
17) (NH4)2SO4
18) SO2
19) Acetic Acid
20) HBr
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(The next 20 questions are from the retake of this quiz.)
21) Carbon tetrachloride
22) CaSO3
23) Cobalt (III) chloride
24) AlPO4
25) CO3226) Na2S
27) H2CO3
28) NH3
29) Sulfurous acid
30) Sodium Nitrate
31) FeCO3
32) Fe2(SO4)3
33) Dinitrogen pentoxide
34) ClO335) Zinc acetate
36) K3PO3
37) NH4NO3
38) SO3
39) Acetate
40) H3PO4
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Significant Figures (“Sigfigs”)
Counting Significant figures
number has a decimal point
number has no decimal point
count significant figures
from the left
count significant figures
from the right
◊ all nonzero digits are significant.
&
◊ only count zeros after a nonzero digit.
Measurement
20.1 g
10005 g
0.0043 kg
0.0500 kg
Sig Figs?
Measure.
345.6 cm
0.99 m
300.2 cm
95.0 m
Sig Figs?
Measure.
0.9 ml
8.7 ml
0.500 cm3
21.0 cm3
Sig Figs?
Measure.
0.12 ms
509 s
710 s
8.820 min
Sig Figs?
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.
1. 34 mol Li = _______ atoms Li
2. 2.5 mol S = _______ atoms S
3. 18.066 x 1023 atoms Fe = _______ mol Fe
4. 67 x 1023 molecules NaCl = _______ mol NaCl
5. 0.25 mol O2 = _______ molecules O2
6. 39 x 1021 molecules H2O = _______ mol H2O
7. 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.
1. 450 g Rb = _______ mol Rb
2. 10 g Cl = _______ mol Cl
3. 1.5 mol He = _______ g He
4. 11 mol Ag = _______ g Ag
5. 45 g C = _______ mol C
6. 0.34 mol C = _______ g C
Mole Level 3
Now convert from atoms to moles to grams and in reverse, too.
1. 12.044 x 1023 atoms Hg = _______ g Hg
2. 12.044 x 1023 atoms Ba = _______ g Ba
3. 238 g Cu = _______ atoms Cu
4. 10.5 g N = _______ atoms N
5. 534 g Xe = _______ atoms Xe
6. 1.5 x 1024 atoms F = _______ g F
Mole Level 4
Determine the molecular mass of any molecule by adding atomic masses.
1. 1 mol H2O = _______ g H2O
2. 1 mol CaCl2 = _______ g CaCl2
3. 1 mol Li3N = _______ g Li3N
4. 1 mol Ni(NO3)2 = _______ g Ni(NO3)2
5. 1 mol Ca(NO3)2 = _______ g Ca(NO3)2
6. 1 mol Ba3(PO4)2 = _______ g Ba3(PO4)2
Mole Level 5
Practice manipulating molecular masses
1. 2 mol CaCl2 = _______ g CaCl2
2. 870 g Li3N = _______ mol Li3N
3. 14 mol O2 = _______ g O2
4. 28.5 x 1023 molecules H2O = _______ g H2O
5. 100.32 g CH4 = _______ molecules CH4
Mole Bonus Level 6 – You Made It!!!
Now, we mix them up.
1. 1599.4 g Sm = _______ atoms Sm
2. 41.99 x 1023 molecules H2SO4 = _______ g H2SO4
3. 33.55 x 1023 atoms Sr = _______ g Sr
4. 25.99 x 1023 molecules NaCl = _______ g NaCl
5. 19.8 mol Si = _______ atoms Si
6. 212.5 g MgCO3 = _______ mol MgCO3
7. 455.7 g Na2O = _______ mol Na2O
8. 7.34 x 1025 molecules N2O5 = _______ mol N2O5
AP Chemistry 2009-10 Unit One Test
Use the following choices for questions 1-3.
a.
b.
c.
d.
e.
Dalton
Thomson
Rutherford
Democritus
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
(C) lead(III) 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
(C) 86.05 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
(C) O-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.
(C) Atoms of a given element are identical; atoms of different elements are
different
(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
1
2
3
length of rod
12.34 cm
12.39 cm
12.33 cm
(A) These people take very accurate measurements
(B) These people take very precise measurements.
(C) These people take very accurate, but not 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
(C) hydronitric acid
(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
(C) 0.438 g/mL
(D) 2.28 g/mL
(E) 2.3 g/mL
12. According to the reaction represented below, how many moles of O 2 are
required to produce 2 moles of H2O?
__C6H12 + ___O2  __CO2 + __H2O
(A) 2 moles
(B) 5/2 moles
(C) 3 moles
(D) 7/2 moles
(E) 4 moles
13. The correct chemical name of Ni2CO3 is
(A) nickel (II) carbonate
(B) nickel(II) chlorate
(C) nickel carbonate
(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
(C) sulfate
(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
(C) calcium 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
(C) the number of liters
(D) the number of moles
(E) the number of grams