Download 1. The Greek philosopher Democritus coined what word for a tiny

1. The Greek philosopher Democritus coined
what word for a tiny piece of matter that
cannot be divided?
A. element
B. atom
C. electron
D. molecule
1. The Greek philosopher Democritus
coined what word for a tiny piece of
matter that cannot be divided?
A. element
B. atom
C. electron
D. molecule
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2. Democritus thought that matter was
made of tiny particles
A. of earth, air, fire, and water.
B. that could not be divided.
C. that could be divided.
D. that were all round and smooth.
2. Democritus thought that matter was
made of tiny particles
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A. of earth, air, fire,
and water.
B. that could not be
divided.
C. that could be
divided.
D. that were all round
and smooth.
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3. If 2 grams of element X combine with 4
grams of element Y to form compound
XY, how many grams of element Y would
combine with 14 grams of X to form the
same compound?
A. 7 grams
B. 14 grams
C. 21 grams
D. 28 grams
3. If 2 grams of element X combine with 4
grams of element Y to form compound XY, how
many grams of element Y would combine with10
14 grams of X to form the same compound?
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A. 7 grams
B. 14 grams
C. 21 grams
D. 28 grams
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4. According to John Dalton’s
observations, when elements combine in a
compound,
A. the ratio of their masses is always the
same.
B. each element contributes an equal
number of atoms.
C. their volumes are always equal.
D. their masses are always equal.
4. According to John Dalton’s
observations, when elements combine in
a compound,
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A. the ratio of their masses
is always the same.
B. each element contributes
an equal number of
atoms.
C. their volumes are always
equal.
D. their masses are always
equal.
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5. Which of the following is NOT part of
John Dalton’s atomic theory?
A. All elements are composed of atoms.
B. All atoms of the same element have the
same mass.
C. Atoms contain subatomic particles.
D. A compound contains atoms of more
than one element.
5. Which of the following is NOT part of
John Dalton’s atomic theory?
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A. All elements are composed of
atoms.
B. All atoms of the same element
have the same mass.
C. Atoms contain subatomic
particles.
D. A compound contains atoms
of more than one element.
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6. Which of the following most accurately
represents John Dalton’s model of the
atom?
A. a tiny, solid sphere with an
unpredictable mass for a given element
B. a hollow sphere with a dense nucleus
C. a tiny, solid sphere with a predictable
mass for a given element
D. a sphere that is hollow throughout
6. Which of the following most accurately
represents John Dalton’s model of the
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atom?
A. a tiny, solid sphere with an
unpredictable mass for a
given element
B. a hollow sphere with a
dense nucleus
C. a tiny, solid sphere with a
predictable mass for a
given element
D. a sphere that is hollow
throughout
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7. J. J. Thomson’s experiments provided
evidence that an atom
A. is the smallest particle of matter.
B. contains negatively charged particles.
C. has a negative charge.
D. has a positive charge.
7. J. J. Thomson’s experiments provided
evidence that an atom
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A. is the smallest
particle of matter.
B. contains negatively
charged particles.
C. has a negative
charge.
D. has a positive
charge.
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Figure 4-1
8. The diagram in Figure 4-1 shows the
results of Rutherford’s gold foil
experiment. What caused some of the
alpha particles to bounce straight back
from the gold foil?
A. electrons in the gold atoms
B. negative charges in the gold atoms
C. other alpha particles
D. nuclei in the gold atoms
8. The diagram in Figure 4-1 shows the results
of Rutherford’s gold foil experiment. What
caused some of the alpha particles to bounce 10
straight back from the gold foil?
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A. electrons in the gold
atoms
B. negative charges in
the gold atoms
C. other alpha particles
D. nuclei in the gold
atoms
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9. Rutherford’s gold foil experiment
provided evidence for which of the
following statements?
A. Negative and positive charges are
spread evenly throughout an atom.
B. Alpha particles have a positive charge.
C. Gold is not as dense as previously
thought.
D. There is a dense, positively charged
mass in the center of an atom.
9. Rutherford’s gold foil experiment
provided evidence for which of the
following statements?
A. Negative and positive charges
are spread evenly throughout
an atom.
B. Alpha particles have a positive
charge.
C. Gold is not as dense as
previously thought.
D. There is a dense, positively
charged mass in the center
of an atom.
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10. Who provided evidence for the
existence of a nucleus in an atom?
A. John Dalton
B. J. J. Thomson
C. Democritus
D. Ernest Rutherford
10. Who provided evidence for the
existence of a nucleus in an atom?
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A. John Dalton
B. J. J. Thomson
C. Democritus
D. Ernest Rutherford
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11. In an atomic model that includes a
nucleus, positive charge is
A. concentrated in the center of an atom.
B. spread evenly throughout an atom.
C. concentrated at multiple sites in an atom.
D. located in the space outside the nucleus.
11. In an atomic model that includes a
nucleus, positive charge is
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A. concentrated in the
center of an atom.
B. spread evenly
throughout an atom.
C. concentrated at multiple
sites in an atom.
D. located in the space
outside the nucleus.
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12. Which statement best describes
Rutherford’s model of the atom?
A. It is like an avocado with the pit
representing the nucleus.
B. It is like an aquarium with swimming fish
representing positive charges.
C. It is like a fried egg with the yolk
representing the nucleus.
D. It is like a huge stadium with a positively
charged marble at the center.
12. Which statement best describes
Rutherford’s model of the atom?
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A. It is like an avocado with the pit
representing the nucleus.
B. It is like an aquarium with
swimming fish representing
positive charges.
C. It is like a fried egg with the
yolk representing the
nucleus.
D. It is like a huge stadium with a
positively charged marble at
the center.
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13. Which subatomic particle has a
negative charge?
A. electron
B. alpha particle
C. neutron
D. proton
13. Which subatomic particle has a
negative charge?
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A. electron
B. alpha particle
C. neutron
D. proton
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14. Which statement about subatomic
particles is NOT true?
A. Protons and neutrons have almost the
same mass.
B. Protons and electrons have opposite
charges.
C. Unlike protons and electrons, neutrons
have no charge.
D. Protons and neutrons have the same
charge.
14. Which statement about subatomic
particles is NOT true?
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A. Protons and neutrons have
almost the same mass.
B. Protons and electrons have
opposite charges.
C. Unlike protons and
electrons, neutrons have no
charge.
D. Protons and neutrons have
the same charge.
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15. Which statement about subatomic
particles is true?
A. Protons, neutrons, and electrons all have
about the same mass.
B. Unlike protons or neutrons, electrons
have no mass.
C. Neutrons have no charge and no mass.
D. An electron has far less mass than either
a proton or neutron.
15. Which statement about subatomic
particles is true?
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A. Protons, neutrons, and
electrons all have about the
same mass.
B. Unlike protons or neutrons,
electrons have no mass.
C. Neutrons have no charge and
no mass.
D. An electron has far less mass
than either a proton or
neutron.
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16. Which of the following is unique for
any given element?
A. the number of neutrons
B. the charge on the electrons
C. the number of protons
D. the mass of a neutron
16. Which of the following is unique for
any given element?
•
•
•
•
the number of
neutrons
the charge on the
electrons
the number of
protons
the mass of a
neutron
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17. The number of protons in one atom of
an element is that element’s
A. mass number.
.
B. balanced charge.
C. atomic number
D. isotope.
18. To find the number of neutrons in an
atom, you would subtract
A. mass number from atomic number.
B. atomic number from mass number.
C. atomic number from electron number.
D. isotope number from atomic number.
19. Suppose an atom has a mass number of
23. Which statement is true beyond any
doubt?
A. The atom has an odd number of
neutrons.
B. The atomic number is less than 11.
C. The atom is not an isotope.
D. The number of protons in the nucleus
does not equal the number of neutrons.
20. Which statement is true about oxygen17 and oxygen-18?
A. They do not have the same number of
protons.
B. Their atoms have an identical mass.
C. They are isotopes of oxygen.
D. The have the same mass number.
20. Which statement is true about
oxygen-17 and oxygen-18?
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A. They do not have the
same number of
protons.
B. Their atoms have an
identical mass.
C. They are isotopes of
oxygen.
D. The have the same
mass number.
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21. In Niels Bohr’s model of the atom,
electrons move
A. like balls rolling down a hill.
B. like planets orbiting the sun.
C. like popcorn in a popcorn popper.
D. like beach balls on water waves.
21. In Niels Bohr’s model of the atom,
electrons move
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A. like balls rolling
down a hill.
B. like planets orbiting
the sun.
C. like popcorn in a
popcorn popper.
D. like beach balls on
water waves.
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22. What can you assume has happened if
an electron moves to a higher energy
level?
A. The atom has become more stable.
B. The electron has lost energy.
C. The electron has gained energy.
D. The atom has lost an electron.
22. What can you assume has happened
if an electron moves to a higher energy
level?
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A. The atom has become
more stable.
B. The electron has lost
energy.
C. The electron has
gained energy.
D. The atom has lost an
electron.
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23. How was Bohr’s atomic model similar to
Rutherford’s model?
A. It assigned energy levels to electrons.
B. It described electron position in terms of
the electron cloud model.
C. It described how electrons gain or lose
energy.
D. It described a nucleus surrounded by a
large volume of space.
23. How was Bohr’s atomic model similar
to Rutherford’s model?
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A. It assigned energy levels to
electrons.
B. It described electron position in
terms of the electron cloud
model.
C. It described how electrons gain
or lose energy.
D. It described a nucleus
surrounded by a large volume
of space.
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24. Which statement accurately represents
the arrangement of electrons in Bohr’s
atomic model?
A. Electrons vibrate in fixed locations around
the nucleus.
B. Electrons travel around the nucleus in
fixed energy levels with energies that vary
from level to level.
C. Electrons travel around the nucleus in
fixed energy levels with equal amounts of
energy.
D. Electrons travel randomly in the relatively
large space outside the nucleus.
24. Which statement accurately represents the
arrangement of electrons in Bohr’s atomic
model?
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A. Electrons vibrate in fixed locations
around the nucleus.
B. Electrons travel around the nucleus in
fixed energy levels with energies
that vary from level to level.
C. Electrons travel around the nucleus in
fixed energy levels with equal
amounts of energy.
D. Electrons travel randomly in the
relatively large space outside the
nucleus.
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25. What do scientists use to predict the
locations of electrons in atoms?
A. Probability
B. algebra
C. geometry
D. ratios and proportions
25. What do scientists use to predict the
locations of electrons in atoms?
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A. probability
B. algebra
C. geometry
D. ratios and
proportions
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26. What does the electron cloud model
describe?
A. the most likely locations of electrons in
atoms
B. the precise locations of electrons in
atoms
C. the number of electrons in an atom
D. the mass of the electrons in an atom
26. What does the electron cloud model
describe?
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A. the most likely locations
of electrons in atoms
B. the precise locations of
electrons in atoms
C. the number of electrons
in an atom
D. the mass of the
electrons in an atom
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27. Which statement about electrons and
atomic orbitals is NOT true?
A. An electron has the same amount of
energy in all orbitals.
B. An orbital can contain a maximum of two
electrons.
C. An electron cloud represents all the
orbitals in an atom.
D. An atom’s lowest energy level has only
one orbital.
27. Which statement about electrons and
atomic orbitals is NOT true?
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A. An electron has the same
amount of energy in all
orbitals.
B. An orbital can contain a
maximum of two electrons.
C. An electron cloud represents all
the orbitals in an atom.
D. An atom’s lowest energy level
has only one orbital.
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28. Which of the following provides the best
analogy for an electron in an atomic
orbital?
A. a bee moving from flower to flower in a
garden
B. a bird resting on a tree branch
C. an ant crawling on the surface of a leaf
D. a bee trying to escape from a closed jar
28. Which of the following provides the
best analogy for an electron in an atomic
orbital?
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A. a bee moving from flower
to flower in a garden
B. a bird resting on a tree
branch
C. an ant crawling on the
surface of a leaf
D. a bee trying to escape
from a closed jar
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29. What is the difference between an atom in
the ground state and an atom in an excited
state?
A. The atom in the ground state has less
energy and is less stable than the atom in an
excited state.
B. The atom in an excited state has one fewer
electron than the atom in the ground state.
C. The atom in an excited state has more
energy and is less stable than the atom in the
ground state.
D. The atom in an excited state has one more
electron than the atom in the ground state.
29. What is the difference between an
atom in the ground state and an atom in
an excited state?
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A. The atom in the ground state has less
energy and is less stable than the
atom in an excited state.
B. The atom in an excited state has one
fewer electron than the atom in the
ground state.
C. The atom in an excited state has more
energy and is less stable than the
atom in the ground state.
D. The atom in an excited state has one
more electron than the atom in the
ground state.
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30. The glowing of a neon light is caused by
electrons emitting energy as they
A. move from lower to higher energy levels.
B. collide with other electrons.
C. move from higher to lower energy levels.
D. collide with the nucleus.
30. The glowing of a neon light is caused
by electrons emitting energy as they
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A. move from lower to
higher energy levels.
B. collide with other
electrons.
C. move from higher to
lower energy levels.
D. collide with the
nucleus.
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