Download Name: Date: AP Chemistry/Chemistry 145 Summer Assignment

Name:
AP Chemistry/Chemistry 145 Summer Assignment
Date:
A. Significant Figures (Sig Figs)
1. How many sig figs are in the following numbers?
0.0450
____________
790
____________
32.10
____________
2. Solve the following problems. Round your answer to the correct number of sig figs (and use the
correct unit on your answer).
825 cm x 32 cm x 0.248 cm
_____________________
2.885 mL
_____________________
15.68 g
B. Density (round your answers to correct number of sig figs and show all work with units)
3. A cube of ruthenium metal 1.5 cm on a side has a mass of 42.0 g. What is the density in g/cm3?
Will ruthenium metal float on water?
4. The density of bismuth metal is 9.8 g/cm3. What is the mass of a sample of bismuth that displaces
65.8 mL of water?
C. Dimensional Analysis (round answers correctly and show work in DA form with units)
5. Make the following conversions:
6.2 ft to m
(1 m = 1.094 yd)
5.44 qt to mL (1 L = 1.057 qt)
45.7 in/s to km/hr
(1 in = 2.54 cm)
23.5 yd3 to m3 (watch the cube)
D. Naming
6. Give the chemical formula for:
Bromite ion
Chloride ion
Nitrate ion
Periodate ion
Hypochlorite ion
7. Provide names for the following ionic compounds:
AlF3
Fe(OH)2
Cu(NO3)2
Mg(ClO4)2
Li3PO4
Hg2S
Cr2(CO3)3
(NH4)2SO4
8. Write the chemical formulas for the following compounds:
Copper(I) oxide
Potassium peroxide
Iron(III) carbonate
Zinc nitrate
Aluminum hydroxide
9. Give the name or chemical formula for each of the following molecular substances:
SF6
XeO3
Dinitrogen tetroxide
Hydrogen cyanide
IF5
Dihydrogen monoxide
Tetraphosphorous hexasulfide
10. Give the name or chemical formula for the following compounds:
Ammonium oxalate
Manganese(III) dichromate
Ti(OH)4
Ni(ClO2)3
Dinitrogen pentoxide
Aluminum oxide
Fe2S3
E. Reactions
11. Balance the following and equations and tell what type of reaction it is (synthesis,
decomposition, single replacement, double replacement, or combustion)
___ KNO3  ___ KNO2 + ___ O2
Type: __________
___ AgNO3 + ___ K2SO4  ___ Ag2SO4 + ___ KNO3
Type: __________
___ CH3NH2 + ___ O2  ___ CO2 + ___H2O + ___ N2
Type: __________
___ N2O5 + ___ H2O  ___HNO3
Type: __________
___ Na + ___ Zn(NO3)2  ___ Zn + ___ NaNO3
Type: __________
12. What are diatomic molecules? List the 7.
F.
Average Atomic Mass
13. Magnesium consists of 3 naturally occurring isotopes with the masses 23.98504, 24.98584,
and 25.98259 amu. The relative abundances of these three isotopes are 78.70%, 10.13 %, and
11.17% respectively. Calculate the average atomic mass.
G. Percent Composition
14. Calculate the percent composition of C12H22O11 (sugar). (Give Percent of each element.) Show
all work.
H. Moles
15. Calculate the number of moles of the following: (SHOW WORK)
42.8 g of KNO3
155.7 L of CO2 at STP
9.25 x 1026 formula units of CaCl2
I. Stoichiometry
16. Limestone, coral, and seashells are composed primarily of solid calcium carbonate. The test
for the identification of a carbonate is to use a few drops of aqueous hydrochloric acid. Solid
calcium carbonate reacts with aqueous hydrochloric acid. The products are calcium chloride,
carbon dioxide, and water.
Write a balanced chemical equation for this reaction.
How many moles of carbon dioxide is released by the reaction of 0.250 moles of calcium
carbonate?
What mass of carbon dioxide gas is produced by the reaction of 0.250 moles of calcium
carbonate?
17. How many grams of ammonia, NH3, can be prepared from 1.40 g of nitrogen gas and 0.60
g of hydrogen gas?
18. Silver nitrate and barium chloride solutions are mixed.
Write a balanced chemical equation for the reaction of silver nitrate and barium chloride.
If a solution that contains 42.5 g silver nitrate is mixed with a solution containing 51.75 g
barium chloride, which is the limiting reactant?
How many grams of each product are formed?
19. A 11.6-g sample of iron ore, containing Fe3O4 (232 g/mol), is reacted with carbon to form
purified iron. The other product of the reaction is carbon dioxide gas. 2.10 g of iron is
recovered from one such trial.
Write a balanced chemical equation for this reaction, including states for each reactant and
product.
What is the theoretical yield of iron from this reaction?
What is the percent yield?