Section 1 The Nature of Science

1. When gathering glassware and equipment for an experiment, you should

a. read all directions carefully to know what equipment is necessary
b. examine all glassware to check for chips or cracks
c. clean any glassware that appears dirty
d. all of the above

2. In the event of a laboratory emergency, you should

a. panic
b. run quickly towards the exit
c. alert the instructor and calmly evacuate the lab
d. wave your arms and scream

3. If you get chemicals in your eye, you should

a. have your partner blow in your eye until it feels better
b. blink until it feels better
c. splash water in your eyes from the sink
d. use the eyewash station for fifteen minutes, holding your eyes open
the whole time

4. Long hair in the laboratory must be

a. held away from the equipment with one hand
b. always neatly groomed
c. tied back or kept entirely out of the way with a hair band, hairpin, or
other confining device
d. cut short

5. Flammable materials, like alcohol, should never be dispensed or used near

a. an open door c. a sink
b. an open flame d. another student

6. You are heating a piece of glass and now want to pick it up. You should
a. use a rag or paper towel
b. pick up the end that looks cooler
c. use tongs
d. pour cold water on it
7. Scientists are trying to find the temperature of a lake. To get an accurate
temperature, they should measure it
a. again and again until they get the same result.
b. only once and only in the center.
c. several times at different places.
d. several times in the same place

8. While working on a class chemistry experiment, Victor dropped a glass test tube
filled with unknown liquid. What should Victor do first?
a. put on gloves c. sweep up the broken glass
b. inform the teacher d. clean up the spilled
chemical

9. Which set of tools will provide the most precise measurements for calculating the
density of an irregularly shaped rock?
a. flask and beaker
b. flask and balance
c. balance and graduated cylinder
d. beaker and graduated cylinder

10. What is the most appropriate tool for measuring 30.0 mL of a sodium chloride
solution?

a. the beaker because it is more stable and the liquid is less likely to spill
b. the beaker because it is calibrated to hold large amounts of liquid
c. the graduated cylinder because it is calibrated to measure the liquid
more precisely
d. the graduated cylinder because it will be nearly filled with liquid

11. Anhydrous copper(II) sulfate is a gray-white powder. When a student heated 250
g of bright blue copper(II) sulfate pentahydrate(CuSO₄ •5H₂O ) in a test tube, the
sample crumbled and turned gray white. The sample also lost 90 g. Based on
this information, what is the most acceptable conclusion?
 a. The color of the sample changed when copper reacted with sulfate ions.
b. The mass of the sample decreased after the copper(II) sulfate evaporated.
c. The sample became dehydrated when it was heated.
d. The sample went from the solid phase to the gaseous phase.

12. Which of the following observations is quantitative?

a. The liquid turns blue litmus paper red.
b. The liquid boils at 100⁰C.
c. The liquid tastes bitter.
d. The liquid is cloudy.

13. A plausible explanation of a body of observed natural phenomena is a scientific

a. control. c. law.
b. experiment. d. theory.

14. The symbols for units of length in order from largest to smallest are
a. m, cm, mm, km. c. km, mm, cm, m.
b. mm, m, cm, km. d. km, m, cm, mm.

15. The density of aluminum is 2.70 g/cm³. What is the mass of a solid piece of
aluminum with a volume of 1.50 cm³?
a. 0.556 g c. 4.05 g
b. 1.80 g d. 4.20 g

16. 0.25 g is equivalent to

a. 250 kg. c. 0.025 mg.
b. 250 mg. d. 0.025 kg.

17. How many minutes are in exactly 1 week?

a. 168 min c. 10,080 min
b. 1440 min d. 100,800 min

18. In a paper chromatography experiment, ink(s) are applied to a piece of paper and
placed in a special solvent. What would happen to a ‘dot’ of ink that was NOT
attracted to the solvent?
a. The ink would separate into its components
b. The ink would not move
c. The ink would change colors
d. The ink would flow up the paper
Section 2 Atoms and Nuclear Reactions

19. According to Dalton's atomic theory, atoms

a. are destroyed in chemical reactions.
b. can be divided.
c. of each element are identical in size, mass, and other properties.
d. of different elements cannot combine.

20. Experiments with cathode rays led to the discovery of the

a. proton. c. neutron.
b. nucleus. d. electron.

21. Rutherford's experiments led him to conclude that atoms contain massive central
regions that have
a. a positive charge. c. no charge.
b. a negative charge. d. both protons and
electrons.

22. An atom is electrically neutral because

a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.

23. Isotopes are atoms of the same element that have different
a. principle chemical b. numbers of neutrons.
properties. c. numbers of protons.
d. numbers of electrons.

24. The least massive particle in an atom is the

a. proton. c. electron.
b. neutron. d. None of the above.
25. The total number of protons and neutrons in the nucleus of an atom is its
a. Atomic number
b. Mass number
c. Avogadro’s number
 d. Average atomic mass
26. The atomic theories of Dalton, Thompson, Rutherford, and Bohr all support which
of the following statements?
a. Atoms are mostly composed of empty space.
b. All matter is composed of tiny, discrete particles called atoms.
c. Electrons orbit the nucleus of an atom at distinct energy levels.
d. Atoms are composed of positively and negatively charged particles.

27. Atoms can be considered the basic building blocks of matter. Which of the
following statements best describes how Atom X and Atom Y are related?

a. X is an ion and Y is a neutral atom

b. X and Y are different elements
c. X is neon and Y is fluorine
d. X and Y are isotopes of the same element.

28. Which element on the periodic table has a total of 16 protons?

a. germanium (Ge) c. oxygen (O)
b. phosphorus (P) d. sulfur (S)

29. Isotopes of an element have different numbers of

a. protons. c. electrons.
b. neutrons. d. positron

30. Which statement best describes the Bohr model of the atom?
a. Electrons are arranged in energy clouds.
b. Electrons have properties similar to waves.
c. Electrons orbit around the nucleus in set paths.
d. Electrons make up most of the mass of an atom.

31. What is Avogadro’s number?

a. How many moles are in 1 particle
b. How many moles are in 1 gram
c. How many grams are in 1 mole
d. How many particles are in 1 mole

32. How many grams are in 1 mole of Nitrogen?

a. 8.43x1024 g
 b. 14.01 g
c. 2.3x10-23 g
d. 1 g

33. 49.35 g of Mg is how many moles?

a. 1 mole
b. 2.030 moles
c. 2.00 moles
d. 8.198x10-23 moles
Section 3 Electrons

34. The highest point of a wave is called what?

a. peak
b. crest
c. trough
d. point

35. Wavelength is the measured distance between what two points?

a. resting point to crest
b. resting point to peak
c. peak to peak
d. crest to crest

36. Given that the speed of light is ~ 3.00x108m/s what is the frequency of a wave if
the wavelength is 7.3x10-7 m? Use the equation c=𝝀𝞶.
a. 4.1x1014 Hz
b. 4.11x1014 Hz
c. 2.4x10-15 Hz
d. 2.43x10-15 Hz
37. The energy of a photon is related to its
a. mass. c. frequency.
b. speed. d. size.

38. The region outside the nucleus where an electron can most probably be found is
the
a. electron configuration. c. s sublevel.
b. quantum. d. electron cloud.

39. The total number of orbitals that can exist in the second energy level is
a. 2
 b. 3
c. 4
d. 8

40. The set of 3 orbitals that are dumbbell shaped and directed along the x, y, and z
axes are called
a. d orbitals. c. f orbitals.
b. p orbitals. d. s orbitals.

41. "Orbitals of equal energy are each occupied by one electron before any is
occupied by a second electron, and all electrons in singly occupied orbitals must
have the same spin" is a statement of
a. the Pauli exclusion b. the Aufbau principle.
principle. c. the quantum effect.
d. Hund's rule.

42. The element with the electron configuration

1s² 2s² 2p⁶ 3s² 3p²

a. Mg c. S
b. C d. Si
43. The figure below represents the periodic table and the location of four different
elements on the table.

a. W c. Y
b. X d. Z

44. Which illustration represents the region in which an electron of a hydrogen atom
is most likely found at ground state?
 a. c.

b. d.

45. Which of the following pieces of evidence best supports Bohr's idea that
electrons occupy specific energy levels within an atom?
a. Sodium atoms become positive ions when they lose electrons.
b. Each element emits a unique bright-line spectrum when it falls from
an excited state to a ground state.
c. Beryllium atoms bombarded with alpha particles produce beams that are
not influenced by magnetic fields.
d. Each element has physical and chemical properties that are unique to that
elementand different from those of other elements.

46. What is the total number of electrons in all s orbitals of a neutral atom of
phosphorus?
a. 2 c. 6
b. 4 d. 8

47. How did the quantum mechanical model of the atom improve on Bohr's Atomic
model?
a. by showing that most of the atom is empty space
b. by establishing the probability clouds of the electrons
c. by predicting the particle nature of the electrons
d. by measuring the absorption spectra of discrete orbits

48. The electron configuration of a neutral atom of calcium is shown.

1s2 2s2 2p6 3s2 3p6 4s2

How many valence electrons are in the atom?

a. 2 c. 8
b. 4 d. 20
49. According to the quantum mechanical model of the atom, what is the maximum
number of electrons that can occupy the second energy level?
a. 2 c. 8
b. 4 d. 10

50. Boron has one electron in the 2p orbital. In which of these orbitals is the electron
likely to be found?

a. c.

b. d.

51. Which of the following statements best explains why potassium (K) react easily
with bromine (Br)?
a. Potassium and bromine both have valence electrons in the fourth energy
level.
b. Potassium and bromine have the same number of electrons in their
highest energy level.
c. Potassium has one electron in its highest energy level, and bromine
needs one electron to complete its highest energy level.
d. Potassium needs one electron to complete its highest energy level, and
bromine has an extra electron in its highest energy level.

52. What types of ions have names ending in -ide?

a. Only metals
b. Only cations
c. Only anions
d. Only gaseous ions

53. Compounds ending in -ite or -ate indicates that the compound contains ____?
a. Fewer electrons than protons
 b. More electrons than protons
c. Only 2 elements
d. A polyatomic ion

54. Which of the following compounds contains the Mn3+ ion?

a. MnS
b. MnBr2
c. Mn2O3
d. MnO

Section 4 The Periodic Table

55. Which of the following elements has the greatest ionization energy?
a. Ga c. K
b. As d. Bi

56. All the alkali metal elements are found on the periodic table in
a. Period 1. c. Period 2.
b. Group 1. d. Group 2.

57. Which of the following elements is not a metal?

a. K c. Fr
b. H d. Na

58. Which periodic group or family of elements is NOT correctly matched with its
common family name?
a. Group 18: noble gases
b. Group 2: alkaline-earth metals
c. Group 17: halogens
d. Group 3: alkali metals

59. Mendeleev organized the chemical elements based on their

a. atomic numbers. c. mass.
b. charges. d. symbols.

60. Which of the following elements is a transition metal?

a. Sulfur c. Iron
b. Calcium d. Sodium

61. Which element has the highest electronegativity?

 a. nitrogen c. fluorine
b. iodine d. selenium

62. Which pair of arrows correctly represents how atomic radii change, from smallest
radius to largest radius, on the periodic table of the elements?

a. c.

b. d.

63. Early in the history of the periodic table, a scientist observed the relationships
between element characteristics and atomic mass. The scientist used this
information to predict the existence of unknown elements with specific atomic
masses and characteristics. How was this information applied by modern
scientists?
a. Scientists were able to predict the properties of new elements.
b. Scientists were able to change the atomic makeup of elements.
c. Scientists were able to make computer parts because of the unpredictable
properties of silicon.
d. Scientists were able to create new elements with unpredictable physical
and chemical properties.

64. Which of the following elements has the same Lewis dot structure as silicon?
a. germanium (Ge) c. arsenic (As)
b. aluminum (Al) d. gallium (Ga)

65. Which of the following atoms has six valence electrons?

a. Sulfur (S) c. Silicon (Si)
b. Magnesium (Mg) d. Argon (Ar

Section 5 Intro to Bonding, Ionic and Metallic

66. The electrons involved in the formation of a chemical bond are called
a. dipoles. b. s electrons.
 c. Lewis electrons. d. valence electrons.

67. If the atoms that share electrons have an unequal attraction for the electrons, the
bond is called
a. nonpolar. c. ionic.
b. polar. d. dipolar.

68. The ions in most ionic compounds are organized into a

a. molecule. c. Lewis structure.
b. polyatomic ion. d. Lattice structure.

69. If a material can be shaped or extended by physical pressure, such as

hammering, which property does the material have?
a. Conductivity c. Malleability
b. Ductility d. Luster

70. Which of these describes how gallium forms a 3⁺ ion?

a. The gallium loses 3 electrons.
b. The gallium loses 3 protons.
c. The gallium gains 3 electrons.
d. The gallium gains 3 protons.

71. Which compound forms when aluminum bonds with fluorine?

a. AlF c. AlF3
b. AlF2 d. Al3F

72. Which diagram shows the correct formation of gallium selenide?

c.

a.

d.
b.
 73. In metals, the valence electrons
a. are attached to particular positive ions.
b. are immobile.
c. are shared by all of the atoms.
d. form covalent bonds.

74. What is the name of the compound PbO2? (** O2- and Pb4+ form Pb2O4 which is
simplified**)
a. lead oxide c. lead oxide (II)
b. lead (II) oxide d. lead (IV) oxide

75. What is the correct name for the compound with the chemical formulaNH4NO3?
a. hydro-nitrogen oxide c. amminia mononitrate
b. nitro-hydrogen nitrate d. ammonium nitrate

76. Limestone is a naturally occuring form of calcium carbonate. The correct formula
for for limestone is
a. Ca(CO3)2 c. Ca2CO3
b. CaCO3 d. Ca2(CO3)2

77. According to the periodic table, which statement correctly describes the change
from a neutral atom of an element to its ion?
a. A fluorine atom forms an F- ion by losing one electron.
b. A sodium atom forms a Na+ ion by losing two electrons.
c. A magnesium atom forms a Mg2+ ion by gaining two electrons
d. A phosphorus atom forms a P3- ion by gaining three electrons.

78. Bonding in molecules that cannot be correctly represented by a single Lewis

structure is
a. polyatomic
b. single bonding
c. double bonding
d. resonance

Unit 6 Covalent Compounds

79. Name the molecule SO3
a. sulfur trioxide c. selenium trioxide
b. silver trioxide d. sulfur oxide

80. What is the formula for dinitrogen trioxide?

a. Ni2O3 c. N2O6
b. NO3 d. N2O3

81. The following molecule has 3 steric regions and 0 unshared pairs. What shape is
it?

a. trigonal pyramidal c. trigonal bipyramidal

b. tetrahedral d. trigonal planar

82. The following molecule has 4 electron regions and no unshared pairs. What
shape is it?

a. tetrahedral c. bent
b. square d. square pyramidal

83. The following molecule has 5 steric regions and no unshared pairs. What shape
is it?
 a. tetrahedral c. trigonal linear
b. octahedral d. trigonal bipyramidal

84. The following molecule has 6 steric regions and no unshared pairs. What shape
is it?

a. tetrahedral c. septahedral
b. octahedral d. pentahedral

85. What is the formula for diphosphorus pentoxide?

a. P2PeO5 c. P2O4
b. PO5 d. P2O5

86. Which of the following Lewis dot structures represents the compound methane
(CH4)

a.
c.

b.
d.

87. Two elements in a molecule have the same electronegativity values. Which of the
following most likely holds the elements together and why?
a. an ionic bond, because electrons transfer from one element to another
 b. a nonpolar covalent bond, because the elements share the electrons
equally
c. a polar covalent bond, because the elements do not share electrons
equally
d. an intermolecular force, because elements do not form a chemical cond

88. Which of the following occurs in an ionic bond?

a. Two ions share electrons
b. Two ions share protons
c. Similarly charged ions attract.
d. Oppositely charged ions attract.

89. The illustration below shows two atoms of a fictional element (M) forming a
diatomic molecule. What type of bonding occurs between these two atoms?

a. covalent c. nuclear
b. ionic d. polar

90. What is the name of the acid with the formula HCl?
a. Chloric acid c. Hydrochloric acid
b. Perchlorous acid d. Chlorous acid
91. What is the name of the acid with the formula H2SO3?
a. Sulfic acid c. Sulfurous acid
b. Sulfuric acid d. Hydrosulfuric acid?

92. What is the formula for Acetic Acid?

a. HC2H3O2 c. H2C2H3O2
b. H(C2H3O2)2 d. H3C2H3O2

93. What is the formula for aluminum hydroxide?

a. AlOH c. AlOH3
b. Al3OH d. Al(OH)3