Summer Assignment

AP CHEMISTRY

SUMMER ASSIGNMENT

2012 - 2013

AP Chemistry is a college level science class that covers a great deal of material and requires up to 22 different labs. This means that you will be responsible for reading each chapter and passing a reading content quiz before lecture so that class time can be used for clarification of points rather than the detailed teaching of each point. Expect to have an hour of homework per class meeting and a half-hour of homework before a lab and one hour afterwards. Study groups are strongly encouraged.

Text: Chemistry, 5th Edition by Zumdahl and Zumdahl

Study Guide: Samples are available in room 602 for you to look through. This will enable you to pick the one best suited for your learning style before making a purchase.

Expectations:

Homework will be assigned, but neither collected nor graded. Solutions will be posted and you will be expected to check the solutions yourself. If you need help with homework, then you must schedule time outside of class to ask questions. Homework will not be reviewed during class.

Bell ringers will be used to gauge your understanding of the material, but will not be graded.

Your grade will be determined by quiz scores, labs, and tests.

Lab:

You need to purchase two lined composition books. These must be permanently bound, not spiral bound.

Labs will be distributed in advance so you have time to prepare your lab notebook before starting the lab. Lab notebooks will be checked before you are permitted to begin the lab.

Assignment:

The first four chapters of the book cover topics learned in your first year of chemistry. Because of this, they will serve as your review. These assignments will be neither graded nor collected; they are provided for your practice. Solutions will be posted on Mr. Chuba’s school web site so you can check your work.

Shortly after the new school year begins we will announce the dates for a series of graded quizzes on the summer assignment. These quizzes will lead up to a full exam on the summer assignment.

Please feel free to contact us at:

703-648-2579

CHAPTER 1

1. Read the entire chapter.

2. Answer the following questions.

3. Solve the following problems – get in the habit of showing all supporting work; you will not receive credit for only the answer on quizzes, tests, and the AP exam.

1. The height of a horse is usually measured in hands. One hand is exactly .33 feet. (a) How tall (in feet) is a horse of 19.2 hands? (b) How tall (in meters) is a horse of 17.8 hands [3.3 feet = 1 meter]?

2. A lap in most tracks that use the English system is .25 mi (English lap). In countries that use the metric system, a metric lap is .50 km. A champion marathon runner covers a mile in about 5.0 min. How many minutes will the runner take to run an English lap at that speed? How many minutes for a metric lap?

3. The cup is a measure of volume widely used in cookbooks. One cup is equivalent to 225 mL. What is the density of clover honey (in g/mL) if ¾ of a cup has a mass of 252 g?

4. Air is 21.0% oxygen by volume. Oxygen has a density of 1.31 g/L. What is the volume,

in L, of 55.0 kg of oxygen?

5. A children’s pain relief medicine contains 80.0 mg of acetaminophen per 0.500 teaspoon. The dosage recommended for a child who weighs between 24.0 and 35.0 lbs is 1.50 teaspoons. What is the range of acetaminophen dosages, expressed in mg acetaminophen per kg body weight, for children who weigh between 24.0 and 35.0 lbs?

6. The density of an irregularly shaped object was determined as follows. The mass of the object was found to be 28.90g. A graduated cylinder was partially filled with water; the reading of the level of water was 6.40 cm3. The object was dropped in the cylinder and the level of the water rose to 9.80 cm3. What is the density of the object?

7. A cylindrical bar of gold that is 1.50 inches high and 0.250 inches in diameter has a mass of 23.1984g, as determined on an analytical balance. An empty graduated cylinder is massed on a triple beam balance and has a mass of 73.47g. After pouring a small amount of liquid into the graduated cylinder, the mass is 79.16g. When the gold cylinder is placed in the graduated cylinder the liquid covers the top of the gold cylinder and the volume indicated on the graduated cylinder is 8.50 mL. Assume that the temperature of the gold bar and the liquid are 86.00F. If the density of the liquid decreases by 1.0% for each 10.00C rise in temperature (over the range 00C to 500C), determine

(a) the density of the gold at 86.00C

(b) the density of the liquid at 40.00F

CHAPTER 2

1. Read the entire chapter.

2. Answer the following questions.

3. Solve the following problems – get in the habit of showing all supporting work; you will not receive credit for only the answer on quizzes, tests, and the AP exam.

1. What is the distinction between atomic number and mass number? What is the distinction between mass number and atomic mass?

Symbol / # of protons / # of neutrons / # of electrons / Net charge
33 / 30
128Te2-
52
16 / 16 / 0
204Tl+
81
78 / 117 / 4+

3. Write the formulas for the following molecules:

(a) disulfur trioxide(b) carbon tetraiodide

(e) silicon dioxide(f) tetraphosphorus decasulfide

(g) sulfur hexafluoride(h) arsenic pentoxide

4. Write the names of the following molecules:

(a) ICl3(b) N2O5

(e) SO3(f) CO

(g) SiC(h) XeF6

(i) P4O10(j) C2H2

5. Write the names of the following ionic compounds:

(a) K2Cr2O7(b) Cu3(PO4)2

(e) Co(NO3)2(f) ScCl3

(g) Sr(OH)2(h) KMnO4

(i) Rb2S(j) Na2CO3

(k) HCl (aq)(l) HClO3

(m) Fe2(SO3)2(n) Ba(NO2)2

6. Write the formulas for the following ionic compounds:

(a) ammonium sulfide(b) sodium nitrite

(e) iron (III) perbromate(f) silver chloride

(g) magnesium dihydrogen sulfate(h) calcium oxalate

(i) ammonium thiocyanate(j) lead (IV) phosphate

(k) cobalt (II) dichromate(l) manganese (VII) carbonate

CHAPTER 3

1. Read the entire chapter.

2. Answer the following questions.

3. Solve the following problems – get in the habit of showing all supporting work; you will not receive credit for only the answer on quizzes, tests, and the AP exam.

1. Chlorine exists mainly as two isotopes, 37Cl and 35Cl. Which is more abundant? How do you know?

2. Assume the element Uus is synthesized and that it has the following stable isotopes:

284Uus (283.4 amu)34.60%

285Uus (284.7 amu)21.20%

288Uus (287.8 amu)44.20%

Determine the value of the average atomic mass for Uus that should be listed on the periodic table.

3. An element is a mixture of two isotopes. One isotope of the element has an atomic mass of 34.96885 amu and has a relative abundance of 75.53%. The other isotope has an atomic mass of 36.96590 amu. Calculate the average atomic mass of the element.

4. A diamond contains 5.00 x 1021 atoms of carbon. How many moles of carbon and how many grams of carbon are in this diamond?

5. Calculate the molar mass of each of the following substances:

a. P4O6

b. Ca3(PO4)2

c. (NH4)2Cr2O7

6. The molecular formula of acetylsalicyclic acid (aspirin) is C9H8O4.

a. Calculate the molar mass of aspirin.

b. A typical aspirin tablet contains 500. mg of aspirin. How many moles of C9H8O4 and how many molecules of C9H8O4 are in a 500. mg tablet?

7. Calculate the percent composition of methyl acrylate, C4H6O2, from which Plexiglas is made.

8. Fungal laccase, a blue protein found in wood-rotting fungi, is 0.390% Cu by mass. If a fungal laccase molecule contains 4 copper atoms, what is the molar mass of fungal laccase?

9. The compound adrenaline contains 56.79% C, 6.56% H, 28.37% O, and 8.28% N by mass. What is the empirical formula for adrenaline?

10. Adipic acid is an organic compound composed of 49.31% C, 43.79% O, and the rest hydrogen. If the molar mass of adipic acid is 146.1 g/mol, what are the empirical and molecular formulas of adipic acid?

11. Balance the following equations:

a. ____ Ca(OH)2 (aq) + ____ H3PO4 (aq) → ____ H2O (l) + ____ Ca3(PO4)2 (s)

b. ____ AgNO3 (aq) + ____ H2SO4 (aq) → ____ Ag2SO4 (s) + ____ HNO3 (aq)

c. ____ Pb(NO3)2 (aq) + ____ H3AsO4 (aq) → ____ PbHAsO4 (s) + ____ HNO3 (aq)

12. Acetaldehyde, CH3CHO, and oxygen react to produce acetic acid, HC2H3O2, as described in the following reaction:

2 CH3CHO (l) + O2 (g) → 2 HC2H3O2 (l)

If 200.0g CH3CHO and 100.0g O2 are used in this reaction, determine:

a. the mass of acetic acid produced

b. the identity of the limiting reactant

c. the identity of the reactant in excess

d. the mass of excess reactant that remains after the reaction is complete

e. If the actual yield is 267.9 g, determine the percent yield for this reaction.

MISCELLANEOUS

The following questions / problems cover topics from your summer reading or from the end of last year’s general chemistry class.

1. Name the following acids:

(a) HNO2(b) HClO

(e) HI(f) HC2H3O2

2. Write the formula for each of the following acids:

(a) phosphoric acid(b) hydrosulfuric acid

(e) oxalic acid(f) carbonic acid

3. Answer the following questions about BeC2O4 and its hydrate.

a. Calculate the mass percent of carbon in the hydrated form of the solid that has the formula

BeC2O4 ∙ 3 H2O

b. When heated to 220.0C, BeC2O4 ∙ 3 H2O (s) dehydrates completely as represented below.

BeC2O4 ∙ 3 H2O (s) → BeC2O4 (s) + 3 H2O (g)

If 3.21 g of BeC2O4 ∙ 3 H2O (s) is heated, calculate

(i) the mass of BeC2O4 (s) formed, and

(ii) the volume of H2O released at 220.0C and 735 mm Hg

4. Calculate the molarity of a solution containing 5.00g of NH4Cl in 500.0 mL of solution.

5. How many grams of NaOH are contained in 250.0 mL of a 0.400 M sodium hydroxide solution?

6. Describe how you would prepare 2.00 L of 0.100 M K2CrO4 from a 1.75 M K2CrO4 stock solution.

7. When the following solutions are mixed together, what precipitate (if any) will form?

a. FeSO4 (aq) and KCl (aq)

b. Al(NO3)3 (aq) and Ba(OH)2 (aq)

c. CaCl2 (aq) and Na2SO4 (aq)

8. Re-write and balance each of the following reactions, then write the net ionic equation:

a. AgNO3 (aq) + BaCl2 (aq)

b. FeSO4 (aq) + K2S (aq)

9. A lake may be polluted with Pb2+ ions. What precipitation reaction might you use to test for the presence of Pb2+ ?

10. Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed:

a. cobalt (III) chloride and sodium hydroxide

b. silver nitrate and ammonium carbonate

c. copper (II) sulfate and mercury (II) chloride

d. strontium nitrate and potassium iodide