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AP Chemistry Summer Assignment 2019ContentsWelcome to AP Chemistry!..........................................................................................................2Summer YouTube Playlist.............................................................................................................2References....................................................................................................................................2Directions.....................................................................................................................................3Summer Due Dates.......................................................................................................................3Assessment Schedule and NEST Help Days (First Block)...............................................................3AP Chemistry Reference Packet...................................................................................................4Worksheet 1: Significant Figures and Dimensional Analysis........................................................7Worksheet 2: Structure of the Atom and the Periodic Table.......................................................9Worksheet 3: Naming Inorganic Compounds.............................................................................11Worksheet 4: Atomic and Molecular Masses.............................................................................13Worksheet 5: Balancing Equations and Patterns of Reactivity...................................................14Worksheet 6: The Mole..............................................................................................................17Worksheet 7: Empirical and Molecular Formulas......................................................................19Worksheet 8: Chemical Equations and Calculations..................................................................21Worksheet 9: Limiting Reactants and Theoretical Yield.............................................................23Worksheet 10: Equilibrium.........................................................................................................25Worksheet 11: Things to Memorize...........................................................................................27

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Welcome to AP Chemistry! We have a lot of material to cover, so it is important that we start the year off strong with a good understanding of the basics. The worksheets in this packet are designed for this purpose. They are review from your first-year chemistry course – they are not exhaustive but go over the most important concepts that students often struggle with.

If you get stuck, take a 15-minute break, then look for a resource to help you and try again. There are directions and planning tools on the next page. You should also review the quiz dates on the next page.

This course will be challenging, but also very rewarding. I truly believe that this course prepares students for college level rigor. Treat it with a positive attitude and you will learn. I will fulfill my end of the bargain by providing useful learning activities, NEST help, flexibility, and expertise.

If you need anything over the summer, I will regularly check my email, so feel free to email me at jleffel@aacps.org.

- Ms. Leffel

Summer YouTube PlaylistI’ve put together several videos that will be helpful in completing these worksheets: http://bit.ly/2K5yQGI

ReferencesWorksheets courtesy of Laura McGuire, Chemistry Teacher, Sun Prairie High School. Modifications were made to reduce length and clarify questions.

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Directionso Complete each worksheet in this packet. Use the table below to set due dates for yourself.o Show all work/ justify your answers. For any questions that require math, write out any

equations. Always use units and box your final answer.o Use any resources you like to help you answer questions.o The entire packet is due on 9/4 (A) and 9/5 (B). o A short, non-redoable quiz on each worksheet will

take place according to the schedule given below.

Summer Due DatesItem Set a Due Date

First Monday of Summer Vacation 6/17Worksheet 1Worksheet 2Worksheet 3Worksheet 4Worksheet 5Worksheet 6Worksheet 7Worksheet 8Worksheet 9Worksheet 10Worksheet 11First Day of School/ Packet Due 9/4 or 9/5

Assessment Schedule and NEST Help Days (First Block)

Quiz Content NEST Help Quiz Date

Worksheet 1 and 2 9/9 9/10 (A) or 9/11 (B)Worksheet 3 and 4 9/13 9/16 (A) or 6/17 (B)Worksheet 5 and 6 9/17 9/18 (A) or 9/19 (B)Worksheet 7 and 8 9/20 9/24 (A) or 9/25 (B)Worksheet 9 and 10 9/25 9/26 (A) or 9/27 (B)Worksheet 11 10/1 10/3 (A) or 10/4 (B)

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Worksheet 1: Significant Figures and Dimensional Analysis

1. Round each of the following numbers to four significant figures, and express the result in scientific notation:

a. 2000.1

b. 456, 500

c. 0.006543210

d. 0.000957830

e. –0.035000

2. Carry out the following operations, and express the answers with the appropriate number of significant figures:

a. 1.24056+75.80=¿

b. 2326−75=¿

c. 890,00×112.3=¿

d. 78,1322.50=¿

e.(15.8+96.17)

(2.0)2=¿

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3. Perform the following conversions using the provided conversion factors:1 mi = 1600 m 1 mi = 5280 ft 1 gal = 3.79 L1 ft3 = 2832 mL 1 cm3 = 1 mLa. 8.60 mi to m

b. $1.55/gal to dollars per liter

c. 75.00 mi/hr to m/s

d. 55.35 ft3 to cm3

4. The density of pure silver is 10.5 g/cm3 at 20°C. If 5.25 g of pure silver pellets are added to a graduated cylinder containing 11.2 mL of water, to what volume level will the water in the cylinder rise?

5. The density of air at ordinary atmospheric pressure and 25°C is 1.19 g/L. What is the mass, in kilograms, of the air in a room that measures 12.5 x 15.5 x 8.0 ft?

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Worksheet 2: Structure of the Atom and the Periodic Table

1. What were the main points of Dalton’s Atomic Theory? Which of these points are still accepted today? Which ones do we no longer accept, and why?

2. Summarize the evidence used by J.J. Thomson to argue that cathode rays consist of negatively charged particles.

3. Let’s pretend you are holding two atoms of carbon that are isotopes. Describe what the two atoms have in common and their differences.

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4. Complete the following:

Symbol K+¿1939 ¿

Protons 25 82

Neutrons 30 64

Electrons 48 56 82

Charge 0

Mass # 137 207

Atomic # 56

5. Write the correct symbol, with both superscripts and subscripts, for each of the following neutral atoms:

a. the isotope of sodium with mass number 23

b. the atom of vanadium that contains 28 neutrons

c. the isotope of chlorine with mass number 37

d. an atom of magnesium that has an equal number of protons and neutrons

6. Color code and label the periodic table in the front of this packet to show the following:a. Metals (blue)b. Non-metals (green)c. Metalloids (red)d. Transition metals (put a thick box around them)e. Common charges for each group

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Worksheet 3: Naming Inorganic Compounds

1. How can you determine the chemical formula of the product formed when the metallic element calcium combines with the nonmetallic element oxygen, O2?

2. Give the name or chemical formula for each of the following ionic compounds:a. Cu(NO3)2

b. Ba(ClO4)2

c. Li3PO4

d. Ca(C2H3O2)2

e. K2CrO4

f. (NH4)2SO4

g. Mercury(I) bromide

h. Iron(III) carbonate

i. Copper(I) oxide

j. Potassium peroxide

k. Iron(II) hydroxide

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3. Give the name or chemical formula for each of the following acids:a. HBrO3

b. HBr

c. H3PO4

d. Hypochlorous acid

e. Iodic acid

f. Sulfurous acid

4. Give the name or chemical formula for each of the following molecular substances:a. SF6

b. IF5

c. XeO3

d. Dinitrogen tetroxide

e. Hydrogen cyanide

f. Tetraphosphorous hexasulfide

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Worksheet 4: Atomic and Molecular Masses

1. What isotope is used as the standard in establishing the atomic mass scale? Explain.

2. The atomic weight of magnesium is reported as 24.3, yet no atom of magnesium has the mass of 24.3 amu. Explain.

3. Only two isotopes of copper occur naturally, Cu–63 (abundance 69.09%) and Cu–65 (abundance 30.91%). Calculate the average atomic mass of copper.

4. Determine the molar mass of each of the following compounds:a. Ca(C2H3O2)2

b. (NH4)3PO4

c. sodium nitrate

d. copper (II) sulfate

5. Calculate the percentage by mass of oxygen in the following compounds:a. NO2

b. CH3COOCH3

c. Cr(NO3) 3

d. (NH4) 2CO3

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Worksheet 5: Balancing Equations and Patterns of Reactivity

1. Balance the following equations:a. ___CO(g) + ___O2(g) → ___CO2(g)

b. ___N2O5(g) + ___H2O(l) → ___HNO3(aq)

c. ___PCl5(l) + ___H2O(l) → ___H3PO4(aq) + ___HCl(aq)

d. ___CH4(g) + ___Br2(g) → ___CBr4(l) + ___HBr(g)

e. ___C5H10O2(l) + ___O2(g) → ___CO2(g) + ___H2O(l)

f. ___Cr(OH)3(s) + ___HClO4(aq) → ___Cr(ClO4)3(aq) + ___H2O(l)

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2. Write balanced chemical equations to correspond to each of the following descriptions:a. Solid calcium carbide, CaC2, reacts with water to form an aqueous solution of

calcium hydroxide and acetylene gas, C2H2.

b. Solid zinc metal reacts with sulfuric acid to form hydrogen gas and an aqueous solution of zinc sulfate.

c. When liquid phosphorous trichloride is added to water, it reacts to form a solution of phosphorous acid and hydrochloric acid.

d. When hydrogen sulfide gas is passes over solid hot iron(III) hydroxide, the reaction produces solid iron(III) sulfide and gaseous water.

e. Zinc carbonate can be heated to form zinc oxide and carbon dioxide.

f. A solution of sodium bromide reactions with a solution of vanadium (III) nitrate to form a brightly colored precipitate.

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3. What products form when a hydrocarbon is completely combusted in air?

4. Write a balanced chemical equation for the reaction that occurs when:a. Liquid octane (C8H18) is combusted in air.

b. Liquid heptane (C7H16), is combusted in air.

c. The gasoline additive MTBE (methyl tertiary-butyl ether), C5H12O(l), burns in air.

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Worksheet 6: The Mole

1. The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet, is C14H18N2O5.

a. What is the molar mass of aspartame?

b. How many moles of aspartame are present in 1.00 mg of aspartame?

c. How many molecules of aspartame are present in 1.00 mg of aspartame?

d. How many hydrogen atoms are present in 1.00 mg of aspartame?

2. A sample of glucose, C6H12O6, contains 2.03 x 1021 atoms of carbon. a. How many atoms of hydrogen does it contain?

b. How many molecules of glucose does it contain?

c. How many moles of glucose does it contain?

d. What is the mass of the sample in grams?

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3. Calculate the following amounts:a. How many moles of chloride ions are in 0.0750 g of magnesium chloride?

b. What is the mass, in grams, of 3.50×10–3 mol of aluminum sulfate?

c. What is the mass, in grams, of 1.75×1020 molecules of caffeine, C8H10N4O2?

d. What is the molar mass of cholesterol if 0.00105 moles weigh 0.406 g?

e. How many molecules are in a 50.0 mg tablet of acetaminophen, C8H9O2N?

4. The allowed concentration of vinyl chloride (C2H3Cl) in the air of a chemical plant is 2.0×10–6 g/L according to OSHA.

a. How many moles of vinyl chloride in each liter does this represent?

b. How many molecules per liter is this?

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Worksheet 7: Empirical and Molecular Formulas

1. Determine the empirical formula if a sample contains:a. 0.104 mol K, 0.052 mol C, and 0.156 mol O

b. 5.28 g Sn and 3.37 g F

c. 21.7% C, 9.6% O, and 68.7% F by mass

2. Determine the empirical and molecular formulas of each of the following substances:a. Ibuprofen, a headache remedy contains 75.69% C, 8.80% H, and 15.51% O by

mass. The molar mass of ibuprofen is 206.29 g/mol.

b. Benzene contains only carbon and hydrogen and is 7.74% hydrogen by mass. The molar mass of benzene is 78.1 g/mol.

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3. Many homes in rural America are heated by propane gas, a compound that contains only carbon and hydrogen. Complete combustion of a sample of propane produced 2.641 g of carbon dioxide and 1.442 g of water as the only products. Find the empirical formula of propane.

4. Menthol, the substance we can smell in mentholated cough drops, is composed of carbon, hydrogen, and oxygen. A 0.1005 g sample of menthol is combusted, producing 0.2829 g of CO2 and 0.1159 g of H2O.

a. Find the empirical formula for menthol.

b. If the compound has a molar mass of 156 g/mol, what is its molecular formula?

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Worksheet 8: Chemical Equations and Calculations

1. Why is it essential to use balanced chemical equations in solving stoichiometry problems?

2. The fermentation of glucose, C6H12O6, produces ethyl alcohol, C2H5OH, and CO2.C6H12O6(aq) → 2 C2H5OH(aq) + 2 CO2(g)

a. How many moles of CO2 are produced when 0.300 mol of C6H12O6 reacts in this fashion?

b. How many grams of C6H12O6 are needed to form 2.00 g of C2H5OH?

c. How many molecules of CO2 form when 2.00 g of C2H5OH are produced?

3. Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. a. Write the balanced chemical equation for this reaction.

b. How many grams of aluminum hydroxide are obtained from 10.5 g of aluminum sulfide?

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4. Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements:

2 NaN3(s) → Na(s) + 3 N2(g)a. How many moles of N2 are produced by 1.50 moles of NaN3?

b. How many grams of NaN3 are required to form 5.00 g of nitrogen gas?

c. How many grams of NaN3 are required to produce 10.0 L of nitrogen gas if the gas has a density of 1.25 g/L?

5. A piece of aluminum foil 0.550 mm thick and 1.00 cm square reacts with bromine to form aluminum bromide.

a. How many moles of aluminum were used? The density of aluminum is 2.69 g/cm3.

b. How many grams of aluminum bromide form if all the aluminum reacts?

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Worksheet 9: Limiting Reactants and Theoretical Yield

1. A manufacturer of bicycles has 50 wheels, 30 frames, and 24 seats.a. How many bicycles can be manufactured using these parts?

b. How many parts of each kind are left over?

c. Which part is like a limiting reactant in that it limits the production of bicycles?

2. The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium bicarbonate, NaHCO3, and citric acid, H3C6H5O7:

3 NaHCO3(aq) + H3C6H5O7 (aq) → 3 CO2(g) + 3 H2O(l) + Na3C6H5O7(aq)In an experiment, 1.00 g of sodium bicarbonate and 1.00 g of citric acid are reacted.

a. Which reactant is the limiting reactant? Show work to support your answer.

b. How many grams of carbon dioxide form?

c. How much of the limiting reactant is left when the reaction is complete?

d. How much of the excess reactant remains after the reaction is complete?

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3. When hydrogen sulfide gas is bubbled into a solution of sodium hydroxide, the reaction forms sodium sulfide and water. How many grams of sodium sulfide are formed if 2.50 g of hydrogen sulfide is bubbled into a solution containing 1.85 g of sodium hydroxide, if the limiting reagent is completely consumed?

4. Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 10.0 g of sulfuric acid and 10.0 g of lead(II) acetate are mixed, calculate the number of grams of sulfuric acid, lead(II) acetate, lead(II) sulfate, and acetic acid present in the mixture after the reaction is complete.

5. A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr.

a. What is the theoretical yield of bromobenzene in this reaction when 30.0 g of benzene reacts with 65.0 g of bromine?

b. If the actual yield of bromobenzene was 56.7 g, what was the percent yield?

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Worksheet 10: Equilibrium

1. Indicate the direction of the shift for the reaction below for each of the following.2H2(g) + O2(g) ⇌ 2H2O(g) + energy

a. Removing H2O as it forms

b. Adding energy

c. Reducing pressure

d. Adding helium gas

2. For the reaction N2O4(g) ⇌ 2NO2(g), Kc = 0.2. a. Write the Kc expression for this reaction.

b. The following concentrations are measured: [N2O4] = 2.0 M, [NO2] = 0.2 M. Is this reaction at equilibrium?

c. Which direction will the reaction proceed? Explain.

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3. Consider the dissolving of calcium chloride into water.a. Write the Ksp expression for calcium chloride.

b. Given that calcium chloride is highly soluble in water, what kind of value would you expect for the Ksp?

4. Explain the relationship between the value of Ka and the strength of an acid.

5. In each of the following reactions, identify the conjugate acid-base pairs. a. HF (aq) + NO3

− (aq) ⇌ HNO3 (aq) + F− (aq)

b. NH4+ (aq) + CO3

2− (aq) ⇌ HCO3− (aq) + NH3 (aq)

6. A buffer system forms when NaHCO3(aq) is mixed with H2CO3(aq).a. Explain the purpose of a buffer.

b. Write a chemical equation showing the buffer neutralizing acid (H+).

c. Write a chemical equation showing the buffer neutralizing base (OH–).

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Worksheet 11: Things to Memorize

Polyatomic IonsIon Name Ion NameH3O+ hydronium CrO4

2– chromateHg2

2+ dimercury (I) Cr2O72– dichromate

NH4+ ammonium MnO4

– permanganateC2H3O2

–

CH3COO– acetate NO2– nitrite

NO3– nitrate

C2O42– oxalate O2

2– peroxideCO3

2– carbonate OH– hydroxideHCO3

– hydrogen (bi)carbonate CN– cyanidePO4

3– Phosphate SCN– thiocyanateClO– hypochlorite SO3

2– sulfiteClO2

– chlorite SO42– sulfate

ClO3– chlorate HSO4

– hydrogen sulfateClO4

– perchlorate S2O32– thiosulfate

Solubility RulesIons that form Soluble Compounds

Exceptions Ions that form Insoluble Compounds Exceptions

Group 1 ions (Li+, Na+, etc.) Carbonate (CO3

2–) When combined with Group 1 ions or ammonium

Ammonium (NH4+) Chromate (CrO4

2–) When combined with Group 1 ions, Ca2+, Mg2+ or ammonium

Nitrate (NO3–) Phosphate (PO4

3–) When combined with Group 1 ions or ammonium

Acetate (C2H3O2– or

CH3COOH) Sulfide (S2–) When combined with Group 1 ions or ammonium

Hydrogen carbonate (HCO3

–) Hydroxide (OH–)When combined with Group 1 ions, Ca2+, Ba2+, Sr2+ or ammonium

Chlorate (ClO3–)

Perchlorate (ClO4–)

Halides (Cl–, Br–, I–) When combined with Ag+, Pb2+, and Hg2

2+

Sulfates (SO42–)

When combined with Ag+, Ca2+, Sr2+, Ba2+, and Pb2+

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Strong Acids and BasesAcids Bases

o HClo HBro HIo HNO3

o HClO4

o H2SO4

o HClO3

o Group 1 hydroxides: LiOH, NaOH, KOH, RbOH, CsOH

o Ca(OH)2*o Sr(OH)2*o Ba(OH)2*

* These bases only show 100% dissociation in dilute solutions (0.1 M or less)

Stoichiometry Conversions

Kinetic Molecular Theoryo Watch the video (http://bit.ly/2EynTKe). You should understand the postulates of

kinetic molecular theory and be able to explain gas laws using kinetic molecular theory.

Intermolecular Forces

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o Watch the video (http://bit.ly/2Ey1Ymy). You should be able to describe the three types of intermolecular forces and use them to explain the physical properties of a substance, such as boiling point.