Download Interim Exam - Review H-Chem 2015

Interim Exam - Review
1. A sample of a substance is heated strongly in a crucible and
the sample increases in mass. This is evidence that the
substance has
1.
2.
3.
4.
5.
melted.
sublimed.
evolved a gas.
expanded
undergone a chemical change.
8. A pure substance that contains more than one type of
atom is called a(n)
1. allotrope.
3. element.
5. isomer.
9. In a chemical change, the total mass of the product(s) is
1.
2.
3.
4.
5.
2. A chemical property of sulfur is that it is
1. solid.
3. odorless.
5. brittle.
2. yellow.
4. combustible.
1. has been known for many centuries.
2. combines with oxygen to form a gas.
3. cannot be chemically decomposed into two or more
substances.
4. is formed when wood is heated without the presence
of air.
5. can be found in many pure forms.
4. An element is identified most accurately by its
1. element
3. compound
5. none of the above
1. any proportion
3. definite proportions
5. one proportion only
2.
Cu2+
3. Cu(II)
1. filtration
3. boiling
5. decomposition
4. Cu(aq) 5. CuO
2. baking a cake.
4. breaking glass.
1.
2.
3.
4.
5.
a change in color.
a change of state.
a change in density.
a change in the number of atoms.
the formation of a new pure substance.
H-Chem 2015-16
2. chlorination
4. distillation
14. Ernest Rutherford concluded from experiments that they
indicated nuclei of atoms are relatively
7. A chemical change involves
1.
2.
3.
4.
5.
soluble in water
different in properties
the same size as every other particle
the same in properties as every other particle
the same phase as every other particle
13. Sea water is made salt–free by
6. An example of a chemical change is
1. grinding rock.
3. heating water.
5. melting ice.
2. equal proportions
4. constant proportions
12. A substance is considered to be homogeneous if every
particle is
1.
2.
3.
4.
5.
5. Which of the following notations correctly indicates that
the substance copper is in the solid state?
2. solution
4. pure substance
11. A mixture consists of two or more components in
mass and color
volume and odor
color and conductivity
density and color
density and conductivity
1. Cu(s)
less than that of the reactants.
a function of the rate of reaction.
the same as that of the reactants.
more than that of the reactants.
less if a catalyst is present.
10. A homogeneous mixture is a(n)
3. Carbon is classified as an element rather than as a
compound because it
1.
2.
3.
4.
5.
2. compound.
4. solution.
Page 1
far apart and positively charged
far apart and negatively charged
close together and positively charged
close together and negatively charged
close together and neutral
Dr. Powell
15. The nucleus of an atom
1.
2.
3.
4.
5.
20. The number of neutrons in one atom of an element is
is electrically neutral
is the densest portion of the atom
occupies most of the atom’s volume
is a low fraction of the atom’s mass
is large compared to the size of the atom
1.
2.
3.
4.
5.
the same in each isotope
the same as the atomic number
equal to the number of protons in the nucleus
equal to the mass number minus the atomic number
equal to the number of electrons minus the number
of protons
21. Naturally occurring gallium is 60% 69Ga and 40% 71Ga by
mass. Based on this data the atomic mass of this element
is
1. 39.0
1. A
3. C
5. None of the above
2. B
4. D
1. 1.0
1.
2.
3.
4.
5.
the mass of the electron
the existence of the neutron
that the electron carries a negative charge
that the atom has a concentrated central mass
that the atom has very little open space
92U
1.
2.
3.
4.
5.
® 14156Ba +
9236Kr
+ 310n
what is the mass number of uranium, U?
1. 92
2. 143
3. 233
4. 235
19 protons, 20 neutrons, 20 electrons
19 protons, 20 neutrons, 18 electrons
20 protons, 19 neutrons, 19 electrons
39 protons, 39 neutrons, 39 electrons
19 protons, 39 neutrons, 18 electrons
H-Chem 2015-16
2. 2.0
3. 3.0
4. 4.0
5. 6.0
protons
neutrons
neutrons and protons
valence electrons and protons
kernel electrons
9 protons, 19 neutrons, 9 electrons
9 protons, 9 neutrons, 19 electrons
19 protons, 19 neutrons, 9 electrons
19 protons, 19 neutrons, 10 electrons
9 protons, 10 neutrons, 9 electrons
25. An element with an atomic number of 12 and a mass
number of 25 contains
5. 236
1.
2.
3.
4.
5.
19. How many protons, neutrons, and electrons are there in
potassium ions, 3919K+?
1.
2.
3.
4.
5.
5. 71.0
24. An atom of fluorine, 199F, contains
18. In the fission reaction,
+
4. 70.0
23. The atomic mass of an element is closely related to the
number of its
17. Rutherford's alpha–particle bombardment of gold foil
helped develop our current model of the atom by
determining
10n
3. 69.8
22. If a new standard for relative atomic masses were chosen
in which the most common atom of oxygen, “O”, had a
mass of 48 the relative atomic mass of hydrogen as
compared to the current stadard would be
16. Which is true?
1.
2.
3.
4.
5.
2. 69.0
12 protons, 13 neutrons, 12 electrons
12 protons, 13 neutrons, 13 electrons
13 protons, 12 neutrons, 13 electrons
13 protons, 13 neutrons, 13 electrons
13 protons, 12 neutrons, 12 electrons
26. The atomic mass unit is defined as
1.
2.
3.
4.
5.
Page 2
the mass of a carbon atom.
1/12 of the mass of the carbon atom.
12 g.
one microgram.
the mass of a hydrogen atom.
Dr. Powell
27. An ion containing 11 protons, 12 neutrons, and 10
electrons has approximately the same mass as
1. 13 protons
3. 22 neutrons
5. 33 protons
33. Which statement is true? All isotopes of the same
element have
2. 21 protons
4. 23 neutrons
1.
2.
3.
4.
5.
28. Atoms of an element all have the same number of
1.
2.
3.
4.
5.
protons
neutrons
nuclear particles
neutrons plus protons
total subatomic particles
34. Boron has two common isotopes, 105B and 115B. The
relative atomic mass of boron is 10.8. The
percent 105B in an average sample of boron is
1. 20%
35. The atom
29. Which property of the elements always increases with
increasing atomic number?
1.
2.
3.
4.
5.
1.
Atomic diameter
Electronegativity
Number of valence electrons
Nuclear charge
Number of protons
1.
3.
5.
2.
3. 50%
4. 67%
5. 80%
is an isotope of
3014Si
3.
2716S
4.
6530Zn
5.
45Rh
2814X, 2815X, 2816X
2.
4.
126X, 168X, 2010X
11X, 21X, 31X
3818X, 3919X, 4020X
128X, 164X, 200X
37. Deuterium, 21D, is an isotope of
1. the same element can have a different number of
neutrons
2. the same element can have a different mass number
3. different elements can have the same number of
electrons
4. different elements can have a different number of
protons
5. different elements can have the same number of
neutrons
1. lithium
3. dubnium
5. hydrogen
1. Chlorine nuclei are smaller than chlorine atoms
2. All chlorine atoms have the same nuclear charge
3. Some naturally occurring chlorine nuclei have 19
protons
4. Some naturally occurring chlorine nuclei have 20
neutrons
5. All chlorine atoms have the same number of protons
2. helium
4. oxygen
38. The symbol
1.
2.
3.
4.
5.
31. Which is false concerning nuclei of chlorine?
indicates this isotope consists of
A
B
C
D
None of the above correctly represent this isotope.
39. The number of neutrons in an atom of
1.
2.
3.
4.
5.
32. Which particle consists of 13 protons, 14 neutrons, and 10
electrons?
2. Silicon atom
4. Phosphide ion
94Be
is
4
5
9
13
The number of neutrons cannot be determined from
the information given.
40. The chlorine atom, 3517Cl, has the same number of
neutrons as
1.
H-Chem 2015-16
2715P
2. 40%
3015X
36. Which set represents isotopes of the same element?
30. Which is of these statements is false?
Neutral atoms of
1. Cobalt atom
3. Aluminum ion
5. Nitrogen isotope
the same number of neutrons
the same number of protons
different numbers of electrons
the same mass
the same nuclear structure
Page 3
3516S
2.
3717Cl
3.
3618Ar
4.
4020Ca
5.
189F
Dr. Powell
41. Which of the following statements about the elements 24
11X and 2512Y is correct?
1.
2.
3.
4.
5.
48. Experimental evidence indicates that the nucleus of an
atom
They are isotopes of the same element
They are non–metals
They are members of the same chemical family
They have the same number of neutrons per atom
The have the same electron configuration
1.
2.
3.
4.
5.
42. If Z represents the atomic number of an element and A
represents its mass number, then the number of neutrons
in one atom of the element is
1. A
2. A + Z
3. A – Z
4. Z – A
5. Z
49. How many nucleons does 2512Mg contain?
1. 12
2. 32
3. 39
4. 57
21H
5. 82
1. They are positive subatomic particles and are found
in the nucleus.
2. They are positive subatomic particles and are found
surrounding the nucleus.
3. They are negative subatomic particles and are found
in the nucleus.
4. They are negative subatomic particles and are found
surrounding the nucleus.
5. They are negative subatomic particles and are
equally distributed throughout the atom
24595Am
1.
+ ? ® 24597Bk + 4 10n
42He
2. 2 11H
3. 4 11H
4. 4 0-1e
5. 2 42He
52. Radioactive plutonium, 21484Pu, emits an alpha particle
and changes to a new element, “X”. This new element
emits a beta particle and is converted to element, “Y”.
Which are representations of elements X and Y?
1.
3.
5.
21082X
and 21083Y
and 21181Y
21083X and 21184Y
2.
4.
21280X
21282X
21080X
and 21081Y
and 21081Y
53. Bismuth, 83Bi, emits a beta particle. Which is correct?
I.
Lead, 82Pb, is formed.
II. Polonium, 84Po, is formed.
III. The mass number increases.
IV. The mass number decreases.
1. charge of +1 and mass of 1 amu
2. charge of +1 and mass of
amu
1. I only
3. I and IV
5. II and IV only
3. charge of –1 and mass of 1 amu
4. charge of –1 and mass of
amu
2. II only
4. II and III only
54. What is “X” in the equation?
21083Bi ® "X" + 0–1e
1.
H-Chem 2015-16
2. proton
4. electron
Which is necessary to complete the equation?
47. What is the charge and mass of a proton?
5. neutral charge and mass of 1 amu
5. 49
51. Consider the nuclear reaction
45. Which statement best describes electrons?
1. 1
2. 11
3. 12
4. 23
5. It is impossible to tell
4. 37
+ 31H ®42He + X
1. triton
3. neutron
5. deuteron
2. isotope
4. nucleon
46. A neutral atom contains 12 neutrons and 11 electrons.
The number of protons in this atom is
3. 25
the missing particle, X, is probably a(n)
44. Which is a synonym for the term “nuclide”?
1. ion
3. electron
5. neutrino
2. 13
50. Consider the nuclear equation below:
43. How many neutrons are in a 5725Mn7+ ion?
1. 25
contains most of the mass of the atom
contains a small percentage of the mass of the atom
has no charge
has a negative charge
contains most of the volume of the atom
Page 4
20983Bi
2.
21082Pb
3.
21084Po
4.
21183Bi
5.
20982Pb
Dr. Powell
55. The equation, E = mc2, computes the quantity of energy
1.
2.
3.
4.
5.
required to start a nuclear reaction
generated during a nuclear reaction
necessary to moderate a nuclear reactor
evolved during radioisotope production
stored in electromagnetic radiation
has a half-life of 8 hours. Starting with 1.00 gram
of the isotope, how much would remain at the end of 24
hours?
2. 0.333 gram
4. 0.125 gram
61. Which statements are correct?
I
The emission of a beta–particle reduces the ratio of
neutrons to protons in the nucleus.
II That the 168O isotope is stable is a reasonable
prediction.
III Radioactive tracers can be used to determine
reaction mechanisms.
IV 90Sr (t½ = 28 y) is more stable than
60Co (t ½ = 5.3 y).
man–made
radioactive
products of nuclear fission
found in naturally occurring uranium
nonmetals
57. A radioactive isotope contains nuclei which
1.
2.
3.
4.
5.
21082Pb
1. 0.500 gram
3. .250 gram
5. 0.000 gram
56. All of the elements in the seventh row of the Periodic
Table are
1.
2.
3.
4.
5.
60.
1. II
3. II and IV
5. All are correct
have unpredictable properties
give off radio waves when heated
undergo change only when energy is absorbed
spontaneously change, liberating energy
are completely stable
2. I and II
4. II, III and IV
62. A sample of an ore contains 100. milligrams of radioactive
phosphorus–32 with a half-life of 14.3 days. How many
milligrams of 32P remain in the sample after 28.6 days?
The symbol for the milligram is mg.
58. The diagram below represents radioactive emanations
passing through an electric field.
1. 0.00 mg
3. 50.0 mg
5. 200 mg
2. 25.0 mg
4. 75.0 mg
63. How long will it take a sample of 6.000 × 1020 atoms of 42K,
with a half life of 12.4 h, to decrease to 1.875 × 1019 atoms
?
1. 0.3875 h
3. 12.4 h
5. 397 h
Which type of emanation is represented by the arrow
labeled 1?
1. alpha particle
3. positron
5. neutron
2. beta particle
4. gamma ray
64. The activity of a sample of La–140 goes from 640. cpm to
40.0 cpm in 160. hours. What is its half-life?
1. 2560. h
3. 160. h
5. 10.0 h
59. In which list can all particles be accelerated by an electric
field?
1.
2.
3.
4.
5.
alpha particles, beta particles, and neutrons
alpha particles, beta particles, and protons
alpha particles, protons, and neutrons
beta particles, protons, and neutrons
neutrons, beta particles, and positrons
H-Chem 2015-16
2. 2.48 h
4. 62.0 h
2. 640. h
4. 40.0 h
65. Mendeleevium–256 emits at a rate of 100. dps after 2.00
hours of experimenting. If the half–life is 30.0 minutes,
what was the original count rate in dps?
1. 100.
3. 1500.
5. 3.28 x 106
Page 5
2. 400.
4. 1,600.
Dr. Powell
66. A nuclear reaction occurs, and the reactants have more
mass than the products. This mass difference represents
1.
2.
3.
4.
5.
73. Given the reaction:
94Be
the energy lost to heat and sound
the energy used to bind the nucleons
the uncertain mass of the neutrino
the kinetic energy of the final products
the potential energy of the electrostatic force
1.
2.
3.
4.
breaking the bonds in the original molecules
forming new bonds
the mass defect
the high energy of large molecules with which fusion
usually occurs
5. the drop of energy level of the electrons in the atoms
involved
68. An increase in the average kinetic energy of a sample of
copper atoms occurs with an increase in
1.
2.
3.
4.
5.
75. I. An atom of 2311Na has 12 neutrons
2. temperature
4. volume
BECAUSE
II. the number of neutrons is the difference between the
mass number and the atomic number.
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
2. 10°C to 1°C
4. 60°C to 50°C
2. gas
4. vapor
76. I. An atom of 23Na has 23 electrons
BECAUSE
71. Which equation represents sublimation?
1. I2(s) ® I2(g)
3. CO2(l) ® CO2(g)
5. O2(g) ® O2(s)
II. the number of protons equals the number of electrons
in a neutral atom.
2. NH3(g) ® NH3(l)
4. H2O(s) ® H2O(l)
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
72. A phase change from the solid directly to the gaseous
state is called
1. fusion
3. sublimation
5. deposition
H-Chem 2015-16
natural transmutation
artificial transmutation
fission
fusion
oxidation-reduction
1. 23892U ® 23490Th + 42He
2. 23490Th ® 23491Pa + 0–1e
3. 21884Po ® 21482Pb + 42He
4. 94Be + 42He ® 126C + 10n
5. none of the above
70. The state of matter which exhibits definite volume but not
a definite shape is
1. liquid
3. solid
5. aqueous
+ 42He
74. Which equation represents artificial transmutation?
69. Which change in the temperature of a 1-gram sample of
water would cause the greatest increase in the average
kinetic energy of its molecules?
1. 1°C to 10°C
3. 50°C to 60°C
5. 500°C to 501°C
63Li
Which type of reaction is represented?
67. Fusion reactions release energy due to
1. concentration
3. pressure
5. density
+ 11H
2. boiling
4. chemical change
Page 6
Dr. Powell
77. I. A sodium atom becomes a positive ion when it loses an
electron
80. I. Chemical properties are more similar for sodium and
magnesium than for sodium and lithium
BECAUSE
BECAUSE
II. electrons have a positive charge.
II. sodium and magnesium are in the same period.
1.
2.
3.
4.
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
81. I. Cl– is a negatively charged ion
78. I. Potassium and carbon exhibit similar properties
BECAUSE
BECAUSE
II. they are in the same period.
II. it has gained an electron and has more electrons than
protons.
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
79. I. Isotopes of different elements can have the same mass
number
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
82. I. Na+ is a positively charged ion
BECAUSE
BECAUSE
II. they can have the same number of neutrons.
II. it has less electrons than protons.
1.
2.
3.
4.
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
H-Chem 2015-16
Page 7
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
Dr. Powell
83. I. An element with an atomic number of “A” and a mass
number of “Z” has A number of neutrons
86. I. Sodium is a metal
BECAUSE
BECAUSE
II. sodium is a solid at room temperature.
II. all elements have the same number of neutrons as
protons.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
1.
2.
3.
4.
87. I. When I2(s) is heated a purple gas is formed
84. I. Most of the alpha particles in Rutherford’s gold foil
experiment were deflected
BECAUSE
II. solid iodine sublimes at standard pressure.
BECAUSE
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
II. the nucleus makes up most of the mass of an atom.
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
88. I. Beta particles are affected by an electric field
BECAUSE
85. I. The atomic mass of chlorine is 35.45
II. beta particles are high energy electrons.
BECAUSE
II. the most abundant isotope of chlorine has 17 protons.
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
H-Chem 2015-16
Page 8
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
Dr. Powell
89. I. In the detonation of a nuclear weapon, a small amount
of mass is gained
BECAUSE
92. What would the correct equation for determining percent
error be in a theoretical experiment where the
experimental value is determined as
J and the
accepted value is
J?
1.
II. the mass defect is regained according to the formula
E=mc2.
2.
1.
2.
3.
4.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
90. I. In order to mix an acid with water, one should quickly
pour the water into the acid
3.
4.
5. none of the above
93. Test tubes containing nonflammable fluids being heated
should be pointed at the nearest
1. sink
3. floor
5. desktop
BECAUSE
II. pouring the acid into the water is too dangerous, since
it increases one’s chances of spilling acid.
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct
explanation of I
5. I and II are BOTH TRUE and II IS a correct explanation
of I
94. Which device is preferred to remove a spill of a large
quantity of a caustic chemical from clothing?
1.
2.
3.
4.
5.
1.
2.
3.
4.
a fire blanket
a safety shower
an eye-wash facility
an approved fire extinguisher
an externally-vented fume hood
95. In the laboratory, never dip a stirring rod into a reagent
bottle because
1.
2.
3.
4.
the bottle may tip
the rod might break
the rod may puncture the bottle
the contents of the bottle may become
contaminated
5. the amount of liquid remaining on the rod is too
small to be used
91. Through experimentation, a student determined the
vapor pressure of water at 60°C to be 140.2 torr. If the
actual vapor pressure of water at 60°C is 149.4 torr, what
is the student's percent error?
1. .0616%
3. 6.16%
5. 6.56%
2. wall
4. ceiling
2. .0656%
4. –6.16%
96. Two samples are massed using different balances.
What is the total mass of the samples to the correct
number of significant digits?
1.
3.
5.
H-Chem 2015-16
Page 9
2.
4.
Dr. Powell
97. How many 100 mg tetracycline capsules can be made
from 1 kg of tetracycline?
1. 10
3. 1,000
5. 100,000
99. Which is the proper reading for the buret?
2. 100
4. 10,000
98. An unknown mass of an element reacts completely with
1.811 g of sulfur and 3.613 g of oxygen to produce 7.124 g
of a compound containing the element, S, and O. What
additional information is required to determine the
unknown mass?
1.
2.
3.
4.
5.
The formula of the product.
The balanced reaction equation.
The molar mass of the unknown element.
The electron configuration of the unknown element.
No additional information is needed.
1. 21.55 mL
3. 22.3 mL
5. 22.60 mL
2. 21.7 mL
4. 22.45 mL
100. Which should be used to accurately measure 185 mL of
an aqueous solution? A 250 mL
1. beaker
3. volumetric flask
5. pipet
2. Florence flask
4. graduated cylinder
101. Which apparatus delivers 50.00 mL of liquid most
accurately?
1.
2.
3.
4.
5.
H-Chem 2015-16
Page 10
50 mL buret
50 mL beaker
50 mL test tube
50 mL graduated cylinder
50 mL flask
Dr. Powell