AP Chemistry Summer Assignment
Name______________________
Show ALL work on separate sheet(s) of paper.
No work = No credit
Summer assignment will be due on the 1st day of class and will be your first graded assignment. (20pts
will be deducted per day you are late) Be prepared for a test comprised of the different components of
the summer assignment the first week of school. Don’t panic…you’ve got this! 
1. How many significant figures are in each of the following?
a. 12
e. 0.0000101
b. 1098
f. 1.01 x 10-5
c. 2001
g. 1000.
d. 2.001 x 103
h. 22.01030
2. Round off each of the following numbers to three significant figure and write the answer in standard
exponential notation.
a. 312.54
d. 0.31254
b. 0.00031254
e. 31.254 x 10-3
c. 31 254 000
3. Perform the following calculations and express each result to the correct number of significant
figures.
a. 97.381 + 4.2502 + 0.99195
b. 171.5 + 72.915 – 8.23
c. (0.102)(0.0821)(273)/1.01
d. (0.14)(6.02 x 1023)
e. 4.181 x 100.62 x (25.7-24.16)
f. (8.925-8.904)/8.925
4. Perform each of the following conversions.
a. 8.43 cm to mm
b. 2.41 x 102cm to m
c. 1.445 X 104m to km
d. 903.3nm to micrometers
5. Convert the following Celsius temperatures to Kelvins.
a. the boiling point of ethyl alcohol, 78.1oC
b. a cold day, -25oC
c. the lowest possible temperature, -273oC
d. the melting point of sodium chloride, 801oC
6. The world record for the hundred meter dash is 9.79s. What is the corresponding speed in units of
m/s, km/h, ft/s, and mi/h?
a. At this speed, how long would it take to run a mile (5820 ft)?
7. Write the atomic symbol (AZX) for each of the atoms described below:
a. z=5, A=12
b. the isotope with 7 protons and 8 neutrons in its nucleus
c. atomic number = 17, number of neutrons = 18
d. z=92, number of neutrons =143
e. number of protons = 6, mass number = 14
f. the isotope of phosphorus with 16 neutrons in its nucleus
8. Complete the following table:
Symbol
Number of
Protons
33
128
252Te
16
81
195
Pt
78
Number of
Neutrons
43
16
123
Number of
Electrons
Net Charge
3+
54
16
1+
9. Classify the following elements as metals, nonmetals or metalloids.
Mg Si Rn Ti Ge Eu Au B Am Si Br
10. What is the distinction between atomic number and mass number?
11. What is the difference between atomic mass and average atomic mass?
12. What is an isotope?
13. An element consists of 1.40% of an isotope with mass of 203.973 amu, 24.10% of an isotope with
mass 205.9745 amu, 22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with
mass 207.9766 amu. Calculate the average atomic mass and identify the element.
14. For each of the following ions, indicate the total number of protons and electrons in the ion. For the
positive ions, predict the formula of the simplest compound formed between itself and oxide. For the
negative ions, predict the simplest compound formed between itself and aluminum.
a. Fe+2
d. Cs+1
g. Br+3
-2
b. Fe
e. S
h. N-3
c. Ba+2
f. P-3
15. An element’s most stable ion forms and ionic compound with bromine, having the formula XBr2. If
the ion of element X has a mass number of 230 and 86 electrons, what is the identity of the element and
how many neutrons does it have.
16. Name each of the following compounds.
a. NaCl
l. CrO3
b. Rb2O
m. SF6
c. CaS
n. Al2O3
d. AlI3
o. SO2
e. CH4
p. CaBr2
f. Hg2O
q. Cr2O3
g. Cos
r. S4N4
h. FeBr3
s. NaH
i. HClO
t. ZnCl2
j. TiCl4
u. CsF
w. TiO2
x. Li3N
y. P2S5
z. C5H8
aa. MnO2
bb. Sr3P2
cc. C3H8
dd. CrH5OH
ee. HC2H3O2
ff. NH4NO2
k. Ag2S
v. ICl
17. Write the formula for each of the following compounds
a. cesium bromide
s. potassium chlorate
b. barium sulfate
t. sodium hydride
c. ammonium chloride
u. sodium oxide
d. chlorine monoxide
v. sodium peroxide
e. silicon tetrachloride
w. potassium cyanide
f. chlorine trifluoride
x. selenium tetrabromide
g. beryllium oxide
y. lead(II) sulfide
h. magnesium fluoride
z. copper(I) chloride
i. sulfur difluoride
aa. gallium arsenide
j. sulfur hexafluoride
bb. nitrous acid
k. sodium dihydrogen
cc. diphosphorus pentoxide
phosphate
dd. silicon dioxide
l. sodium sulfite
ee. nitrogen trichloride
m. lithium nitride
ff. hydrobromic acid
n. chromium(II) carbonate
gg. cesium perchlorate
o. ammonium acetate
p. ammonium hydrogen sulfate
q. cobalt(II) nitrate
r. mercury(I) chloride
18. List the names and formulas of the 6 strong acids.
19. List the names and formulas of the 9 strong bases.
20. Write the symbol and charge for each of the following polyatomic ions.
(you were to memorize these in pre-AP, so you should know them well!)
a. nitrite
j. nitrate
s. sulfite
b. sulfate
k. hydroxide
t. hydrogen sulfate
c. cyanide
l. phosphate
u. hydrogen phosphate
d. carbonate
m. hydrogen carbonate v. chlorate
e. hypochlorite
n. chlorite
w. iodate
f. perchorate
o. bromate
x. dichromate
g. chromate
p. permanganate
y. oxalate
h. acetate
q. peroxide
i. borate
r. thiosulfate
21. Write balanced chemical equations to correspond to each of the following descriptions.
a. when solid potassium chlorate is heated, it decomposes to form solid potassium chloride and
oxygen
b. solid zinc metal reacts with sulfuric acid to form hydrogen gas and an aqueous solution of
zinc sulfate
c. when liquid phosphorus trichloride is added to water, it reacts to form aqueous phosphorous
acid and hydrochloric acid
d. when hydrogen sulfide gas is passed over solid hot iron(III) hydroxide, the resultant reaction
produces solid iron(III) sulfide and water vapor.
22. 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 3769.4g of aspartame?
c. How many molecules of aspartame are present in 345.9g of aspartame?
d. How many oxygen atoms are present in 23.6g of aspartame?
23. What is the mass, in grams, of 0.0438 moles of iron(III) phosphate?
24. What is the molar mass of diazepam(Valium) if 0.05570 mol has a mass of 15.86g?
25. Determine the empirical formula of a compound that is 10.4%C, 27.8%S and 61.7%Cl.
26. Find the molecular formula of a compound that is 73.8%C, 8.7%H, 17.5%N and has a molar mass =
166.0g/mol.
27. Given the reaction: S + O2 SO2
a. How many grams of sulfur must be burned to give 100.0g of SO2?
b. How many grams of oxygen must be required for the reaction in part (a)?
28. 6NaOH + 2Al 2Na3AlO3 + 3H2
a. How much aluminum is required to produce 17.5g of hydrogen?
b. How much Na3AlO3 can be formed from 165.0g of sodium hydroxide?
c. How many moles of NaOH are required to produce 3.0g of hydrogen?
d. How many moles of hydrogen can be prepared from 1.0g of aluminum?
29. The following unbalanced equation takes place at high temperatures.
Cr2O3(s) + Al(l)  Cr(l) _ Al2O3(l)
If 42.7g Cr2O3 and 9.8g Al are mixed and reacted until one of the reactants is used up.
a. Which reactant will be left over?
b. How much will be left?
c. How many grams of chromium will be formed?
30. Calculate the mass of water produced when 42.0g of propane, C3H8, is burned with 115g of oxygen.
CONGRATULATIONS…you did it! Be proud of yourself and get ready for a fun-filled and challenging year
which will push you to your limits, but will make you a better student, get you better prepared for
college and prove to yourself how brilliant you really are!
See you in August!!!
Mrs. B