PART 1 : MATTER AND MEASUREMENT
1. Solids have a __________ shape and are not appreciably __________.
A) definite, compressible
B) definite, incompressible
C) indefinite, compressible
D) indefinite, incompressible
E) sharp, convertible
2. A separation process that depends on differing abilities of substances to form gases is called
__________.
A) filtration
B) solvation
C) distillation
D) chromatography
E) all of the above are correct
3. In the following list, only __________ is not an example of matter.
A) planets
B) light
C) dust
D) elemental phosphorus
E) table salt
4. The law of constant composition applies to __________.
A) solutions
B) heterogeneous mixtures
C) compounds
D) homogeneous mixtures
E) solids
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5. Which states of matter are significantly compressible?
A) gases only
B) liquids only
C) solids only
D) liquids and gases
E) solids and liquids
6. For which of the following can the composition vary?
A) pure substance
B) element
C) homogeneous mixture
D) heterogeneous mixture
7. In the following list, only __________ is not an example of a chemical reaction.
A) dissolution of a penny in nitric acid
B) the condensation of water vapor
C) a burning candle
D) the formation of polyethylene from ethylene
E) the rusting of iron
8. Gases and liquids share the property of __________.
A) compressibility
B) definite volume
C) incompressibility
D) indefinite shape
E) definite shape
9. Which one of the following is (are) not an intensive property?
A) density
B) temperature
C) melting point
D) mass
E) volume
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10. Which of the following are chemical processes?
A) rusting of a nail
B) freezing of water
C) decomposition of water into hydrogen and oxygen gases
D) compression of oxygen gas
11. Precision refers to __________.
A) how close a measured number is to other measured numbers
B) how close a measured number is to the true value
C) how close a measured number is to the calculated value
D) how close a measured number is to zero
E) how close a measured number is to infinity
12. Accuracy refers to __________.
A) how close a measured number is to zero
B) how close a measured number is to the calculated value
C) how close a measured number is to other measured numbers
D) how close a measured number is to the true value
E) how close a measured number is to infinity
13. Expressing a number in scientific notation __________.
A) changes its value
B) removes ambiguity as to the significant figures
C) removes significant zeros
D) allows to increase the number's precision
E) all of the above
14. Of the objects below, __________ is the densest.
A) an object with a volume of 2.5 L and a mass of 12.5 kg
B) an object with a volume of 139 mL and a mass of 93 g
C) an object with a volume of 0.00212 m3 and a mass of 4.22 × 104 mg
D) an object with a volume of 3.91 × 10-24 nm3 and a mass of 7.93 × 10-1 ng
E) an object with a volume of 13 dm3 and a mass of 1.29 × 103 g
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LECTURE 2: ATOMS
1. Of the following processes, which one changes the atomic number?
A) Alpha emission
B) Beta emission
C) Electron capture
D) Positron emission
E) All of these processes change the atomic numbers
2. All atoms of a given element have the same
A) Mass number.
B) Number of nucleons.
C) Atomic mass.
D) Number of neutrons.
E) Atomic number.
3. The atomic number indicates __________.
A) The number of neutrons in a nucleus
B) The total number of neutrons and protons in a nucleus
C) The number of protons or electrons in a neutral atom
D) The number of atoms in 1 g of an element
E) The number of different isotopes of an element
4. Elements in Group 2A are known as the __________.
A) alkaline earth metals
B) alkali metals
C) chalcogens
D) halogens
E) noble gases
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5. Elements in Group 6A are known as the __________.
A) Alkali metals
B) Chalcogens
C) Alkaline earth metals
D) Halogens
E) Noble gases
6. __________ are found uncombined, as monatomic species in nature.
A) Noble gases
B) Chalcogens
C) Alkali metals
D) Alkaline earth metals
E) Halogens
7. The formula of a salt is XCl2 . The X-ion in this salt has 28 electrons. The metal X is __________.
A) Ni
B) Zn
C) Fe
D) V
E) Pd
8. Which one of the following is not one of the postulates of Dalton's atomic theory?
A) Atoms are composed of protons, neutrons, and electrons.
B) All atoms of a given element are identical; the atoms of different elements are different and have
different properties.
C) Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are
neither created nor destroyed in chemical reactions.
D) Compounds are formed when atoms of more than one element combine; a given compound always
has the same relative number and kind of atoms.
E) Each element is composed of extremely small particles called atoms.
9. Consider the following selected postulates of Dalton's atomic theory:
A) Each element is composed of extremely small particles called atoms.
B) Atoms are indivisible.
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C) Atoms of a given element are identical.
D) Atoms of different elements are different and have different properties.
Which of the postulates is(are) no longer valid?
10. The gold foil experiment performed in Rutherford's lab __________.
A) Confirmed the plum-pudding model of the atom
B) Led to the discovery of the atomic nucleus
C) Was the basis for Thompson's model of the atom
D) Utilized the deflection of beta particles by gold foil
E) Proved the law of multiple proportions
11. Cathode rays are deflected away from a negatively charged plate because __________.
A) They are not particles
B) They are positively charged particles
C) They are neutral particles
D) They are negatively charged particles
E) They are emitted by all matter
12. The molecular formula of a compound is always __________ the empirical formula.
A) More complex than
B) Different from
C) An integral multiple of
D) The same as
E) Simpler than
13. The species __________ contain(s) 16 neutrons
A) 31P
B) 32S
C) 35Cl
D) 36Kr
E) 16O
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14. Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon
for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g
of hydrogen, a ratio of 4:1 by mass. This is a statement of the law of __________.
A) Constant composition
B) Multiple proportions
C) Conservation of matter
D) Conservation of mass
E) Octaves
15. Different isotopes of a particular element contain different numbers of __________.
A) Protons
B) Protons and neutrons
C) Protons, neutrons, and electrons
D) None of the above is correct.
16. An unknown element is found to have three naturally occurring isotopes with atomic masses of
35.9675 (0.337%), 37.9627 (0.063%), and 39.9624 (99.600%). Which of the following is the unknown
element?
A) Ar
B) K
C) Cl
D) Ca
E) None of the above could be the unknown element.
17. An atom of 15N contains __________ neutrons.
A) 7
B) 22
C) 8
D) 10
E) 15
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18. In the Rutherford nuclear-atom model, __________.
A) The heavy subatomic particles, protons and neutrons, reside in the nucleus
B) The three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same
mass
C) The light subatomic particles, protons and neutrons, reside in the nucleus
D) Mass is spread essentially uniformly throughout the atom
E) The three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same
mass and mass is spread essentially uniformly throughout the atom
19. Which atom has the greatest number of neutrons?
A) Carbon-14
B) Nitrogen-14
C) Oxygen-16
D) Argon-39
E) Potassium-39
20. Which atom has the smallest number of neutrons?
A) Carbon-14
B) Nitrogen-14
C) Oxygen-16
D) Neon-19
PART 5: PERIODIC TABLE
1. Elements __________ exhibit similar physical and chemical properties.
A) with similar chemical symbols
B) with similar atomic masses
C) in the same period of the periodic table
D) on opposite sides of the periodic table
E) in the same group of the periodic table
2. Which pair(s) of elements would you expect to exhibit the greatest similarity in their physical and
chemical
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properties?
A) H, Li
B) Ne, Kr
C) Ca, Ni
D) Ga, Ge
E) O, Se
3. Which pair(s) of elements would you expect to exhibit the greatest similarity in their physical and
chemical
properties?
A) O, S
B) C, Si
C) K, Ca
D) H, He
E) N, P
4. Of the choices below, which one is (are) not an ionic compound?
A) PCl5
B) MoCl6
C) RbCl
D) H2SO4
E) NaCl
5. Which one of the following is (are) most likely to lose electrons when forming an ion?
A) F
B) P
C) Rh
D) Sr
E) N
6. Elements in the same group of the periodic table typically have __________.
A) similar mass numbers
B) similar physical properties
C) similar chemical properties
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D) similar atomic masses
7. An element in the upper right corner of the periodic table __________.
A) is either a metal or metalloid
B) is definitely a metal
C) is either a metalloid or a non-metal
D) is definitely a non-metal
E) is definitely a metalloid
8. An empirical formula always indicates __________.
A) which atoms are attached to which in a molecule
B) how many of each atom are in a molecule
C) the simplest whole-number ratio of different atoms in a compound
D) the isotope of each element in a compound
E) the geometry of a molecule
9. Atomic radius generally increases as we move __________.
A) down a group and from right to left across a period
B) up a group and from left to right across a period
C) down a group and from left to right across a period
D) up a group and from right to left across a period
E) down a group; the period position has no effect
10. The first ionization energies of the elements __________ as you go from left to right across
a period of the periodic table, and __________ as you go from the bottom to the top of a group
in the table.
A) increase, increase
B) increase, decrease
C) decrease, increase
D) decrease, decrease
E) are completely unpredictable
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11. The most common and stable allotrope of sulfur is __________.
A) S
B) S2
C) S4
D) S8
E) Sulfur does not form allotropes.
12. The first noble gas to be incorporated into a compound was __________.
A) Ar
B) Kr
C) He
D) Ne
E) Xe
13. All the elements in group 8A are gases at room temperature. Of all the groups in the
periodic table, only group_________ contains examples of elements that are gas, liquid, and
solid at room temperature.
A) 2A
B) 1A
C) 7A
D) 5A
E) 6A
14. In general, as you go across a period in the periodic table from left to right:
(1) the atomic radius __________;
(2) the electron affinity becomes __________ negative; and
(3) the first ionization energy __________.
A) decreases, decreasingly, increases
B) increases, increasingly, decreases
C) increases, increasingly, increases
D) decreases, increasingly, increases
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E) decreases, increasingly, decreases
15. Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?
A) Mg > Na > P > Si > Ar
B) Ar > Si > P > Na > Mg
C) Si > P > Ar > Na > Mg
D) Na > Mg > Si > P > Ar
E) Ar > P > Si > Mg > Na
16. Screening by the valence electrons in atoms is __________.
A) less efficient than that by core electrons
B) more efficient than that by core electrons
C) essentially identical to that by core electrons
D) responsible for a general increase in atomic radius going across a period
E) both more efficient than that by core electrons and responsible for a general increase in atomic radius
going across a period
17. The atomic radius of main-group elements generally increases down a group because __________.
A) effective nuclear charge increases down a group
B) effective nuclear charge decreases down a group
C) effective nuclear charge zigzags down a group
D) the principal quantum number of the valence orbitals increases
E) both effective nuclear charge increases down a group and the principal quantum number of the
valence orbitals increases
18. Which one of the following atoms has the largest radius?
A) O
B) F
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C) S
D) Cl
E) Ne
19. Of the choices below, which gives the order for first ionization energies?
A) Cl > S > Al > Ar > Si
B) Ar > Cl > S > Si > Al
C) Al > Si > S > Cl > Ar
D) Cl > S > Al > Si > Ar
E) S > Si > Cl > Al > Ar
20. Of the following species, __________ has the largest radius.
A) Rb+
B) Sr2+
C) Br-
D) Kr
E) S2-
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