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CST Practice Test
Young
NAME
CST Practice Test
Multiple Choice Questions
1) At 1 atm and 298 K, which of the Ka values listed below
represents the strongest acid?
(a) 1.1 × 10−7
(b) 1.8 × 10−5
(c) 5.6 × 10−11
(d) 4.6 × 10−4
5) Which electron-dot symbol represents an atom of chlorine in the ground state?
(a)
(c)
(b)
(d)
2) Given the system at equilibrium:
PbCO3 (s) Pb2+ (aq) + CO3 2− (aq)
How will the addition of Na2 CO3 (aq) affect [Pb2+ ](aq)
and the mass of PbCO3 (s)?
(a) [Pb2+ ](aq) will decrease and the mass of PbCO3 (s)
will decrease.
(b) [Pb2+ ](aq) will decrease and the mass of PbCO3 (s)
will increase.
(c) [Pb2+ ](aq) will increase and the mass of PbCO3 (s)
will decrease.
(d) [Pb2+ ](aq) will increase and the mass of PbCO3 (s)
will increase.
3) When a catalyst is added to a system at equilibrium, a
decrease occurs in
(a) the heat of the reaction
(b) activation energy
6) Which statement describes the elements in Period 3?
(a) Each successive element has a greater atomic radius.
(b) Each successive element has a lower electronegativity.
(c) All elements have similar chemical properties.
(d) All elements have valence electrons in the same
principal energy level.
7) What volume will a 300.-milliliter sample of a gas at
STP occupy when the pressure is doubled at constant
temperature?
(a) 150. mL
(b) 450. mL
(c) 300. mL
(d) 600. mL
(c) potential energy of the reactants
(d) potential energy of the products
8) Which type of bond is formed when an atom of potassium transfers an electron to a bromine atom?
4) Given the reaction at equilibrium:
X + Y 2Z + heat
The concentration of the product could be increased by
(a) adding a catalyst
(b) adding more heat to the system
(c) increasing the concentration of Y
(d) decreasing the concentration of X
(a) metallic
(c) nonpolar covalent
(b) ionic
(d) polar covalent
9) C3 H8 + 5O2 → 3CO2 + 4H2 O
Which of these could be added to the above reaction to increase the rate of reaction over time?
(a)
(b)
(c)
(d)
14) A student observed that when sodium hydroxide was
dissolved in water, the temperature of the water increased. The student should conclude that the dissolving of sodium hydroxide
(a) is endothermic
(b) is exothermic
(c) produces an acid solution
C3 H8 and O2
C3 H8 and CO2
O2 and CO2
O2 and H2 O
(d) produces a salt solution
10) The heat energy required to change a unit mass of a
solid into a liquid at constant temperature is called
(a) heat of vaporization
(c) heat of solution
(b) heat of formation
(d) heat of fusion
15) Given the nuclear equation:
14
16
2
N+X→
O+
H
7
8
1
What is particle X?
(a) an alpha particle
(c) a deuteron
(b) a beta particle
(d) a triton
11) Given the reaction at equilibrium:
2A(g) + 3B(g) A2 B3 (g) + heat
Which change will not affect the equilibrium concentrations of A(g), B(g), and A2 B3 (g)?
(a) adding more A(g)
16) Given the reaction:
N2 (g) + 3H2 (g) 2NH3 (g) + energy
If the temperature is increased and the pressure is kept
constant, the new equilibrium concentration will be
(b) adding a catalyst
(c) increasing the temperature
(a) less for NH3 (g)
(c) less for N2 (g)
(d) increasing the pressure
(b) the same for NH3 (g)
(d) the same for N2 (g)
12) What occurs when a substance melts?
(a) It changes
sorbed.
(b) It changes
leased.
(c) It changes
sorbed.
(d) It changes
leased.
from solid to liquid, and heat is abfrom solid to liquid, and heat is refrom liquid to solid, and heat is ab-
17) In a mixture of water, sugar, and salt, which ingredient(s), if any, are solvents?
(a) Water only
(b) Water and sugar only
(c) Sugar and salt only
(d) Water, sugar, and salt
from liquid to solid, and heat is re-
18) Which property do most acids share?
13) Which phase change is exothermic?
(a) solid to liquid
(c) liquid to solid
(b) solid to gas
(d) liquid to gas
(a) Bitter taste
(b) Sour taste
(c) Slippery feel
(d) Faint color
19) Given the reaction:
2N2 (g) + O2 (g) 2N2 O(g)
Which statement is true when this closed system
reaches equilibrium?
(a) All of the N2 (g) has been consumed.
(b) All of the O2 (g) has been consumed.
(c) Pressure changes no longer occur.
(d) The forward reaction no longer occurs.
20) Which type of bond exists between an atom of carbon
and an atom of fluorine?
(a) ionic
(c) polar covalent
(b) metallic
(d) nonpolar covalent
21) Which of these is the best conductor of electricity?
(a)
(b)
(c)
(d)
Distilled water
Salt water
Carbonated water
Sugar water
25) In a reversible chemical reaction, which factors must
be equal when the reaction is at equilibrium?
(a) rate at which reactants are formed and rate at
which products are formed
(b) concentration of reactants and concentration of
products
(c) potential energy of reactants and potential energy
of products
(d) activation energy of reactants and activation energy of products
26) In a reversible reaction, chemical equilibrium is attained when the
(a) rate of the forward reaction is greater than the
rate of the reverse reaction
(b) rate of the reverse reaction is greater than the rate
of the forward reaction
(c) concentration of the reactants reaches zero
(d) concentration of the products remains constant
27) What are the characteristics of a neutron?
(a) It has no charge and no mass.
(b) It has no charge and a mass of 1 amu.
22) The ability of H2 SO4 (aq) to change blue litmus red is
mainly due to the presence of
(a) SO2 molecules
(c) H3 O+ (aq) ions
(b) H2 O molecules
(d) SO4 2− (aq) ions
(c) It has a charge of +1 and no mass.
(d) It has a charge of +1 and a mass of 1 amu.
28) Given the solution at equilibrium:
PbI2 (s) Pb2+ (aq) + 2I− (aq)
23) If equal volumes of 0.1 M NaOH and 0.1 M HCl are
mixed, the resulting solution will contain a salt and
(a) HCl
(b) NaOH
(c) H2 O
(d) NaCl
24) Carbon dioxide gas is most soluble in water under conditions of
(a) high pressure and low temperature
(b) high pressure and high temperature
(c) low pressure and low temperature
(d) low pressure and high temperature
The addition of which nitrate salt will cause a decrease
in the concentration of I− (aq) ?
(a) Pb(NO3 )2
(c) LiNO3
(b) Ca(NO3 )2
(d) KNO3
29) Which properties are most common in nonmetals?
(a) low ionization energy and low electronegativity
(b) low ionization energy and high electronegativity
(c) high ionization energy and low electronegativity
(d) high ionization energy and high electronegativity
30) Which ion has the largest radius?
(a) Na+
(b) Mg2+
(c) K+
(d) Ca2+
31) The forces between atoms that create chemical bonds
are the result of interactions between
(a) nuclei
(b) electrons
(c) protons and electrons
34) What happens when NaCl(s) is dissolved in water?
(a) Cl− ions are attracted to the oxygen atoms of water molecules.
(b) Na+ ions are attracted to the oxygen atoms of
water molecules.
(c) Cl− ions are repelled by the hydrogen atoms of
water molecules.
(d) Na+ ions are repelled by the oxygen atoms of water molecules.
35) Which pair of atoms is held together by a covalent
bond?
(d) protons and nuclei
32) The graph below represents the uniform cooling of a
substance, starting with the substance as a gas above
its boiling point.
(a) HCl
(b) LiCl
(c) NaCl
(d) KCl
36) A condensation polymerization reaction is best described as the
(a) joining of monomers by the removal of oxygen
(b) joining of monomers by the removal of water
(c) oxidation of a hydrocarbon by oxygen
(d) oxidation of a hydrocarbon by water
37) As the number of neutrons in the nucleus of a given
atom of an element increases, the atomic number of
that element
During which interval is the substance completely in
the liquid phase?
(a) AB
(b) BC
(c) CD
(d) DE
33) The energy absorbed when ammonium chloride dissolves in water can be measured in
(a) degrees
(c) moles per liter
(b) kilocalories
(d) liters per mole
(a) decreases
(b) increases
(c) remains the same
38) Experiments performed to reveal the structure of
atoms led scientists to conclude that an atom’s
(a) positive charge is evenly distributed throughout its
volume
(b) negative charge is mainly concentrated in its nucleus
(c) mass is evenly distributed throughout its volume
(d) volume is mainly unoccupied
39) The nucleus of which atom contains 48 neutrons?
(a)
32
S
16
(c)
85
Rb
37
(b)
48
Ti
22
(d)
112
Cd
48
40) When an atom loses an electron, the atom becomes
an ion that is
(a) positively charged and gains a
mass
(b) positively charged and loses a
mass
(c) negatively charged and gains a
mass
(d) negatively charged and loses a
mass
42) The atomic mass unit is defined as exactly
of an atom of
small amount of
H
O
(d)
(c)
24
Mg
12
(b)
14
C
6
(d)
26
Mg
12
small amount of
small amount of
43) Which type of radiation continues in a straight line
when passed through an electric field?
(a) alpha
(c) gamma
(b) beta
(d) proton
44) Which atom in the ground state has five electrons in
its outer level and ten electrons in its kernel?
(b)
(c)
12
C
6
the mass
H
H
O
(a)
small amount of
41) Which shows the correct Lewis structure for H2 O?
(a)
1
12
(a) C
(b) Cl
H
(c) Si
(d) P
H O H
H
O
H
45) Which list of substances is in order of increasing intermolecular forces?
(a) Ice, soda, honey, helium
(b) Soda, ice, honey, helium
(c) Helium, soda, honey, ice
(d) Helium, soda, ice, honey
For question 46
46) The forward reaction is best described as an
(a) exothermic reaction in which energy is released
(b) exothermic reaction in which energy is absorbed
(c) endothermic reaction in which energy is released
(d) endothermic reaction in which energy is absorbed
47) As HCl(g) is added to water, the pH of the water
solution
(a) decreases
(b) increases
(c) remains the same
52) Which of these has base units made up of amino acids?
(a) Protein
(b) Phospholipids
(c) Sucrose
(d) DNA
53) Which of these combine together to form proteins?
(a) Amino acids
(b) Lipids
(c) Sugars
(d) Nucleic acids
48) Which list is in order of increasing penetrating
strength?
(a) Alpha, gamma, beta
54) Which element in Group 1 has the greatest tendency
to lose an electron?
(b) Alpha, beta, gamma
(a) cesium
(c) potassium
(c) Gamma, alpha, beta
(b) rubidium
(d) sodium
(d) Gamma, beta, alpha
49) An increase in the temperature of a system at equilibrium favors the
(a)
(b)
(c)
(d)
55) The diagram below represents radiation passing
through an electric field.
endothermic reaction and decreases its rate
endothermic reaction and increases its rate
exothermic reaction and decreases its rate
exothermic reaction and increases its rate
50) How are protons held together in the nucleus of an
atom?
(a) Nuclear forces
(b) Electromagnetic attraction
(c) Electromagnetic repulsion
(d) Rotational inertia
51) What is the concentration of a solution of 10. moles
of copper (II) nitrate in 5.0 liters of solution?
(a) 0.50 M
(b) 2.0 M
(c) 5.0M
(d) 10. M
The arrow labeled A most likely represents
(a) a positron
(c) alpha radiation
(b) an electron
(d) gamma radiation
56) What is the total number of valence electrons in an
atom of xenon?
(a) 0
(b) 2
(c) 8
(d) 18
57) The bond between hydrogen and oxygen in a water
molecule is classified as
62) In the equation
234
234
Th →
Pa + X the symbol
90
91
X represents
(a) ionic and nonpolar
(b) ionic and polar
(a)
0
e
+1
(c)
1
n
0
(b)
0
e
−1
(d)
1
H
1
(c) covalent and nonpolar
(d) covalent and polar
58) When ionic bonds are formed, metallic atoms tend to
(a) lose electrons and become negative ions
(b) lose electrons and become positive ions
63) A gas sample has a volume of 25.0 milliliters at a pressure of 1.00 atmosphere. If the volume increases to
50.0 milliliters and the temperature remains constant,
the new pressure will be
(c) gain electrons and become negative ions
(d) gain electrons and become positive ions
(a) 1.00 atm
(b) 2.00 atm
(c) 0.250 atm
(d) 0.500 atm
59) Which phase change is exothermic?
64) Which noble gas has the highest first ionization energy?
(a) H2 O(s) → H2 O(`)
(b) H2 O(`) → H2 O(s)
(a) radon
(b) krypton
(c) H2 O(s) → H2 O(g)
(c) neon
(d) helium
(d) H2 O(`) → H2 O(g)
65) Which statement explains why fusion reactions are difficult to initiate?
60) Given the reaction:
A2 (g) + B2 (g) 2AB(g) + heat
An increase in the concentration of A2 (g) will
(a) decrease the production of AB(g)
(b) decrease the frequency of collisions between A2 (g)
and B2 (g)
(a) Positive nuclei attract each other.
(b) Positive nuclei repel each other.
(c) Neutrons prevent nuclei from getting close enough
to fuse.
(d) Electrons prevent nuclei from getting close enough
to fuse.
(c) increase the production of B2 (g)
(d) increase the frequency of collisions between A2 (g)
and B2 (g)
66) Given the reaction:
Cl(g) + Cl(g) → Cl2 (g) + energy
61) Which subatomic particle is found in the nucleus of
all isotopes of hydrogen?
(a) proton
(c) electron
(b) neutron
(d) positron
Which statement best describes the reaction?
(a) A bond is formed and energy is absorbed.
(b) A bond is formed and energy is released.
(c) A bond is broken and energy is absorbed.
(d) A bond is broken and energy is released.
67) The reaction during which monomers are combined
and water is released is called
73) Hotter temperatures generally make
in water.
(a) saponification
(a) gases
(b) neutralization
(c) addition polymerization
(b) solids
(c) liquids
(d) condensation polymerization
(d) salts
68) A catalyst will affect the rate of the forward reaction
by changing the
less soluble
74) Why does a spoonful of loose salt crystals dissolve
faster in water than does a block of the same amount
of salt?
(a) activation energy
(a) The loose salt crystals require less energy to dissolve than the block of salt.
(b) The loose salt crystals have more surface area exposed to the water than the block of salt.
(b) heat of reaction
(c) heat of formation
(d) potential energy of the products
(c) The loose salt crystals are less soluble than the
block of salt.
(d) The loose salt crystals have fewer chemical bonds
to break than the block of salt.
69) What is the correct formula for magnesium fluoride?
(a) MgF
(b) Mg2 F
(c) Mg2 F2
75) Which two elements have chemical properties that are
most similar?
(d) MgF2
(a) Cl and Ar
(b) Li and Na
(c) K and Ca
(d) C and N
70) If M represents an alkali metal, what is the formula
for the compound formed by M and oxygen?
(a) MO2
(b) M2 O
(c) M2 O3
(d) M3 O2
76)
71) Which formula correctly represents antimony (V) oxide?
(a) SbO5
(b) Sb5 O
(c) Sb2 O5
(d) Sb5 O2
72) Which acid-base pair will always undergo a reaction
that produces a neutral solution?
(a) a weak acid and a weak base
(b) a weak acid and a strong base
(c) a strong acid and a weak base
(d) a strong acid and a strong base
Carbonated beverages are bottled and canned under
pressure, because pressure greatly−
(a) decreases the solubility of solids in liquids.
(b) increases the solubility of solids in liquids.
(c) decreases the solubility of gases in liquids.
(d) increases the solubility of gases in liquids.
77) How does the temperature of water influence the solubility of different substances?
82) Adding a catalyst to a chemical reaction changes the
rate of reaction by causing
(a) Hotter water generally makes solids more soluble.
(a) a decrease in the activation energy
(b) Colder water generally makes liquids more soluble.
(b) an increase in the activation energy
(c) Hotter water generally makes gases more soluble.
(c) a decrease in the heat of reaction
(d) an increase in the heat of reaction
(d) Water temperature does not affect the solubility
of substances.
78) When HCl is dissolved in water, the only positive ion
present in the solution is the
(a) hydrogen ion
(c) hydride ion
(b) hydroxide ion
(d) chloride ion
83) In which pair of elements do the nuclei of the atoms
contain the same number of neutrons’ ?
(a)
7
9
Li and
Be
3
4
(c)
23
24
Na and
Mg
11
12
(b)
14
16
N and
O
7
8
(d)
32
35
S and
Cl
16
17
79) Given the solution at equilibrium:
CaSO4 (s) Ca2+ (aq) + SO4 2− (aq)
When Na2 SO4 is added to the system, how will the
equilibrium shift?
84) The properties of carbon are expected to be most similar to those of
(a) boron
(b) aluminum
(c) silicon
(d) phosphorus
(a) The amount of CaSO4 (s) will decrease, and the
concentration of Ca2+ (aq) will decrease.
(b) The amount of CaSO4 (s) will decrease, and the
concentration of Ca2+ (aq) will increase.
(c) The amount of CaSO4 (s) will increase, and the
concentration of Ca2+ (aq) will decrease.
(d) The amount of CaSO4 (s) will increase, and the
concentration of Ca2+ (aq) will increase.
85) Which type of radiation is most similar to high-energy
x rays?
(a) alpha
(c) neutron
(b) beta
(d) gamma
86) When an acid is dissolved in water, it will−
80) Given the nuclear reaction:
9
12
1
Be + X →
C+
n
4
6
0
What is the identity of particle X?
(a) alpha particle
(c) proton
(b) beta particle
(d) neutron
(a)
(b)
(c)
(d)
release H+ ions into the water.
release H− ions into the water.
release OH− ions into the water.
not release ions into the water.
87) Which atom will form an ionic bond with a Br atom?
81) In which list can all particles be accelerated by an
electric field?
(a) N
(b) Li
(c) O
(d) C
(a) alpha particles, beta particles, and neutrons
(b) alpha particles, beta particles, and protons
(c) alpha particles, protons, and neutrons
(d) beta particles, protons, and neutrons
88) What is the pH of a solution that results from the complete neutralization of an HCl solution with a KOH
solution?
(a) 1
(b) 7
(c) 10
(d) 4
89) Which atoms are isotopes of the same element?
(a)
24
25
X and
X
12
12
(b)
20
20
X and
X
10
11
(c)
31
32
X and
X
15
16
(d)
31
31
X and
X
19
19
94) Which change of phase is exothermic?
(a) solid to liquid
(c) solid to gas
(b) gas to liquid
(d) liquid to gas
95) Proteins are produced through the process of
90) Which subatomic particles have a mass of approximately 1 atomic mass unit each?
(a) addition
(c) polymerization
(b) substitution
(d) combustion
(a) proton and electron
(b) proton and neutron
96) The mass of a calcium atom is due primarily to the
mass of its
(c) neutron and positron
(d) electron and positron
(a) protons, only
(b) neutrons, only
91) Given the reaction at equilibrium:
(c) protons and neutrons
(d) protons and electrons
A(g) + B(g) C(g) + D(g)
The addition of a catalyst will
(a) shift the equilibrium to the right
(b) shift the equilibrium to the left
97) Which statement about the mass of an electron is correct?
(c) increase the rate of forward and reverse reactions
equally
(a) The mass of an electron is equal to the mass of a
proton.
(d) have no effect on the forward or reverse reactions
(b) The mass of an electron is less than the mass of
a proton.
92) Given the reaction at equilibrium:
BaCrO4 (s) Ba2+ (aq) + CrO2−
4 (aq)
Which substance, when added to the mixture, will
cause an increase in the amount of BaCrO4 (s)?
(a) K2 CO3
(b) CaCO3
(c) BaCl2
(d) CaCl2
93) Given the reaction:
2SO2 (g) + O2 (g) 2SO3 (g)
The value of the equilibrium constant (Keq ) will be
changed by increasing the
(a) pressure
(b) temperature
(c) concentration of SO2 (g)
(d) concentration of SO3 (g)
(c) The mass of an electron is equal to the mass of a
neutron.
(d) The mass of an electron is greater than the mass
of a neutron.
98) A potential energy diagram of a chemical reaction is
shown below.
102) What is the molarity of a solution that contains 40.
grams of NaOH in 0.50 liter of solution?
(a) 1.0 M
(b) 2.0 M
(c) 0.50 M
(d) 0.25 M
103) Which graph best shows the relationship between
Kelvin temperature and average kinetic energy?
(a)
(c)
(b)
(d)
What is the difference between the potential energy
of the reactants and the potential energy of the products?
(a) 20 kcal
(b) 40 kcal
(c) 60 kcal
(d) 80 kcal
99) What is the atomic number of an element that has six
protons and eight neutrons?
(a) 6
(b) 2
(c) 8
(d) 14
104) When alpha particles are used to bombard gold foil,
most of the alpha particles pass through undeflected.
This result indicates that most of the volume of a
gold atom consists of
100) Given the reaction:
226
222
Ra →
Rn + X
88
86
(a) neutrons
(b) protons
(c) deuterons
(d) unoccupied space
Which type of emanation is represented by X?
(a) alpha particle
(c) proton
(b) beta particle
(d) positron
105) Atoms of metals tend to
(a) lose electrons and form negative ions
(b) lose electrons and form positive ions
101) Given the system at equilibrium:
H2 (g) + F2 (g) 2HF(g) + heat
(c) gain electrons and form negative ions
(d) gain electrons and form positive ions
Which change will not shift the point of equilibrium?
(a) changing the pressure
(b) changing the temperature
(c) changing the concentration of H2 (g)
(d) changing the concentration of HF(g)
106) Which of the following 0.1 M solutions has the lowest
pH’ ?
(a) 0.1 M NaOH
(b) 0.1 M CH3 OH
(c) 0.1 M NaCl
(d) 0.1 M HCl
107) Which of the following elements has the strongest
attraction for electrons?
(a) boron
(c) oxygen
(b) aluminum
(d) sulfur
110) Given the reaction at equilibrium:
N2 (g) + 3H2 (g) 2NH3 (g) + 22 kcal
Which stress would cause the equilibrium to shift to
the left?
(a) increasing the temperature
108) Which particles may be gained, lost, or shared by an
atom when it forms a chemical bond?
(a) protons
(c) neutrons
(b) electrons
(d) nucleons
(b) increasing the pressure
(c) adding N2 (g) to the system
(d) adding H2 (g) to the system
111) What is the total number of valence electrons in an
atom of boron in the ground state?
109) The potential energy diagram of a chemical reaction
is shown below.
(a) 1
(b) 7
(c) 3
(d) 5
112) What is the total number of protons and neutrons in
86
an atom of
Rb?
37
(a) 37
(b) 49
(c) 86
(d) 123
113) Which type of radiation has zero mass and zero
charge?
Which arrow represents the part of the reaction most
likely to be affected by the addition of a catalyst?
(a) A
(b) B
(a) alpha
(c) neutron
(b) beta
(d) gamma
(c) C
(d) D
114) The elements known as the alkaline earth metals are
found in Group
(a) 1
(b) 2
(c) 16
(d) 17
CST Practice Test
Young
Answer Key
Multiple Choice Questions
1) d
2) b
3) b
4) c
5) d
6) d
7) a
8) b
9) a
10) d
11) b
12) a
13) c
14) b
15) a
16) a
17) a
18) b
19) c
20) c
21) b
22) c
23) c
24) a
25) a
26) d
27) b
28) a
29) d
30) c
31) c
32) c
33) b
34) b
35) a
36) b
37) c
38) d
39) c
40) b
41) d
42) a
43) c
44) d
45) c
46) d
47) a
48) b
49) b
50) a
51) b
52) a
53) a
54) a
55) b
56) c
57) d
58) b
59) b
60) d
61) a
62) b
63) d
64) d
65) b
66) b
67) d
68) a
69) d
70) b
71) c
72) d
73) a
74) b
75) b
76) d
77) a
78) a
79) c
80) a
81) b
82) a
83) c
84) c
85) d
86) a
87) b
88) b
89) a
90) b
91) c
92) c
93) b
94) b
95) c
96) c
97) b
98) a
99) a
100) a
101) a
102) b
103) a
104) d
105) b
106) d
107) c
108) b
109) b
110)
111)
112)
113)
114)
a
c
c
d
b