Chemistry First Semester Exam Review
1. How many liters are in 500 milliliters?
2. How many kilojoules are in 500 joules?
3. List some possible units for volume.
4. What is the volume of a cube that is 5 centimeters on all sides?
5. If the mass of the cube in #4 is 55.5 grams, what is the density of the cube?
6. What is the solution concentration in percent mass when 155 grams of sugar is dissolved
in 750 grams of water?
7. What is the molar mass of sodium hydroxide?
8. What is the molar mass of pentane?
9. How many moles are in 45 grams of oxygen gas? Remember that oxygen is diatomic!
10. The specific heat capacity of water is 4.184
J
. How many joules of energy does it take
gC
to heat 25g of water from 15°C to 28°C?
11. If the molar heat of combustion for propane is 560 kJ mol , how much energy will be
released by burning 6.5 moles of propane?
12. What is the molar mass of Na2CO3?
13. Ten kilograms of candy contains 590g of chocolate, 880g of sugar, and 250g of pecans.
What is the percent sugar in this candy?
14. Write the correct chemical formula for the ionic compounds formed by the following
pairs of ions. Then name the compound.
a. Na+ and Fb. K+ and S-2
c. Ni+2 and SO4-2
d. Al+3 and O-2
e. Ca+2 and ClO3-1 (chlorate)
f. NH4+1 (ammonium) and P-3
g. Cu+1 and NO3-1
h. Cu+2 and NO3-1
15. Classify each of the following as chemical or physical properties or both.
a. Conducts electricity
b. Is a liquid at room temperature
c. Reacts with acids to form gas bubbles and a solid precipitate
d. Used to distinguish metals from nonmetals
e. Changes from a metallic solid to a purple gas when heated
16. What is the molar mass of Cu2Fe3S2(CO3)2?
17. How many grams of water are in 2.5 moles of water?
18. Answer the questions using the following reaction: BaCO3  BaO + CO2
a. Name the reactant and both products.
b. Calculate the molar mass of the reactant and both products.
c. If ten moles of BaO are formed, how many moles of BaCO3 were decomposed?
d. If ten moles of BaO are formed, how many grams of BaCO3 were decomposed?
19. Refer to the metal reactivity series in your book to answer the questions:
a. Which is the least active solid metal that can be obtained using the reduction
process involving heat with coke (carbon) or carbon monoxide (CO)?
b. Will the metal sodium react with a solution of silver ions?
c. Will the metal sodium react with a solution of potassium ions?
d. Write the balanced redox reaction that occurs when magnesium reacts with an
aqueous solution of copper (II) nitrate.
20. In Materials Lab A.3 you examined and determined the metallic character of a number of
substances. Name three criteria that allow you to distinguish between a metal, nonmetal,
and metalloid.
21. Write and balance the following reactions:
a. hydrogen gas + chlorine gas ⇒ hydrogen chloride gas
b. silver ion in solution + sulfuric acid solution ⇒ hydrogen ion in solution + solid
silver sulfate
c. solid calcium carbonate ⇒ solid calcium oxide + carbon dioxide gas
d. solid zinc + hydrogen ion in solution ⇒ zinc ion in solution + hydrogen gas
e. CaSO4 + H3PO4 ⇒ Ca3(PO4)2 + H2SO4
f. Fe3O2 + SO2 ⇒ Fe + SO3
22. Which of the following ores is most economical to extract silver from? Determine your
response by calculating the percent silver in each.
a. Tampaprepionate
AgNO3
b. tampapreionette
Ag2S
c. tampapreionite
Ag2O
23. Draw an example of the following compounds:
a. a carboxylic acid
b. an alcohol
c. an alkene
d. a cycloalkane
e. an inorganic acid
f. a base
24. List the Earth's composition in terms of spheres. What are the major chemicals in each?
25. Trace the path of a drop of water from the Hillsborough River all the way to an iceberg in
Greenland. Name the cycle you are describing.
26. From the following data, indicate whether the mixture is a solution, suspension, or
colloid.
Appearance
Clarity
Tyndall Effect
Mixture A
yellow
clear
yes
Mixture B
white solid
cloudy
yes
Mixture C
clear (water-like)
clear
no
Mixture D
blue
clear
no
27. For butane, write the:
a. molecular formula
b. structural formula
c. electron dot structure
d. condensed formula
28. Describe the pH scale.
29. Name both heavy metal ions and the consequences of ingesting each.
30. In the electroplating of copper, the following two reactions occur at the electrodes:
Process I:
Cu+2(aq) + 2e- ⇒ Cu(s)
Process II:
Cu(s) ⇒ Cu+2(aq) + 2e-
a. Which process is reduction?
b. Which process occurs on the item being electroplated?
31. Draw the electron dot diagram for 2-butene.
32. Draw the structural formula for 3-methyl pentane.
33. What is the molecular formula for cyclohexane?
34. What are the structural and molecular formulas for benzene?
35. Draw and name five isomers of octane.
36. Write the structural formula for 4-methyl nonyne.
37. Fill in the following chart and answer the questions pertaining to it.
Element symbol
a.
Number of protons
Number of electrons
18
18
20
20
239
88
S
b.
c.
Number of neutrons
20
U
d. What is the mass number of a above?
e. What is the ionic charge of b above?
f. What is the ionic charge of c above?
38. Draw models for the following:
a. a mixture of elemental gases: monatomic A and diatomic B
b. a diatomic compound in three states of matter, all in the same container
c. the chemical reaction: combustion of propane
d. a solution of potassium bromide in water
39. Write the balanced chemical equation for the complete combustion of octane, including
the quantity of thermal energy released. Refer to your book for the molar heat of
combustion of octane.