Download Atomic Structure Worksheet

Atomic Structure
11/9/04
Name
Multiple Choice
Identify the letter of 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.
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.
____ 3.
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.
____ 4.
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 predictable mass for a given element
d. a sphere that is hollow throughout
____ 5.
J.J. Thomson’s experiments provided evidence that an atom
a. is the smallest particle of matter.
c. has a negative charge.
b. contains negatively charged particles. d. has a positive charge.
____ 6.
J.J. Thomson’s model of an atom can best be described as
a. “soup – like”
c. “ Jello – model”
b. “ solar system – like”
d. “solid – model”
____ 7.
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.
____ 8.
In an atomic model that includes a nucleus, positive charge is
a. concentrated in the center of an atom. c. concentrated at multiple sites in an
atom.
b. spread evenly throughout an atom.
d. located in the space outside the
nucleus.
____ 9.
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.
Figure 4-1
____ 10.
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
____ 11.
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.
____ 12.
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.
____ 13.
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.
____ 14.
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
____ 15.
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.
____ 16.
The glowing of a neon light is caused by electrons emitting energy as they
a. move from lower to higher energy
c. move from higher to lower energy
levels.
levels.
b. collide with other electrons.
d. collide with the nucleus.
____ 17.
Which subatomic particle has a negative charge?
a. electron
c. neutron
b. alpha particle
d. proton
____ 18.
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.
____ 19.
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.
____ 20.
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
____ 21.
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.
____ 22.
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.
____ 23.
Suppose an atom has a mass number of 35. Which statement is true beyond
any doubt?
a. The atom has an odd number of neutrons.
b. The atomic number is less than 17.
c. The atom is not an isotope.
d. The number of protons in the nucleus does not equal the number of neutrons.
____ 24.
Which statement is true about oxygen-17 and oxygen-18?
a. They do not have the same number of protons.
b. Their atoms have identical mass.
c. They are isotopes of oxygen.
d. The have the same mass number.
atomic struct ws
Answer Section
MULTIPLE CHOICE
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B
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