Download Unit Two Test Review

Unit Two Test Review
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According to the law of definite proportions,
any two samples of water, H2O,
A.
B.
C.
D.
will be made up of only particles consisting of two
atoms of hydrogen and one atom of oxygen.
will have the same ratio of mass of hydrogen to
mass of oxygen.
will have a 2:1 ratio of mass of hydrogen to mass
of oxygen.
Both (A) and (B)
(1)
According to the law of definite proportions,
any two samples of water, H2O,
A.
B.
C.
D.
will be made up of only particles consisting of two
atoms of hydrogen and one atom of oxygen.
will have the same ratio of mass of hydrogen to
mass of oxygen.
will have a 2:1 ratio of mass of hydrogen to mass
of oxygen.
Both (A) and (B)
(1)
The law that states that mass cannot be
created or destroyed in ordinary chemical
and physical changes is known as the law of
A.
B.
C.
D.
conservation of mass.
mass action.
multiple proportions.
definite composition.
(2)
The law that states that mass cannot be
created or destroyed in ordinary chemical
and physical changes is known as the law of
A.
B.
C.
D.
conservation of mass.
mass action.
multiple proportions.
definite composition.
(2)
“When two elements combine to form two or
more compounds, the mass of one element
that combines with a given mass of the other
element is in the ratio of small whole
numbers.” This statement is known as the
law of
A.
B.
C.
D.
conservation of mass.
mass action.
multiple proportions.
definite composition.
(3)
“When two elements combine to form two or
more compounds, the mass of one element
that combines with a given mass of the other
element is in the ratio of small whole
numbers.” This statement is known as the
law of
A.
B.
C.
D.
conservation of mass.
mass action.
multiple proportions.
definite composition.
(3)
Which two compounds are examples of the
law of multiple proportions?
A.
B.
C.
D.
FeCl3 and Fe2(SO4)3
O2 and O3
CO and CO2
FeCl2 and Fe(NO3)2
(4)
Which two compounds are examples of the
law of multiple proportions?
A.
B.
C.
D.
FeCl3 and Fe2(SO4)3
O2 and O3
CO and CO2
FeCl2 and Fe(NO3)2
(4)
The law of multiple proportions can be partly
explained by the idea that
A. elements can combine in only one way to
form compounds.
B. whole atoms of the same two elements
combine to form different compounds.
C. elements in a compound always occur in a
1:1 ratio
D. only atoms of the same element can
combine.
(5)
The law of multiple proportions can be partly
explained by the idea that
A. elements can combine in only one way to
form compounds.
B. whole atoms of the same two elements
combine to form different compounds.
C. elements in a compound always occur in a
1:1 ratio
D. only atoms of the same element can
combine.
(5)
The observation that the mass of carbon
dioxide formed from the reaction of carbon
and oxygen equals the combined masses of
the carbon and oxygen that reacted supports
the law of
A.
B.
C.
D.
mass action
multiple proportions
definite proportions
conservation of mass.
(6)
The observation that the mass of carbon
dioxide formed from the reaction of carbon
and oxygen equals the combined masses of
the carbon and oxygen that reacted supports
the law of
A.
B.
C.
D.
mass action
multiple proportions
definite proportions
conservation of mass.
(6)
An atomic theory based on scientific
observations started about
A.
B.
C.
D.
400 BCE.
1800
1900
1930
(7)
An atomic theory based on scientific
observations started about
A.
B.
C.
D.
400 BCE.
1800
1900
1930
(7)
Dalton’s atomic theory helped explain the
law of conservation of mass because is stated
that atoms
A.
B.
C.
D.
could not combine.
could not be created or destroyed.
all had the same mass.
were invisible.
(8)
Dalton’s atomic theory helped explain the
law of conservation of mass because is stated
that atoms
A.
B.
C.
D.
could not combine.
could not be created or destroyed.
all had the same mass.
were invisible.
(8)
Dalton’s atomic theory does NOT support
which of the following observations?
A. Matter is neither created nor destroyed in
chemical and physical changes.
B. Atoms of most elements are made up of
protons, neutrons, and electrons.
C. NO and NO2 are compounds of nitrogen and
oxygen.
D. Hydrogen atoms differ from oxygen atoms.
(9)
Dalton’s atomic theory does NOT support
which of the following observations?
A. Matter is neither created nor destroyed in
chemical and physical changes.
B. Atoms of most elements are made up of
protons, neutrons, and electrons.
C. NO and NO2 are compounds of nitrogen and
oxygen.
D. Hydrogen atoms differ from oxygen atoms.
(9)
Dalton failed to recognize that substances
can exist in the form
A.
B.
C.
D.
AB
A2B
A2
AB2
(10)
Dalton failed to recognize that substances
can exist in the form
A.
B.
C.
D.
AB
A2B
A2
AB2
(10)
From observing that, within a cathode tube,
cathode rays could move a paddle wheel
placed in their path, J.J. Thomson concluded
that
A. a magnetic field was produced.
B. particles were passing from the cathode to the
anode.
C. there was a high-pressure gas within the tube.
D. atoms are indivisible.
(11)
From observing that, within a cathode tube,
cathode rays could move a paddle wheel
placed in their path, J.J. Thomson concluded
that
A. a magnetic field was produced.
B. particles were passing from the cathode to the
anode.
C. there was a high-pressure gas within the tube.
D. atoms are indivisible.
(11)
The rays produced in a cathode tube in early
experiments were
A.
B.
C.
D.
only affected by magnetic fields.
only affected by electric fields.
were attracted by the positive electrode.
All of the above.
(12)
The rays produced in a cathode tube in early
experiments were
A.
B.
C.
D.
only affected by magnetic fields.
only affected by electric fields.
were attracted by the positive electrode.
All of the above.
(12)
The behavior of cathode rays led scientists to
conclude that the rays were composed of
A.
B.
C.
D.
energy.
positively charged particles.
negatively charged particles.
uncharged particles.
(13)
The behavior of cathode rays led scientists to
conclude that the rays were composed of
A.
B.
C.
D.
energy.
positively charged particles.
negatively charged particles.
uncharged particles.
(13)
Because cathodes made of different metallic
elements produced cathode rays, scientists
generalized that
A.
B.
C.
D.
all atoms have electrons.
atoms are indivisible.
atoms carry a positive charge.
electrons vary in charge.
(14)
Because cathodes made of different metallic
elements produced cathode rays, scientists
generalized that
A.
B.
C.
D.
all atoms have electrons.
atoms are indivisible.
atoms carry a positive charge.
electrons vary in charge.
(14)
Because most of the alpha particles in
Rutherford’s gold-foil experiments passed
through the foil, he concluded that
A.
B.
C.
D.
atoms contained no charged particles.
atoms were mostly empty space.
electrons formed in the nucleus.
atoms contained a positively charged,
pudding-like material.
(15)
Because most of the alpha particles in
Rutherford’s gold-foil experiments passed
through the foil, he concluded that
A.
B.
C.
D.
atoms contained no charged particles.
atoms were mostly empty space.
electrons formed in the nucleus.
atoms contained a positively charged,
pudding-like material.
(15)
Because a few alpha particles were deflected
back from the foil in Rutherford’s gold-foil
experiments, he concluded that the particles
were
A. striking electrons.
B. indivisible.
C. repelled by tiny regions of high positive
charge.
D. magnetic.
(16)
Because a few alpha particles were deflected
back from the foil in Rutherford’s gold-foil
experiments, he concluded that the particles
were
A. striking electrons.
B. indivisible.
C. repelled by tiny regions of high positive
charge.
D. magnetic.
(16)
Which of the following descriptions is not a
characteristic of the nucleus of an atom?
A.
B.
C.
D.
positively charged
contains uncharged particles
accounts for most of the atom’s volume
accounts for most of the atom’s mass
(17)
Which of the following descriptions is not a
characteristic of the nucleus of an atom?
A.
B.
C.
D.
positively charged
contains uncharged particles
accounts for most of the atom’s volume
accounts for most of the atom’s mass
(17)
29
A neutral atom of 14
Si
A. has an atomic number of 29.
B. contains a total of 43 electrons, protons, and
neutrons.
C. contains 15 protons and 14 neutrons.
D. Both (A) and (C)
(18)
29
A neutral atom of 14
Si
A. has an atomic number of 29.
B. contains a total of 43 electrons, protons, and
neutrons.
C. contains 15 protons and 14 neutrons.
D. Both (A) and (C)
(18)
Which of the following atoms contains the
most neutrons?
A.
B.
C.
D.
43
20
Ca
45
21 Sc
49
22 Ti
50
24 Cr
(19)
Which of the following atoms contains the
most neutrons?
A.
B.
C.
D.
43
20
Ca
45
21 Sc
49
22 Ti
50
24 Cr
(19)
Each of the three isotopes of hydrogen,
hydrogen-1, hydrogen-2, and hydrogen-3,
A.
B.
C.
D.
contains one neutron and one proton.
contains at least one neutron.
has one proton in its nucleus.
is equally abundant.
(20)
Each of the three isotopes of hydrogen,
hydrogen-1, hydrogen-2, and hydrogen-3,
A.
B.
C.
D.
contains one neutron and one proton.
contains at least one neutron.
has one proton in its nucleus.
is equally abundant.
(20)
Which of the following atomic models could
be referred to as the “solar-system” model of
the atom?
A.
B.
C.
D.
Thomson’s plum-pudding model
Rutherford model
Bohr model
quantum model
(21)
Which of the following atomic models could
be referred to as the “solar-system” model of
the atom?
A.
B.
C.
D.
Thomson’s plum-pudding model
Rutherford model
Bohr model
quantum model
(21)
According to the Bohr model of the atom,
which particles are allowed to exist in any
one of a number of energy levels?
A.
B.
C.
D.
electrons
protons
neutrons
both (A) and (B)
(22)
According to the Bohr model of the atom,
which particles are allowed to exist in any
one of a number of energy levels?
A.
B.
C.
D.
electrons
protons
neutrons
both (A) and (B)
(22)
Which model was developed in an attempt to
explain hydrogen’s line emission spectrum?
A.
B.
C.
D.
Thomson’s plum-pudding model
Rutherford model
Bohr model
quantum model
(23)
Which model was developed in an attempt to
explain hydrogen’s line emission spectrum?
A.
B.
C.
D.
Thomson’s plum-pudding model
Rutherford model
Bohr model
quantum model
(23)
The line-emission spectrum of an atom is
caused by the energies released when
electrons
A. jump from a lower energy level to a higher
energy level.
B. jump from a higher energy level to a lower
energy level.
C. jump from the ground state to an excited state.
D. None of the above.
(24)
The line-emission spectrum of an atom is
caused by the energies released when
electrons
A. jump from a lower energy level to a higher
energy level.
B. jump from a higher energy level to a lower
energy level.
C. jump from the ground state to an excited state.
D. None of the above.
(24)
Because excited hydrogen atoms always
produced the same line-emission spectrum,
scientists concluded that hydrogen
A.
B.
C.
D.
had no electrons.
did not release energy.
released energy of only certain values.
could only exist in the ground state.
(25)
Because excited hydrogen atoms always
produced the same line-emission spectrum,
scientists concluded that hydrogen
A.
B.
C.
D.
had no electrons.
did not release energy.
released energy of only certain values.
could only exist in the ground state.
(25)
The flame color produced by heated metal
ions is due to electrons that
A. jump from a lower energy level to a higher
energy level.
B. jump from a higher energy level to a lower
energy level.
C. jump from the ground state to an excited state.
D. None of the above.
(26)
The flame color produced by heated metal
ions is due to electrons that
A. jump from a lower energy level to a higher
energy level.
B. jump from a higher energy level to a lower
energy level.
C. jump from the ground state to an excited state.
D. None of the above.
(26)
If electromagnetic radiation A has a lower
frequency that electromagnetic radiation B,
then, compared to B
A. the wavelength of A is shorter.
B. the energy of A is lower.
C. A is more particle-like.
D. Both (A) and (C).
(27)
If electromagnetic radiation A has a lower
frequency that electromagnetic radiation B,
then, compared to B
A. the wavelength of A is shorter.
B. the energy of A is lower.
C. A is more particle-like.
D. Both (A) and (C).
(27)
Quantum number n provides what
information regarding the location of
electrons in an atom?
A.
B.
C.
D.
orbital shape
orbital orientation (tilt)
electron spin
energy level
(28)
Quantum number n provides what
information regarding the location of
electrons in an atom?
A.
B.
C.
D.
orbital shape
orbital orientation (tilt)
electron spin
energy level
(28)
How many orbitals are in a p-sublevel (psubshell)?
A.
B.
C.
D.
1
3
5
7
(29)
How many orbitals are in a p-sublevel (psubshell)?
A.
B.
C.
D.
1
3
5
7
(29)
What is the maximum number of electrons
that can be located in a d-sublevel (d-subshell)?
A.
B.
C.
D.
2
6
10
14
(30)
What is the maximum number of electrons
that can be located in a d-sublevel (d-subshell)?
A.
B.
C.
D.
2
6
10
14
(30)
What information does an orbital give us
about the location of electrons in an atom?
A. The path or orbit of an electron around the
nucleus.
B. The location of an electron at any given point
in time.
C. The region of space outside of the nucleus
where an electron can be found 90% of the
time.
D. The direction of spin of an electron.
(31)
What information does an orbital give us
about the location of electrons in an atom?
A. The path or orbit of an electron around the
nucleus.
B. The location of an electron at any given point
in time.
C. The region of space outside of the nucleus
where an electron can be found 90% of the
time.
D. The direction of spin of an electron.
(31)
What is the maximum number of electrons
that can be located in any one orbital?
A.
B.
C.
D.
1
2
6
10
(32)
What is the maximum number of electrons
that can be located in any one orbital?
A.
B.
C.
D.
1
2
6
10
(32)
27
The electron configuration of 13
A.
B.
C.
D.
Al
1s2 2s2 2p6 3s1 3d2
1s2 2s2 2p5 3s2 3p2
1s2 2s2 2p6 3s2 3p1
[Ne]3s1 3p1 3d1
(33)
27
The electron configuration of 13
A.
B.
C.
D.
Al
1s2 2s2 2p6 3s1 3d2
1s2 2s2 2p5 3s2 3p2
1s2 2s2 2p6 3s2 3p1
[Ne]3s1 3p1 3d1
(33)
40
The electron configuration of 19
A.
B.
C.
D.
K
1s2 2s2 2p6 3s2 3p6 3d1
[Ar] 4s1
[Kr] 4s1
1s2 2s2 2p6 3s3 3p6
(34)
40
The electron configuration of 19
A.
B.
C.
D.
K
1s2 2s2 2p6 3s2 3p6 3d1
[Ar] 4s1
[Kr] 4s1
1s2 2s2 2p6 3s3 3p6
(34)
Which of the following orbital diagrams for
phosphorus is correct?
A.     
1s 2s
2p

3s
  __
3p
B.     
1s 2s
2p

3s
  
3p
C.     
1s 2s
2p

3s
  
3p
D.     
1s 2s
2p

3s
  __
3p
(35)
Which of the following orbital diagrams for
phosphorus is correct?
A.     
1s 2s
2p

3s
  __
3p
B.     
1s 2s
2p

3s
  
3p
C.     
1s 2s
2p

3s
  
3p
D.     
1s 2s
2p

3s
  __
3p
(35)
Which of the following pairs of atomic
symbols represent isotopes?
A.
B.
C.
D.
235
238
U and U
P and P8
32
83
P and Pb
50
51
Sn and Sb
4
(36)
Which of the following pairs of atomic
symbols represent isotopes?
A.
B.
C.
D.
235
238
U and U
P and P8
32
83
P and Pb
50
51
Sn and Sb
4
(36)
In developing his periodic table, Mendeleev
listed on cards each element’s name, atomic
mass, and
A.
B.
C.
D.
atomic number.
electron configuration.
isotopes.
properties.
(37)
In developing his periodic table, Mendeleev
listed on cards each element’s name, atomic
mass, and
A.
B.
C.
D.
atomic number.
electron configuration.
isotopes.
properties.
(37)
Mendeleev’s periodic table did not always
list elements in order of increasing atomic
mass because he grouped together elements
with similar
A.
B.
C.
D.
properties.
atomic numbers.
densities.
colors.
(38)
Mendeleev’s periodic table did not always
list elements in order of increasing atomic
mass because he grouped together elements
with similar
A.
B.
C.
D.
properties.
atomic numbers.
densities.
colors.
(38)
Mendeleev predicted that the gaps in his
periodic table represented
A.
B.
C.
D.
isotopes.
radioactive elements.
permanent gaps.
undiscovered elements.
(39)
Mendeleev predicted that the gaps in his
periodic table represented
A.
B.
C.
D.
isotopes.
radioactive elements.
permanent gaps.
undiscovered elements.
(39)
Moseley’s work with X-ray spectral lines led
to the discovery of a periodic law based on
increasing
A.
B.
C.
D.
atomic mass.
isotopes.
atomic number.
properties.
(40)
Moseley’s work with X-ray spectral lines led
to the discovery of a periodic law based on
increasing
A.
B.
C.
D.
atomic mass.
isotopes.
atomic number.
properties.
(40)
An electron that is found in the outermost
shell of an atom and determines the atom’s
chemical properties is called a(n)
A. paired electron.
B. p electron.
C. valence electron.
D. octave electron.
(41)
An electron that is found in the outermost
shell of an atom and determines the atom’s
chemical properties is called a(n)
A. paired electron.
B. p electron.
C. valence electron.
D. octave electron.
(41)
The periodic law states that the physical and
chemical properties of elements are functions
of their atomic
A.
B.
C.
D.
masses.
numbers.
radii.
structures.
(42)
The periodic law states that the physical and
chemical properties of elements are functions
of their atomic
A.
B.
C.
D.
masses.
numbers.
radii.
structures.
(42)
Refer to a periodic table. In which period is
calcium?
A.
B.
C.
D.
Period 2
Period 3
Period 4
Period 5
(43)
Refer to a periodic table. In which period is
calcium?
A.
B.
C.
D.
Period 2
Period 3
Period 4
Period 5
(43)
Refer to a periodic table. In which group is
calcium?
A.
B.
C.
D.
Group 1 (1A)
Group 2 (2A)
Group 17 (7A)
Group 18 (8A)
(44)
Refer to a periodic table. In which group is
calcium?
A.
B.
C.
D.
Group 1 (1A)
Group 2 (2A)
Group 17 (7A)
Group 18 (8A)
(44)
An element that has the electron
configuration [Ne]3s23p5 is in which period?
A.
B.
C.
D.
Period 2
Period 3
Period 5
Period 7
(45)
An element that has the electron
configuration [Ne]3s23p5 is in which period?
A.
B.
C.
D.
Period 2
Period 3
Period 5
Period 7
(45)
An element that has the electron
configuration [Ne]3s23p5 is in which group?
A.
B.
C.
D.
Group 2 (2A)
Group 5 (5A)
Group 7 (7B)
Group 17 (7A)
(46)
An element that has the electron
configuration [Ne]3s23p5 is in which group?
A.
B.
C.
D.
Group 2 (2A)
Group 5 (5A)
Group 7 (7B)
Group 17 (7A)
(46)
Elements in the s- or p- blocks of the
periodic table are called
A.
B.
C.
D.
alloys.
main-group elements.
metals.
transition metals.
(47)
Elements in the s- or p- blocks of the
periodic table are called
A.
B.
C.
D.
alloys.
main-group elements.
metals.
transition metals.
(47)
Elements in Group 18 (8A) have
A.
B.
C.
D.
very low reactivity.
good conductivity.
very high reactivity.
metallic character.
(48)
Elements in Group 18 (8A) have
A.
B.
C.
D.
very low reactivity.
good conductivity.
very high reactivity.
metallic character.
(48)
Nonmetallic elements in Group 17 (7A) that
react with metals to form salts are
A.
B.
C.
D.
alkali-metals.
halogens.
lanthanides.
noble gases.
(49)
Nonmetallic elements in Group 17 (7A) that
react with metals to form salts are
A.
B.
C.
D.
alkali-metals.
halogens.
lanthanides.
noble gases.
(49)
The outer shell electron configuration of an
alkaline-earth metal has
A.
B.
C.
D.
one electron in the s orbital.
two electrons in the s orbital.
one electron in the p orbital.
two electrons in the p orbital.
(50)
The outer shell electron configuration of an
alkaline-earth metal has
A.
B.
C.
D.
one electron in the s orbital.
two electrons in the s orbital.
one electron in the p orbital.
two electrons in the p orbital.
(50)
The alkali metals are found on Earth only in
compounds because they
A.
B.
C.
D.
have small atoms.
are very reactive elements.
are rare elements.
are metallic elements.
(51)
The alkali metals are found on Earth only in
compounds because they
A.
B.
C.
D.
have small atoms.
are very reactive elements.
are rare elements.
are metallic elements.
(51)
To which group does hydrogen belong?
A.
B.
C.
D.
Group 1 (1A)
Group 2 (2A)
Group 18 (8A)
None of the above.
(52)
To which group does hydrogen belong?
A.
B.
C.
D.
Group 1 (1A)
Group 2 (2A)
Group 18 (8A)
None of the above.
(52)
A metal is expected to be a(n)
A.
B.
C.
D.
nonconductor.
insulator.
conductor.
fluid at room temperature.
(53)
A metal is expected to be a(n)
A.
B.
C.
D.
nonconductor.
insulator.
conductor.
fluid at room temperature.
(53)
An element found in Groups 3 – 12
(3B – 2B) of the periodic table is classified
as a(n)
A.
B.
C.
D.
alkali metal.
alloy.
actinide.
transition metal.
(54)
An element found in Groups 3 – 12
(3B – 2B) of the periodic table is classified
as a(n)
A.
B.
C.
D.
alkali metal.
alloy.
actinide.
transition metal.
(54)
An element that has an outer shell electron
configuration consisting of two electrons in
the s orbital and two electrons in the d orbital
is in which group?
A.
B.
C.
D.
alkali metals.
alkaline earth metals.
transition metals.
halogens.
(55)
An element that has an outer shell electron
configuration consisting of two electrons in
the s orbital and two electrons in the d orbital
is in which group?
A.
B.
C.
D.
alkali metals.
alkaline earth metals.
transition metals.
halogens.
(55)
Lanthanide elements are found in which
block of the periodic table?
A.
B.
C.
D.
s
p
d
f
(56)
Lanthanide elements are found in which
block of the periodic table?
A.
B.
C.
D.
s
p
d
f
(56)
In which series of elements do all of the
elements undergo radioactive decay?
A.
B.
C.
D.
Period 5
Period 6
lanthanides
actinides
(57)
In which series of elements do all of the
elements undergo radioactive decay?
A.
B.
C.
D.
Period 5
Period 6
lanthanides
actinides
(57)
Ionization energy is the energy required to
remove ______ from an atom of an element.
A.
B.
C.
D.
the electron cloud.
all electrons.
one electron.
an ion.
(58)
Ionization energy is the energy required to
remove ______ from an atom of an element.
A.
B.
C.
D.
the electron cloud.
all electrons.
one electron.
an ion.
(58)
Across a period in the periodic table,
ionization energy generally
A.
B.
C.
D.
decreases.
decreases then increases.
increases.
remains constant.
(59)
Across a period in the periodic table,
ionization energy generally
A.
B.
C.
D.
decreases.
decreases then increases.
increases.
remains constant.
(59)
The decrease in ionization energy down a
group is due to
A. increased electron shielding.
B. decreased charge of the nucleus.
C. increased distance between the
nucleus and valence electrons.
D. Both (A) and (C)
(60)
The decrease in ionization energy down a
group is due to
A. increased electron shielding.
B. decreased charge of the nucleus.
C. increased distance between the
nucleus and valence electrons.
D. Both (A) and (C)
(60)
When determining the size of an atom by
measuring bond radius, the radius of an atom
is
A.
B.
C.
D.
equal to the distance between nuclei.
one-half the distance between nuclei.
twice the distance between nuclei.
one-fourth the distance between nuclei.
(61)
When determining the size of an atom by
measuring bond radius, the radius of an atom
is
A.
B.
C.
D.
equal to the distance between nuclei.
one-half the distance between nuclei.
twice the distance between nuclei.
one-fourth the distance between nuclei.
(61)
Across a period in the periodic table, atomic
radii generally
A.
B.
C.
D.
decrease.
decrease, then increase.
increase.
increase, then decrease.
(62)
Across a period in the periodic table, atomic
radii generally
A.
B.
C.
D.
decrease.
decrease, then increase.
increase.
increase, then decrease.
(62)
Down a group in the periodic table, atomic
radii generally
A.
B.
C.
D.
decrease.
decrease, then increase.
increase.
increase, then decrease.
(63)
Down a group in the periodic table, atomic
radii generally
A.
B.
C.
D.
decrease.
decrease, then increase.
increase.
increase, then decrease.
(63)
An element with the lowest electronegativity
would be located where in the periodic
table?
A.
B.
C.
D.
Group 1 (1A), Period 7
Group 13 (A), Period 4
Group 15 (5A), Period 3
Group 17 (7A), Period 2
(64)
An element with the lowest electronegativity
would be located where in the periodic
table?
A.
B.
C.
D.
Group 1 (1A), Period 7
Group 13 (A), Period 4
Group 15 (5A), Period 3
Group 17 (7A), Period 2
(64)
An element with the highest electronegativity
would be located where in the periodic table?
A.
B.
C.
D.
Group 1 (1A), Period 7
Group 13 (A), Period 4
Group 15 (5A), Period 3
Group 17 (7A), Period 2
(65)
An element with the highest electronegativity
would be located where in the periodic table?
A.
B.
C.
D.
Group 1 (1A), Period 7
Group 13 (A), Period 4
Group 15 (5A), Period 3
Group 17 (7A), Period 2
(65)
Refer to a periodic table and determine which
element below has the lowest electron
affinity.
A.
B.
C.
D.
Cl
Se
Cs
Te
(66)
Refer to a periodic table and determine which
element below has the lowest electron
affinity.
A.
B.
C.
D.
Cl
Se
Cs
Te
(66)
As the atomic number of the metals of
Group 1 (1A) increases, the ionic radius
A.
B.
C.
D.
increases.
decreases.
remains the same.
no particular trend is noted.
(67)
As the atomic number of the metals of
Group 1 (1A) increases, the ionic radius
A.
B.
C.
D.
increases.
decreases.
remains the same.
no particular trend is noted.
(67)
An element with the smallest anionic
(negative-ionic) radius would be located
where in the periodic table?
A.
B.
C.
D.
Group 1(1A), Period 7
Group 3 (3B), Period 4
Group 15 (5A), Period 3
Group 17 (7A), Period 2
(68)
An element with the smallest anionic
(negative-ionic) radius would be located
where in the periodic table?
A.
B.
C.
D.
Group 1(1A), Period 7
Group 3 (3B), Period 4
Group 15 (5A), Period 3
Group 17 (7A), Period 2
(68)
Which of the following elements behaves
similarly to calcium? Be able to explain
your answer!
A.
B.
C.
D.
magnesium
sodium
sulfur
chlorine
(69)
Which of the following elements behaves
similarly to calcium? Be able to explain
your answer!
A.
B.
C.
D.
magnesium
sodium
sulfur
chlorine
(69)
Which of the following elements behaves
most like aluminum? Be able to explain
your answer!
A.
B.
C.
D.
boron
magnesium
silicon
gallium
(70)
Which of the following elements behaves
most like aluminum? Be able to explain
your answer!
A.
B.
C.
D.
boron
magnesium
silicon
gallium
(70)
How many electrons does fluorine have
in its outermost shell in its ground state?
A.
B.
C.
D.
1
5
7
8
(71)
How many electrons does fluorine have
in its outermost shell in its ground state?
A.
B.
C.
D.
1
5
7
8
(71)
How many electrons does the fluoride
ion (F1-) have in its outermost shell in its
ground state?
A.
B.
C.
D.
1
5
7
8
(72)
How many electrons does the fluoride
ion (F1-) have in its outermost shell in its
ground state?
A.
B.
C.
D.
1
5
7
8
(72)
Highly reactive metallic elements that
react with water to form alkaline
solutions are called
A.
B.
C.
D.
actinides.
alkali metals.
halogens.
noble gases.
(73)
Highly reactive metallic elements that
react with water to form alkaline
solutions are called
A.
B.
C.
D.
actinides.
alkali metals.
halogens.
noble gases.
(73)
Which of the following properties is
NOT periodic, and when graphed versus
atomic number would show a continuous
upward trend?
A.
B.
C.
D.
ionization energy
electronegativity
atomic mass
atomic radius
(74)
Which of the following properties is
NOT periodic, and when graphed versus
atomic number would show a continuous
upward trend?
A.
B.
C.
D.
ionization energy
electronegativity
atomic mass
atomic radius
(74)
Compared to a calcium atom, a calcium
ion (Ca2+) has
A.
B.
C.
D.
fewer protons
fewer electrons
more electrons
more protons
(75)
Compared to a calcium atom, a calcium
ion (Ca2+) has
A.
B.
C.
D.
fewer protons
fewer electrons
more electrons
more protons
(75)
What is the total charge of the nucleus of
a helium atom?
A.
B.
C.
D.
+4
0
+2
-2
(76)
What is the total charge of the nucleus of
a helium atom?
A.
B.
C.
D.
+4
0
+2
-2
(76)