Honors Chem Midterm Review Sheet
Exam - Wed. Dec. 17, 2008
a)
b)
c)
d)
We can order the material from the first semester into 4 broad categories
The “fundamentals” of chemistry
Basic Atomic Theory
Balancing and predicting chemical reactions
Stoichiometry
Listed below is a detailed outline of each of these areas to help you study. However,
even if something is not specifically listed below, it is still fair game. Your notes, old
problem sets, and tests will prove invaluable in helping to study for the exam. In terms of
the textbook, we have covered Chapters 1, 2, 3, 4, 5, 6, part of 7, 8, and 9.
Foundations of Chemistry (Test I)
a) Definition of and branches of chemistry
b) Understand differences between mixtures (heterogeneous and homogeneous) and
pure substances
c) Classification of a pure substance as either a compound or an element
d) Physical and chemical properties and changes
e) States of matter and their characteristics
f) Chemical reactions – reactants and products
g) Intensive and extensive properties
h) Methods to separate mixtures
i) Intro to periodic table – metals metalloids, and nonmetals, families and groups,
periods, transition vs. representative elements.
j) Properties of metals and nonmetals
k) What is special about elements in the same family
l) Scientific method
m) Models, theories, and hypothesis
n) Units of measurement, why must we have a standard?
o) KNOW ALL METRIC CONVERSIONS FROM MEGA TO PICO
p) Density, mass, and volume
q) Conversion factors – how do you derive them and use them
r) Easy and difficult conversions
Sig figs, history of the atom, modern atomic structure, and
early chemical calculations (Test II)
a) Accuracy, precision, and percent error
b) Scientific notation.
c) Significant Figures. How do you determine how many in a number? How do you
add, subtract, multiply, and divide with them?
d) Exact numbers – how do they effect sig. figs.
e) History of the atom : Know scientists in chronological order from Democritus to
Rutherford, their experiments, and contributions.
f) Laws of Definite Proportions, Multiple Proportions, and Conservation of Matter,
and how to apply them.
g) Dalton’s Atomic Theory (know the statements) and how the theory explains the
laws of definite prop, multiple prop, and conservation of mass.
h) Modern atomic theory: subatomic particles
i) Atomic symbols, mass number, atomic number
j) Isotopes, and average atomic mass
k) The mole
l) Conversions between numbers of things, moles, and grams for both atoms and
molecules.
Balancing and predicting chemical reactions (Chapt. 5, 6, and part of 7 )
a)
b)
c)
d)
e)
f)
g)
h)
i)
j)
k)
l)
You are now responsible for all polyatomic ions on pp. 127 + class sheet)
Word, formula, and balanced chemical equations.
Symbols and states in chemical equations.
How to balance a chemical equation.
Ionization and Dissociation (this is from 15-1)
Strong, and nonelectrolytes (from 15-1)
Be able to identify and predict the following kinds of reactions:
Synthesis
Decomposition
Combustion
Double Replacement
How to use the solubility rules and the activity series in the prediction of double and
single replacement reactions.
m) How to write molecular, complete ionic, and net ionic equations for double
replacement rxns.
n) What reactions produce gases?
Stoichiometry – Chapt. 8 and 9
a)
b)
c)
d)
e)
What does a balanced chemical equation tell you?
Mole – Mole conversions
Mass – Mass conversions
Mole – molecule, and mass – molecule conversions
Percent composition
The format of the exam will be a mixture of multiple choice and problems. I would bet
there will be 30-50 multiple choice and 3 - 5 problems, each taking up about one half of
the exam time period.
EXAMPLES:
Consider Silicon, an element widely used in semi-conductors
a) It consists of three isotopes with atomic masses 27.977 amu, 28.977 amu, and
29.974 amu. Their abundances are 92.18%, 4.71%, and 3.12% respectively.
What is the average atomic mass of silicon?
b) What is the mass, in grams, of a silicon atom?
Cisplatin, an antitumor ingredient, has the formula Pt(NH3)2Cl2.
o) Calculate the molar mass of cisplatin
p) How many moles of nitrogen are there in 3.4 moles of cisplatin?
q) How many grams of platinum are there in 250.0 g of cisplatin?
r) How many atoms of chlorine are there in 2.0 moles of cisplatin?
i)
Fill in the gaps in the following table:
Symbol
Protons
Neutrons
Electrons
Atomic #
Mass #
Net Charge
31
P 3-
70
Ga
33
42
56
137
0
2+
Reaction review questions:
1) Balance the following chemical equations and name each product and reactant:
a) Ca(OH)2 + HCl  CaCl2 + H2O
b) Fe2O3 + C  Fe + CO2
c) P4O10 + H2O  H3PO4
d) Al + H2SO4  Al2(SO4)3 + H2
Write balanced net ionic equations for the reactions that may occur when each of the
following pairs is mixed. Identify any spectator ions in these reactions. If there is no
reaction, write NR.
a) AgNO3 (aq) and Na2CO3(aq)
b) NaCl (aq) and (NH4)2SO4 (aq)
c) KOH (aq) and HNO3 (aq)
d) Pb(NO3)2 (aq) and MgSO4 (aq)
e) Hg(NO3)2 (aq) and HBr (aq)
f) HF(aq) and NaOH (aq)
1) Write balanced equations, with states for the following reactions. If indicated, write
down what kind of reaction occurred.
a) Solid copper(I) oxide is heated to decompose it into its elements.
b) Synthesis reaction between solid calcium and solid carbon to form a solid
product.
c) The combustion of decane, C10H22(l)
Stoichiometry Review Problems
1) The combustion of a sample of butane, C4H10, produces 3.46 g of water, as well as
CO2
a) Write the balanced equation for the reaction
b) How many moles of water were formed? How many molecules?
c) How many moles of butane burned?
d) How many grams of butane burned?
e) How many grams and moles of oxygen gas were used up?
f) What is the mass percentage of carbon in butane?
In the late 1700’s the father of modern chemistry, Antoine Lavoisier, performed a
chemical reaction in which he fermented wine. Some information about this experiment
is given in the table below: Use this information to answer the questions that follow.
Quantitative Experiment on the Fermentation of Wine
Reactants
Water
Sugar
Yeast
Mass (g)
400
100
10
Products
Carbon dioxide
Alcohol
Acetic acid
Water
Sugar (unreacted)
Yeast (unreacted)
a) Is wine a pure substance, heterogeneous mixture, or a solution? Explain
b) Write out the chemical reaction that occurred during the fermentation.
Mass (g)
35
58
3
409
4
1
c) Lavoisier stated that this experiment demonstrated the law of conservation of matter?
Is this true? Explain by stating this law and showing if the data in the table can
support it.
d) Why is the word “quantitative” and not “qualitative” used in the title of the table? Is
there any qualitative information in the table? Explain.
4) Express the following numbers in proper scientific notation
a) 602,300,000,000,000,000,000,000 –
b) 5 –
c) 0.0000104 –
5) Express each of the following as a decimal number
i) 9.012 x 10-2 –
ii) 6.91193901 x 107 –
iii) 285.345 x 10-6 –
6) Indicate the number of significant figures in each of the following
i) 12 –
ii) 2001 –
iii) 0.0000101 –
iv) 900 –
v) 2.00 x 10-4 –
vi) 10.
7) Round each of the following to the number of significant figures in parenthesis and
write the number in scientific notation
a) 73,000 (3) –
b) 0.00562 (2) –
c) –12 (1) –
8) Evaluate each of the following and write the answer to the correct number of
significant figures
a) 212.2 + 26.7 + 402.09
b) (0.14)(6.022 x 1023)
c) 4.03 x 10-2 – 2.044 x 10-3 + 10.111 x 10-1
d) (2.0944 + 0.0003233 + 12.22) / (7.001)
e) (7.239)(23.4)(3.416 + 2) / (19.278 – 23.37)
f) [(100.2 x 103)(3.417 x 104 + 4.576 x 104) / (.000027)] * 100 (note 100 is exact)
2) Silver dollars contain 90% silver. A silver dollar has a mass of 27.0 g. In September
1995 silver sold for $5.18 an ounce. In September 1995 did the silver dollar have
more value as currency or as a source of silver?
3) During earlier times in England, land was measured in units such as fardells, nookes,
yards, and kides.
2 fardells = 1 nooke
4 nookes = 1 yard
4 yards = 1 kide
vii) How many kides are there in 27 fardells?
viii)
What is the area in square yards of land that measures 15 fardells by 12 kides?