Atomic Theory

A single ion of an unnamed element is found to have 157 neutrons, 106 protons, and 103 electrons. What is the atomic number of this element?
A. 103
B. 106
C. 157
D. 263

The number of protons in N^3- is
A. 3.
B. 5.
C. 7.
D. 10.

The number of electrons in N^3- is
A. 3.
B. 4.
C. 7.
D. 10.

The number of protons in Ca²⁺ is
A. 18.
B. 20.
C. 22.
D. 24.

The number of electrons in ^Ca2+ is
A. 18.
B. 20.
C. 22.
D. 24.

The number of protons in Al³⁺ is
A. 7.
B. 10.
C. 13.
D. 16.

The symbol, Fe³⁺, has
A. 26 electrons and 26 protons.
B. 26 electrons and 23 protons.
C. 23 electrons and 26 protons.
D. 29 electrons and 26 protons.

The symbol, K¹⁺, has
A. 19 electrons and 18 protons.
B. 18 electrons and 19 protons.
C. 18 electrons and 18 protons.
D. 19 electrons and 19 protons.

The symbol, P^3-, has
A. 15 electrons and 18 protons.
B. 18 electrons and 18 protons.
C. 12 electrons and 15 protons.
D. 18 electrons and 15 protons.

Which of the following has the most number of neutrons?
A. ²³⁸U
B. ²³²Th
C. ²³⁷Np
D. ²⁴³Am

Which of the following has the most number of neutrons?
A. ¹⁴⁵Pm
B. ¹⁴⁶Nd
C. ¹⁴⁷Sm
D. ¹⁴⁴Pr

Which of the following has the fewest number of neutrons?
A. ¹⁴⁵Pm
B. ¹⁴⁶Nd
C. ¹⁴⁷Sm
D. ¹⁴⁴Pr

The number of electrons in Cl1- is
A. 16.
B. 17.
C. 18.
D. 20.

The number of electrons in Mg²⁺ is
A. 10.
B. 12.
C. 14.
D. 16.

The compound GaAs is used in electronic displays in some calculators. How many electrons are in the ion Ga³⁺?
A. 38
B. 31
C. 34
D. 28
E. 39

The number of protons(p), neutrons(n), and electrons(e) represented by the symbol ³⁷Cl^1- is
A. 18 p, 37 n, 17 e.
B. 17 p, 20 n, 17 e.
C. 20 p, 18 n, 20 e.
D. 17 p, 20 n, 18 e.
E. 20 p, 17 n, 17 e.

A neutral atom of the isotope Cesium-131 has
A. 55 protons, 131 neutrons and 55 electrons.
B. 131 protons, 55 neutrons and 131 electrons.
C. 55 protons, 76 neutrons and 76 electrons.
D. 55 protons, 76 neutrons and 55 electrons.
E. 76 protons, 55 neutrons and 76 electrons.

A neutral atom of the isotope Americium-243 has
A. 95 protons, 243 neutrons and 95 electrons.
B. 95 protons, 243 neutrons and 243 electrons.
C. 95 protons, 148 neutrons and 148 electrons.
D. 148 protons, 95 neutrons and 95 electrons.
E. 95 protons, 148 neutrons and 95 electrons.

A neutral atom of the isotope Thorium-230 has
A. 90 protons, 230 neutrons and 90 electrons.
B. 90 protons, 140 neutrons and 90 electrons.
C. 140 protons, 140 neutrons and 90 electrons.
D. 90 protons, 90 neutrons and 140 electrons.
E. 90 protons, 140 neutrons and 140 electrons.

How many neutrons are present in a 1- ion of the isotope chlorine -37?
A. 16
B. 17
C. 18
D. 20

Which particle has the greatest number of protons?
A. 13C
B. 14C
C. 14N
D. 14B

The element rhenium (Re) exists as two stable isotopes and 18 unstable isotopes. Rhenium -185 has in its nucleus
A. 75 protons, 130 neutrons
B. 130 protons, 75 neutrons
C. 75 protons, 75 neutrons
D. 75 protons, 110 neutrons

How many electrons surround the nucleus of a 2+ ion of calcium - 44?
A. 18
B. 20
C. 22
D. 24

A fluroine ion with a 1- charge is found to have a mass number of 19. Which of the following correctly describes its structure?
A. 8 protons, 9 electrons, 10 neutrons
B. 9 protons, 8 electrons, 10 neutrons
C. 9 protons, 10 electrons, 10 neutrons
D. 10 protons, 9 electrons, 9 neutrons

Which particle has the greatest number of neutrons?
A. 13C
B. 14C
C. 14N
D. 14B

The ion 30 Si²⁺ consists of
A. 16 neutrons, 5 protons and 2 electrons
B. 16 neutrons, 14 protons and 28 electrons
C. 14 neutrons, 16 protons and 12 electrons
D. 16 neutrons, 14 protons and 12 electrons
E. 16 neutrons, 14 protons and 16 electrons

The isotope ¹¹⁰Ag⁺¹ contains
A. 47 protons, 110 neutrons and 46 electrons
B. 47 protons, 63 neutrons and 48 electrons
C. 47 protons, 63 neutrons and 46 electrons
D. 63 protons, 47 neutrons and 46 electrons
E. 63 protons, 47 neutrons and 48 electrons

The isotope ¹⁹⁷Au³⁺ contains
A. 79 protons, 197 neutrons and 76 electrons
B. 79 protons, 118 neutrons and 76 electrons
C. 79 protons, 79 neutrons and 82 electrons
D. 118 protons, 79 neutrons and 76 electrons
E. 82 protons, 115 neutrons and 79 electrons

The isotope ³⁵ Cl^-1 contains
A. 17 protons, 35 neutrons and 16 electrons
B. 35 protons, 35 neutrons and 36 electrons
C. 18 protons, 17 neutrons and 19 electrons
D. 16 protons, 19 neutrons and 16 electrons
E. 17 protons, 18 neutrons and 18 electrons

The isotope ²¹⁰At^-1 contains
A. 85 protons, 125 neutrons and 86 electrons
B. 85 protons, 86 neutrons and 125 electrons
C. 85 protons, 125 neutrons and 84 electrons
D. 125 protons, 85 neutrons and 126 electrons
E. 84 protons, 126 neutrons and 85 electrons

The isotope ²⁰⁹ Po³⁺ contains
A. 84 protons, 81 neutrons and 125 electrons
B. 125 protons, 84 neutrons and 122 electrons
C. 209 protons, 209 neutrons and 206 electrons
D. 84 protons, 125 neutrons and 81 electrons
E. 87 protons, 122 neutrons and 84 electrons

The isotope ²²² Rn⁺¹ contains
A. 86 protons, 136 neutrons and 85 electrons
B. 136 protons, 86 neutrons and 86 electrons
C. 86 protons, 86 neutrons and 136 electrons
D. 87 protons, 135 neutrons and 86 electrons
E. 87 protons, 86 neutrons and 135 electrons

The isotope ¹²⁶ Te^2- contains
A. 52 protons, 74 neutrons and 50 electrons
B. 52 protons, 74 neutrons and 52 electrons
C. 74 protons, 52 neutrons and 76 electrons
D. 74 protons, 52 neutrons and 72 electrons
E. 52 protons, 74 neutrons and 54 electrons

An element has two isotopes, X and Y, with mass numbers of 52.0 and 53.0 respectively. The relative atomic mass is 52.2. The percentage abundance of the two isotopes is
A. X - 20% Y - 80%
B. X - 25% Y - 75%
C. X - 80% Y - 20%
D. X - 75% Y - 25%
E. X - 50% Y - 50%

An element has two isotopes, X and Y, with mass numbers of 52.0 and 54.0 respectively. The relative atomic mass is 53.5. The percentage abundance of the two isotopes is
A. X - 20%
Y - 80%

B. X - 25% Y - 75%
C. X - 80% Y - 20%
D. X - 75% Y - 25%
E. X - 50% Y - 50%

The relative atomic mass of the element bromine is 79.90. Which of the following statements could represent the approximate percent abundance of the isotopes of bromine?
A. The isotopes 79Br and 80Br are in about equal abundance.
B. The isotopes 79Br and 81Br are in about equal abundance.
C. The isotopes 80Br and 81Br are in about equal abundance.
D. The isotope 79Br is about 2 times as abundant as the isotope 81Br.
E. The isotope 81Br is about 2 times as abundant as the isotope 79Br.

The relative atomic mass of the element rhenium is 186.2. Which of the following statements could represent the approximate percent abundance of the isotopes of rhenium?
A. The isotopes ¹⁸⁵Re and ¹⁸⁷Re are in equal abundance.
B. The isotopes ¹⁸⁶Re and ¹⁸⁷Re are in equal abundance.
C. The isotopes ¹⁸⁶Re and ¹⁸⁸Re are in equal abundance.
D. The isotope ¹⁸⁵Re is a little greater in abundance than isotope ¹⁸⁷Re.
E. The isotope ¹⁸⁷Re is a little greater in abundance than isotope ¹⁸⁵Re.

The relative atomic mass of the element europium is 151.96. Which of the following statements could represent the approximate percent abundance of the isotopes of europium?
A. The isotopes ¹⁵¹Eu and ¹⁵³Eu are in equal abundance.
B. The isotopes ¹⁵²Eu and ¹⁵³Eu are in equal abundance.
C. The isotopes ¹⁵¹Eu and ¹⁵²Eu are in equal abundance.
D. The isotope ¹⁵¹Eu is 2 times as abundant as the isotope ¹⁵³Eu.
E. The isotope ¹⁵³Eu is 2 times as abundant as the isotope ¹⁵¹Eu.

The relative atomic mass of the element boron is 10.81. Which of the following statements could represent the approximate percent abundance of the isotopes of boron?
A. The isotopes ¹⁰B and ¹¹B are in equal abundance.
B. The isotope ¹⁰B is 2 times as abundant as the isotope ¹¹B.
C. The isotope ¹¹B is 2 times as abundant as the isotope ¹⁰B.
D. The isotope ¹⁰B is 4 times as abundant as the isotope ¹¹B.
E. The isotope ¹¹B is 4 times as abundant as the isotope ¹⁰B.

A sub-atomic particle with a 1+ charge is the
A. proton.
B. neutron.
C. photon.
D. electron.

A sub-atomic particle with a 1- charge is the
A. proton.
B. neutron.
C. photon.
D. electron.

A sub-atomic particle that is not charged is the
A. proton.
B. neutron.
C. photon.
D. electron.

The statement that best compares a proton and an electron is that their masses are
A. similar and charges are similar.
B. similar and charges are different.
C. different and charges are different.
D. different and charges are similar..

The statement that best compares a proton and a neutron is that their masses are
A. similar and charges are similar.
B. similar and charges are different.
C. different and charges are different.
D. different and charges are similar..

The statement that best compares an electron and a neutron is that their masses are
A. similar and charges are similar.
B. similar and charges are different.
C. different and charges are different.
D. different and charges are similar..

The statement that best compares an electron and a neutron is that their charges are
A. similar and they are located in the same part of the atom.
B. similar and they are located in different parts of the atom.
C. different and they are located in the same part of the atom.
D. different and they are located in different parts of the atom.

The statement that best compares a proton and a neutron is that their charges are
A. similar and they are located in the same part of the atom.
B. similar and they are located in different parts of the atom.
C. different and they are located in the same part of the atom.
D. different and they are located in different parts of the atom.

The statement that best compares a proton and an electron is that their charges are
A. similar and they are located in the same part of the atom.
B. similar and they are located in different parts of the atom.
C. different and they are located in the same part of the atom.
D. different and they are located in different parts of the atom.

The statement that best compares a proton and an electron is that their masses are
A. similar and they are located in the same part of the atom.
B. similar and they are located in different parts of the atom.
C. different and they are located in the same part of the atom.
D. different and they are located in different parts of the atom.

The statement that best compares a proton and a neutron is that their masses are
A. similar and they are located in the same part of the atom.
B. similar and they are located in different parts of the atom.
C. different and they are located in the same part of the atom.
D. different and they are located in different parts of the atom.

The atomic number of an element is based on the number of
A. protons.
B. neutrons.
C. photons.
D. electrons.

The mass number of an element is based on the number of
A. protons and electrons.
B. neutrons and electrons.
C. protons and neutrons.
D. electrons, protons and neutrons.

The positively charged particles in the nucleus of an atom are called
A. electrons.
B. protons.
C. neutrons.
D. neutrinos.
E. positrons.

The negatively charged particles around the nucleus of an atom are called
A. electrons.
B. protons.
C. neutrons.
D. negatrons.
E. positrons.

Which of the following is NOT a subatomic particle?
A. neutron
B. proton
C. electron
D. nucleus
E. A,B,C and D are subatomic particles

The particles in the nucleus of an atom that possess no charge are called
A. electrons.
B. protons.
C. neutrons.
D. neutrinos.
E. positrons.

Given an atom of element X, select the false statement in the following list.
A. Adding an electron produces an ion of X.
B. Removing a neutron produces a new isotope of X.
C. Adding a neutron changes the mass of the atom.
D. Removing two electrons produces a negtive ion of X.

The particle which has the least mass is
A. proton.
B. neutron.
C. alpha particle.
D. electron.

The neutrons of an atom
A. revolve around the nucleus.
B. contribute to the atomic mass.
C. are positively charged.
D. determine the atomic number.

In the Bohr model of the atom:
A. the positive charge is evenly distributed.
B. electrons circle the nucleus in orbits or shells.
C. electrons occupy regions of high probability called orbitals.
D. electrons are inside the nucleus.
E. the atom is a small indestructable particle.

An element's spectrum is the result of energy released by
A. collisions between its atoms.
B. high energy electrons returning to their normal shells.
C. the breakup of its nucleus.
D. high energy particles striking the nucleus.

Analysis of an atom indicates that there are three electrons in the third energy level. The element is
A. Na
B. Al
C. N
D. P

Analysis of an atom indicates that there are five electrons in the third energy level. The element is
A. V
B. Al
C. N
D. P

Analysis of an atom indicates that there are two electrons in the third energy level. The element is
A. Mg
B. Al
C. Be
D. P

Analysis of an atom indicates that there are two electrons in the second energy level. The element is
A. Mg
B. Al
C. Be
D. P

Analysis of an atom indicates that there are three electrons in the second energy level. The element is
A. Mg
B. Al
C. Be
D. B

Analysis of an atom indicates that there are six electrons in the second energy level. The element is
A. Ne
B. O
C. Ba
D. B

Analysis of an atom indicates that there is one electron in the second energy level. The element is
A. Li
B. He
C. Na
D. B

Analysis of an atom indicates that there is one electron in the fourth energy level. The element is
A. Li
B. C
C. Na
D. K

According to Bohr, the electron distribution in the element fluorine is
A. 1, 8
B. 2, 8
C. 1, 7
D. 2, 7

According to Bohr, the electron distribution in the element magnesium is
A. 1, 8, 1
B. 2, 8, 2
C. 1, 8, 2
D. 2, 8, 1

According to Bohr, the electron distribution in the element aluminum is
A. 1, 8, 3
B. 2, 8, 2
C. 2, 7, 2
D. 2, 8, 3

According to Bohr, the electron distribution in the element sulfur is
A. 1, 8, 5
B. 2, 8, 4
C. 2, 8, 6
D. 2, 8, 3

According to Bohr, the electron distribution in the element argon is
A. 2, 8, 7
B. 2, 8, 4
C. 2, 8, 8
D. 2, 7, 8

In the Periodic Table, an element with the electron distribution 2e-, 8e-, 3e-, is located in
A. period 2, group 13.
B. period 3, group 2.
C. period 3, group 13.
D. period 3, group 14.

In the Periodic Table, an element with the electron distribution 2e-, 3e-, is located in
A. period 2, group 13.
B. period 3, group 2.
C. period 3, group 13.
D. period 3, group 14.

In the Periodic Table, an element with the electron distribution 2e-, 8e-, 4e-, is located in
A. period 4, group 13.
B. period 3, group 2.
C. period 3, group 13.
D. period 3, group 14.

In the Periodic Table, an element with the electron distribution 2e-, 8e-, 5e-, is located in
A. period 5, group 13.
B. period 5, group 2.
C. period 3, group 15.
D. period 3, group 14.

In the Periodic Table, an element with the electron distribution 2e-, 8e-, 7e-, is located in
A. period 3, group 17.
B. period 5, group 2.
C. period 3, group 15.
D. period 7, group 13.

In the Periodic Table, the element identified by period 3, group 17 is
A. Ac.
B. La.
C. Cl.
D. F.

In the Periodic Table, the element identified by period 3, group 15 is
A. Y.
B. In.
C. Cl.
D. P.

In the Periodic Table, the element identified by period 4, group 2 is
A. Sc.
B. Si.
C. Ca.
D. C.

In the Periodic Table, the element identified by period 5, group 13 is
A. In.
B. Y.
C. P.
D. Cl.

In the Periodic Table, the element identified by period 5, group 16 is
A. Po.
B. Mo.
C. Ta.
D. Te.

An atom of an element forms a stable ion by easily losing 3 electrons. The ion has a charge of
A. 3- and is in Group 13.
B. 3+ and is in Group 13.
C. 3- and is in Group 15.
D. 3+ and is in Group 15.

An atom of an element forms a stable ion by easily losing 2 electrons. The ion has a charge of
A. 2- and is in Group 2.
B. 2+ and is in Group 2.
C. 2- and is in Group 16.
D. 2+ and is in Group 16.

An atom of an element forms a stable ion by easily losing 1 electron. The ion has a charge of
A. 1- and is in Group 1.
B. 1+ and is in Group 1.
C. 1- and is in Group 17.
D. 2+ and is in Group 17.

An atom of an element forms a stable ion by easily gaining 1 electron. The ion has a charge of
A. 1- and is in Group 1.
B. 1+ and is in Group 1.
C. 1- and is in Group 17.
D. 2+ and is in Group 17.

An atom of an element forms a stable ion by easily gaining 2 electrons. The ion has a charge of
A. 2- and is in Group 2.
B. 2+ and is in Group 2.
C. 2- and is in Group 16.
D. 2+ and is in Group 16.

An atom of an element forms a stable ion by easily gaining 3 electrons. The ion has a charge of
A. 3- and is in Group 13.
B. 3+ and is in Group 13.
C. 3- and is in Group 15.
D. 3+ and is in Group 15.

In Bohr's Atomic Theory, when an electron moves from one energy level to another energy level more distant from the nucleus
A. energy is emitted.
B. energy is absorbed.
C. no energy change occurs.
D. light is emitted.

Element "X" has three naturally occuring isotopes. The isotopes and their percent abundances in nature are listed below:

X-118 has an abundance of 35.5%
X-119 has an abundance of 15.5%
X-122 has an abundance of 49.0%

The average atomic mass of element "X" is:
A. 119.667 u.
B. 1144.532 u.
C. 120.115 u.
D. 119 u.
E. 120.0 u.

Element "X" has three naturally occuring isotopes. The isotopes and their percent abundances in nature are listed below:

X-129 has an abundance of 45.3%
X-132 has an abundance of 31.8%
X-134 has an abundance of 22.9%

The average atomic mass of element "X" is:
A. 131.667 u.
B. 131.60 u.
C. 131.099 u.
D. 132.0 u.
E. 130.0 u.

Element "X" has three naturally occuring isotopes. The isotopes and their percent abundances in nature are listed below:

X-126 has an abundance of 31.5%
X-128 has an abundance of 19.5%
X-129 has an abundance of 49.0%

The average atomic mass of element "X" is:
A. 127.86 u.
B. 127.667 u.
C. 127.60 u.
D. 128.0 u.
E. 127.5 u.

Who is known for using alpha particles in his famous "Gold Foil Experiment?
A. Chadwick
B. Schrodinger
C. Thomson
D. Rutherford

Who is known for using a modified cathode ray tube in order to determine the properties of the cathode rays--later to be known as electrons?
A. Chadwick
B. Schrodinger
C. Thomson
D. Rutherford

The wild deflections of alpha particles in Rutherford's Scattering Experiment led him to suggest that:
A. atoms have a uniform positive charge.
B. the alpha particles were deflected when they hit fast moving electrons in the atom.
C. his detector was malfunctioning.
D. some alpha particles were deflected by dense nuclei.
E. the atoms of gold were radioactive.

Rutherford's experiment was important because it showed that
A. an atom is mostly empty space.
B. radioactive elements gave off alpha particles.
C. the mass of the atom is uniformly distributed throughout the atom.
D. gold foil can be made to be only a few atoms thick.

Alpha particles travelling toward thin gold foil may
A. go straight through without changing direction.
B. be slightly deflected by repulsion of protons in the nucleus.
C. bounce back due to collisions with nucleii.
D. A and B only.
E. A, B and C.

Alpha particles travelling toward thin gold foil may
A. bounce back due to collisions with nucleii.
B. go straight through without changing direction.
C. be deflected at sharp angles by the attraction of electrons.
D. A and B only.
E. A and C only.

Alpha particles travelling toward thin gold foil may
A. go straight through without changing direction.
B. be slightly deflected by repulsion of neutrons in the nucleus.
C. bounce back due to collisions with nucleii.
D. A and B only.
E. A and C only.

The mass of protons and neutrons has been assigned a whole number value-- 1 amu is an integer; however, the atomic mass of an element is a fractional number. This is because
A. electrons contribute significantly to the mass.
B. the mass is the weighted average of the natural isotopes.
C. the mass is only an estimate.
D. the protons weigh more than the neutrons.

Two atoms have different masses. They are said to be isotopes of the same element if they have the same numbers of
A. protons and the same numbers of neutrons.
B. neutrons but different numbers of electrons.
C. neutrons but a different numbers of protons.
D. protons but different numbers of neutrons.

The element chlorine is mixture of the two isotopes: chlorine-35 and chlorine-37. A sample of this element contains
A. equal amounts of C1-35 and C1-37.
B. much more C1-35 than C1-37.
C. much less C1-35 than C1-37.
D. slightly less C1-35 than C1-37.

Of the atoms described in the following chart, which two are isotpes of the same element?

Atom Neutrons Protons Mass Number
A 90 63 153
B 90 66 156
C 94 66 160
D 96 64 160

A. A and B
B. B and C
C. C and D
D. A and D

Consider the following data:

Atom Protons Neutrons Mass Number
A 52 72 124
B 52 78 130
C 54 76 130
D 56 76 132

Which atoms are isotopes of the same element?
A. A and B
B. C and D
C. B and C
D. A and D

Dalton's Atomic Theory contain statements which are no longer considered to be true. Which of the following statements have been proven invalid?
I. Each element is made up of tiny units called atoms.
II. Atoms are indivisible.
III. All atoms of a given element are identical in every way.
IV. Atoms of one element are different from atoms of every other
element.
V. Compounds are formed when atoms of different elements link together.
A. II
B. III
C. II, IV
D. II, V
E. II, III, IV

A true statement about atoms is that
A. Most of the volume of an atom is occupied by the nucleus.
B. The nucleus contains neutrons only.
C. Most of the mass of the atom is centered in the nucleus.
D. All atoms occupy the same volume.

A true statement about atoms is that
A. Most of the volume of an atom is empty space.
B. The nucleus contains neutrons and electrons.
C. The mass of the atom is evenly distributed throughout its volume.
D. All atoms occupy the same volume.

A true statement about atoms is that
A. Most of the volume of an atom is occupied by the nucleus.
B. The nucleus contains neutrons and protons.
C. The mass of the atom is evenly distributed throughout its volume.
D. Atoms of the same element must have identical nuclei.

A false statement about atoms is that
A. Most of the volume of an atom is occupied by the nucleus.
B. The nucleus contains neutrons and protons.
C. The mass of the atom is concentrated in its centre.
D. Atoms of the same element can have different mass.

A false statement about atoms is that
A. Most of the volume of an atom is occupied by empty space.
B. The nucleus always contains the same number of neutrons and protons.
C. The mass of the atom is concentrated in its centre.
D. Atoms of the same element can have different mass.

A false statement about atoms is that
A. Most of the volume of an atom is occupied by empty space.
B. The nucleus is positively charge.
C. The mass of the atom is evenly distributed throughout its volume.
D. Atoms of the same element can have different mass.

A false statement about atoms is that
A. Most of the volume of an atom is occupied by empty space.
B. The nucleus has no charge.
C. The mass of the atom is concentrated in the nucleus.
D. Atoms of the same element can have different numbers of neutrons.

A false statement about atoms is that
A. Most of the volume of an atom is occupied by empty space.
B. Atoms have no charge.
C. The mass of the atom is concentrated in the nucleus.
D. Atoms of the same element must have the same number of neutrons.

John Dalton's atomic theory included all of the following except that atoms
A. are the smallest particle of matter.
B. are shaped like spheres.
C. of the same element are identical.
D. contain electrons.

J.J. Thomson's atomic model included all of the following except that atoms
A. have an overall neutral charge.
B. contain electrons in set orbits.
C. have a uniform density.
D. have a main bulk that is postively charged.

J.J. Thomson's atomic model included all of the following except that atoms
A. are made of smaller particles.
B. contain electrons embedded in the bulk of mass.
C. have an overall neutral charge.
D. have a main bulk that is negatively charged.

Who was responsible for reviving the idea of atoms by proposing what has been called the "Billiard Ball Model"?
A. Democritus
B. Dalton
C. Thomson
D. Rutherford

Who proposed the "Plum Pudding" Model of the atom--a positively charged bulk with an equivalent number of negatively charged electrons dispersed throughout?
A. Democritus
B. Dalton
C. Thomson
D. Rutherford

Who proposed the "Nuclear" Model of the atom--negatively charged electrons moving randomly in the space around a small, dense and positively charged nucleus.
A. Bohr
B. Dalton
C. Thomson
D. Rutherford

J. J. Thomson was incorrect when he
A. said that electrons inhabited orbitals.
B. gave the proton a positive charge.
C. said that the positive charge was concentrated in the nucleus.
D. thought that the positive charge in an atom was uniformly spread out.

J. J. Thomson
A. regarded atoms as solid and indivisible.
B. devised the "plum-pudding" model of the atom.
C. discovered the neutron.
D. started the science of quantum mechanics.
E. did an experiment which led to the discovery of the nucleus.

J.J. Thomson
A. regarded atoms as solid and indivisible.
B. devised the "planetary" model of the atom.
C. started the science of quantum mechanics.
D. discovered the properties of the electron.
E. did an experiment which led to the discovery of the nucleus.

Ernest Rutherford's main contribution to the study of the atom was
A. the oil-drop experiment which led to the determination of the charge on an electron
B. the scattering experiment which led to the nuclear model of the the atom
C. the model which explained the observed spectra of elements
D. the determination of energy levels of the hydrogen atom
E. the development of the wave equation and quantum mechanics

Which of the following is not part of the theory of electrons today?
A. Electrons have certain energy levels or orbitals.
B. An electron's location is based on probability.
C. Electrons may be viewed as "charged" clouds.
D. Electrons orbit the nucleus like planets around the sun.
E. Electron jumps between energy levels are responsible for the light spectrum for an atom.

Who used a modified cathode ray tube to investigate the electron--he determined that it had mass and was negatively charged?
A. Crookes
B. Dalton
C. Thomson
D. Rutherford

Who was the first person responsible for the idea that matter consisted of tiny, invisible particles called atoms.
A. Democritus
B. Dalton
C. Thomson
D. Crookes

Who suggested that the negatively charged electrons moving in the space around the nucleus, actually moved in set orbits?
A. Bohr
B. Dalton
C. Thomson
D. Rutherford

Who suggested that the electrons existing in the space around the nucleus actually occupy set orbitals according to a probability set out by quantum mechanics.
A. Bohr
B. Schrodinger
C. Thomson
D. Rutherford

Who was responsible for organizing the modern Periodic Table?
A. Newlands
B. Mendeleev
C. Berzelius
D. Avogadro

Which scientist's model of the atom was a uniformly dense, solid sphere that entered into chemical reactions but was unchanged by the reaction?
A. Rutherford
B. Dalton
C. Thomson
D. Bohr

Earnest Rutherford's main contribution to the study of the atom was:
A. the oil-drop experiment which led to the determination of the charge on an electron.
B. the scattering experiment which led to the nuclear model of the atom.
C. the model which explained the observed spectra of elements.
D. the determination of energy levels of the hydrogen atom.
E. the development of the wave-equation and quantum mechanics.

The scientist who came up with a model of the atom which first explained the light spectrum of hydrogen was:
A. Dalton.
B. Rutherford.
C. Thomson.
D. Bohr.
E. Schrodinger.