Download TEST-Atomic Structure

Atomic Structure Test
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. The Greek philosopher Democritus coined what word for a tiny piece of matter that cannot be divided?
a. element
c. electron
b. atom
d. molecule
____
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.
____
3. 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. 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 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. 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.
Figure 4-1
____
7. 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
c. other alpha particles
b. negative charges in the gold atoms
d. nuclei in the gold atoms
____
8. 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. Who provided evidence for the existence of a nucleus in an atom?
a. John Dalton
c. Democritus
b. J. J. Thomson
d. Ernest Rutherford
____ 10. 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. 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 subatomic particle has a negative charge?
a. electron
c. neutron
b. alpha particle
d. proton
____ 13. 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 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 of the following is unique for any given element?
a. the number of neutrons
c. the number of protons
b. the charge on the electrons
d. the mass of a neutron
____ 16. The number of protons in one atom of an element is that element’s
a. mass number.
c. atomic number.
b. balanced charge.
d. isotope.
____ 17. To find the number of neutrons in an atom, you would subtract
a. mass number from atomic number.
c. atomic number from electron number.
b. atomic number from mass number.
d. isotope number from atomic number.
____ 18. 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.
____ 19. Which statement is true about oxygen-17 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. In Niels Bohr’s model of the atom, electrons move
a. like balls rolling down a hill.
c. like popcorn in a popcorn popper.
b. like planets orbiting the sun.
d. like beach balls on water waves.
____ 21. What can you assume has happened if an electron moves to a higher energy level?
a. The atom has become more stable.
c. The electron has gained energy.
b. The electron has lost energy.
d. The atom has lost an electron.
____ 22. 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. 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. What do scientists use to predict the locations of electrons in atoms?
a. probability
c. geometry
b. algebra
d. ratios and proportions
____ 25. 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. 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 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. 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. 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. In figure 4-2, what is the main difference between the atomic model in panel 1 and the mdoel in panel 2?
a. Panel 1 shows an atom that has a
c. Panel 1 depicts an atom as a solid sphere
subatomic structure. Panel 2 shows an
without any subatomic particles. Panel 2
atom as a solid sphere without any
shows an atom that has a nucleus
subatomic particles.
surrounded by an electron cloud.
b. Panel 1 depicts an atom as a solid sphere
without any subatomic particles. Panel 2
shows an atom that has a subatomic
structure.
____ 31. In figure 4-2, what is the main difference between the atomic model in panel 2 and the model in panel 3?
a. The main difference is the wat in which
c. There is no real difference between panel
electron motion is depicted. In panel 2,
2 and panel 3.
the movement of electrons is represented
by fixed circular orbits. In panel 3, the
probable locations of the moving electrons
are represented by a cloud.
b. The main difference is in the nucleus. In
panel 2, the movement of electrons is
represented by fixed circular orbits. In
panel 3, the probable locations of the
moving electrons are represented by a
cloud.
____ 32. How is the atomic model in panel 2 helpful to your understanding of the atom? In what ways is it not
helpful?
a. It is helpful because it has protons and
c. It is helpful because it shows the general
electrons. It is not helpful because it
location of the subatomic particles in an
shows electrons in an electron cloud.
atom. It is not helpful because it implies
that electrons travel in fixed paths around
the nucleus.
b. It is helpful because it has subatomic
particles. It is not helpful because it has
the charges backwards.
____ 33. What are the atomic and mass numbers of the atom shown?
a. Atomic number of 17 and a mass number c. Atomic number of 8 and a mass number of
of 8.
9.
b. Atomic number of 8 and a mass number of
17.
____ 34. Would Dalton have recognized the model of a nucleus shown in Figure 4-3? Explain your answer.
a. Yes; because he thought of the atom as a c. No; because he thought of the atom as a
solid indivisible ball and had no
solid, indivis1ble ball and had no
knowledge of subatomic particles.
knowledge of subatomic particles.
b. Yes; because he thought of the atom as
d. No; because he thought of the atom as
having subatomic particles.
having subatomic particles.
____ 35. Would Rutherford have recognized the model of a nucleus in Figure 4-3? Explain your answer.
a. No; Rutherford demonstrated the
c. No, he thought of the atom as a solid
existence of a nucleus, named subatomic
sphere.
particles with a positive charge protons,
and predicted the existence of neutrons.
b. Yes; Rutherford demonstrated the
d. Yes, because it demonstrates the electron
existence of a nucleus, named subatomic
cloud model.
particles with a positive charge protons,
and predicted the existence of neutrons.
____ 36. Skip this question.
a. Alrighty
b. No problem
____ 37. Skip this question, too.
a. Rock on!
b. Woot!
c. Huzzah!
d. Skip what question?
Atomic Structure Test
Answer Section
MULTIPLE CHOICE
1. ANS: B
PTS: 1
DIF: L1
OBJ: 4.1.1 Describe ancient Greek models of matter.
2. ANS: B
PTS: 1
DIF: L2
OBJ: 4.1.1 Describe ancient Greek models of matter.
3. ANS: A
PTS: 1
DIF: L1
OBJ: 4.1.2 List the main points of Dalton’s atomic theory and describe his evidence for the existence of
atoms.
4. ANS: C
PTS: 1
DIF: L1
OBJ: 4.1.2 List the main points of Dalton’s atomic theory and describe his evidence for the existence of
atoms.
5. ANS: C
PTS: 1
DIF: L2
OBJ: 4.1.2 List the main points of Dalton’s atomic theory and describe his evidence for the existence of
atoms.
6. ANS: B
PTS: 1
DIF: L2
OBJ: 4.1.3 Explain how Thomson and Rutherford used data from experiments to produce their atomic
models.
7. ANS: D
PTS: 1
DIF: L1
OBJ: 4.1.3 Explain how Thomson and Rutherford used data from experiments to produce their atomic
models.
8. ANS: D
PTS: 1
DIF: L2
OBJ: 4.1.3 Explain how Thomson and Rutherford used data from experiments to produce their atomic
models.
9. ANS: D
PTS: 1
DIF: L1
OBJ: 4.1.3 Explain how Thomson and Rutherford used data from experiments to produce their atomic
models.
10. ANS: A
PTS: 1
DIF: L1
OBJ: 4.1.3 Explain how Thomson and Rutherford used data from experiments to produce their atomic
models.
11. ANS: D
PTS: 1
DIF: L2
OBJ: 4.1.3 Explain how Thomson and Rutherford used data from experiments to produce their atomic
models.
12. ANS: A
PTS: 1
DIF: L1
OBJ: 4.2.1 Identify three subatomic particles and compare their properties.
STA: MS.PS.3.a
13. ANS: D
PTS: 1
DIF: L1
OBJ: 4.2.1 Identify three subatomic particles and compare their properties.
STA: MS.PS.3.a
14. ANS: D
PTS: 1
DIF: L2
OBJ: 4.2.1 Identify three subatomic particles and compare their properties.
STA: MS.PS.3.a
15. ANS: C
PTS: 1
DIF: L2
OBJ: 4.2.1 Identify three subatomic particles and compare their properties.
STA: MS.PS.3.a
16. ANS: C
PTS: 1
DIF: L1
OBJ: 4.2.2 Distinguish the atomic number of an element from the mass number of an isotope, and use
these numbers to describe the structure of atoms.
STA: MS.PS.3.e
17. ANS: B
PTS: 1
DIF: L1
OBJ: 4.2.2 Distinguish the atomic number of an element from the mass number of an isotope, and use
these numbers to describe the structure of atoms.
STA: MS.PS.3.e
18. ANS: D
PTS: 1
DIF: L2
OBJ: 4.2.2 Distinguish the atomic number of an element from the mass number of an isotope, and use
these numbers to describe the structure of atoms.
STA: MS.PS.3.e
19. ANS: C
PTS: 1
DIF: L2
OBJ: 4.2.2 Distinguish the atomic number of an element from the mass number of an isotope, and use
these numbers to describe the structure of atoms.
STA: MS.PS.3.e
20. ANS: B
PTS: 1
DIF: L1
OBJ: 4.3.1 Describe Bohr’s model of the atom and the evidence for energy levels.
STA: MS.PS.3.a
21. ANS: C
PTS: 1
DIF: L1
OBJ: 4.3.1 Describe Bohr’s model of the atom and the evidence for energy levels.
STA: MS.PS.3.a
22. ANS: D
PTS: 1
DIF: L2
OBJ: 4.3.1 Describe Bohr’s model of the atom and the evidence for energy levels.
STA: MS.PS.3.a
23. ANS: B
PTS: 1
DIF: L2
OBJ: 4.3.1 Describe Bohr’s model of the atom and the evidence for energy levels.
STA: MS.PS.3.a
24. ANS: A
PTS: 1
DIF: L2
OBJ: 4.3.2 Explain how the electron cloud model represents the behavior and locations of electrons in
atoms. STA:
MS.PS.3.a
25. ANS: A
PTS: 1
DIF: L1
OBJ: 4.3.2 Explain how the electron cloud model represents the behavior and locations of electrons in
atoms. STA:
MS.PS.3.a
26. ANS: A
PTS: 1
DIF: L2
OBJ: 4.3.2 Explain how the electron cloud model represents the behavior and locations of electrons in
atoms. STA:
MS.PS.3.a
27. ANS: D
PTS: 1
DIF: L1
OBJ: 4.3.2 Explain how the electron cloud model represents the behavior and locations of electrons in
atoms. STA:
MS.PS.3.a
28. ANS: C
PTS: 1
DIF: L1
OBJ: 4.3.3 Distinguish the ground state from excited states of an atom based on electron configurations.
29. ANS: C
PTS: 1
DIF: L2
OBJ: 4.3.3 Distinguish the ground state from excited states of an atom based on electron configurations.
30. ANS: B
PTS: 1
31. ANS: A
PTS: 1
32. ANS: C
PTS: 1
33. ANS: B
PTS: 1
34. ANS: C
PTS: 1
35. ANS: B
PTS: 1
36. ANS: A
PTS: 1
37. ANS: B
PTS: 1
OTHER
38. ANS:
Panel 1 depicts an atom as a solid sphere without any subatomic particles. Panel 2 shows an atom that has a
subatomic structure.
PTS: 1
DIF: L1
OBJ: 4.1.2 List the main points of Dalton’s atomic theory and describe his evidence for the existence of
atoms. | 4.2.1 Identify three subatomic particles and compare their properties. | 4.3.1 Describe Bohr’s
model of the atom and the evidence for energy levels.
STA: MS.PS.3.a
39. ANS:
Protons have a positive charge, while neutrons have no charge. This atom has an atomic number of 8 and a
mass number of 17.
PTS: 1
DIF: L2
OBJ: 4.2.1 Identify three subatomic particles and compare their properties.
STA: MS.PS.3.a