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Unit 2 Practice Questions
I.
Atomic Theory
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Proton
Neutron
Electron
Isotope
Ion
1.
2.
3.
4.
Neutral charge; 1 amu
Positive charge
Negligible weight
Negative charge; pairs with opposite spin
1
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Atom
Ion
Neutron
Proton
electron
1. The smallest representative particle of helium
2. Loss or gain creates positively or negatively
charged ion, respectively
3. Particle responsible for positive nuclear charge
4. Isotopes of uranium always differ in their number
of this particle
5. Their number in the nucleus determines an
element’s atomic number
2
II
I
The periodic table
does not report
mass numbers
Addition of an
electron to an
atom creates a
positively charged
ion
BECAUSE
A mass number can be
assigned to one isotope of
an element but not to an
element in general
BECAUSE
Every electron carries a
negative charge
3
II
I
Ca is a neutral
atom
An element (X)
with an atomic
number of 16 has
14 electrons in X-2
BECAUSE
It has the same number of
protons and electrons
BECAUSE
Two protons bind the
two outermost
electrons
4
II
I
Two isotopes of the
same element have
the same mass
number
An atom of 12C
contains 12
protons
BECAUSE
Isotopes have the same
number of protons
BECAUSE
The identity of an
element is determined
by the number of
protons in the nuclei of
its atoms
5
II
I
The atomic number
of a neutral atom
that has a mass of
39 and has 19
electrons is 19
A large number of
alpha particles
were deflected in
the Rutherford
experiment
BECAUSE
The number of protons in a
a neutral atom is equal to
the number of electrons
BECAUSE
Alpha particles that
came close to the
nucleus of the gold
atoms were deflected
6
II
I
The isotope Cl-37
has 17 protons, 17
neutrons, and 17
electrons
BECAUSE
The atomic mass of
chlorine is 35.43 amu
7
Which of the following is not a conclusion
Rutherford made from his experiment with alpha
particles being shot at a thin sheet of gold foil?
(A)
(B)
(C)
(D)
(E)
An atom has a very small, compact nucleus
An atom is mainly empty space
An atom’s mass is concentrated in the nucleus
An atom has a very dense nucleus
An atom has a negatively charged nucleus
8
Which of the following statements is false regarding
sub-atomic particles?
(A) The proton has a positive one charge
(B) The neutron has no charge
(C) The electrons are found in regions of the atom
called orbitals
(D) The electrons have a greater mass than the
protons
(E) Protons and neutrons are the nucleons of the
atom
9
The two main regions of an atom are the
(A)
(B)
(C)
(D)
Principal energy levels and energy sublevels
Nucleus and kernel
Nucleus and energy levels
Planetary electrons and energy levels
10
An atom of beryllium consists of 4 protons, 5
neutrons and 4 electrons. The mass number of this
atom is
(A)
(B)
(C)
(D)
13
9
8
5
11
A mysterious element has the following relative
abundances: X-34 15%, X-35 20%, X-36 65%
Which of the following is true?
(A) The atomic mass of the element is closer to 34.1
(B) The atomic mass of the element is closer to 34.9
(C) The atomic mass of this element cannot be
determined without knowing exactly what X is
(D) A mass spectrophotometer would not be
helpful in determining the percentages of the
isotopes
(E) The atomic mass of this element is
approximately 35.5
12
Atoms of 235U and 238U differ in structure by three
(A)
(B)
(C)
(D)
Electrons
Isotopes
Neutrons
protons
13
Which of the following pairs of compounds can be
used to illustrate the Law of Multiple Proportions?
(A)
(B)
(C)
(D)
(E)
NO and NO2
CH4 and CO2
ZnO2 and ZnCl2
NH3 and NH4Cl
H2O and HCl
14
Two different sodium atoms or ions may differ in all
of the following ways EXCEPT
(A)
(B)
(C)
(D)
(E)
The number of electrons outside their nuclei
The overall charge they carry
Their mass numbers
The number of neutrons in their nuclei
The number of protons in their nuclei
15
Which of the following isotopes has the greatest
number of neutrons?
(A)
(B)
(C)
(D)
(E)
35Cl
31P
40Ar
41Ca
14C
16
Which is inconsistent with the concept of an
isotope?
(A)
(B)
(C)
(D)
(E)
Same atomic number
Different number of neutrons
Same mass number
Same name of the element
Same number of protons
17
Two isotopes of the same element will always differ
in
(A)
(B)
(C)
(D)
(E)
Mass number but never in atomic number
Atomic number but never in mass number
Charge outside but never inside their nuclei
Nuclear charge but never in overall charge
The number of electrons outside their nuclei
but never in the number of neutrons inside
their nuclei
18
What is the number of protons and neutrons in an
atom with mass number 89 and atomic number 39?
(A)
(B)
(C)
(D)
(E)
50 protons and 50 neutrons
50 protons and 39 neutrons
39 protons and 89 neutrons
39 protons and 50 neutrons
39 protons and 39 neutrons
19
Twenty-five percent of element X exists as 210X and
seventy-five percent of it exists as 214X. What is the
atomic weight of element X in amu?
(A)
(B)
(C)
(D)
(E)
85
211
212
213
214
20
Which of the following combinations represents an
element with a net charge of +1 with a mass
number of 75?
(A)
(B)
(C)
(D)
(E)
35 neutrons, 35 protons, 34 electrons
40 neutrons, 40 protons, 39 electrons
40 neutrons, 35 protons, 34 electrons
37 neutrons, 38 protons, 39 electrons
40 neutrons, 35 protons, 35 electrons
21
Of the following statements about the number of
subatomic particles in an ion of 3216S-2, which are
true?
I. 16 protons
II. 14 neutrons
III. 18 electrons
(A)
(B)
(C)
(D)
(E)
II only
III only
I and II only
I and III only
I, II and III
22
Isotopes of an element are related because which
of the following are the same in these isotopes?
I. Atomic mass
II. Atomic number
III. Arrangement of orbital electrons
(A)
(B)
(C)
(D)
(E)
I only
II only
I and II only
II and III only
I, II and III
23
For the radioactive element 99Tc, what is the correct
number of protons and neutrons?
(A)
(B)
(C)
(D)
(E)
43 protons and 56 neutrons
43 protons and 99 neutrons
56 protons and 43 neutrons
56 protons and 99 neutrons
Cannot be determined
24
II. Nuclear
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Alpha particle
Beta particle
Gamma radiation
Neutron
Positron
1.
2.
3.
4.
Has a negative charge
Has no mass and no charge
Has the greatest positive charge
Is very similar to an electron
25
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
Alpha decay
Beta decay
Positron emission
Gamma decay
Electron capture
1. Often accompanies other radioactive processes
2. Causes an atom to reduce its atomic number by 2
and its mass number by 4
3. Occurs when a neutron is converted into a proton in
a nucleus
26
II
I
is an isotope of
BECAUSE
The nuclei of both atoms
have the same number of
neutrons
Alpha particles are
the heaviest type
of radiation decay
BECAUSE
Alpha emission particles
consist of 2 protons and
2 neutrons
12C
14C
27
II
I
Nuclear fusion on
the sun converts
hydrogen to helium
with a release of
energy
The “bullet”
usually used to
initiate the fusion
of 235U is a
neutron
BECAUSE
BECAUSE
Some mass is converted to
energy in a solar fusion
Capture of the neutron
by the 235U nucleus
causes an unstable
condition that leads to
its disintegration
28
II
I
Radioactive
elements can emit
alpha particles,
beta particles, and
gamma rays
BECAUSE
Radioactive elements have
extremely stable nuclei
If a radioactive
sample with a
half-life of 40
years decays for
80 years, 25% of
the sample will
remain
BECAUSE
One half of 100% is 50%,
and one half of 50% is
25%
29
6 Li +
In the artificial transmutation 94Be + X
3
4 He, the particle represented by the letter X is a(n)
2
(A)
(B)
(C)
(D)
(E)
Beta particle
Positron
Deuteron
Proton
Alpha particle
30
14 C
6
What is X?
(A) 42He
(B) 0+1e
(C) 0-1e
(D) 11H
(E) 126C
14 N
7
+X
This reaction is an example of
(A) Alpha decay
(B) Beta decay
(C) Fusion
(D) Gamma decay
(E) Positron emission
31
226 Rn
86
218 Po
84
+ 42He
The radioactive decay shown above is an example of
(A) Positron emission
(B) Gamma ray emission
(C) Alpha decay
(D) Beta decay
(E) Ionization
32
131 I
53
131 Xe
54
+ 0-1e
The radioactive decay shown above is an example of
(A) Positron emission
(B) Gamma ray emission
(C) Alpha decay
(D) Beta decay
(E) Ionization
33
Which equation is an example of an artificial
transmutation?
(A)
(B)
(C)
(D)
(E)
238U
4He
+ 234Th
27Al + 4He
30P + 1 n
0
14C
14N + 0 e
-1
226Ra
4He + 222Rn
99 Tc
99 Tc + g
43
43
34
Which nuclear equation below demonstrates beta
decay?
(A) 238U
X + 234Th
3H
(B) 1H + X
17O + 1H
(C) 14N + X
(D) 234Pa
X + 234U
(E) None of the above demonstrates beta decay
35
Element 10220X is formed as a result of 3 alpha and 2
beta decays. Which of the following is the parent
element?
(A)
(B)
(C)
(D)
90 A
16
114 Z
24
114 Q
28
12 J + 90 L
8
12
36
Radioactive emanations can be detected by using
(A)
(B)
(C)
(D)
(E)
A person’s DNA
A block of lead
A Geiger counter
An x-ray machine
Graphite and heavy water
37
Sodium-24, a radioactive isotope used medically in
blood studies, decays by beta decay and has a halflife of 15.0 hours. What is the product of the
radioactive decay of sodium-24?
(A)
(B)
(C)
(D)
(E)
F-20
Ne-24
Ne-23
Na-23
Mg-24
38
After 62.0 hours, 1.0 gram remained unchanged
from a sample of potassium-42 (half life is 12.4
hours). What was the mas of potassium-42 in the
original sample?
(A)
(B)
(C)
(D)
(E)
64 grams
32 grams
16 grams
8 grams
4 grams
39
The emission of a beta particle results in a new
element with the atomic number
(A)
(B)
(C)
(D)
Increased by 1
Increased by 2
Decreased by 1
Decreased by 2
40
The energy released by the detonation of an atomic
bomb is NOT related to
(A)
(B)
(C)
(D)
(E)
Fission of the atom’s nucleus
Fusion of the atom’s nucleus
A chain reaction
The release of many neutrons
The uncontrolled speed of many neutrons
41
As a nucleus of a particular isotope disintegrates,
another nuclide is formed. This change in the
nucleus to form a new nuclide is called
(A)
(B)
(C)
(D)
(E)
Binding energy
Transmutation
Stability
Generation
Synthesis
42
Which element has no known stable isotope?
(A)
(B)
(C)
(D)
(E)
Carbon
Silver
Radon
Phosphorus
Lead
43
Which pair below would not be deflected or
attracted by the charged plates in an electric field?
(A)
(B)
(C)
(D)
(E)
An alpha particle and a neutron
A beta particle and a positron
A quark and a deuteron
A proton and gamma radiation
Gamma radiation and a neutron
44
In 6.20 hours, a 50.0 gram sample of silver-112
decays to 12.5 grams. What is the half-life of silver112?
(A)
(B)
(C)
(D)
(E)
1.60 hours
3.10 hours
6.20 hours
12.4 hours
18.6 hours
45
A physicist starts out with 320 grams of a
radioactive element Z and after 20 minutes he has
only 20 grams left. What is the half-life of element
Z?
(A)
(B)
(C)
(D)
(E)
2 minutes
3 minutes
4 minutes
5 minutes
10 minutes
46
Which of the following is closest in mass to a
proton?
(A)
(B)
(C)
(D)
Alpha particle
Positron
Neutron
Electron
47
The daughter nucleus formed when 18F undergoes
positron emission is
(A)
(B)
(C)
(D)
(E)
14N
16O
18O
19F
20Ne
48
In 12.4 hours, a 100 gram sample of an element
decays so that its mass is 25 grams. What is the
approximate half-life of this radioactive substance?
(A)
(B)
(C)
(D)
(E)
1.6 hours
3.1 hours
6.2 hours
24.8 hours
49.6 hours
49
Which of the following transmutations
demonstrates beta decay?
I. Bi-212
II. Pb-212
III. Ra-228
(A)
(B)
(C)
(D)
(E)
Po-212
Bi-212
Ac-228
I only
II only
II and III only
I and II only
I , II, and III
50
Which of the following forms of radioactive decay
have no electrical charge?
I. Alpha decay
II. Beta decay
III. Gamma decay
(A)
(B)
(C)
(D)
(E)
II only
III only
I and II only
I and III only
II and III only
51
Which of the following are uses for radiation and
radioactivity that are of benefit to us?
I. nuclear waste
II. radioisotopes
III. Excess exposure
(A)
(B)
(C)
(D)
(E)
I only
II only
III only
I and II only
I and III only
52
A patient undergoing treatment for thyroid cancer
receives a dose of radioactive iodine, which has a
half-life of 8.05 days. If the original dose contained 12
mg of iodine-131, what mass of iodine-131 remains
after 16.1 days?
53
III. Electrons
Questions 1-4 refer to the following:
(A) 1s
(B) 2s
(C) 3s
(D) 3p
(E) 3d
1. Contains up to 10 electrons
2. Contains one pair of electrons in the ground state
of lithium
3. Is exactly half filled in the ground state of
phosphorus
4. Contains a filled orbital in the ground state of
helium
54
II
I
Two electrons in
the 2s subshell
must have opposite
spins
Gas-phase
elements absorb
or emit only
specific
wavelengths of
visible light when
excited by an
electric current
BECAUSE
The Pauli exclusion
principle states that no two
electrons in the same atom
can have identical quantum
numbers
BECAUSE
The energy levels that
electrons can occupy in
gas-phase atoms and
molecules are
continuous
55
II
I
The 4s orbital fills
before the 3d
orbitals
The ground state
electron
configuration of
Cu is [Ar]4s13d10
BECAUSE
Subshells fill in the order
from lower to higher
energy
BECAUSE
Completely filled and
half-filled d orbitals
bestow special
electronic stabilization
56
II
I
An element that
has the electron
configuration
1s22s22p63s23p64s2
3d3 is a transition
element
BECAUSE
The transition elements
from scandium to zinc are
filling the 3d orbitals
57
In a hydrogen atom, when an electron jumps from
an excited energy state to a more stable energy
state,
(A) Electromagnetic radiation is emitted by the
atom
(B) Electromagnetic radiation is absorbed by the
atom
(C) The atom becomes a positively charged ion
(D) The atom becomes a negatively charged ion
(E) The atom undergoes nuclear decay
58
Which principal energy level has exactly four
sublevels?
(A)
(B)
(C)
(D)
(E)
1
2
3
4
5
59
Which metal is not correctly paired with its color
when put into a flame?
(A)
(B)
(C)
(D)
(E)
Lithium-red
Potassium-lilac
Sodium-yellow
Copper-orange
Magnesium-white
60
All of the following statements are consistent with
Bohr’s model of the atom EXCEPT
(A) An electron may assume an infinite number of
velocities
(B) An atom is most stable when its electron
configuration is that of the ground state
(C) The electron shell numbers represent the
principal energy levels
(D) Electrons in orbitals closest to the nucleus have
the lowest energy
(E) They are all consistent
61
The maximum number of electrons in a shell with the
principal quantum number equal to 4 is
(A)
(B)
(C)
(D)
2
10
16
32
62
If the principal quantum number of a shell is equal to
2, what types of orbitals will be present?
(A) s
(B) s and p
(C) s, p, and d
(D) s, p, d and f
63
An element with an atomic number of 26 has how
many electrons in the 3d sublevel?
(A) 0
(B) 2
(C) 6
(D) 8
(E) 10
64
Which of the following orbitals has the lowest
energy?
(A) 2p
(B) 3s
(C) 3d
(D) 4s
(E) 3p
65
How many valence electrons are in an atom with the
configuration 1s22s22p63s23p2?
(A)
(B)
(C)
(D)
(E)
6
5
4
3
2
66
The electron configuration 1s22s22p63s23p64s23d7
represents an atom of the element
(A)
(B)
(C)
(D)
(E)
Br
Co
Cd
Ga
Mg
67
The lowest principal quantum number that an
electron can have is
(A)
(B)
(C)
(D)
0
1
2
3
68
The sublevel that has only one orbital is identified by
the letter
(A)
(B)
(C)
(D)
s
p
d
f
69
The sublevel that can be occupied by a maximum of
10 electrons is identified by the letter
(A)
(B)
(C)
(D)
s
p
d
f
70
An orbital may never be occupied by
(A)
(B)
(C)
(D)
1 electron
2 electrons
3 electrons
0 electrons
71
A neutral species whose electron configuration is
1s22s22p63s23p64s23d104p65s24d105p6 is
(A)
(B)
(C)
(D)
(E)
Highly reactive
A positively charged ion
A noble gas
A transition metal
A lanthanide element
72
In going from1s22s22p63s23p64s1 to
1s22s22p63s23p54s2 , an electron would
(A)
(B)
(C)
(D)
(E)
Absorb energy
Emit energy
Relax to the ground state
Bind to another atom
Undergo no change in energy
73
Which of the following atoms does
1s22s22p63s23p63d2 represent?
(A)
(B)
(C)
(D)
(E)
An excited state Ca atom
A ground state Ca atom
An excited state Sc atom
An excited state K atom
None of the above
74
Which electron configuration shows that of an
excited atom?
(A)
(B)
(C)
(D)
(E)
1s22s22p63s1
1s22s22p63s23p63d1
1s22s22p4
1s22s22p63s23p64s2
1s22s22p63s23p3
75
Which of the following correctly represents an
excited state of scandium?
(A)
(B)
(C)
(D)
(E)
1s22s22p63s23p64s23d1
1s22s32p53s23p64s23d1
1s22s22p63s23p64s13d2
1s22s22p63s23p64s23d2
1s22s22p63s23p64s03d1
76
The electron configuration for an atom of the
element Tc is
(A)
(B)
(C)
(D)
(E)
1s22s22p63s23p64s23d104p55s25p6
1s22s22p63s23p64s23d104p35s24d5
1s22s22p63s23p64s23d104p3
1s22s22p63s23p63d15
1s22s22p63s23p64s23d104p65s24d5
77
IV. Periodic Table
Questions 1-3 refer to the following:
(A) F
(B) Li
(C) Fe
(D) He
(E) Si
1. Shows both the properties of metals and nonmetals
2. Has the greatest ionization energy
3. Has the greatest electronegativity
78
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
K
As
Be
Se
Ir
1.
2.
3.
4.
Metalloid
Nonmetal
Group 1A metal
Is an alkaline earth metal
79
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
Alkali metal
Alkaline earth metal
Transition metal
Halogen
Noble gas
1.
2.
3.
4.
Reacts most vigorously with water
Is chemically inert
Has the highest first ionization energy in its period
Contains elements in the solid, liquid and gas
phases at STP
80
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
Ionization energy
Electronegativity
Atomic radius
Atomic number
Mass number
1. Is the measure of the pull of the nucleus of an
atom on the electrons of other atoms bonded to it
2. Is the energy required to remove an electron from
an atom
3. Is equal to the number of protons in an atom
81
I
K is considered to
be a metal
As you go from
left to right across
the periodic table
the elements tend
to become more
metallic in
character
II
BECAUSE
When K becomes an ion its
atomic radius increases
BECAUSE
As you go from left to
right across the periodic
table the elements tend
to lose electrons
82
II
I
Elemental fluorine
is more reactive
than elemental
neon
Isotopes of a
particular element
have nearly
identical chemical
behavior
BECAUSE
Neon has a larger atomic
weight than fluorine
BECAUSE
They have identical
electron configurations
83
II
I
The element with
an electron
configuration of
[He]2s1 has a larger
atomic radius than
fluorine
Atomic radii
increase down a
group
BECAUSE
The element with an
electron configuration of
[He]2s1 has a greater
nuclear charge than
fluorine
BECAUSE
The higher the atomic
number within a group,
the smaller the atom
84
Which of the following substances are liquids at
room temperature?
I. Hg
II. Br2
III. Si
(A)
(B)
(C)
(D)
(E)
I only
II only
I and II only
II and III only
I , II, and III
85
According to placement in the periodic table, which
statements regarding the first ionization energies of
certain elements should be true?
I. Li has a higher value than Na
II. K has a higher value than Cs
III. Na has a higher value than Al
(A)
(B)
(C)
(D)
(E)
I only
III only
I and II only
II and III only
I , II, and III
86
The modern periodic table is arranged based upon
atomic
(A)
(B)
(C)
(D)
(E)
Isotopes
Number
Density
Radius
Mass
87
Which of the following elements has the lowest
electronegativity?
(A)
(B)
(C)
(D)
(E)
Cesium
Strontium
Calcium
Barium
Potassium
88
Where are the highest ionization energies found in
the periodic table?
(A)
(B)
(C)
(D)
(E)
Upper left corner
Lower left corner
Upper right corner
Lower right corner
Middle of transition elements
89
The most active nonmetal has
(A)
(B)
(C)
(D)
(E)
A high electronegativity
A low electronegativity
A medium electronegativity
Large atomic radii
A deliquescent property
90
Which of the following metals is most reactive?
(A)
(B)
(C)
(D)
(E)
Na
Mg
Cu
Au
Cl
91
Which of the following is NOT true regarding nickel,
Ni?
(A)
(B)
(C)
(D)
(E)
It is malleable
It is ductile
It is lustrous
It is an insulator
It forms colored compounds
92
Which of the following represents an ordering of the
period 4 elements by increasing atomic size?
(A)
(B)
(C)
(D)
(E)
K, Kr, Ca, Br
K, Ca, Br, Kr
Kr, Br, Ca, K
Ca, K, Br, Kr
Br, Kr, Ca, K
93
An element has the following properties: shiny,
brittle, poor electrical conductivity, and high melting
point. This element can be best classified as a
(A)
(B)
(C)
(D)
(E)
Alkali metal
Halogen
Metalloid
Transition metal
Noble gas
94
The order of the elements in the periodic table is
based on
(A)
(B)
(C)
(D)
(E)
The number of neutrons
The radius of the atom
The atomic number
The atomic weight
The number of oxidation states
95
The elements within each column of the periodic
table
(A)
(B)
(C)
(D)
(E)
Have similar valence electron configurations
Have similar atomic radii
Have the same principal quantum number
Will react to form stable elements
Have no similar chemical properties
96
Which element has the greatest electronegativity?
(A)
(B)
(C)
(D)
(E)
Chlorine
Oxygen
Sulfur
Phosphorus
Fluorine
97
Which of these elements is the most electronegative?
(A)
(B)
(C)
(D)
(E)
S
Cl
Na
Mg
P
98
The elements that display the greatest nonmetallic
character are located toward which corner of the
periodic table?
(A)
(B)
(C)
(D)
(E)
Upper left
Dead center
Lower right
Lower left
Upper right
99
Which group contains elements in the solid, liquid
and gas phases at 298K and 1 atm?
(A)
(B)
(C)
(D)
(E)
1
2
16
17
18
100
An element that has a high first ionization energy and
is chemically inactive would most likely be
(A)
(B)
(C)
(D)
(E)
A noble gas
A transition element
An alkali metal
A halogen
An alkaline earth metal
101
As the elements of period 2 are considered from left
to right, there is generally a decrease in
(A)
(B)
(C)
(D)
(E)
Ionization energy
Electronegativity
Metallic character
Nonmetallic character
None of the above
102
Which of the following has the greatest affinity for
electrons?
(A)
(B)
(C)
(D)
(E)
Na
Cl
Br
K
C
103
All members of Group 1A have similar reactivity
because
(A) They have the same number of protons
(B) They have the same number of electrons
(C) They have similar outer-shell electron
configurations
(D) They have valence electrons with the same
quantum numbers
(E) They have the same number of neutrons
104
Arrange the following elements in order of
decreasing nonmetallic character:
Ge,Sn,Pb,Si
(A)
(B)
(C)
(D)
Pb, Sn, Ge, Si
Ge, Sn, Pb, Si
Si, Ge, Sn, Pb
They all have equal nonmetallic character since
they are all in the same column of the periodic
table
(E) None of the above
105
Which of the following is NOT a property of Group IA
elements?
(A)
(B)
(C)
(D)
(E)
Low ionization energies
Low electronegativities
High melting points
Metallic bonding
Electrical conductivity
106
Which of the following elements would have the
largest atomic radius?
(A)
(B)
(C)
(D)
(E)
Cl
F
Li
Ne
Na
107
Which of the following elements would have the
lowest first ionization energy?
(A)
(B)
(C)
(D)
(E)
Fluorine
Oxygen
Nitrogen
Carbon
Boron
108