AP Chemistry Summer Assignment
Short Answer
Each of the following is an example of some of the types of questions that you had answered while in Honors
Chemistry I. Please answer each of these questions, and show all work with appropriate units and significant
digits. A short quiz will be given on these problems once this sheet has been reviewed. Please note that you do
NOT need a textbook to complete this assignment; it is a review, and referring to your notes from Honors Chemistry
I will provide any assistance that you may need.
1. The following length measurements were taken by students using several different measuring devices. Find
the average of the measurements. Make sure that your answer has the correct number of significant figures.
10.05 cm, 10.1 cm, 9.741 cm, 10.6 cm, 10.5 cm
2. What is the sum of 2.7 g and 2.47 g expressed in the correct number of significant digits?
3. Perform the following operation: 3.43 cm
significant figures.
5.2 cm. Make sure that your answer has the correct number of
4. What is the temperature 128 K expressed in degrees Celsius?
5. What is the volume of an object with a density of 7.73 g/cm3 and a mass of 5.40
10 g?
6. A cube of a gold-colored metal with a volume of 59 cm has a mass of 980 g. The density of pure gold is
19.3 g/cm3. Is the metal pure gold? Show calculations to justify your answer.
7. List the number of protons, neutrons, and electrons in
C.
8. Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the
isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0%
abundant. What is the average atomic mass for element Z?
9. Give the electron configuration for a neutral atom of beryllium.
10. Write the electron configuration for chromium.
11. What is the frequency of ultraviolet light with wavelength 2.94
10
m? (c = 3.00
10 m/s)
12. What is the wavelength of gamma ray electromagnetic radiation with a frequency of 2.73
3.00 10 m/s)
13. What is the energy of a microwave photon that has a frequency of 1.12
10
10
Hz? (h = 6.63
Hz? (c =
10
J s)
14. Which group of elements in the periodic table is known as the alkali metals?
15. Which group in the periodic table is known as the noble gases?
16. What is the electron configuration of sulfur?
17. From which orbital in a lithium atom is an electron transferred to form Li ?
18. What orbital is filled when iodine gains an electron to become a negative ion?
19. In which group in the periodic table do the elements have the highest electronegativity values?
20. Give the electron configurations for mercury and its 2 ion.
21. Write the formula for the compound barium oxide.
22. Write the formula for the compound rubidium phosphide.
23. Write the formula for the compound boron chloride.
24. How many representative particles are in 1.45 g of a molecular compound with a molar mass of 237 g?
25. Find the mass in grams of 3.10
10
molecules of F .
26. What is the percent composition of NiO, if a sample of NiO with a mass of 41.9 g contains 33.1 g Ni and
8.8 g O?
27. Calculate the molecular formulas of the compounds having the following empirical formulas and molar
masses: C H , 58 g/mol; CH, 78 g/mol; and HgCl, 236.1 g/mol.
28. Complete and balance the following equation.
Cd(NO )
NH Cl
29. Write a balanced equation for the following:.
Sodium chlorate undrgoes decomposition to form soldium chlorde and oxygen.
30. Write a balanced net ionic equation for the following reaction.
H PO (aq) Ca(OH) (aq)
Ca (PO ) (aq) H O(l)
31. If 8.00 mol of NH reacted with 17.0 mol of O , how many moles of H O will be produced?
4NH (g) + 7O (g)
4NO + 6H O(g)
32. If 8.6 L of H reacted with 4.0 L of O at STP, what is the volume of the gaseous water collected (assuming
that none of it condenses)?
2H (g) + O (g) 2H O(g)
33. Assuming STP and a stoichiometric amount of NH and NO in an expandable container originally at 15 L,
what is the final volume if the reaction goes to completion?
4NH (g) + 6NO(g)
5N (g) + 6H O(g)
34. If 5.0 g of H are reacted with excess CO, how many grams of CH OH are produced, based on a yield of
86%?
CO(g) + 2H (g)
CH OH(l)
35. The volume of a gas is 250 mL at 340.0 kPa pressure. What will the volume be when the pressure is
reduced to 50.0 kPa, assuming the temperature remains constant?
36. A balloon filled with helium has a volume of 30.0 L at a pressure of 100 kPa and a temperature of 15.0 C.
What will the volume of the balloon be if the temperature is increased to 80.0 C and the pressure remains
constant?
37. A gas has a volume of 590 mL at a temperature of –55.0 C. What volume will the gas occupy at 30.0 C?
38. A gas has a pressure of 710 kPa at 227 C. What will its pressure be at 27 C, if the volume does not
change?
39. A gas storage tank has a volume of 3.5 10 m when the temperature is 27 C and the pressure is 101 kPa.
What is the new volume of the tank if the temperature drops to –10 C and the pressure drops to 95 kPa?
40. How many moles of N are in a flask with a volume of 250 mL at a pressure of 300.0 kPa and a
temperature of 300.0 K?
41. What is the pressure exerted by 32 g of O in a 22.0-L container at 30.0 C?
42. A mixture of gases at a total pressure of 95 kPa contains N , CO , and O . The partial pressure of the CO
is 24 kPa and the partial pressure of the N is 48 kPa. What is the partial pressure of the O ?
43. Use Graham’s law to calculate how much faster fluorine gas, F , will effuse than chlorine gas, Cl , will.
The molar mass of F = 38.0; the molar mass of Cl = 70.9.
44. Determine the oxidation number of each element in the following compound: HMnO4.
45. Balance the following using the oxidation number change method:
KClO3 + H2SO4 --> KHSO4 + O2 + ClO2 + H2O
46. Identify the oxidizing and reducing agents in #45.
47. Balance the following using the ion electron method:
K3Fe(CN)6(aq) + Cr2O3(s) + KOH(aq) --> K4Fe(CN)6(aq) + K2CrO4(aq) + H2O(l)
48. For H2SO4, determine the following (note – assume the central atom obeys the octet rule):
a. A Lewis Structure
b. The hybrid type of the central atom
c. The bond angles
d. The molecular geometry
e. The polarity of the molecule.
f.
Draw any and all possible resonance strucutres
49. 50.0 g of a metal at 100.0 degrees C is placed into 20.0 grams of water at 30.0 degrees C. After mixing, the
temperature is 57.0 degrees celsius. What is the specific heat of the metal?
50. In what type of medium is the reaction in #47 occurring?