Download the ap chemistry summer assignment

AP Chemistry Summer Assignment 2015
Mr. Edelman
[email protected]
Welcome to AP Chemistry! You already have a background in chemistry from your
general chemistry class, but AP Chemistry is very different. Rather than memorizing how
to do particular types of problems, you must really understand the chemistry and be able
to apply it to different kinds of problems. AP Chemistry is a difficult course. To succeed
you must keep up with the assignments and be willing to spend time working through the
material. The College Board recommends that students spend one hour outside of class
studying and practicing for every hour in class. I think this is an underestimation of
what is necessary to be successful.
Like most AP classes, AP Chemistry comes with a summer assignment. It is due the first
Friday of school and will count as your first quiz grade. We will have a test over the
concepts in this summer assignment on that first Friday. The summer assignment is a
review of your first year chemistry course. If you do not know how to complete problems
in this assignment, use your notes from your first year class or find an online tutorial or
website to help you. There are buckets of them.
I hope you will enjoy your AP Chemistry class. Be ready for an academic challenge. I
know you will learn a lot in AP Chemistry and it will be an excellent way for you to prepare
for college, as it will enhance work-habits, organizational skills and your ability to learn
independently and think creatively.
Have a great summer. See you in August!
Mr. Edelman
You may write your answers on these pages or use notebook paper.
Unit One – Math and Measurement
1. Write the following measurements in scientific notation.
A. 369 g
_______________________
B. 540,000 mL (3 sig figs) _______________________
C. 0.4560 mi
_______________________
D. 0.000000060
_______________________
2. Express the following as whole numbers or decimals.
A. 2.85 x 10-3
______________________
B. 1.5 x 108
C. 4.00 x 10-2
______________________
______________________
3. How many significant figures are there in each of the following values?
A. 0.01359456
____________
B. 12.0000
____________
C. 133.45
____________
D. 120.3
____________
E. 2200
____________
F. 0.0040
____________
G. 45.006
____________
4. Perform the indicated calculations on the following measured values. Give the
answer with the correct number of significant figures and units.
A. 16.81 m + 3.226 m =___________________
B. 326.8 N x 4.4 m2 = ______________________
C. C. 7.442 s – 7.52 s = ______________________
D. 91 g ÷ 1.86 cm3 = _______________________
5. Using conversion factors, convert 4.1 liters to:
A. kiloliters ____________________
B. milliliters ____________________
C. microliters
____________________
D. cubic centimeters ____________________
6. A velocity is 9.21 x 104 cm per minute. Use unit analysis (dimensional analysis) to
calculate the velocity in meters per second.
7. A team of students determined the density of a sample of wood to be 0.62 grams per
centimeter3. A handbook of tree physiology reported the density to be 0.631 for the
same type of wood. What is the percent error of the student’s value?
8. A leaky faucet drips at a rate of 1 drop/s. If one drop of water is 0.1 mL, how many
gallons of water will be wasted in one day?
9. An aluminum bar is 5.0 cm x 4.0 cm x 10.4 mm and has a mass of 54.000 g. Find the
density of the bar in lb/ft3.
10. What is the diameter, in Angstroms, of an atom of element X, if 6.89 x 107 atoms laid
side by side is 1.8000 inches in length?
11. A. Compare and contrast the Kelvin scale and the Celsius scale.
B. Convert 450. Kelvin to Celsius
C. Convert 200. Celsius to Kelvin
D. Convert -230 Celsius to Kelvin
In addition to the above items be sure you know
•
•
•
The difference between accuracy and precision
How to determine the uncertainty of a measurement
Metric prefixes (mega, kilo, hecto, deka, deci, centi, milli, micro, nano, pico)
Unit Two – Basic Atomic Structure, Naming Compounds and Writing Formulas
12. How many protons, neutrons and electrons are in each of the following ions?
A. Fe3+ (mass # 56) ____p____n____e
B. Ca2+ (mass # 40) ____p____n____e
C. F- (mass # 19) ____p____n____e
D. P3- (mass# 31) ____p____n____e
E. I- (mass # 127) ____p____n____e
13. Name the family or group of the Periodic Table to which each of the following
elements belong:
A. Ar ________________________
B. Sr _________________________
C. Fe _________________________
D. Cl _________________________
E. Nd ________________________
F. Rb _________________________
14. Name each of the following compounds:
A. PbI2
__________________________________________
B. B. NH4Cl
__________________________________________
C. Fe2O3 __________________________________________
D. LiH __________________________________________
E. CsCl __________________________________________ F.
NaH __________________________________________
G. Cr(OH)3 __________________________________________
H. NaC2H3O2 __________________________________________
I. K2Cr2O7 __________________________________________
J. Na2SO4 ___________________________________________
K. KH2PO4 ___________________________________________
15. Name each of the following compounds:
A. NI3 __________________________________________
B. B. PCl5 __________________________________________
C. C. CO __________________________________________
D. D. P4O10 __________________________________________
E. E. N2O4 __________________________________________
F. NH3 __________________________________________
16. Write formulas for each of the following compounds:
A. iron (III) oxide ____________________________________
B. B. hydrogen iodide ____________________________________
C. C. tin (II) fluoride) ____________________________________
D. calcium phosphate___________________________________
E. lead (II) nitrate ____________________________________
F. sodium cyanide ____________________________________
G. sodium hydrogen sulfate ______________________________
H. sodium bromate ____________________________________
17. Write formulas for each of the following compounds:
A. rubidium nitrate ________________________________________
B.
sodium iodate ________________________________________
C.
dinitrogen tetroxide ______________________________________
D.
tin (IV) oxide ________________________________________
E.
potassium carbonate ______________________________________
F.
iron (III) chloride ________________________________________
G.
sulfurous acid ___________________________________________
H.
magnesium hydroxide ____________________________________
I.
carbon tetrachloride ______________________________________
J.
potassium hydrogen phosphate ______________________________
K.
potassium permanganate ___________________________________
L.
potassium chlorate ________________________________________
M.
hypoiodous acid __________________________________________
N.
ammonium acetate ________________________________________
O.
hydroiodic acid __________________________________________
18. Give the names of the following acids:
A. H2SO3 _____________________________________________
B. HI ________________________________________________
C. HBr _______________________________________________
D. HNO2______________________________________________
E. H3PO4 _____________________________________________
F. HCl _______________________________________________
19. Give formulas for the following acids:
A. hydrocyanic acid ____________________________________
B. hydrofluoric acid ____________________________________
C. acetic acid _________________________________________
D. sulfuric acid ________________________________________
E. nitric acid __________________________________________
F. hydrosulfuric acid ___________________________________
20. Give the names of the seven diatomic elements.
21. Define the word isotope.
22. What does the law of definite composition say?
23. What does the law of multiple proportions say?
In addition to the above items, be sure you read about and understand the
following:
•
•
•
•
Dalton’s Atomic Theory
Thomson’s cathode ray tube experiment
Rutherford’s gold foil experiment
The difference between a molecule and an ion
Unit Three – The Mole, Percent Composition, Empirical and Molecular Formulas
24. An element, E, has only two naturally occurring isotopes. E-10 has a mass of 10.01
amu and a natural abundance of 19.78%. E-11 has a mass of 11.01 amu and a
natural abundance of 80.22%. What is the average atomic mass of E?
25. Chlorine has two stable isotopes. The mass of one isotope is 34.97 amu. Its relative
abundance is 75.53%. What is the mass of the other stable isotope?
26. How many atoms are in 2.4 moles of neon gas? How many grams?
27. How many grams of zinc are in 1.16 x 1022 atoms of zinc?
28. How many mg of Br2 are 4.6 x 1020 molecules of bromine?
29. How many grams are there in 0.36 moles of cobalt (III) acetate , Co(C2H3O2)3? How
many grams of cobalt are in the sample? How many atoms of cobalt?
30. Calculate the mass percent of chlorine in each of the following compounds:
A.
ClF
B.
CuCl2
31. Chlorophyll a is essential for photosynthesis. It contains 2.72% magnesium by mass.
What is the molar mass of chlorophyll a assuming there is one atom of magnesium in
every molecule of chlorophyll a?
32. Which of the following formulas can be empirical? Circle them.
A. CH4
F. NH4Cl
B. CH2
G. Sb2S3
C. KMnO4
H. N2O
D. N2O5
I. CH2O
E. B2H8
33. A compound is found to contain 49.67 % carbon, 48.92 % chlorine, and 1.39 %
hydrogen. The molar mass of the compound is 289.9 g/mole. Determine the
empirical and molecular formulas of the compound.
Unit Four – Reaction Stoichiometry
34. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon
dioxide. A. Write a balanced chemical equation for this reaction.
B. How many grams of calcium oxide will be produced after 12.25 grams of
calcium carbonate are completely decomposed?
C. What is the volume of carbon dioxide gas produced when the 12.25 grams of
calcium carbonate completely decompose at STP?
35. When ammonia gas, oxygen gas and methane (CH4) gas are combined, the products
are hydrogen cyanide gas and water.
A. Write a balanced chemical equation for the reaction.
B. Calculate the mass of each product produced when 225 grams of oxygen gas
is reacted with an excess of the other two reactants.
C. If the actual yield of the experiment in (B) is 105 grams of HCN, calculate the
percent yield.
36. DDT, an insecticide harmful to fish, birds and humans, is produced by the following
reaction:
2C6H5Cl
+
chlorobenzene
C2HOCl3 → C14H9Cl5 + H2O
chloral
DDT
In a government lab, 1142 grams of chlorobenzene is reacted with 485 grams of
chloral.
A. What mass of DDT is formed?
B. Which reactant is limiting? Which is excess?
C. What mass of the excess reactant is left over?
D. If the actual yield of DDT is 200.0 grams, what is the percent yield?
Unit Five - Solutions
37. Differentiate between what happens when the following are dissolved in water. A.
Polar solute versus nonpolar solute
B. KF versus C6H12O6
C. RbCl versus AgCl
38. Write a reaction to show how solid calcium chloride breaks apart when dissolved in
water.
39. What is molarity?
40. Calculate the molarity of the solution made by dissolving 5.263 grams of NaHCO3 in
enough water to make 250.0 mL of solution.
41. A solution of ethanol (C2H5OH) in water is prepared be dissolving 75.0 mL of ethanol
(density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the
molarity of the solution?
42. Which of the following solutions of strong electrolytes contains the largest number of
moles of chloride ions?
A. 100.0 mL of 0.30 M AlCl3
B. 50.0 mL of 0.60 M MgCl2
C. 200.0 mL of 0.40 M NaCl
43. How would you prepare 2.00 L of 0.250 M NaOH A. from a 1.00 M stock solution?
B. from solid NaOH?
In addition to the above, know the following:
• the difference between an electrolyte and a nonelectrolyte
• the difference between a strong electrolyte and a weak electrolyte
• three strong acids and three strong bases
• one weak acid and one weak base
You need to know the polyatomic ions available on my CPHS website. You need to
know the name, formula and charge of each. Make some flash cards. You do need to
know these for the first test.