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 non charged 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 non charged 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.
B. it claimed atoms could be divided.
C.
it explained what electrons are.
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.
B. it claimed atoms could be divided.
C.
it explained what electrons are.
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: mass A. as negative particles scattered in a positive 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: mass A. as negative particles scattered in a positive 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.
B. Knowing that neutrons are in the nucleus C. Measuring the energy in different colors of light given off by excited atoms D. Knowing that protons are in the nucleus.
Evidence to support Bohr’s model comes from: A. Measuring the mass of different elements.
B. Knowing that neutrons are in the nucleus C. Measuring the energy in different colors of light given off by excited atoms D. Knowing that protons 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 B. only protons C. only neutrons D. anodes
What is an atom’s nucleus made of?
A. protons and neutrons B. only protons C. only neutrons 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.
B.
protons.
neutrons.
C.
D.
nuclei protons and neutrons.
An element’s atomic number is equal to its number of A.
B.
protons.
neutrons.
C.
D.
nuclei protons and neutrons.
Two different isotopes of an element have different A.
B.
numbers of neutrons.
numbers of protons.
C. atomic numbers.
D. numbers of electrons.
Two different isotopes of an element have different A.
B.
numbers of neutrons.
numbers of protons.
C. atomic numbers.
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.