Download Name________________________ Midterm Review Date

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Midterm Review
1. In which process does a solid change directly
into a vapor?
A) sublimation
C) condensation
B) C2H3
D) C6H9
3. Two substances, A and Z, are to be identified.
Substance A can not be broken down by a
chemical change. Substance Z can be broken
down by a chemical change. What can be
concluded about these substances?
A) Substance A is a compound and substance Z
is an element.
B) Both substances are compounds.
C) Both substances are elements.
D) Substance A is an element and substance Z
is a compound.
4. The element in Group 14, Period 3 on the
Periodic Table is classified as a
A) nonmetal
C) metal
A)
B)
C)
D)
HClO 4 (gram-formula mass = 100. g/mol)
HClO 3 (gram-formula mass = 84 g/mol)
HClO 2 (gram-formula mass = 68 g/mol)
HClO (gram-formula mass = 52 g/mol)
6. Which particles are found in the nucleus of an
atom?
A)
B)
C)
D)
Which particle diagram best represents this same
substance after a physical change has taken
place?
B) metalloid
D) noble gas
5. In which compound is the percent composition
by mass of chlorine equal to 42%?
A)
B)
C)
D)
7. Given the particle diagram representing four
molecules of a substance:
B) deposition
D) solidification
2. What is the molecular formula of a compound
that has a molecular mass of 54 and the empirical
formula C 2H3?
A) C4H6
C) C8H12
Date_______________________
electrons, only
protons and electrons
neutrons, only
protons and neutrons
8. A mixture of crystals of salt and sugar is added to
water and stirred until all solids have dissolved.
Which statement best describes the resulting
mixture?
A) The mixture is homogeneous and can be
separated by filtration.
B) The mixture is homogeneous and cannot be
separated by filtration.
C) The mixture is heterogeneous and can be
separated by filtration.
D) The mixture is heterogeneous and cannot be
separated by filtration.
Midterm Review
9. Which must be a mixture of substances?
A) liquid
C) solid
B) gas
D) solution
10. A sample of an element has a mass of 34.261
grams and a volume of 3.8 cubic centimeters.
To which number of significant figures should
the calculated density of the sample be
expressed?
A) 3
B) 2
C) 4
D) 5
11. Which of these elements has an atom with the
most stable outer electron configuration?
A) Cl
B) Ca
C) Ne
D) Na
12. What is the chemical formula for copper(II)
hydroxide?
A) Cu(OH) 2
C) Cu2(OH)
B) CuOH
D) CuOH2
13. A sample of a gas is contained in a closed rigid
cylinder. According to kinetic molecular theory,
what occurs when the gas inside the cylinder is
heated?
A) The number of gas molecules increases.
B) The number of collisions between gas
molecules per unit time decreases.
C) The volume of the gas decreases.
D) The average velocity of the gas molecules
increases.
14. A sample of helium gas has a volume of 900.
milliliters and a pressure of 2.50 atm at 298 K.
What is the new pressure when the temperature
is changed to 336 K and the volume is
decreased to 450. milliliters?
A) 0.177 atm
C) 14.1 atm
B) 5.64 atm
D) 4.43 atm
15. Which element is a noble gas?
A) krypton
C) manganese
B) chlorine
D) antimony
16. What is the chemical formula for sodium
sulfate?
A) NaSO 4
C) NaSO 3
B) Na2SO 4
D) Na2SO 3
17. Which conclusion is based on the “gold foil
experiment” and the resulting model of the
atom?
A) An atom is mainly empty space, and the
nucleus has a negative charge.
B) An atom has hardly any empty space, and
the nucleus has a negative charge.
C) An atom is mainly empty space, and the
nucleus has a positive charge.
D) An atom has hardly any empty space, and
the nucleus has a positive charge.
18. Which element is an alkali metal?
A) sodium
C) hydrogen
B) calcium
D) zinc
19. Which element has chemical properties that are
most similar to those of calcium?
A) N
B) Sr
C) K
D) Co
20. Which mass measurement contains four
significant figures?
A) 0.431 g
C) 1003 g
B) 0.086 g
D) 3870 g
21. Which trends are observed as each of the
elements within Group 15 on the Periodic Table
is considered in order from top to bottom?
A) Their metallic properties increase and their
atomic radii decrease.
B) Their metallic properties increase and their
atomic radii increase.
C) Their metallic properties decrease and their
atomic radii increase.
D) Their metallic properties decrease and their
atomic radii decrease.
22. Which list consists of types of chemical
formulas?
A)
B)
C)
D)
empirical, molecular, structural
synthesis, decomposition, neutralization
atoms, ions, molecules
metals, nonmetals, metalloids
23. A correct name for N2O3 is
A)
B)
C)
D)
nitrogen (I) oxide
nitrogen (II) oxide
nitrogen (III) oxide
nitrogen (IV) oxide
Midterm Review
24. Which symbol represents a particle that has the
same total number of electrons as S 2–?
A) Ar
B) O2– C) Si
D) Se 2–
25. What is the mass number of an atom that has six
protons, six electrons, and eight neutrons?
A) 6
B) 14
C) 12
D) 20
26. If 4.00 moles of oxygen gas, 3.00 moles of
hydrogen gas, and 1.00 mole of nitrogen gas are
combined in a closed container at standard
pressure, what is the partial pressure exerted by
the hydrogen gas?
A) 1.00 atm
C) 3.00 atm
B) 0.125 atm
D) 0.375 atm
27. During a laboratory activity to investigate
reaction rate, a student reacts 1.0-gram samples
of solid zinc with 10.0-milliliter samples of
HCl(aq). The table below shows information
about the variables in five experiments the
student performed.
29. Which trends are observed when the elements in
Period 3 on the Periodic Table are considered in
order of increasing atomic number?
A) The atomic radius decreases, and the first
ionization energy generally decreases.
B) The atomic radius decreases, and the first
ionization energy generally increases.
C) The atomic radius increases, and the first
ionization energy generally increases.
D) The atomic radius increases, and the first
ionization energy generally decreases.
30. A metal, M, forms an oxide compound with the
general formula M 2O. In which group on the
Periodic Table could metal M be found?
A) Group 2
C) Group 16
B) Group 1
D) Group 17
31. What is the empirical formula of a compound
that contains 28% iron, 24% sulfur, and 48%
oxygen by mass?
A) FeSO 3
C) Fe 2(SO4) 3
B) Fe 2(SO3) 3
D) FeSO 4
32. Which statement concerning elements is true?
Which two experiments can be used to
investigate the effect of the concentration of
HCl(aq) on the reaction rate?
A) 1 and 3
C) 1 and 5
B) 4 and 3
D) 4 and 2
28. The average kinetic energy of water molecules
is greatest in which of these samples?
A)
B)
C)
D)
100 g of water at 45°C
100 g of water at 25°C
10 g of water at 55°C
10 g of water at 35°C
A) Different elements must have different
numbers of isotopes.
B) All atoms of a given element must have
the same mass number.
C) All atoms of a given element must have
the same atomic number.
D) Different elements must have different
numbers of neutrons.
33. What occurs when an atom of chlorine and an
atom of hydrogen become a molecule of
hydrogen chloride?
A) A chemical bond is broken and energy is
released.
B) A chemical bond is formed and energy is
absorbed.
C) A chemical bond is broken and energy is
absorbed.
D) A chemical bond is formed and energy is
released.
Midterm Review
34. Which compound forms a green aqueous
solution?
A) RbCl
C) ZnCl2
B) NiCl 2
D) CaCl2
35. The temperature of a sample of a substance
changes from 10.°C to 20.°C. How many
Kelvin does the temperature change?
A) 20.
B) 10.
C) 283 D) 293
36. Which element forms an ion that is larger than
its atom?
A) aluminum
C) magnesium
B) sodium
D) chlorine
37. Which properties are most common in
nonmetals?
A) low ionization energy and high
electronegativity
B) high ionization energy and high
electronegativity
C) high ionization energy and low
electronegativity
D) low ionization energy and low
electronegativity
38. Which group contains elements composed of
diatomic molecules at STP?
A) 11
B) 2
C) 7
D) 17
39. Which process is a chemical change?
A)
B)
C)
D)
decomposing of water
subliming of ice
melting of ice
boiling of water
40. The gram formula mass of NH4Cl is
A) 22.4 g/mole
C) 53.5 g/mole
B) 28.0 g/mole
D) 95.5 g/mole
41. Which phase change results in the release of
energy?
A)
B)
C)
D)
H2O( ) ® H2O(g)
H2O(s) ® H2O(g)
H2O(s) ® H2O( )
H2O(g) ® H2O( )
42. How many electrons are in the outermost
principal energy level (shell) of an atom of
carbon in the ground state?
A) 6
B) 2
C) 3
D) 4
43. Which set of procedures and observations
indicates a chemical change?
A) Ethanol is added to an empty beaker and
the ethanol eventually disappears.
B) Large crystals are crushed with a mortar
and pestle and become powder.
C) A solid is gently heated in a crucible and
the solid slowly turns to liquid.
D) A cool, shiny metal is added to water in a
beaker and rapid bubbling occurs.
44. What is the total number of oxygen atoms in the
formula MgSO 4 • 7 H 2O? [The • represents
seven units of H 2O attached to one unit of
MgSO4 .]
A) 11
B) 7
C) 5
D) 4
45. The temperature of a sample of water changes
from 10.°C to 20.°C when the water absorbs
420 Joules of heat. What is the mass of the
sample?
A) 1.0 g
C) 100 g
B) 10. g
D) 1000 g
46. Which notation represents an atom of sodium
with an atomic number of 11 and a mass
number of 24?
A)
C)
B)
D)
47. Based on bond type, which compound has the
highest melting point?
A) C6H14
C) CH 3OH
B) CaCl2
D) CCl4
Midterm Review
48. A student investigated the physical and
chemical properties of a sample of an unknown
gas and then identified the gas. Which
statement represents a conclusion rather than an
experimental observation?
A) When placed in the gas, a flaming splint
stops burning.
B) When the gas is bubbled into limewater,
the liquid becomes cloudy.
C) The gas is carbon dioxide.
D) The gas is colorless.
49. A student calculated the percent by mass of
water in a sample of
to be
, but the accepted value is
. What
was the student's percent error?
A)
B)
C)
D)
50. What is the formula of titanium(II) oxide?
A) TiO2
C) Ti 2O3
B) TiO
D) Ti 2O
54. In comparison to an atom of
in the ground
state, an atom of
in the ground state has
A)
B)
C)
D)
three more valence electrons
three more neutrons
three fewer valence electrons
three fewer neutrons
55. The molecular formula of glucose is C 6H12O6.
What is the empirical formula of glucose?
A) CH 2O
C) CHO
B) C12H24O12
D) C6H12O6
56. A sample of a compound contains 65.4 grams of
zinc, 12.0 grams of carbon, and 48.0 grams of
oxygen. What is the mole ratio of zinc to carbon
to oxygen in this compound?
A) 1:4:6
C) 5:1:4
B) 1:1:2
D) 1:1:3
57. Which diagram represents the nucleus of an
atom of
?
A)
B)
C)
D)
51. Which Lewis electron-dot diagram is correct for
a S 2– ion?
A)
B)
C)
D)
52. Under which conditions of temperature and
pressure would helium behave most like an
ideal gas?
A)
B)
C)
D)
50 K and 20 kPa
750 K and 600 kPa
50 K and 600 kPa
750 K and 20 kPa
53. When a quantity of electricity is converted to
heat, the heat energy produced is measured in
A) volts
C) degrees
B) amperes
D) joules
58. The modern model of the atom is based on the
work of
A)
B)
C)
D)
one scientist over a short period of time
many scientists over a long period of time
many scientists over a short period of time
one scientist over a long period of time
59. Which element is malleable and can conduct
electricity in the solid phase?
A) iodine
C) tin
B) phosphorus
D) sulfur
60. What amount of heat is required to completely
melt a 29.95-gram sample of H2O(s) at 0°C?
A) 334 J
C) 1.00 × 10 4 J
B) 2260 J
D) 1.00 × 10 3 J
Midterm Review
61. Element X is a solid that is brittle, lacks
luster,and has six valence electrons. In which
group on the Periodic Table would element X
be found?
A) 16
B) 15
C) 1
D) 2
62. What is the total number of orbitals containing
only one electron in an atom of nitrogen in the
ground state?
A) 1
B) 2
C) 3
D) 4
63. A gas occupies a volume of 444 mL at 273 K
and 79.0 kPa. What is the final kelvin
temperature when the volume of the gas is
changed to 1880 mL and the pressure is
changed to 38.7 kPa?
A) 31.5 K
C) 566 K
B) 2360 K
D) 292 K
64. The data table below gives the temperature and pressure of four different gas samples, each in a
2-liter container.
Which two gas samples contain the same total number of particles?
A) CH 4 and CO 2 B) He and Ne
C) CH 4 and Ne
D) He and CO2
Midterm Review
65. Which substance contains bonds that involved
the transfer of electrons from one atom to
another?
67. The diagram below represents a Celsius
thermometer recording a certain temperature.
A) KBr B) CO 2 C) NH 3 D) Cl 2
66. The graph below represents the uniform heating
of a substance, starting below its melting point,
when the substance is solid.
Which line segments represent an increase in
average kinetic energy?
A)
C)
and
and
B)
D)
and
and
What is the correct reading of the thermometer?
A) 5°C
C) 0.3°C
B) 4.3°C
D) 4°C
68. Which is a binary compound?
A) MgSO4
C) NaNO3
B) KOH
D) CaCl2
69. A compound is made up of iron and oxygen,
only. The ratio of iron ions to oxide ions is 2:3
in this compound. The IUPAC name for this
compound is
A) iron(II) oxide
C) iron trioxide
B) iron(III) oxide
D) triiron dioxide
70. Which quantity of heat is equal to 200. joules?
A) 20.0 kJ
C) 0.200 kJ
B) 2.00 kJ
D) 0.0200 kJ