AP Chemistry - AP Summer Homework, 2014



AP Chemistry

Units 1-2-3

Summer Homework

To perform well on the Unit 1-2-3 Test, you should be able to do the following:

1. Compare and contrast the definite shape, volume, and/or compressibility, or lack thereof, for the three common states of matter.

2. Provide examples of elements, compounds, heterogeneous mixtures, and homogeneous mixtures.

3. Provide an example of the law of constant composition.

4. Compare and contrast physical and chemical properties/changes.

5. Compare and contrast intensive and extensive properties.

6. Convert between °C and K and vice versa. Define “absolute zero.”

7. Calculate density and percent error.

8. Compare and contrast accuracy and precision.

9. Identify the number of significant figures.

10. Report answers with the correct number of significant figures for addition/subtraction and multiplication/division.

11. Provide an example of the law of multiple proportions.

12. Compare and contrast the three subatomic particles—protons, neutrons, and electrons.

13. Report numbers of protons, neutrons, and electrons for elements and ions.

14. Discuss the history of the atom.

15. Identify isotopes from among a list.

16. Calculate the average atomic mass, the fractional abundance, or the mass of one isotope.

17. Identify how elements are grouped on the periodic table, including by families and by metal/nonmetal/metalloid.

18. Name the special families/groups of the periodic table.

19. Name the seven diatomic elements.

20. Compare and contrast empirical and molecular formulas.

21. Compare and contrast the exchange of electrons for metals and nonmetals.

22. Name and identify ionic, molecular-covalent, and acidic compounds.

23. Predict formulas for ionic compounds based on cationic and anionic charges.

24. Balance equations. Describe combustion reactions.

25. Predict the products in a given reaction.

26. Write balanced chemical equations with correct formulas from word equations.

27. Classify reactions according to reaction type.

28. Calculate molar mass.

29. Calculate percent composition of a substance.

30. Convert using the mole road, i.e., mass ( molecules, atoms ( mass, moles ( molecules, etc.

31. Calculate the empirical formula from percent composition of the elements.

32. Calculate the molecular formula from percent composition of the elements and from the molar mass.

33. Convert using the new mole road, i.e., mass A ( mass B, moles A ( mass B, volume A ( mass B, etc., including the mass of two reactants (limiting reactant).

34. Calculate the percent yield of a limiting reactant example.

AP Chemistry Name_________________________

Unit 1 Review

1. Write down all of the terms that could be used to describe the substance pictured in each diagram.

Diagram A Diagram B Diagram C

[pic] [pic] [pic]

2. Identify the following as homogeneous mixture, heterogeneous mixture, compound, or element.

a. water e. sodium chloride

b. nitrogen f. salt water

c. brass g. air

d. orange juice h. salad dressing (i.e., oil and water)

3. Define and give an example of the law of constant composition?

4. Which of the following are physical and which are chemical properties?

a. malleability e. color

b. flammability f. density

c. shape g. boiling point

d. corrosiveness h. brittleness

5. Which of the following are physical and which are chemical changes?

a. alcohol burns e. gold bends

b. apples turn brown f. iron rusts

c. dry ice bubbles in water g. magnesium reacts with oxygen

d. salt dissolves in water h. a solid forms when NaCl and AgNO3 mix

6. What is the difference between an intensive and an extensive property?

7. What is the means to separate

a. a solid from a liquid?

b. a mixture of two liquids?

c. different colors of ink or different ions that have various abilities to adhere to solid surfaces?

8. Show conversion factors for the following problems, reflect the correct number of significant figures in your answer, and include proper units. Remember that definitions such as “1 foot = 12 inches” do not count in determining the number of significant figures.

a. 0.20 cL to L

b. 5.4 gal to L (1 L = 0.264 gal)

c. 85 m/s to km/hr

d. The FM station B-96 broadcasts at a wavelength of 3.11 m. What is the corresponding value in (m if 1 m has 1,000,000 μm?

e. If you went to Paris, France, and charged 5250 euros to your credit card, a debit of how many U.S. dollars will appear on your credit card statement? (as of 5/8/08, 1.00 euro = U.S. $1.53574)

f. In lower Slovobia, 3 cattle can be traded for 7 sheep, and 12 sheep are required to purchase a pig. If I have 25 pigs, but I want cattle, for how many cattle will I be able to trade?

9. Name and describe the three temperature scales. What is the value of absolute zero?

10. Convert the following temperatures.

a. 89 K to °C

b. 27°C to K

11. Given the following lab data, what is the density of metal pellets?

• A graduated cylinder + water has a mass of 48.56 g and the volume of water is 10.2 mL.

• After the pellets are added, the graduated cylinder + water + pellets have a mass of 98.24 g and the volume reads 16.8 mL.

12. The calculated density you obtained in the above problem is called the experimental density. The accepted density of the pellets is 7.81 g/mL. Using the below equation, find the percent error.

% error = | accepted – experimental | × 100

accepted

|Densities (g/cm3) |

|Cork |0.24 |

|Ice |0.92 |

|Aluminum |2.70 |

|Iron |7.86 |

13. Calculate the density of a rectangular solid that is 27.0 cm long, 14.55 cm wide, and 9.3 cm high and has a mass of 805 g. Then identify the solid using the table to the right.

14. A 54-gram sample has a density of 8.0 g/mL. What is the volume of the sample?

15. A 5.4-cm3 sample has a density of 0.30 g/cm3. What is the mass of the sample?

Provide short answers to the following.

16. An ice cube floats in water but sinks in gasoline. Moreover, a cork floats on top of both the water and gasoline. What can you conclude about the relative densities of ice, cork, water, and gasoline?

17. What is the difference between accuracy and precision? What do the dartboards look like for each of the three scenarios?

AP Chemistry Name_________________________

Unit 2 Review

1. Define and give an example of the law of multiple proportions?

2. Label the information for the three subatomic particles.

|Subatomic Particle |Symbol |Charge |Location |Mass (amu) |

|Proton | | | | |

|Neutron | | | | |

|Electron | | | | |

3. Label the information for the three types of radioactivity.

|Type of Radiation |Greek |Isotopic Symbol |Particle or Ray? |

| |Symbol | | |

|Alpha | | | |

|Beta | | | |

|Gamma | | | |

4. Label the history of the atom chart.

|Model |Neutron|Protons|Electro|Nucleus|Signficance |Experiments |Illustration |

| |s? |? |ns? |? | | | |

|Dalton | | | | | | | |

|Rutherford | | | | | | | |

|Modern Quantum | | | | | | |

|Model | | | | | | |

|calcium-40 atom | | | | | | |

| | |4 |9 | | |4 |

|iodine-127 ion | | | | | |54 |

| |30P | | | | | |

| |15 | | | | | |

| | | | |36 |48 |36 |

|potassium-39 ion | | | | | |18 |

6. Of the following atoms, which are isotopes of the same element? (Circle them.)

20X 22X 22X 19X 21X

10 11 10 9 10

7. Given the following information, determine the average atomic mass for carbon. The abundance of carbon-12 is 98.90% with a mass of 12.000 amu. The abundance of carbon-13 is 1.10% with a mass of 13.003 amu.

8. Silicon naturally occurs as a mixture of three different isotopes. Their masses and the abundance of each are given in the below table. Find the average atomic mass of silicon.

|Isotope |Mass in amu |% abundance |

|28Si |27.98 |92.21 |

|14 | | |

|29Si |28.98 |4.70 |

|14 | | |

|30Si |29.97 |3.09 |

|14 | | |

9. The element silver, a metal found in jewelry, has two stable isotopes: silver-107, with a mass of 106.905 amu; and silver-109, with a mass of 108.905 amu. If the average atomic mass of silver is 107.878 amu, then what is the relative abundance of these isotopes?

10. Label the periodic table below with the names of appropriate families and their charges.

| | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | |

11. What is the difference between a period and a family or group? On which does chemical similarity rely?

12. Where are the metals, nonmetals, and metalloids found on the periodic table? Which gain electrons? Lose?

13. What are the seven diatomic elements?

14. What is the difference between molecular and empirical formulas?

15. What is the empirical formula for

a. CH4?

b. C3H6?

AP Chemistry Name_________________________

Unit 3 Review

1. Balance the following equations:

a. ____Al(NO3)3 + ____Na2S → ____Al2S3 + ____NaNO3

b. ____K(s) + ____H2O(l) → ____KOH(aq) + ____H2(g)

c. ____B2O3 + ____Mg → ____MgO + ____B

2. Identify the type of reaction for each of the following:

a. 3NiSO4 + 2Na3PO4 → Ni3(PO4)2 + 3Na2SO4

b. NH4NO2 → 2H2O + N2

c. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag

d. C2Cl4 + Cl2 → C2Cl6

e. CH4 + 2O2 → CO2 + 2H2O

3. What is the molar mass of ammonium sulfate, (NH4)2SO4?

4. What is the mass % of H in methane, CH4?

5. How many molecules of CH4 are in 48.2 g of this compound?

6. How many grams of sodium carbonate, Na2CO3, contain 1.773 × 1017 formula units?

7. How many molecules of CH4 are in 0.123 mol?

8. What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?

9. A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molar mass of the compound is 136 amu. What is the molecular formula?

10. The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O.

4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(g)

The combustion of 43.9 g of ammonia consumes how many grams of NO2?

11. What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water?

Mg(s) + 2H2O(l) → Mg(OH)2(s) + H2(g)

12. Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide.

4Al(s) + 3O2(g) → 2Al2O3(s)

In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. What is the percent yield of the reaction?

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