Date:
Chemistry Midyear Exam Review Topics 2014-2015
Thursday January 29, 2014
Juniors: 8:00 AM – 11:00 AM then to Technical Area
Seniors: 11:50AM – 2:30PM from Technical Area in the morning
Chapters: 1-4, 6, 18 : Holt: Chemistry
Weighting: 20% of first semester grade (~13% of grade for the whole year)
Format: 100 multiple choice questions (Honors 120 multiple choice questions)
Provided:
periodic table, polyatomic ions, electronegativity values
Bring:
calculator, # 2 pencils, eraser
In the following packet are the topics studied during the first semester of chemistry. Sample test questions
are also included.
Study Resources:
 Your worksheets, your labs (Chromatography, Half-Life, Flame Test, Periodic Trends, etc.), your
tests (You may come in and look them over). You will see some of these questions on your
midterm.

Content Review problems at the end of each chapter.
 The SparkNotes website has a chemistry section at
http://www.sparknotes.com/chemistry
 Questions from previous MCAS tests are archived on the internet at
http://www.doe.mass.edu/mcas/testitems.html . They are organized by year, and then by subject
within each year.
Ways to Study:
 Start studying NOW.
 Review in short study sessions.
 Quiz a friend over the material and practice explaining topics to each other.
 DO NOT look at the answers until you have tried the problems! If you get stuck DO NOT look at
the answers until you have tried as hard to get yourself unstuck as you would try in the real exam.
 Schedule study sessions with friends (and chemistry teachers). Try explaining how to do the
problems to each other—by the time you’ve finished explaining something completely, you’ll
understand it well.
 Review the “objectives” at the beginning of each chapter and the summaries at the end. Quiz
yourself. Anything you don’t remember or have trouble with is something you need to re-read,
study, or ask about.
Go to sleep no later than 10:00 P.M. the night before the exam! Then eat a Healthy breakfast. Yes, really!
You are much more likely to think clearly during the test if you are well rested and relaxed.
Chapter Topics
Chapter 1: The Science of Chemistry and 2: Matter & Energy
 What is chemistry?
 Percent error calculations
 Lab Safety
 Density problems
 Scientific Method
 Temperature scales (Kelvin – Celsius)
 Metric and SI units (prefixes)
 Categorize matter (heterogeneous,
compound, etc)
 Accuracy and Precision
 Techniques to separate mixtures,
 Measuring
Chromatography lab
 What are significant figures?

Four states of matter
 Rules of significant figures (honors)

Chemical and Physical properties &
 Significant Figures in calculations
changes
(honors)

Laws of conservation of energy, matter
 Scientific Notation
Book problems: p. 9 #3,4,5,12,13,14, p.14 #1-3, p.19 #3, 6-12, p.28 # 1-8, 13, 14, p. 31 #1-15, p. 32 # 21
23, 26-28, p.45 # 1,-3, 5-10, p.53 #1-7, p.59 # 1,2 p.63 #1,4-6,8,9, p.66#17, 19, p.67#20-26, 30-34, 36-40
Chapters: 3 Atoms & Moles and 18 Nuclear Chemistry:
 Models of atom
 Isotopes
 Laws: Multiple Proportions, Definite
 Radioactivity and stability of nucleus
Composition
 Nuclear reactions (alpha, beta, gamma)
 Development of atom
 Fusion, Fission
(history/scientists/experiments)
 Half life, Carbon dating (half-Life lab)
 Dalton’s Atomic Theory
 Write Electron Configurations
 Rutherford’s experiment
 Valence electrons and Octet Rule
 Structure of atom
 Predict charge of ions formed from
 Subatomic particles
Periodic Table
 Atomic number, mass number vs.
 Noble gases – stability
average atomic mass
 Write orbital diagrams
Book problems: p.78 #1-6, p.86 # 1-4, p.89 # 1, 2, & 1-6, p. 99 # 1, 2, 4-8, p.1071-11, 25, p.108# 30-35,
p.109 # 52, 55, 65, 66, p. 653 #1-4, p.657 #2 ,5, p.660 # 3, p.662 # 1-3, p.669 #4, 5, 8, 18, 19, p.670 # 34
Chapter 4: The Periodic Table
 Historical development of modern periodic table
 Identify different parts/ families on periodic table
 Write electron configuration of element based on location on periodic table
o Aufbau, Pauli Exclusion principles
o Hund’s Rule
 Predict properties of elements
 Know 4 trends across period and down family:
o Atomic radius
o Ionic radius
o Ionization energy
o Electronegativity
 Flame test lab and light emission
 Atomic Emission Spectra
 Quantum theory
o Describe energy levels, sublevels, orbitals & electron spin
Book problems: p. 122 # 4-7, 12, 13, p.131 # 1, 5, 7, 13 p.141 #1, 3, 5, 10, 13, p.150# 1-3,7, 9, 12, 14, 21,
31, 32, , 41, p.15359-64, p.155 # 11,12
Chapter 5: Ions & Ionic Compounds and Chapter 6: Covalent Compounds
 Valence electrons and Octet Rule
 Predict charge of ions formed from Periodic Table
 Noble gases – stability
 Transition metals – how to determine charge from name or formula
 Lewis Dot diagrams
 Describe Ionic bonding, Covalent bonding, metallic bonding
 Identify, name and write cations, anions, polyatomic ions, & the 7 diatomic elements
 Identify if compound is ionic or molecular
 Lewis dot diagrams/structures of covalent molecules
 Shapes (geometry) of covalent molecules, VSEPR Theory
 Polarity of covalent bonds and molecules
 Write names & formulae for ionic, covalent, and acid compounds
Book problems: p.165 # 1-4, 7,8,10,11,12 p.175 # 1, 2, p.180 #2-8 but not 8b, p. 183 # 1-4, 7, 17-19,
p.202, # 1, p.205 # 1,2, p.207 # 3,6,7,9,10, p. 213 # 1,2,4,6-8, p.216 # 8,9,11,15,16,17,20,22,25-27,30,32,
33, 35,38,39, p.220 #3
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Midyear Exam Review Questions
1. Chemistry is best defined as the study of
a. The structure of matter
b. All substances and the changes that they can undergo
c. The substances found on the periodic table and the compounds they form
d. What happens when two elements are mixed together
2. Which group of measurements is the most precise? (Each group of measurements is for a different
object).
a.
2 g,
3 g,
4g
b.
2.0 g, 3.0 g, 4.0 g
c.
2.0 g, 2.5 g, 3.0 g
d.
2.0 g, 3.0 g, 4.0 g, 5.0 g
3. Measurements which closely agree with the accepted value are said to be
a. precise
b. reliable
c. significant
4. The gram is a unit of
a. length
b. area
c. mass
d. accurate
d. volume
5. The number 149,000,000 is usually written in scientific notation as
a.
0.149 × 109
b.
1.49 × 108
c.
14.9 × 107
d.
149 × 106
e.
1490 × 105
6. The correct scientific notation for 0.000850 is
a. 8 × 10 −3
b. 850 × 10−6
c. 85 × 10−5
d. 8.50 × 10 −4
7. In the measurement 0.503 L, which digit is the estimated digit?
a. 5
b. the 0 between 5 and 3
c. 3
d. the 0 to the left of the decimal point
e. there is no estimated digit in this measurement
8. How many significant figures are there in the measurement 0.0035 kg?
a. 2
b. 3
c. 4
d. 5
e. this cannot be determined
9. How many of the zeroes in the measurement 0.00004020 meters are significant?
a. 1
b. 2
c. 6
d. 7
10. How many significant figures does the measurement 0.0023 m have?
a. 1
b. 2
c. 3
d. 4
________________________________________________________________________
Solve the following and round to the proper number of significant figures (HONORS)
11. 20.5 m + 80.36 m =
a. 101 m
b. 100.9 m
c. 100. m
d. 100.86 m
e. 5
12. 4.5 m × 347 m =
a. 1561.5 m2
b. 1562 m2
c. 1560 m2
d. 1500 m2
e. 1600 m2
________________________________________________________________________
3
13. Most student thermometers have an uncertainty of 0.2 Celsius degrees.
Which is the proper reading of the thermometer shown in the illustration at the right?
a. l6. °C b. 16.4 °C
c. 16.40 °C
d. 16.45 °C
14. A student reads a balance as 38.81 g. The correct reading is 38.41 g.
What is the percent error?
a. 0.0104%
b. 0.104%
c. 0.400%
d. 1.04%
15. Which temperature on the Celsius scale corresponds to 273 K on the Kelvin
scale?
a. 0 °C
b. 260 °C
c. 273 °C
d.
373°C
e.
546 °C
16. Which of the following is a statement of the law of conservation of energy?
a. Energy must be conserved in order to have enough energy for the future
b. In chemical processes, it is best to conserve as much energy as possible
c. In any process, energy is neither created nor destroyed
d. Energy cannot be transformed from one kind of energy to another.
17. What are the parts of the atom?
a. proton with positive charge, neutron with negative charge, electron with neutral charge
b. proton with positive charge, neutron with neutral charge, electron with negative charge
c. proton with neutral charge, neutron with negative charge, electron with positive charge
d. proton with negative charge, neutron with positive charge, electron with neutral charge
18. Which property would be most helpful in identifying a substance?
a. mass
b. state
c. volume
d. melting point
19. Which state of matter is characterized by definite shape and definite volume?
a. plasma.
b. liquid
c. solid
d. gas
20. Which of the following is a physical change?
a.
cooking
b. burning
c. rusting
d. crushing
21. A substance that cannot be separated into simpler substances by a chemical change is called a(n)
a. compound
b. mixture
c. element
d. crystal
22. Which of the following is an example of a homogeneous mixture?
a. oil and water
c. sawdust and nails
b. salt and pepper
d. seawater
23. Which of the following is NOT an example of a chemical change?
a. rusting iron
c. cutting paper
b. an apple ripening
d. a piece of wood burning
24. A chemical change must produce which of the following?
a. a mixture
b. an element
c. water d. a new substance
25. A compound:
a. can be separated into its elements by physical means
b. has a variable composition
c. has a constant composition
d. has properties similar to its elements
26. An example of a chemical change is
a.
freezing of water.
b.
burning a match.
c.
boiling carbon tetrachloride.
d.
dissolving alcohol in water.
4
e.
stretching a rubber band.
27. Which involves a chemical change?
a.
powdering sugar
d. condensing steam
b.
magnetizing an iron bar
e. separating cream from milk
c.
exposing photographic film to light
28. The purpose of filtration is to
a. form precipitates.
b. remove water from solutions.
c. separate dissolved ions from the solvent.
d. separate insoluble substances from a solution.
29. When Pb-214 gives off a beta particle, the new nucleus produced is
a. Hg-210
b. Po-218
c. Tl-214
d. Bi-214
30. J. J. Thomson
a. was the first to observe cathode rays
b. determined both the charge and the mass of the electron
c. concluded that the particles in the cathode beam were the same for all
gases
d. could not determine the charge-to-mass ratio of the electron
31. Given the nuclear reaction:
What is X?
a. A proton, 11 p
c. A neutron, 01 n
234
90
Th 
234
91
Pa + X
b. A positron, +10 e
d. A beta particle, −1 0 e
32. Isotopes of an element have a different
a. number of protons
c. atomic number
b. number of electrons
d. mass number
33. The discovery of the electron was made by
a. J.J. Thomson
c. Henri Becquerel
b. Ernst Rutherford
d. Robert Millikan
34. Where in the atom is each particle located?
a. all of them are in the nucleus
b. protons and electrons are in the nucleus, neutrons move around the outside
c. only protons are in the center, electrons move around the outside
d. protons and neutrons are in the center, called the nucleus and electrons move around the outside
in a space called the electron cloud
35. What is the number of electrons of:
a. 51
b. 23
51
23V
7+
c. 30
d. 44
e. 16
36. Which of the following is not a part of Dalton's atomic theory?
a. all elements are composed of atoms
b. atoms are always in motion
c. atoms of the same element are alike in mass and size
d. atoms that combine do so in simple whole number ratios.
37. Nuclear reactions are different from chemical reactions because in nuclear reactions
a. new compounds are formed.
b. atoms are rearranged into new compounds.
5
c. changes in the nuclei of atoms produce different elements.
d. electrons are transferred from one atom to another.
38. Which one of the following is the most penetrating type of radiation given off by radioactive atoms?
a. alpha b. beta c. gamma
d. ultraviolet
39. Suppose a radioactive isotope has a half-life of 16 years. After 48 years a 100 gram sample will be
reduced to
a. 50 g
b. 25 g
c. 12.5 g
d. about 6 g
40. What is the mass number of an atom that consists of 20 protons, 22
neutrons and 20 electrons?
a. 18
b. 20
c. 42
d. 40
41. A chlorine atom (Cl) differs from a chloride ion (Cl −) in that a chlorine atom
a. has a positive nucleus while the ion’s nucleus is negative.
b. has a neutral nucleus while the ion’s nucleus is positive.
c. contains one electron less than the ion.
d. contains one electron more than the ion.
e. contains one proton more in the nucleus.
42. An atom is defined as the smallest part of an element that
a. contains at least one proton, neutron, and electron
b. retains the chemical identity of that element
c. can carry an electric charge
d. is affected in a cathode ray tube
43. Metals have the following properties: (Circle all that apply)
a. conductivity b. brittleness
c. malleability
d. ductility
e. luster
f. negative charges
44. The nucleus of an atom has all of the following characteristics EXCEPT that it
a. is positively charged.
b. is very dense.
c. contains nearly all of the atom’s mass
d. contains nearly all of the atom’s volume.
45. The physicist who determined experimentally both the charge and the mass of a single electron was
a. John Dalton
b. Sir William Crookes
c. J.J. Thomson
d. Robert Millikan
46. The atomic number of an atom is defined as its
a. mass in amu
b. number of electrons
c. number of neutrons
d. number of protons
47. Two atoms are isotopes if they contain
a. different numbers of electrons
b. different numbers of protons, and different numbers of neutrons
c. the same number of protons, but different number of neutrons
d. the same number of neutrons, but different number of protons
48. Dalton’s modern atomic theory was accepted because
a. Aristotle believed in atoms
b. it explained some basic laws of nature
c. it was such a revolutionary idea
49. Rutherford’s gold foil experiment was significant because
a. it demonstrate how alpha particles react with matter
6
b. it discovered the electron
c. it demonstrated that the atom was made up of a dense nucleus and a large empty space that
contained the electrons
d. it discovered the neutron
50. Compared to one atom of 5927 Co, one atom of 5826 Fe contains the same number of
a. protons.
b. nucleons.
c. neutrons.
d.. electrons
218
51. What particle is needed to complete this nuclear reaction: 222Rn 
Po + __________
0
a. 42He α
b.
β
c. H
d. 01n
−1e
52. How many electrons are in a chromium (III) ion, Cr 3+ ? a. 52
b. 27
c. 24
d. 21
53. The metallic elements in the periodic table are located toward the ________ compared to the staircase:
a. right
b. left c. left and the right
54. When a radioactive atom emits an alpha particle, the atom is changed to
one with:
a. a higher mass number and a higher atomic number
b. a lower mass number and a lower atomic number
c. a higher mass number and a lower atomic number
d. a lower mass number and a higher atomic number
55. Identify the set of isotopes below.
a. copper (I) ion and copper (II) ion
b. copper (I) ion and copper atom
c. copper-63 and copper-65
d. copper-63 and nickel-63
56. Circle one from each pair that represents the smaller particle.
a. F or Fb. F or Cl
c. F or C
57. In which state of matter are the particles able to move past each other and moving moderately around
their container?
a. solid
b. liquid
c. gas
d. plasma
e. Bose-Einstein condensate
58. Suppose a radioactive isotope has a half-life of 12 years. If you started with a 100.00 grams sample of
the substance, how many years would it take to reduce the sample to 6.25 g?
a. 12 years
b. 24 ye c.
36 years d. 48 years
e. 93.75 years
59. How are the elements arranged on the periodic table?
a. similarity in size and electrons
b. similarity in properties and atomic number
c. similarity in symbol and protons
d. similarity in date of discovery
60. Which of the following is a nonmetal?
a. Pt
b. Sc
c. V
d. Li
61. What is the energy required to remove an electron from an atom:
a. activation energy
b. electronegativity
c. ionization energy
e. Kr
d. potential energy
62. _____________ is a property that indicates how strongly an atom of an element attracts electrons in a
chemical bond.
a. electronegativity
b. electron affinity
c. ionization energy
d. none of the above
63. As you move down the periodic table from magnesium through barium, the ionization energy
a. remains constant b. decreases.
c. increases.
7
64. The person credited with developing the modern periodic table is
a. Dalton
b. Mendeleev
c. Rutherford
d. Thomson
65. The d block of elements corresponds to which section of the periodic table?
a. transition metals b. alkaline metal c. halogens
d. nonmetals
66. The electron configuration for fluorine is
a. 1s22s22p63s23p5
b. 1s22s22p6
c. 1s22s22p5
d. 1s22p7
67. Which elements tend to have similar properties?
a. elements in the same vertical column.
b. elements in the same horizontal row
c. all of them
d. none of them
68. Which of the following is a noble gas?
a. fluorine
b. nitrogen
c. xenon
d. oxygen
69. As you move across the periodic table from potassium to krypton, in general the atomic radii
a. remain constant
b. decrease
c. increase
70. The radius of the calcium ion is (larger than, smaller than, the same size as) the calcium atom.
a. larger than
b. smaller than c. the same size as
71. What is the charge on the ion that would most readily be formed by chlorine?
a. 1+
b. 2+
c. 1−
d. 2−
72. Which of these ions has the same electron configuration as Ar?
a. Na +
b. Ca+
c. S−
d. Cl−
73. Which of the following is the Lewis dot diagram of the element fluorine?
74. What is the electron configuration of the element Mg?
a. 1s2 2s2 2p2 3s2
c. 1s2 2s2 2p2 3s6
b. 1s2 2s2 2p6 3s2
d. 1s2 2s6 2p2 3s6
75. Which element has the electron configuration of [Ar] 4s2?
a. Ge
b. Ca
c. Na
d. Mg
76. When writing electron configurations, the s block elements on the periodic table are
a. columns 1A and 2A
b. columns 3A to 8A
c. columns 3B to 2B
d. the bottom two rows of the periodic table
77. When the electrons of an element become excited, they
a. jump to a lower energy level
b. jump to a higher energy level
c. emit light
d. jump to a higher energy level and emit light
78. An atomic emission spectrum consists of
a. all the colors of the rainbow
b. all wavelengths of visible light
8
c. a characteristic few colors of visible light, depending on the element
d. the same colors of light as other elements
79. Electrons fill the lowest energy level sublevels first. This is a statement of
a. Hund’s Rule
b. Heisenberg Uncertainty Principle
c. Aufbau Principle
d. Pauli Exclusion Principle
80. The element oxygen has ____ valence electrons. a. 2
b. 4
c. 6
d. 8
81. What are valence electrons?
a. the number of electrons in an atom of an element
b. the total number of electrons in the p sublevel
c. the number of electrons that become excited in an atom
d. the outermost energy level electrons in the atom of an element
82. The element F would most likely
a. gain 1 electron b. lose 1 electron c. gain 7 electrons
d. lose 7 electrons
83. When Sr forms an ion, what charge would it most likely have?
a. +6
b. −6
c. +2
d. −2
84. Noble gases will most likely
a. gain electrons b. lose electrons c. neither gain or lose electrons
85. How many centimeters are contained within 40.3 meters?
a. ]0.403 cm
b. 4.03 cm
c. 403.0 cm
d. 4030 cm
86. A metric unit of mass is the
a. kilogram
b. meter
c. milliliter
87. What is the correct measure for the graduated cylinder below?
a. 5.0 cm3
b. 6.0 cm3
c. 7.0 cm3
d. degree Celsius
d. 7.5 cm3
88. The combining of two smaller massed atoms into one larger massed atom in a nuclear reaction is called
a.
Fusion
b. fission
c. bombardment
d. half life
89. The half-life of an element is
a. half the time it takes for an element to react
b. half the time it takes for an element to decay
c. the time it takes for half of an element to explode
d. the time it takes for half of an element to decay into another element
90. Which of the following statements is true concerning the composition of ionic compounds?
a.
They are composed of anions and cations
b.
They are composed of anions only
9
c.
d.
e.
They are composed of cations only
They are formed from two or more nonmetallic elements
They are formed from two or more metallic elements
91. The Lewis dot diagram of carbon would have ___ dots.
a. 1
b. 2
c. 4
d. 6
92. Which of the following correctly describes a covalent bond?
a. two atoms stay together because of opposite charges that form
b. two atoms stay together because 1 or more electrons have been permanently transferred
between them.
c. two atoms stay together because 2 or more electrons are shared between them
d. two atoms stick together
93. A group of atoms united by covalent bonds is a(n)
a. cation
b. molecule.
c. ionic compound.
94. What is the formula for dinitrogen pentoxide?
a. 2N5O
b. N5O2
c. N2O5
95. What is the name of SiO4?
a. silicon oxygen
d. O5N2
b. silicon oxide
96. What is the name of NH3?
a. mononitrogen trihydrogen
d. octet.
c. silicon tetraoxide
b. nitrogen trihydride
97. What is the formula for xenon heptafluoride?
a. XeF9
b. Xe7F
c. XeFl7
d. silicate
c. ammonium
d. ammonia
d. XeF7
98. While performing a chemistry lab, goggles should be worn
a.
only when the teacher is looking
b.
only when heating a substance
c.
only when using acids and bases
d.
always
99. NH3 is best described as a(n):
a. ionic compound
b. covalent (molecular) compound
c. metallic compound
d. need more information
100. Which has more energy blue light, microwaves, yellow light or radio waves?
a. blue light
b. microwaves c. yellow light d. radio waves
101. Which compound below would have a tetrahedral shape? (hint: draw them out before answering.)
a. CH4
b. H2O
c. BF3
d. AsCl3
102) Which compound below would have polar bonds but be a nonpolar molecule? (hint: draw them out
before answering the question)
a. CH4
b. H2O
c. BF3
d. AsCl3
103) In the Lewis dot diagram of the molecule PF3, phosphorus has
a.
1 bonding pair and 3 nonbonding pair of electrons
b.
2 bonding pairs and 2 nonbonding pair of electrons
c.
3 bonding pairs and 1 nonbonding pair of electrons
d.
4 bonding pairs of electrons
104) A group of atoms united by covalent bonds is a(n)
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a. cation
b. molecule.
c. ionic compound.
d. octet.
105) What is the major determining factor in the shapes of molecules?
a. the charge of each nucleus in the molecule
b. the shielding effect
c. repulsion between valence shell electron pairs
d. the number of energy levels in each atom in the molecule
e. the repulsion of neighboring nuclei
106) What can cause a molecule to be polar?
a. one type of atom in the molecule attracts electrons more than another type of atom in the
molecule.
b. the molecule gives up an electron.
c. the molecule "steals" an electron from another molecule or atom.
d. all of the above.
107) What shape does a molecule of CH4 have?
a. linear
b. pyramidal
c. trigonal planar
108) NH3 is best described as a(n):
a. ionic compound
b. covalent (molecular) compound
d. bent
e. tetrahedral
c. metallic compound
d. need more information
109) Which of the following compounds contains both ionic and covalent bonds?
a. LiBr
b. SO2
c. XeF6
d. Mg3(PO3)2
110) What is the correct name for the compound Cu(C2H3O2)2?
a. copper (IV) acetate b. copper(II) oxalate
c. copper (IV) oxalate
111) What is the name of H3PO3 (aq)?
a. phosphate
b. hydrogen phosphate c. phosphorous acid
112) What is the name of CuCl2?
a. copper chloride
b. copper dichloride
d. copper(II) acetate
d. phosphoric acid
c. copper I chloride
d. copper II chloride
113) What is the formula for strontium carbonate?
a. SrCO3 b. Sr2(CO3)2
c. SrC
d. Sr2CO32
114) What is the shape of a molecule that has a central atom with two lone pairs of electrons and two
bonded atoms?
a. linear
b. tetrahedral
c. trigonal planar
d. bent
e.pyramidal
115) What is the formula for ammonium sulfide?
a. NH3S
b. NH4S
c. NH42S
116) What is the name of HBr?
a. hydrobromic acid b. hydrogen bromine
d. (NH4)2S
c. hydrogen bromide
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e. (NH4)2SO4
d hydrogen monobromide