2014-15 Hon Chemistry Midterm Exam Topics and Review Guide
The following questions and problems are meant to serve as an overall review for the midterm
exam. It is only a guide. You should also review all notes, worksheets, labs, and returned tests
for chapters 2 through 8.
Chapter 2
1. Express each in scientific notation:
a. 9360000
b. 0.7728
c. 0.000037001
2. Write each in standard notation.
a. 8.2001112 x 105
b. 3.23800 x 10-4
d. 190000000000
c. 1.09857 x 101
d. 5.63 x 10-2
3. Significant Figures. Review rules for using significant figures. How many sig. figs. in each of the following
numbers?
a. 0.5
b. 500
c. 500.
d. 500.0
e. 0.05
f. 0.050
6
g. 56008
h. 6.53 x 10
4. Rounding.
a. 3.41236 to 3 sig figs
d. 0.853479 to 4 sig figs
b. 3459.23 to 3 sig figs
e. 49673.56 to 4 sig figs
c. 2.0104 to 4 sig figs
f. 0.00256 to 1 sig fig
5. Rounding/Sig Figs.
Round each of the following to 3 significant figures and express in scientific notation:
a. 73623409
b. 0.0035681230
c. 0.865487
d. 209.825097
e. 723549.09
6. Math with Significant Figure. Calculate each with the correct amount of significant figures
a. 5.2 x 1.00 = ______
b. 6.3489 + 7.7 = _____
c. (3.4 x 103) – (2.1 x 102) = _______
d. 8.940 / 2.39 = ______
e. 149.0 kg + 3388.228 kg + 2.98 kg = ______
f. (1.092 x 103m) – (4.33 x 106m) = _____
9
7
) = ______
g. (4.932 x10 4 )(5.43x10
2
(4.32 x10 )(9 x10 )
7. Dimensional analysis. Show all work. Make sure that your answer has the correct number of significant figs
and is in scientific notation.
a.
b.
g.
j.
m.
8.
7,500,000 μL to mL
89,751,236 lbs to mg
111,109 g to lbs
36 cm to miles
5.72 g to kg
Temperature conversions
Convert to Celsius:
Convert to Kelvin:
b.
e.
h.
k.
n.
15673.35 dL/hour to mL/week
52.30 km/hr to m/s
5400 in to mi
16 weeks to sec
275.6 mL to L
a. 350 K
a. 8.50 oC
b. 17 K `
b. 191 oC
c.
f.
i.
l.
1.56 x 10-4 L to quarts
5.25 x 103 kg to mg
19 cm to ft
54 yds to mm
c. 212 K
c. -40 oC
1
9.
Density. What is the equation for density? ___________ What are the units? __________________
Round the answers to the following problems to the correct number of significant figures.
a. The density of an item is 0.933 kg/L. find the volume of a 4.9909 g sample.
b. The mass of an item is 4234 g and the volume is 893 cm3. What is the density in kg/L?
c. An object measures 5.60 cm by 3.3 cm by 1.456 cm and has a mass of 2.34 g. What is its density?
d. An irregularly shaped object with a density of 3.556 g/mL is dropped into a graduated cylinder filled
with 22.56 mL of water. If the water level rises to 44.5 mL, what is the mass of the object?
e. What is the volume of an object with a density of 8.03 g/cm3 and a mass of 6.00 x 102 g?
Chapter 3
10. Matter.
a. Define the following: heterogeneous, homogeneous, mixture, compound, element, distillation,
filtration, chemical property, physical property, isotope, metal, nonmetal, metalloid, ductile, malleable.
b.
Classify each of the following as an element [E], a compound [C], or a mixture [M].
Distilled Water
Ocean water Ice (from tap water)
A chocolate sundae
Carbon dioxide
Silver
Sugar
A Big Mac®
c.
Classify the following as pure substances [P] or as mixtures [M]:
Black coffee
Distilled water
mercury
oxygen
Kool aid
Beach sand
Gold
Air
Air
Gold
Alcohol
d. Classify the following as heterogeneous [He] or as homogeneous [Ho]:
sand & salt mixture
hydrogen
iron
unfiltered air
iron with rust
pure water
tossed salad
Can of pepsi
Bucket of ocean water
11. Physical vs Chemical Properties/Changes
a. Salt dissolves in water.
c. A piece of copper is cut in half.
e. Water is heated and changed to steam.
g. Ethyl alcohol evaporates.
i. density
b.
d.
f.
h.
sugar
salt water
dirt
salt water
Chocolate chip cookie
Cup of black coffee
HCl acid reacts with Mg to produce H2 gas.
A sugar cube is ground up.
Iron rusts.
Ice melts.
2
Chapter 4
12. Know how to obtain information about elements from the periodic table.
13. Isotope Symbols:
a. Write the chemical symbol for the magnesium isotope with 13 neutrons.
b. Write the chemical symbol for the copper isotope with a mass number of 65.
c. Write the complete chemical symbol for the ion with 84 protons, 125 neutrons, and 80 electrons.
d. Write the complete chemical symbol for the ion with 27 protons, 32 neutrons, and 25 electrons.
e. Write the complete chemical symbol for the ion with 73 protons, 108 neutrons, and 68 electrons.
14. Subatomic Particles. How many protons and neutrons are in the following:
a. 244Pu
b. 133Cs
c. 227Ac
d. 57Fe
15. Ions. Determine the number of protons, electrons and neutrons
a. O-2
How many protons and electrons? What is the atomic number?
b. Na+1 How many protons and electrons? What is the atomic number?
c. Na+1 Is this a cation or an anion? Explain.
d. O-2
Is this a cation or an anion? Explain.
16. Average Atomic Mass. Calculating Average Atomic Mass:
Copper has two common isotopes 63Cu and 65Cu. If the abundance of 63Cu is 69.15% and the abundance
of 65Cu is 30.85%, calculate the average atomic mass of copper.
17. Subatomic particles with ions and isotopes. Fill in the following chart:
Element
Symbol
Atomic
Number
Mass
Number
1
1
2
Cl 1-
Neutrons
Electrons
Gained/Lost
Family/Group
Name
Metal/
nonmetal
/metalloid
0
2
35
K 1+
6
0
35
Lost 2
39
Zinc
Au3+
Electrons
2
6
Gold
Protons
79
118
3
Chapter 5
18. Naming Compounds. Name the following:
a. SeO
b. B2O3
c. AsBr3
h. AgNO3
i. Ba(OH)2 j. KC2H3O2
o. HNO2
d. SnO2
k. Li2CO3
e. CuS
l. Fe2(SO4)3
f. Ca3N2
m. HBr
g. NH4NO2
n. HC2H3O2
19. Formula Writing. Write formulas for the following compounds:
a. barium nitride
b. silver iodide
c. sulfur hexafluoride
d. carbon tetrachloride
e. magnesium acetate
f. iron (II) sulfate
g. zinc chromate
h. cobalt (II) carbonate
i. calcium bromide
j. lithium sulfite
k. nitric acid
l. sulfurous acid
m. copper (II) permanganate
n. phosphoric acid
o. iron (III) oxide
20. More Naming Compounds. Name the following:
a. H3PO4
b. CsOH
c. Li2O
g. H2SO4
h. FeCO3
i. SO3
m. Na2SO3
n. H2CO3
o. LiH
s. N2O
t. NH4F
u. HCO3-
d. Ca(OH)2
j. BaCO3
p. CO
v. K2O
e. CaBr2
k. Al(OH)3
q. MgBr2
f. Fe2O3
l. NaC2H3O2
r. SnBr2
Chapters 6 and 7
21. Products vs Reactants. Identify the product(s) and reactant(s) of the following reaction:
a. NaOH + HCl  NaCl + H2O
b. H2O  H2 + O2
22. Writing Chemical Equations with states.
For the following descriptions of chemical reactions, write and balance the chemical equations. Include the
physical states (aq, s, l, g).
a. When zinc metal and sulfur powder are heated, they form solid zinc sulfide.
b. When sodium metal is placed in a beaker of water, hydrogen gas and sodium hydroxide solution are
formed.
c. Aqueous iron (III) chloride will react with aqueous sodium hydroxide to produce aqueous iron (III)
hydroxide and aqueous sodium chloride.
a. The Haber process is a chemical process by which hydrogen gas reacts with nitrogen gas to form
ammonia. Write and balance a chemical equation for this reaction.
b. One of the problems with space travel is the building up of carbon dioxide produced by the
astronauts. The typical procedure is to react the carbon dioxide with lithium hydroxide to form
lithium carbonate and liquid water. Write and balance a chemical equation for this reaction.
c. Aluminum metal burns in pure oxygen to produce solid aluminum oxide.
d. Hydrogen sulfide gas reacts with oxygen gas to form water vapor and solid sulfur.
e. Hydrogen gas and iron (III) oxide powder react to form liquid water and solid iron powder.
23. Types of Reactions. Determine the type of reaction for each equation:
a. H3PO4 + 3KOH  K3PO4 + 3H2O
b. Ag2O  Ag + O2(g)
c. N2 + H2  NH3
d. C12H22O11(s)  12C(s) + 11H2O(g)
e. AgNO3 + NaCl  AgCl + NaNO3
f. HCl + NaOH  H2O + NaCl
g. H2(g) + O2(g)  H2O(g)
h. Zn(s) + H2SO4(aq)  ZnSO4(aq) + H2(g)
4
24. Predicting Products. Write balanced molecular equations for the following: If they are double replacement
or acid base then also show states of all parts of reaction. Some may not have reactions.
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
magnesium reacts with nitric acid
dicarbon dihydride reacts with oxygen
calcium chloride reacts with sulfurous acid
zinc reacts with copper (II) sulfate
ammonium sulfate reacts with lead (II) nitrate
iron (III) chloride decomposes
sodium reacts with oxygen
dicarbon hexoxide reacts with oxygen
sodium carbonate reacts with potassium chloride
tricarbon octohydride reacts with oxygen
aluminum reacts with sulfuric acid
barium chloride reacts with sodium sulfate
25. Redox Reactions. Determine which of the following are redox (oxidation-reduction) reactions. For the
reactions that are redox, determine which element was oxidized and which was reduced.
a. Ag + S  Ag2S
b. Al + CuCl2  AlCl3 + Cu
c. ZnBr2 + AgNO3  Zn(NO3)2 + AgBr
d. NaI + F2  NaF + I2
Chapter 8:
26. Molar Conversions. Complete the following table. (Show all work.)
Mass of Sample
Moles of Sample
Particles of Sample
4.24 g hexacarbon hexahydride
0.224 mol water
2.71 x 1022 molecules carbon dioxide
0.297 g nitric acid
1.26 mol hydrochloric acid
4.21 x 1024 molecules magnesium acetate
1478 mg ammonium carbonate
1.400 x 103 mol beryllium
permanganate
9.97654 x 1023 molecules hypochlorous
acid
5
27. Percent composition: Find the percent compositions of the elements in the following compounds:
a. CuBr2
d. hydrochloric acid
b. NaOH
f. Mg(NO3)2
c. ammonium sulfide
e. aluminum sulfate
28. Empirical Formulas: Determine the empirical formulas for the following compounds.
a. An oxide of chromium has the following percent composition: 68.4% Cr and 31.6% O.
b. The percent composition of a new compound is 63.5% silver, 8.2% nitrogen and 28.3% oxygen.
c. A 170.00g sample of an undentified compound contains 29.84 g sodium, 67.49 g chromium and 72.67 g
of oxygen.
d. A 60.00 g sample of tetraethyl lead contains 38.43 g of lead, 17.83 g of carbon, and 3.74 g of hydrogen.
29. Molecular formulas: Determine the empirical and molcular formulas for the following compounds.
a. A compound containing 5.93% H and 94.07% O has an estimated molar mass of 34.00 grams.
b. The empirical formula for trichloroisocyanuric acid, the active ingrediant in many household bleaches, is
OCNCl. The molar mass of this compound is 232.41 grams.
c. Determine the molecular formula of a compound with an empirical formula of NH2 and an empirical
formula mass of 32.06 amu.
d. An important reagent used in the synthesis of organic chemical compounds contains 39.74% C, 2.78% H,
13.41% Mg and 44.07% Br. It has a molar mass of 181.31 grams. Determine its molecular formulas.
6