CHEMISTRY – 1st SEMESTER EXAM REVIEW
STRATEGY: Start by reading through your notes and study guides to refresh your memory. Look over the Chapter Highlights for
Chapters 1-7. Then, use this review sheet as a starting point to identify the areas on which you need to spend more study time. For
those areas, go back to homework assignments, text resources, and notes to practice more problems. Prepare an index card with
notes to help with difficult concepts. These questions are only samples and do not include specific examples of how vocabulary and
other conceptual information might appear in a multiple-choice test. The questions will be similar to those on chapter tests.
FORMAT:
 Questions will include no more than 100 multiple-choice questions and 1 essay from those that I give you.
 You will be given a periodic table.
 You may use 1 handwritten small (3.5”x5”) index card to prompt your memory.
Chapter 1: Matter and Change
1. What is the difference between an element and a
compound?
2. What is the difference between a heterogeneous and
homogeneous mixture?
3. Compare and contrast a solution, colloid, and suspension.
4. Classify the following as element, compound,
heterogeneous mixture, or solution.
a. graphite (carbon)
c. table salt (NaCl)
b. grape juice
d. vegetable soup
5. Classify the following as chemical or physical changes.
a. cutting wire
c. apple slices turning brown
b. melting ice
d. compressing a gas
6. Classify the following properties as physical or chemical.
a. melts at 68.0C
c. decomposes in air
b. corrosive
d. conductive
Chapter 2: Measurements and Calculations
11. What is the meaning behind the Law of Conservation of
Mass and the Law of Multiple Proportions?
12. What is the difference between a quantitative and a
qualitative observation?
13. What is density? How is it determined experimentally and
mathematically?
14. List the metric prefixes from mega to nano, the symbols
for each, and list what they represent numerically.
15. What is the difference between precision and accuracy?
16. Complete the following conversions significantly:
a. 340.0 mm to km
c. 9.00 ns to s
-3
b. 0.0320 Mg to g
d. 3.05 x 10 km to cm
Chapter 3: Atoms: The Building Blocks of Matter
20. List the particles that makeup an atom. Where are each of
the particles located in an atom? What kind of charge
do each of the particles have? What is the relative size
of each particle?
21. Identify the scientists who made the following discoveries
and name their experiments.
a. Atoms contain negatively charged particles called
electrons.
b. Atoms contain a dense, positive nucleus.
22. What is the primary difference between the modern model
of the atom and Bohr’s model?
23. Write the nuclear representation, which includes atomic
number & mass number, for the following isotopes.
a. carbon-14
c. nickel-63
b. chromium-53
d. zirconium-92
24. What are valence electrons and where are they located?
7. Classify the following characteristic as either being that of
a metal or a nonmetal.
a. dull
c. shiny
b. malleable
d. brittle
8. What are the 4 states of matter and how would you
distinguish between each?
9. What is a change of state? Is it physical or
chemical…why? Give some examples of the
change of state.
10. Determine where each of the following are on the periodic
table: groups/families, noble gases, periods, alkali metals,
metals, transition metals, nonmetals, halogens, metalloids,
alkaline earth metals, rare earth metals, lanthanides, and
actinides.
17. In a lab, the average measured density for Pre-1982
3
pennies was 7.98 g/cm . Given that the literature value
3
for the density is 8.92 g/cm , calculate the percent error.
18. Determine the number of significant figures in each of the
following numbers.
a. 0.000357
d. 3,004
b. 8.7010
e. 700.00
3
c. 100,000
f. 6.2030 x 10
19. Convert a and b into scientific notation and c and d into
standard form.
-3
a. 548,000
c. 1.200 × 10
7
b. 0.0000770
d. 9.25 × 10
25. Calculate the average atomic mass of copper if 69.17% of
63
the copper atoms occurring in nature are Cu and 30.83%
65
are Cu.
26. Complete the table for the following isotopes.
Symbol
Zn
Atomic #
20
Mass #
65
74
40
# of protons
34
# of neutrons
21
# of electrons
18
27. Determine the mass in grams of each of the following.
a. 6.50 moles of Cu
18
b. 1.05 x 10 atoms of Hg
28. How many moles are there in each of the following?
2
a. 1.50 x 10 grams ZnS
25
b. 2.25 x 10 molecules of CO2
Chapter 4: Arrangement of Electrons in Atoms
29. What is electromagnetic radiation and what are the
seven types listed from lowest energy to highest
energy?
30. What is wavelength? What is frequency? How are
wavelength and frequency related?
31. What formulas can be used to calculate wavelength
and frequency?
32. What formula is used to either calculate energy or
frequency.
33. What is the meaning of the ground state of an electron and
excited state of an electron?
34. What happens as an electron goes from its ground state to
an excited state?
35. What occurs when an electron goes from an excited state
to its ground state?
36. What is the maximum number of electrons that an orbital
can contain? That the s, p, d, and f sublevels can
contain?
37. Define the following: Heisenberg Uncertainty Principle,
Aufbau Principle, Pauli Exclusion Principle, and Hund’s
Rule?
Chapter 5: The Periodic Table
40. Describe the periodic trends for atomic radius, ionic radius,
ionization energy, and electron affinity.
41. Explain the trends listed above. (Think of the energy levels
involved within a group and the increasing number of
protons across a period.)
42. Which group on the periodic table has the largest atomic
radii?
43. Which group on the periodic table has the highest first
ionization energy?
44. According to trends, what elements on the periodic table
st
have the highest /lowest 1 ionization energy?
45. Compare the element Fe and Cu when answering the
following.
a. Which element has the smallest atomic radius?
b. Which element has the largest first ionization energy?
46. How many valence electrons are in each of the following
elements?
a. Ba
b. Pb
c. Po
d. Rn
38. Complete the orbital notation and electron configuration
notation (box and spectroscopic) for the following. Circle the
valence electrons.
# electrons
Symbol
electron configuration
F
Ca
P
N
Se
39. Predict the ions that will form from the following atoms,
show the Noble Gas it will be like when it forms an ion,
and give the Noble Gas configuration of the neutral atom.
Atom
Ion
Noble Gas
Electron Configuration
K
Cl
O
Mg
47. In each pair of elements, circle the one that has the largest
atomic radius.
a. Cs or Fr
b. Sn or Pb
c. Ag or Cd
48. In each pair of elements, circle the one that has the largest
first ionization energy.
a. Cs or Ba
c. Au or Hg
49. How are the elements arranged in the current periodic
table?
50. Circle the particle with the LARGER radius. Which is larger
in each example, the neutral atom or the ion?
–1
2+
a. Cl Cl
b. Mg Mg
51. Circle the atom with the HIGHER electronegativity.
a. C Si
b. Cs W
c. F Cl
52. Based on the electronegativity of each element in the
following compounds, are the bonds in the compound
IONIC, COVALENT or POLAR COVALENT?
a. MgO
c. LiCl
b. H2O
d. Br2
Chapter 6: Chemical Bonding and Molecular Geometry
53. Atoms that have very similar electronegativities are
expected to form _________bonds.
54. Metals typically have ______________________
ionization energies.
55. Metals and non-metals form ___________ bonds.
56. Non-metals share electrons in __________ bonds.
57. The ability of an atom in a molecule to attract shared
electrons to itself is called _______.
58. Compare & contrast single, double, and triple bonds.
59. Atoms having greatly differing electronegativities are
expected to form _________ bonds.
60. Metallic bonds can be described as metal atoms
surrounded by a __________ ___ __________
61. According to the Octet Rule, chemical bonds form
because atoms gain, lose, or share electrons to have
a full outer energy level ( __ electrons in most
atoms). What is the difference between an ionic
compound and a covalent compound?
62. List general characteristics of ionic compounds.
63. Why is it more difficult to list general characteristics of
covalent compounds.
64. Draw Lewis dot diagrams for the following
compounds:
a. CBr4
b. Li2S c. CO2
65. For water,
a. Determine the general VSEPR form (ABxEy)
b. Draw the Lewis dot diagram.
c. Draw the geometric structure indicating a 3-D
structure.
d. Indicate the name of the molecular shape.
e. Indicate the polarity of the molecule.
66. Explain what VSEPR stands for and how VSEPR
theory is used to predict the shape of molecules.
Chapter 7: Chemical Formulas and Chemical Compounds
67. How many atoms of each element are shown in each compound?
a. CaC2O4
c. Pb(C2O4)2
b. Zn(NO3)2
d. Li3PO4
68. State the number of molecules / formula units that are represented by each of the following.
How many atoms of each element are shown in each?
compound?
a. 4 AlBr3
c. N2O4
b. 2 Fe(NO3)2
d. 3 HBr
69. Classify the following ions as either a monatomic or
polyatomic.
+3
-1
a. Al
d. H
+2
-1
b. Hg2
e. MnO4
-2
-2
c. CO3
f. O
70. Classify the following ions as either cations or anions.
+3
+1
a. Al
d. NH4
-1
-2
b. MnO4
e. CO3
-2
+1
c. O
f. Na
71. Write formulas for the following compounds
(HINT: First determine the type of compound - ionic / covalent).
a. calcium bromide
f. tin (IV) oxide
b. magnesium hydroxide
g. silicon dioxide
c. iron (III) sulfate
h. dinitrogen tetroxide
d. hydrogen fluoride
i. hydrogen sulfide
e. potassium sulfite
j. ammonium acetate
72. Write the names for the following compounds
(HINT: First determine the type of compound - ionic / covalent).
a. P4O6
h. MgSO4
b. Cu2CO3
i. CrCl3
c. Zn(MnO4)2
j. NH4OH
d. AuCl3
k. HClO3
e. Li2Cr2O7
l. Cu3(PO4)2
f. Be3P2
m. LiH
g. PbSO4
n. BaCl2
73. Write the formula for copper (II) sulfate pentahydrate.
74. Name the following acids:
a. HCl
b. HClO3
c. HClO2
75. What is the % composition of AgNO3?
76. What is the empirical formula for a compound made up of 66.0% Ba 34.0% Cl?
77. What is the molecular formula for a molecule with empirical formula CH2O and molar mass 120.12 g/mol?
POSSIBLE ESSAY QUESTIONS:
The test will include 2 of these 4 questions. You will choose 1 of those 2 to answer.
You will be asked to answer the question with a well-structured essay, using proper grammar.
Follow every detail in the prompts of each question to earn full credit.
Use sufficient detail to convey understanding, and use proper scientific terminology related to the subject. I will be looking for certain key
terms that must be used to answer each question completely. Review your notes and text to figure out what these are for each topic, and
build your essay around them.
1. Describe what the Hydrogen Line Emission Spectrum is and how it led to Bohr’s Model of the Atom. Use a sketch of
Bohr’s model of the hydrogen atom to help explain the concepts. Use appropriate terminology to earn full credit.
2. Describe the quantum model of the atom. List the 4 quantum numbers and describe the information that is provided by
each quantum number. Draw sketches of 2 types of orbitals. Use appropriate terminology to earn full credit.
3. Describe the three principles that guide the electron configuration of an atom. Demonstrate with an example using arrow
or box notation and spectroscopic notation. Use appropriate terminology to earn full credit.
4. Compare and contrast the ionic, polar covalent, non-polar covalent, and metallic chemical bonds in terms of the electrons
that are involved. Describe properties typical of compounds that are formed from the different types of bonds. Use
appropriate terminology to earn full credit.