Question 1

Which of the following concepts underlies all the others: ionization energy, effective nuclear charge, atomic size.

Accepted Answer

A)  ionization energy 
B)  effective nuclear charge 
C)  atomic size 
D)  none of the above 
A)  ionization energy 
B)  effective nuclear charge 
C)  atomic size 
D)  none of the above

Question 2

Which of the following atoms is the smallest?

Accepted Answer

A)  Br 
B)  Ga 
C)  As 
D)  Ca 
E)  K 
A)  Br 
B)  Ga 
C)  As 
D)  Ca 
E)  K

Question 3

If an element has 9 protons and 10 neutrons and 9 electrons, which expression correctly identifies the element?

Accepted Answer

A)    F 
B)    F 
C)    K 
D)    K 
E)    K 
A)    F 
B)    F 
C)    K 
D)    K 
E)    K

Question 4

What prompted early scientists to propose that the ray of the cathode ray tube was due to the cathode?

Accepted Answer

A)  The ray was present regardless of gas, or even without a gas. 
B)  The ray was attracted to positively charge electric plates. 
C)  The ray was not seen from the positively charged anode. 
D)  The ray could be diverted by a magnetic field. 
E)  The ray would change colors depending on which gas was used inside the tube. 
A)  The ray was present regardless of gas, or even without a gas. 
B)  The ray was attracted to positively charge electric plates. 
C)  The ray was not seen from the positively charged anode. 
D)  The ray could be diverted by a magnetic field. 
E)  The ray would change colors depending on which gas was used inside the tube.

Question 5

What color do you see when you close your eyes while in a dark room? Explain.

Accepted Answer

A)  dark violet; Since no light is entering, you would tend to see the fringes of color from the ultra-violet region of the spectrum. 
B)  flashes of white; Although white is not really a color, you perceive all the frequencies of the spectrum as they flash by the retina of the eye. 
C)  black; Since no light is hitting the eye all you see is the absence of color, known as black. 
D)  all colors; The harder you close your eyes the more colors you will see. 
A)  dark violet; Since no light is entering, you would tend to see the fringes of color from the ultra-violet region of the spectrum. 
B)  flashes of white; Although white is not really a color, you perceive all the frequencies of the spectrum as they flash by the retina of the eye. 
C)  black; Since no light is hitting the eye all you see is the absence of color, known as black. 
D)  all colors; The harder you close your eyes the more colors you will see.

Question 6

Neon, Ne, (number 10) has a relatively large effective nuclear charge, yet it cannot attract any additional electrons because ________.

Accepted Answer

A)  of the repulsion of neighboring electrons 
B)  the outermost shell has gotten too small 
C)  the outermost shell is too far away from the nucleus 
D)  its outermost shell is already filled to capacity 
A)  of the repulsion of neighboring electrons 
B)  the outermost shell has gotten too small 
C)  the outermost shell is too far away from the nucleus 
D)  its outermost shell is already filled to capacity

Question 7

How might you distinguish a sodium-vapor street lamp from a mercury-vapor street lamp?

Accepted Answer

A)  use binoculars to look for printing adjacent to the bulb 
B)  look at the street lamps through a spectroscope and match their spectral patterns to their respective atomic spectra 
C)  ask your local utility company to identify these lamps for you 
D)  The shadows cast from a sodium-vapor street lamp tend to be more diffuse around the edges. 
A)  use binoculars to look for printing adjacent to the bulb 
B)  look at the street lamps through a spectroscope and match their spectral patterns to their respective atomic spectra 
C)  ask your local utility company to identify these lamps for you 
D)  The shadows cast from a sodium-vapor street lamp tend to be more diffuse around the edges.

Question 8

Which of the following experiments helped to determine the charge of an electron and (indirectly) its mass?

Accepted Answer

A)  J.J. Thompson's cathode ray deflection experiments 
B)  R. Millikan's oil drop experiments 
C)  E. Rutherford's gold foil experiments 
D)  Avogadro's number experiments 
E)  Franklin's kite experiments 
A)  J.J. Thompson's cathode ray deflection experiments 
B)  R. Millikan's oil drop experiments 
C)  E. Rutherford's gold foil experiments 
D)  Avogadro's number experiments 
E)  Franklin's kite experiments

Question 9

The following statement describes which subatomic particle best? It is located outside of the nucleus.

Accepted Answer

A)  an electron 
B)  a proton 
C)  a neutron 
D)  A and B 
E)  B and C 
A)  an electron 
B)  a proton 
C)  a neutron 
D)  A and B 
E)  B and C

Question 10

In Rutherford's gold foil experiment, alpha particles ________.

Accepted Answer

A)  passed through the atomic nucleus 
B)  touched the atomic nucleus 
C)  were deflected by the atomic nucleus 
D)  were invisible to the atomic nucleus 
A)  passed through the atomic nucleus 
B)  touched the atomic nucleus 
C)  were deflected by the atomic nucleus 
D)  were invisible to the atomic nucleus

Question 11

If the particles of a cathode ray had a greater electric charge, the ray passing through a magnetic field would bend ________.

Accepted Answer

A)  more because of a greater electromagnetic attraction 
B)  less because of greater electrical inertia 
C)  more because the particles would be traveling faster 
D)  by the same amount regardless of its charge 
A)  more because of a greater electromagnetic attraction 
B)  less because of greater electrical inertia 
C)  more because the particles would be traveling faster 
D)  by the same amount regardless of its charge

Question 12

Which experiences a greater effective nuclear charge, an electron in the outer shell of neon (atomic number 10) or an electron in the outer shell of sodium (atomic number 11)?

Accepted Answer

A)  sodium because it contains more protons 
B)  neon because of less inner shell shielding 
C)  sodium because it contains a greater number of shells 
D)  neon because it is a smaller atom 
A)  sodium because it contains more protons 
B)  neon because of less inner shell shielding 
C)  sodium because it contains a greater number of shells 
D)  neon because it is a smaller atom

Question 13

What do the components of a conceptual model have in common?

Accepted Answer

A)  All components interact with each other. 
B)  All components are mutually independent of each other. 
C)  The components have nothing in common. This is what differentiates a conceptual model from a physical model. 
D)  Each component must correlate with a corresponding component of a physical model. 
A)  All components interact with each other. 
B)  All components are mutually independent of each other. 
C)  The components have nothing in common. This is what differentiates a conceptual model from a physical model. 
D)  Each component must correlate with a corresponding component of a physical model.

Question 14

The isotope lithium-7 has a mass of 7.0160 atomic mass units, and the isotope lithium-6 has a mass of 6.0151 atomic mass units. Given the information that 92.58 percent of all lithium atoms found in nature are lithium-7 and 7.42 percent are lithium-6, calculate the atomic mass of lithium, Li (atomic number 3).

Accepted Answer

A)  7.0160 amu 
B)  6.942 amu 
C)  6.495 amu 
D)  13.031 amu 
A)  7.0160 amu 
B)  6.942 amu 
C)  6.495 amu 
D)  13.031 amu

Question 15

Which of the above has the least energy?

Accepted Answer

A)  a 
B)  b 
C)  c 
D)  d 
E)  e 
A)  a 
B)  b 
C)  c 
D)  d 
E)  e

Question 16

Rutherford assumed that the atomic nucleus was positively charged because ________.

Accepted Answer

A)  electrons were already established to be negatively charged 
B)  the alpha particles that ricocheted off of the nucleus are also positively charged 
C)  he had a very optimistic outlook on life 
D)  Two of the above are reasonable answers 
A)  electrons were already established to be negatively charged 
B)  the alpha particles that ricocheted off of the nucleus are also positively charged 
C)  he had a very optimistic outlook on life 
D)  Two of the above are reasonable answers

Question 17

The mass number of an element is ________.

Accepted Answer

A)  the sum of the protons and the neutrons 
B)  the sum of the electrons and the protons 
C)  the sum of the electrons and the neutrons 
D)  the sum of the isotopes 
E)  the number of protons 
A)  the sum of the protons and the neutrons 
B)  the sum of the electrons and the protons 
C)  the sum of the electrons and the neutrons 
D)  the sum of the isotopes 
E)  the number of protons

Question 18

Using the following generic atom description, choose the correct method for determining the number of neutrons.   X

Accepted Answer

A)  subtract G from F 
B)  subtract F from G 
C)  add F and G 
D)  divide F by G 
E)  look it up on the periodic table 
A)  subtract G from F 
B)  subtract F from G 
C)  add F and G 
D)  divide F by G 
E)  look it up on the periodic table

Question 19

What do the electron configurations for all the group 18 noble gases have in common?

Accepted Answer

A)  They have the same number of electrons. 
B)  They occupy the same number of shells. 
C)  Their outermost occupied shells are filled to capacity. 
D)  all of the above 
A)  They have the same number of electrons. 
B)  They occupy the same number of shells. 
C)  Their outermost occupied shells are filled to capacity. 
D)  all of the above

Question 20

Evidence for the existence of neutrons did not come until many years after the discoveries of the electron and the proton. Give a possible explanation.

Accepted Answer

A)  The neutron is nearly massless. 
B)  The neutron is only slightly more massive than the proton. 
C)  The discovery required the use of ultrafast computers. 
D)  The neutron lacks an electrical charge. 
A)  The neutron is nearly massless. 
B)  The neutron is only slightly more massive than the proton. 
C)  The discovery required the use of ultrafast computers. 
D)  The neutron lacks an electrical charge.

Which of the following concepts underlies all the others: ionization energy, effective nuclear charge, atomic size.

Which of the following atoms is the smallest?

If an element has 9 protons and 10 neutrons and 9 electrons, which expression correctly identifies the element?

What prompted early scientists to propose that the ray of the cathode ray tube was due to the cathode?

What color do you see when you close your eyes while in a dark room? Explain.

Neon, Ne, (number 10) has a relatively large effective nuclear charge, yet it cannot attract any additional electrons because ________.

How might you distinguish a sodium-vapor street lamp from a mercury-vapor street lamp?

Which of the following experiments helped to determine the charge of an electron and (indirectly) its mass?

The following statement describes which subatomic particle best? It is located outside of the nucleus.

In Rutherford's gold foil experiment, alpha particles ________.

If the particles of a cathode ray had a greater electric charge, the ray passing through a magnetic field would bend ________.

Which experiences a greater effective nuclear charge, an electron in the outer shell of neon (atomic number 10) or an electron in the outer shell of sodium (atomic number 11)?

What do the components of a conceptual model have in common?

Which of the above has the least energy?

Rutherford assumed that the atomic nucleus was positively charged because ________.

The mass number of an element is ________.

Using the following generic atom description, choose the correct method for determining the number of neutrons. X

What do the electron configurations for all the group 18 noble gases have in common?

Evidence for the existence of neutrons did not come until many years after the discoveries of the electron and the proton. Give a possible explanation.

About Science

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The Atomic Nucleus

How Atoms Bond

How Molecules Mix

How Water Behaves

How Chemicals React

Acids and Bases in Our Environment

Oxidations and Reductions Charge the World

Organic Compounds

Nutrients of Life

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Exam 4: Subatomic Particles

Which of the following concepts underlies all the others: ionization energy, effective nuclear charge, atomic size.

Which of the following atoms is the smallest?

If an element has 9 protons and 10 neutrons and 9 electrons, which expression correctly identifies the element?

What prompted early scientists to propose that the ray of the cathode ray tube was due to the cathode?

What color do you see when you close your eyes while in a dark room? Explain.

Neon, Ne, (number 10) has a relatively large effective nuclear charge, yet it cannot attract any additional electrons because ________.

How might you distinguish a sodium-vapor street lamp from a mercury-vapor street lamp?

Which of the following experiments helped to determine the charge of an electron and (indirectly) its mass?

The following statement describes which subatomic particle best? It is located outside of the nucleus.

In Rutherford's gold foil experiment, alpha particles ________.

If the particles of a cathode ray had a greater electric charge, the ray passing through a magnetic field would bend ________.

Which experiences a greater effective nuclear charge, an electron in the outer shell of neon (atomic number 10) or an electron in the outer shell of sodium (atomic number 11)?

What do the components of a conceptual model have in common?

Which of the above has the least energy?

Rutherford assumed that the atomic nucleus was positively charged because ________.

The mass number of an element is ________.

Using the following generic atom description, choose the correct method for determining the number of neutrons. X

What do the electron configurations for all the group 18 noble gases have in common?

Evidence for the existence of neutrons did not come until many years after the discoveries of the electron and the proton. Give a possible explanation.

About Science

Particles of Matter

Elements of Chemistry

The Atomic Nucleus

How Atoms Bond

How Molecules Mix

How Water Behaves

How Chemicals React

Acids and Bases in Our Environment

Oxidations and Reductions Charge the World

Organic Compounds

Nutrients of Life

Medicinal Chemistry

Optimizing Food Production

Protection Water and Air Resources

Capturing Energy

Filters