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.

Unit 3 ExamReview

Question 1Dalton’s atomic theory was accepted because

A. There was evidence to support it.B. Democritus said that it was correctC. Dalton invented the electron

microscopeD. Dalton showed how molecules are

formed

Question 1Dalton’s atomic theory was accepted because

A. There was evidence to support it.B. Democritus said that it was correctC. Dalton invented the electron

microscopeD. Dalton showed how molecules are

formed

Question 2Atoms are neutral (no net electric charge) when they

A. have an equal number of charged and non-charged particles

B. have neutrons in their nucleiC. have an equal number of electrons

and protonsD. have an equal number of neutrons and

protons

Question 2Atoms are neutral (no net electric charge) when they

A. have an equal number of charged and non-charged particles

B. have neutrons in their nucleiC. have an equal number of electrons

and protonsD. have an equal number of neutrons and

protons

Question 3The 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.

Question 3The 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.

Question 4

A. Atoms cannot be divided.B. Atoms of an element are alike.C. Atoms are made of electrons.D. 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?

Question 4

A. Atoms cannot be divided.B. Atoms of an element are alike.C. Atoms are made of electrons.D. 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?

Question 5A subatomic particle that has a negative charge is called a(n)

A. molecule

B. electron

C. element

D. compound

Question 5A subatomic particle that has a negative charge is called a(n)

A. molecule

B. electron

C. element

D. compound

Question 6

A. thermal energy. C. electrical current and a sealed gas tube

B. kinetic energy. D. X rays.

Thomson made his discovery about the atom during an experiment using

Question 6

A. thermal energy. C. electrical current and a sealed gas tube

B. kinetic energy. D. X rays.

Thomson made his discovery about the atom during an experiment using

Question 7What particle did Thomson discover?

A. nucleusB. electronC. protonD. neutron

Question 7What particle did Thomson discover?

A. nucleusB. electronC. protonD. neutron

Question 8Thompson’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 nucleusC. as positive particles scattered in a

negative massD. has neutrons and electrons

Question 8Thompson’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 nucleusC. as positive particles scattered in a

negative massD. has neutrons and electrons

Question 9By using his gold foil experiment, Rutherford was responsible for discovering that an atom contains

A. electronsB. moleculesC. anodesD. nucleus

Question 9By using his gold foil experiment, Rutherford was responsible for discovering that an atom contains

A. electronsB. moleculesC. anodesD. nucleus

Question 10

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

Question 10

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

Question 11

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

Question 11

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

Question 12

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 are in the nucleus

D. Knowing that protons are in the nucleus.

Evidence to support Bohr’s model comes from:

Question 12

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 are in the nucleus

D. Knowing that protons are in the nucleus.

Evidence to support Bohr’s model comes from:

Question 13

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?

Question 13

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?

Question 14

Which of these particles could be a neutron?A. Particle “A”B. Particle “B”C. Particle “C”

Question 14

Which of these particles could be a neutron?A. Particle “A”B. Particle “B”C. Particle “C”

Question 15

Which of these particles could be an electron?A. Particle “A”B. Particle “B”C. Particle “C”

Question 15

Which of these particles could be an electron?A. Particle “A”B. Particle “B”C. Particle “C”

Question 16

Which of these particles could be an proton?A. Particle “A”B. Particle “B”C. Particle “C”

Question 16

Which of these particles could be an proton?A. Particle “A”B. Particle “B”C. Particle “C”

Question 17

A. protons and neutrons

C. only neutrons

B. only protons D. anodes

What is an atom’s nucleus made of?

Question 17

A. protons and neutrons

C. only neutrons

B. only protons D. anodes

What is an atom’s nucleus made of?

Question 18

The atomic mass of the element shown above would be:

A.9 B. 17 C. 25D. 8

Question 18

The atomic mass of the element shown above would be:

A.9 B. 17 C. 25D. 8

Question 19

The atomic number of the element shown above would be:

A.9 B. 17 C. 25 D. 8

Question 19

The atomic number of the element shown above would be:

A.9 B. 17 C. 25 D. 8

Question 20An 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. 26D. 82

Question 20An 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. 26D. 82

Question 21

A. protons. C. nuclei

B. neutrons. D. protons and neutrons.

An element’s atomic number is equal to its number of

Question 21

A. protons. C. nuclei

B. neutrons. D. protons and neutrons.

An element’s atomic number is equal to its number of

Question 22

A. numbers of neutrons.

C. atomic numbers.

B. numbers of protons.

D. numbers of electrons.

Two different isotopes of an element have different

Question 22

A. numbers of neutrons.

C. atomic numbers.

B. numbers of protons.

D. numbers of electrons.

Two different isotopes of an element have different

Question 23What is the mass number of an element that has 19 protons, 19 electrons, and 20 neutrons?

A. 19 B. 20 C. 39D. 58

Question 23What is the mass number of an element that has 19 protons, 19 electrons, and 20 neutrons?

A. 19 B. 20 C. 39D. 58

Question 24Use a periodic table to answer this: A neutral sodium atom has how many electrons?

A. 0 B. 11 C. 12D. 23

Question 24Use a periodic table to answer this: A neutral sodium atom has how many electrons?

A. 0 B. 11 C. 12D. 23

Question 25

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

Question 25

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

Question 26The number of energy levels filled in an atom is determined by the number of

A. protonsB. electronsC. neutronsD. photons

Question 26The number of energy levels filled in an atom is determined by the number of

A. protonsB. electronsC. neutronsD. photons

Question 27

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?

Question 27

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?

Question 28

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

Question 28

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

Question 29

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?

Question 29

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?

Question 30

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

Question 30

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