Transcript PPT - Unit 3 Exam Review

Review
Dalton’s atomic theory was accepted because
A. There was evidence to support it.
B. Democritus said that it was correct
C. Dalton invented the electron microscope
D. Dalton showed how molecules are formed
Dalton’s atomic theory was accepted because
A. There was evidence to support it.
B. Democritus said that it was correct
C. Dalton invented the electron microscope
D. Dalton showed how molecules are formed
Atoms are neutral (no net electric charge) when they
A. have an equal number of charged and noncharged particles
B. have neutrons in their nuclei
C. have an equal number of electrons and
protons
D. have an equal number of neutrons and
protons
Atoms are neutral (no net electric charge) when they
A. have an equal number of charged and noncharged particles
B. have neutrons in their nuclei
C. have an equal number of electrons and
protons
D. have an equal number of neutrons and
protons
The atomic theory of the ancient Greek philosopher
Democritus was revised because
A. it claimed matter is
made of atoms.
C.
it explained what
electrons are.
B. it claimed atoms
could be divided.
D. scientists found new
evidence.
The atomic theory of the ancient Greek philosopher
Democritus was revised because
A. it claimed matter is
made of atoms.
C.
it explained what
electrons are.
B. it claimed atoms
could be divided.
D. scientists found new
evidence.
In 1803 Dalton was the first person to develop an atomic
theory based on lab experiments. Which of these
statements is not part of Dalton’s atomic theory
?
A.
B.
C.
D.
Atoms cannot be divided.
Atoms of an element are alike.
Atoms are made of electrons.
Atoms of different elements form compounds.
In 1803 Dalton was the first person to develop an atomic
theory based on lab experiments. Which of these
statements is not part of Dalton’s atomic theory
?
A.
B.
C.
D.
Atoms cannot be divided.
Atoms of an element are alike.
Atoms are made of electrons.
Atoms of different elements form compounds.
A subatomic particle that has a negative charge is called
a(n)
A. molecule
B. electron
C. element
D. compound
A subatomic particle that has a negative charge is called
a(n)
A. molecule
B. electron
C. element
D. compound
Thomson made his discovery about the atom during an
experiment using
A. thermal energy.
B. kinetic energy.
C. electrical current and a
sealed gas tube
D. X rays.
Thomson made his discovery about the atom during an
experiment using
A. thermal energy.
B. kinetic energy.
C. electrical current and a
sealed gas tube
D. X rays.
What particle did Thomson discover?
A. nucleus
B. electron
C. proton
D. neutron
What particle did Thomson discover?
A. nucleus
B. electron
C. proton
D. neutron
Thompson’s “plum pudding” (or chocolate chip ice
cream) atomic model showed the atom:
A. as negative particles scattered in a positive
mass
B. has a negatively charged nucleus
C. as positive particles scattered in a negative
mass
D. has neutrons and electrons
Thompson’s “plum pudding” (or chocolate chip ice
cream) atomic model showed the atom:
A. as negative particles scattered in a positive
mass
B. has a negatively charged nucleus
C. as positive particles scattered in a negative
mass
D. has neutrons and electrons
By using his gold foil experiment, Rutherford was
responsible for discovering that an atom contains
A. electrons
B. molecules
C. anodes
D. nucleus
By using his gold foil experiment, Rutherford was
responsible for discovering that an atom contains
A. electrons
B. molecules
C. anodes
D. nucleus
Rutherford’s experiment produced evidence that the
center of an atom
A. Contains a small region with a highly concentrated
negative charge.
B. Contains a large region with a slight negative charge
C. Contains a small region with a highly concentrated
positive charge.
D. Contains a small region with a highly concentrated
neutral charge.
Rutherford’s experiment produced evidence that the
center of an atom
A. Contains a small region with a highly concentrated
negative charge.
B. Contains a large region with a slight negative charge
C. Contains a small region with a highly concentrated
positive charge.
D. Contains a small region with a highly concentrated
neutral charge.
According to Bohr’s theory, an electron’s path around
the nucleus defines its
A. electric charge.
C. energy level
B. atomic mass.
D. speed.
According to Bohr’s theory, an electron’s path around
the nucleus defines its
A. electric charge.
C. energy level
B. atomic mass.
D. speed.
Evidence to support Bohr’s model comes from:
A. Measuring the mass of
different elements.
C. Measuring the energy
in different colors of
light given off by
excited atoms
B. Knowing that neutrons D. Knowing that protons
are in the nucleus
are in the nucleus.
Evidence to support Bohr’s model comes from:
A. Measuring the mass of
different elements.
C. Measuring the energy
in different colors of
light given off by
excited atoms
B. Knowing that neutrons D. Knowing that protons
are in the nucleus
are in the nucleus.
Which of the following statements not true?
A. Protons have a positive charge.
B. A nucleus has a positive charge.
C. Neutrons have no charge.
D. Neutrons have a negative charge.
Which of the following statements not true?
A. Protons have a positive charge.
B. A nucleus has a positive charge.
C. Neutrons have no charge.
D. Neutrons have a negative charge.
Which of these particles could be a neutron?
A. Particle “A”
B. Particle “B”
C. Particle “C”
Which of these particles could be a neutron?
A. Particle “A”
B. Particle “B”
C. Particle “C”
Which of these particles could be an electron?
A. Particle “A”
B. Particle “B”
C. Particle “C”
Which of these particles could be an electron?
A. Particle “A”
B. Particle “B”
C. Particle “C”
Which of these particles could be an proton?
A. Particle “A”
B. Particle “B”
C. Particle “C”
Which of these particles could be an proton?
A. Particle “A”
B. Particle “B”
C. Particle “C”
What is an atom’s nucleus made of?
A. protons and
neutrons
C. only neutrons
B. only protons
D. anodes
What is an atom’s nucleus made of?
A. protons and
neutrons
C. only neutrons
B. only protons
D. anodes
The atomic mass of the element shown above would be:
A.9
B. 17
C. 25
D. 8
The atomic mass of the element shown above would be:
A.9
B. 17
C. 25
D. 8
The atomic number of the element shown above would be:
A.9
B. 17
C. 25
D. 8
The atomic number of the element shown above would be:
A.9
B. 17
C. 25
D. 8
An iron atom has an atomic mass of 56. Its atomic
number is 26. How many neutrons does the iron atom
have?
A. 30
B. 56
C. 26
D. 82
An iron atom has an atomic mass of 56. Its atomic
number is 26. How many neutrons does the iron atom
have?
A. 30
B. 56
C. 26
D. 82
An element’s atomic number is equal to its number of
A.
protons.
C.
nuclei
B.
neutrons.
D.
protons and
neutrons.
An element’s atomic number is equal to its number of
A.
protons.
C.
nuclei
B.
neutrons.
D.
protons and
neutrons.
Two different isotopes of an element have different
A.
numbers of
neutrons.
C. atomic numbers.
B.
numbers of
protons.
D. numbers of
electrons.
Two different isotopes of an element have different
A.
numbers of
neutrons.
C. atomic numbers.
B.
numbers of
protons.
D. numbers of
electrons.
What is the mass number of an element that has 19
protons, 19 electrons, and 20 neutrons?
A. 19
B. 20
C. 39
D. 58
What is the mass number of an element that has 19
protons, 19 electrons, and 20 neutrons?
A. 19
B. 20
C. 39
D. 58
Use a periodic table to answer this: A neutral sodium
atom has how many electrons?
A. 0
B. 11
C. 12
D. 23
Use a periodic table to answer this: A neutral sodium
atom has how many electrons?
A. 0
B. 11
C. 12
D. 23
An electron jumps to a new energy level when
A. the atom becomes charged.
B. the atom becomes unstable.
C. the electron’s location is pinpointed.
D. the atom gains or loses energy.
An electron jumps to a new energy level when
A. the atom becomes charged.
B. the atom becomes unstable.
C. the electron’s location is pinpointed.
D. the atom gains or loses energy.
The number of energy levels filled in an atom is
determined by the number of
A. protons
B. electrons
C. neutrons
D. photons
The number of energy levels filled in an atom is
determined by the number of
A. protons
B. electrons
C. neutrons
D. photons
Which statement about the atom’s nucleus is correct?
A. The nucleus is made of protons and neutrons, and
has a negative charge.
B. The nucleus is made of protons and neutrons, and
has a positive charge.
C. The nucleus is made of electrons, and has a positive
charge.
D. The nucleus is made of electrons, and has a negative
charge.
Which statement about the atom’s nucleus is correct?
A. The nucleus is made of protons and neutrons, and
has a negative charge.
B. The nucleus is made of protons and neutrons, and
has a positive charge.
C. The nucleus is made of electrons, and has a positive
charge.
D. The nucleus is made of electrons, and has a negative
charge.
Oxygen’s atomic number is 8. This means that an
oxygen atom has
A. eight neutrons in its nucleus.
B. a total of eight protons plus neutrons.
C. eight protons in its nucleus.
D. a total of eight neutrons plus electrons.
Oxygen’s atomic number is 8. This means that an
oxygen atom has
A. eight neutrons in its nucleus.
B. a total of eight protons plus neutrons.
C. eight protons in its nucleus.
D. a total of eight neutrons plus electrons.
Which statement about an element’s average atomic mass is
correct?
A. It is determined by counting the number of isotopes
in a sample of the element.
B. It is equal to one-twelfth the mass of the most
common isotope.
C. It is a weighted average, so common isotopes have a
greater effect than uncommon ones.
D. It is based on an isotope’s charge, so negatively
charged isotopes have a greater effect than positive
ones.
Which statement about an element’s average atomic mass is
correct?
A. It is determined by counting the number of isotopes
in a sample of the element.
B. It is equal to one-twelfth the mass of the most
common isotope.
C. It is a weighted average, so common isotopes have a
greater effect than uncommon ones.
D. It is based on an isotope’s charge, so negatively
charged isotopes have a greater effect than positive
ones.
An atom’s mass number equals the number of
A.
protons plus the number of electrons.
B.
protons plus the number of neutrons.
C.
protons.
D. neutrons.
An atom’s mass number equals the number of
A.
protons plus the number of electrons.
B.
protons plus the number of neutrons.
C.
protons.
D. neutrons.