advanced placement chemistry summer 2020 packet

Advanced Placement

Chemistry

Summer 2020 packet

Student name: _________________

June 1, 2020 Dr.Naumova

Dear prospective AP Chemistry 2020-2021 students:

Welcome to the AP Chemistry class! I look forward to working with all of you to help you succeed in this

course and earn credit toward your future college degree.

This is your AP Chemistry Summer assignment. It is due on the first day of school; absolutely no

excuses.

1) Complete the attached packet. The packets will be collected and graded.

2) Please purchase the student lab notebook for this course that you will use throughout the year.

Composition notebook for labs is not acceptable. Below is an example of the lab notebook that will

work (you may buy a different brand but make sure that the notebook has duplicate/”carbon” pages). If

you have a similar lab notebook left from another course (with at least half of pages blank), you can use

it for AP Chemistry. Please have the notebook with you on the first day of school.

If you need to reach me during the summer, you may email me at [email protected]. I may also be

contacting you via email with updates and any announcements that I need to make so please check your email

periodically.

Have a great summer! Dr. Naumova

Assignment

1. All assignments in the summer packet are organized by TOPICS. The specific concepts that need to be

reviewed in each topic are listed. Please review/refresh the first 3 topics thoroughly as they cover the

foundation of the course. Review other topics as needed to complete the remaining problems in the

packet.

2. You can use the following websites to find information:

● https://chem.libretexts.org/

● http://www.bozemanscience.com/ap-chemistry/

● https://www.khanacademy.org/science/chemistry/ap-chemistry

● http://www.learnapchemistry.com/

● https://www.youtube.com/user/mrfarabaugh/videos ● or another AP Chemistry website

3. Get very familiar with the Periodic Table used by the College Board (included). Note that the table

does not have the names of the elements. Please know the names and symbols of all representative and

transition elements.

4. Memorize the most common solubility rules.

5. Memorize the names, formulas, and charges of the polyatomic ions and most common monatomic ions

(attached).

Most Common Solubility Rules of Ionic Compounds:

https://chem.libretexts.org/

http://www.bozemanscience.com/ap-chemistry/

https://www.khanacademy.org/science/chemistry/ap-chemistry

http://www.learnapchemistry.com/

https://www.youtube.com/user/mrfarabaugh/videos

TOPIC 1: Matter and Measurement

MAKE SURE you review the following concepts:

▪ Three states of matter, their general properties and the methods for their interconversion

▪ Physical and chemical change ▪ Elements, mixtures and compounds

▪ Heterogeneous and homogeneous mixtures ▪ Scientific notation

▪ SI units and prefixes ▪ Conversion between units, including derived units such as density ▪ Uncertainties in measurements and significant figures

▪ Accuracy, precision, percentage error ▪ Conversion between the three different temperature units

Problems:

All answers must be in scientific notation to the correct number of significant figures.

1) What is the volume in liters of .0098 x 10-5 mg of benzene if the density of benzene is 0.879 g/mL?

Answer:________________

2) What is the mass in kg of 3.000×104 L of benzene if the density of benzene is 0.879 g/mL?

Answer:________________

TOPIC 2: Atoms, Molecules, and Ions


▪ Five main aspects of Dalton's Atomic Theory

▪ Three subatomic particles, their relative charges, masses and locations in the atom

▪ Calculating the numbers of protons, neutrons and electrons present in the isotope using the Atomic

Number (Z) and Mass Number (A)

▪ Calculation of the atomic mass of element using the abundances and masses of isotopes ▪ Locations of metals, nonmetals and metalloids on the periodic table

▪ Common anions and cations (including polyatomic ions) and their charges ▪ Nomenclature (names and formulas) of the following types of compounds:

▪ binary ionic compounds of a metal and a nonmetal

▪ ionic compounds containing polyatomic anions ▪ hydrated salts

▪ binary molecular compounds of two nonmetals ▪ binary acids

▪ oxoacids and compounds containing oxoanions

Problems:

1. Complete the following table. Include atomic and mass numbers for all nuclides:

Symbol 12276Os

Protons 13 66 76

Neutrons 34 116 74

Electrons 54

Mass number 115 2+ 1-

2. There are four naturally occurring isotopes of iron: iron – 56 (91.754% and 55.935 amu), iron – 54

(5.845% and 53.940 amu), iron – 57 (2.119% at 56.935 amu), and iron – 58 (0.2830% at 57.933 amu).

Calculate the average atomic mass of iron.

Answer:________________

3. There are two naturally occurring isotopes of nitrogen: N-14 and N-15. Which isotope is more

abundant? Why?

4. Name the following ionic compounds:

Formula Name Formula Name

LiCl PbO2

Fe2O3 Mg3(PO4)2

ZnCl2 NaHCO3

AgNO3 KCN

5. Write the formula of the following ionic compounds:

Name Formula Name Formula

Sodium acetate Silver cyanide

Tin(II) chloride Nickel (II) chlorite

Calcium hydroxide Lead (II) nitrate

Zinc sulfate Sodium chloride

6. Name the following covalent compounds:


CO SiO2

CO2 N2O

N2O3 S2Cl2

7. Write molecular formula of the following compounds:


Xenon hexafluoride Nitrogen tribromide

Tetranitrogen tetraoxide Dinitrogen tetrasulfide

8. Write chemical formulas for the following compounds:


Carbon monoxide Sodium acetate

Potassium permanganate Sulfur trioxide

Nickel (II) sulfate Silver sulfide

9. Name the acids:


CH3COOH (or

HC2H3O2)

HF

HBrO3 HCN

H2CO3 H2SO3

10. Write chemical formulas for the following acids:


Perchloric acid Nitrous acid

Nitric acid Hydrochloric acid

Iodic acid Bromic acid

11. Write chemical formulas for the following hydrates:

Name Formula

Magnesium perchlorate hexahydrate

Calcium chromate hexahydrate

Copper (II) sulfate penhahydrate

Iron (III) chloride hexahydrate

Barium chloride dihydrate

TOPIC 3: Stoichiometry


▪ Write balanced chemical equations using chemical formulas and symbols including states of matter. ▪ Calculations using percentage by mass

▪ Calculate empirical formulas from percentage by mass data ▪ Convert empirical formula to molecular formula using molar mass

▪ Calculate chemical quantities using the mole, Avogardo’s number, and molar mass ▪ Calculate the quantities of reactants and products using the mole ratios, Avogardo’s number, and molar

mass. ▪ Determine the type of chemical reactions (synthesis, decomposition, combustion, single replacement,

or double replacement).

Problems

Part I: Composition stoichiometry problems. Always report the correct amount of sig. figures.

a) Write the formula for magnesium chloride__________

b) What is the molar mass of magnesium chloride_________

c) How many moles of magnesium chloride formula units are represented by 9.67×10 25 formula units?

Answer:________________

d) How many chloride atoms are represented by 5.29 mg of magnesium chloride?

Answer:________________

e) What mass of Mg 2+ ions do you have if you have 6.78×10 9 formula units of magnesium chloride?

Answer:________________

Part II: Empirical and molecular formula problems.

1. A hydrated compound has an analysis of 18.29% Ca, 32.37% Cl, and 49.34% H2O. What is the

formula?

Answer:________________

2. Determine the empirical and molecular formula of ibuprofen, a headache remedy that contains 75.69%

C, 8.80% H and 15.51% O by mass; molar mass of 206 g/mol.

Answer:________________

Part III: Write balanced chemical equations for each of the following. Indicate the states of matter

(phases) for each reactant and product.

1. Nitric acid reacts with sodium hydroxide to produce sodium nitrate and water.

2. Magnesium reacts with silver nitrate to produce magnesium nitrate and silver.

3. Potassium chlorate decomposes with manganese oxide as a catalyst into potassium chloride and oxygen

gas.

4. Lithium reacts with water to produce lithium hydroxide and hydrogen gas.

5. Sodium phosphate reacts with chromium (III) permanganate producing sodium permanganate and

chromium (III) phosphate.

6. Chlorine gas, an oxidizing agent, is bubbled into a solution of potassium bromide producing bromine gas

and potassium chloride.

Part IV: Balance each of the following chemical equations and write the reaction type on line next to

the equation:

1. Li2O + H2O → LiOH ___________________________________

2. Ca(ClO3)2 → CaCl2 + O2 ___________________________________

3. C8H8 + O2 → CO2 + H2O ___________________________________

4. BaO + H2O → Ba(OH)2 ___________________________________

5. Xe + F2 → XeF6 ___________________________________

6. Ca + AlCl3 → CaCl2 + Al ___________________________________

7. NH4NO3 → N2O + H2O ___________________________________

8. N2 + H2 → NH3 ___________________________________

9. C4H10 + O2 → CO2 + H2O ___________________________________

10. Si + S8 → Si2S4 ___________________________________

11. SrBr2 + (NH4)2CO3 → SrCO3 + NH4Br ___________________________________

12. BaCl2 + Al2(SO4)3 → BaSO4 + AlCl3 ___________________________________

TOPIC 4: Thermochemistry


● Recall the units of energy and interconversions between J, kJ, cal and kcal.

● Calculate the amount of heat using the specific heat capacity of a substance.

● Calculate the enthalpy change of the reaction using Hess’s Law.

Problems:

1. The specific heat of toluene (C7H8) is 1.13 J/g-K. How many J of heat are needed to raise the

temperature of 62.0g of toluene from 16.3oC to 38.8 oC ?

Answer:________________

2. Use Hess’s Law to calculate ΔH for the reaction of ethylene with F2

Overall reaction: C2H4(g) + 6F2(g) → 2CF4(g) +4HF(g) ΔH = ?

Use the reactions below to solve this problem.

○ H2(g) + F2(g) → 2HF(g) ΔH= -537kJ

○ C(s) + 2F2(g) → CF4 (g) ΔH= -680kJ

○ 2C(s) + 2H2(g) → C2H4(g) ΔH= +52.3kJ

Answer:________________

TOPIC 5: Chemical Bonding


● Determine the type of bonding that exists between the two atoms in a binary compound.

● Differentiate between polar and nonpolar covalent bonds

Complete the following table (Place a checkmark in the correct box)

Molecule Ionic Polar Covalent Non-Polar Covalent

NO2

CaO

H2O

K2O

AlF3

CuCl2

HF

NBr3

Fe2O3

TOPIC 6: Gases


● Use the Ideal Gas Law to calculate one of the variables of gas (volume, pressure, number of moles,

temperature)

● Solve stoichiometry problems that have gases as reactants or products

1. Ammonium sulfate, an important fertilizer, can be prepared by the reaction of ammonia with sulfuric

acid:

2NH3(g) + H2SO4(aq) → (NH4)2SO4(aq)

Calculate the volume of NH3(g) needed at 42oC at 15.6 atm to react with 87 kg of H2SO4.

Answer:________________

TOPIC 7: Equilibrium


● Write expression for the Equilibrium constant, Keq

● Calculate the equilibrium constant for a reverse reaction given the Keq for the forward reaction

● Use the magnitude of Keq to predict the relative amounts of reactants and products

Problems:

1. Write the expression for Keq for the following reactions

○ 3NO(g) ↔ N2O(g) + NO2(g)

○ Ni(CO)4(g) ↔ Ni(s) + 4CO(g)

○ Ti(s) +2Cl2(g) ↔ TiCl4 (l)

○ Co(s) + 2H+(aq) ↔ Co2+(aq) + H2(g)

2. The equilibrium constant for the reaction 2SO3(g) ↔ 2SO2(g) + O2(g) is Keq=2.4x10-3 at 200oC.

Calculate the new Keq for 2SO2(g) + O2(g) ↔ 2SO3(g).

Does the new equilibrium favor SO2 and O2, or does it favor SO3 at this temperature? Explain.

TOPIC 8: Acids and Bases


● In an acid-base equation, identify Bronsted-Lowery acids, bases, and conjugate acids and bases

1. Label the Bronsted-Lowry acid and base on the left side of the equation, and label their conjugate

acid/base on the right side

○ NH4+(aq) + CN-(aq) ↔ HCN(aq) + NH3(aq)

○ (CH3)3N(aq) + H2O(l) ↔ (CH3)3NH+(aq) + OH-(aq)

○ HCHO2(aq) + PO43-(aq) ↔ CHO2

-(aq) +HPO42- (aq)

○ CHO2-(aq) + H2O(l) ↔ HCHO2(aq) + OH-(aq)

○ HSO4- (aq) + HCO3

+ (aq) ↔ SO42-(aq) + H2CO3 (aq)

TOPIC 9: Entropy and Gibbs Energy


● Identify whether reaction is endothermic or exothermic based on the sign of enthalpy change

● Identify if the disorder of the system increases or decreases based on the sign of entropy change

● Identify if the disorder of the system increases or decreases based on chemical equation

● Identify if the reaction is spontaneous or nonspontaneous based on the sign of Gibbs Energy change

1. A certain reaction has ΔH = -19.5k and ΔS = 42.7kJ.

a. Is the reaction exothermic or endothermic?

b. Does the reaction lead to an increase or decrease in the disorder of the system?

c. ΔG for this reaction at 298K is negative. Is the reaction spontaneous at this temperature?

2. Predict the sign of the entropy change (ΔS) of the system for each of the following reactions

a. 2SO2(g) + O2(g) → 2SO3 (g)

b. Ba(OH)2(s) → BaO(s) + H2O (g)

c. CO(g) + 2H2(g) → CH3OH(l)

d. FeCl2(s) + H2(g) → Fe(s) + 2HCl(g)

Chapter 20: Electrochemistry

Concepts to review:

● Determine the oxidation number of elements in the formula of a compound or ion

● Determine whether the reaction is oxidation-reduction or not

● Balance oxidation-reduction reactions in acidic and basic solution using the method of half-reactions

1. Assign the oxidation numbers of the atoms in the following compounds or ions.

(a) Al2O3 Al: _____ O: _____

(b) XeF4 Xe: _____ F: _____

(c) K2Cr2O7 K: _____ Cr: _____ O: _____

(c) SO42- S: _____ O: _____

(c) H2PO3- H: _____ P: _____ O: _____

2. Indicate whether the following balanced equations involve oxidation-reduction. If they do, identify the

elements that undergo changes in oxidation number. Hint: determine the oxidation number of each

element in the reaction and see whether it changes from the reactant to the product sign.

a. PBr3(l) + 3H2O(l) → H3PO3(aq) + 3HBr(aq)

REDOX or Not REDOX (circle one)

Element oxidized:_______________

Element reduced:_______________

b. NaI(aq) + 3HOCl(aq) → NaIO3 (aq) + 3HCl(aq)




c. 3SO2(aq) + 2HNO3(aq) + 2H2O(l) → 3H2SO4(aq) + 2NO(g)




d. 2H2SO4(aq) + 2NaBr(s) → Br2 (l) + SO2 (g) + Na2SO4 (aq) + 2H2O(l)




e. I2 (s) + OCl- (aq) → IO3- (aq) + Cl- (aq)

3. Balance the following equation in basic solution using the method of half-reactions. Show all work.

a. MnO4-(aq) + Br- (aq) → MnO2 (s) + BrO3

- (aq)

advanced placement chemistry summer 2020 packet

Documents