, TESTBANK For Chemistry The Molecular
Nature of Matter 8th Edition Jespersen
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,Chemistry: Molecular Nature of Matter, 8e (Jespersen)
Chapter 0 A Very Brief History of Chemistry
1) Which of the following is the logical progression of elements formed in a star?
A) Hydrogen → Helium → Argon → Carbon
B) Hydrogen → Helium → Carbon → Argon
C) Helium → Hydrogen → Argon → Carbon
D) Helium → Hydrogen → Carbon → Argon
E) Argon → Carbon → Helium → Hydrogen
Answer: B
Diff: 2
Section: 0.2
2) Why is iron the heaviest element formed in a star prior to the formation of a supernova?
A) The formation of iron in a star starts a cooling process of the star, ending nucleosynthesis.
B) Iron reacts with the hydrogen in stars to cause a violet explosion that leads to a super nova.
C) Iron is the heaviest element that is stable at high temperatures; all others are radioactive.
D) The formation of iron in a star causes a reaction with helium that causes nucleosynthesis to
end.
E) When iron is formed in the outer layers of a star, the iron has enough kinetic energy to leave
the gravity of the star.
Answer: A
Diff: 1
Section: 0.2
3) One would expect a fairly even distribution of elements on the earth; instead, the distribution
is uneven. Which of the following best describes why we observe this?
A) The nebula that formed the earth had elements that were not evenly distributed.
B) Winds on the surface of the earth have moved the heavy and light elements into bands.
C) The early earth liquefied, resulting in heavier elements migrating toward the core and lighter
elements moving toward the surface. This migration to the surface was largely by lava flows,
which were inconsistent.
D) Some water-soluble elements were washed by water into pockets on the surface.
E) The magnetic properties of the core caused the metals to pool into certain areas between the
poles on the earth.
Answer: C
Diff: 2
Section: 0.2
4) The relative number of atoms of each element in a particular compound
A) is always l:l.
B) is the same as the density ratio.
C) is the same as the weight ratio.
D) is definite and constant.
E) cannot be determined experimentally.
Answer: D
Diff: 2
Section: 0.3 (was 0.2)
1
,5) Which of the following postulates from Dalton's atomic theory are now considered incorrect?
I. All atoms of a given element are identical.
II. Matter consists of very small particles known as atoms.
III. Atoms are indestructible and indivisible.
A) III only
B) II only
C) I only
D) I and II
E) I and III
Answer: E
Diff: 1
Section: 0.4
6) Which of the following statements is/are consistent with Dalton's atomic theory?
I. The atoms in a given sample of an element do not share any common properties.
II. Matter consists of particles called atoms.
III. In chemical reactions, atoms merely rearrange and do not disintegrate.
A) III only
B) II only
C) I only
D) II and III
E) I and III
Answer: D
Diff: 2
Section: 0.5 (was 0.4)
7) Which of the following statements is/are NOT consistent with Dalton's atomic theory?
I. The atoms in a given sample of an element do not share any common properties.
II. Matter consists of tiny particles called molecular substances.
III. In chemical reactions, atoms merely rearrange and do not disintegrate.
A) III only
B) II only
C) I only
D) II and III
E) I and II
Answer: E
Diff: 2
Section: 0.4
2
,8) Which of the following postulates from Dalton's atomic theory is incorrectly stated?
A) The atoms in a given sample of an element are identical.
B) Matter consists of tiny particles called atoms.
C) In chemical reactions, atoms merely rearrange and do not disintegrate.
D) In a given chemical compound, the atoms can be present in various numerical ratios.
E) The atoms of different elements differ in mass and other properties.
Answer: D
Diff: 2
Section: 0.4
9) Which of the following is consistent with the postulates from Dalton's atomic theory?
A) The atoms in a given sample of an element are not necessarily identical.
B) Matter consists of tiny particles called ions.
C) In chemical reactions, atoms both rearrange and disintegrate in smaller subatomic particles.
D) The atoms of different elements can be identical in mass and other properties.
E) In a given chemical compound, the atoms are always present in the same fixed numerical
ratio.
Answer: E
Diff: 2
Section: 0.4
10) Which one of the statements below is true?
A) When two atoms combine to form a chemical compound, they do so in many different
proportions by mass.
B) When two different compounds combine to form an element, they do so in definite
proportions by mass.
C) When two different elements combine to form a chemical compound, they do so in definite
proportions by mass.
D) When two molecules combine in a chemical reaction, a number of different elements can be
generated depending on the masses used.
E) When two different elements combine to form a mixture, they do so in definite proportions by
atomic number.
Answer: C
Diff: 2
Section: 0.4
11) Which one of the statements below is false?
A) In chemical reactions, atoms are rearranged.
B) In a given compound, the atoms are always present in the same fixed numerical ratio.
C) Matter is made up of tiny particles called atoms.
D) In a sealed reaction flask, the total mass after the reaction is over, is the same as before the
reaction started.
E) When hydrogen and oxygen react to form water, the mass of oxygen atoms is equal to the
mass of hydrogen atoms.
Answer: E
Diff: 1
Section: 0.4
3
,12) Which of the following examples is consistent with the postulates from Dalton's atomic
theory?
Hint: Be sure to keep the definitions of atoms and molecules straight!
A) The atoms in a sample of chlorine are similar to the atoms in a sample of elemental sulfur.
B) Matter consists of extremely tiny particles that are always either positively or negatively
charged.
C) When water is formed from oxygen and hydrogen molecules, the atoms in water are grouped
differently compared to the atoms in molecules of hydrogen and oxygen.
D) A sample of water contains hydrogen and oxygen atoms combined in two different ratios by
mass.
E) There are eight different types of sulfur atoms in any naturally occurring sample of elemental
sulfur.
Answer: C
Diff: 2
Section: 0.4
13) To form hydrogen sulfide, H2S, 4.03 g of molecular hydrogen (H2) are reacted with 62.13 g
of sulfur (S). If all of the hydrogen and sulfur completely react to form hydrogen sulfide, how
many grams of hydrogen sulfide should be formed?
A) 66.16 g
B) 58.10 g
C) 4.03 g
D) 70.19 g
E) 33.03 g
Answer: A
Diff: 3
Section: 0.4
14) Which of these scientists developed the atomic theory?
A) John Dalton
B) J. J. Thomson
C) Robert Millikan
D) Henry Moseley
E) Ernest Rutherford
Answer: A
Diff: 1
Section: 0.4
4
,15) When J. J. Thomson discovered the electron, what physical property of the electron did he
measure?
A) charge
B) charge-to-mass ratio
C) temperature
D) mass
E) atomic number
Answer: B
Diff: 1
Section: 0.4
16) Which one of the following contributes to the charge of an atom, but does NOT contribute
significantly to the mass of an atom?
A) electrons
B) nuclei
C) photons
D) neutrons
E) protons
Answer: A
Diff: 2
Section: 0.5 (was 0.4)
17) Which of the following have roughly the same mass?
A) a proton and an electron
B) a neutron and an electron
C) a neutron and a proton
D) an electron and an alpha particle
E) none of these options
Answer: C
Diff: 1
Section: 0.5
18) Which of the following have opposite electric charges?
A) a proton and an electron
B) a neutron and an electron
C) a neutron and a proton
D) an electron and an alpha particle
E) none of these options
Answer: A
Diff: 1
Section: 0.5
5
,19) Consider the atoms of 65Cu and 65Zn. Both of these atoms have the same
A) number of electrons.
B) atomic mass.
C) number of neutrons.
D) mass number.
E) number of protons.
Answer: D
Diff: 1
Section: 0.5
20) Which of the following particles will not be deflected by charged plates?
A) hydrogen atoms
B) cathode rays
C) alpha particles
D) protons
E) These are all deflected by charged plates.
Answer: A
Diff: 2
Section: 0.5
21) Uranium exists in nature in the form of several isotopes and the different isotopes have
different
A) atomic numbers.
B) charges.
C) numbers of electrons.
D) numbers of neutrons.
E) numbers of protons.
Answer: D
Diff: 2
Section: 0.5
22) Two isotopes of an element differ only in their
A) symbol.
B) atomic number.
C) mass number.
D) number of protons.
E) number of electrons.
Answer: C
Diff: 1
Section: 0.5
6
,23) Which answer below best describes all atoms of a given isotope of a particular element?
A) They possess the same mass but their other properties differ.
B) They possess similar chemical properties and the same mass but have nothing else in
common.
C) They possess the same atomic number but have nothing else in common.
D) They possess the same number of electrons, the same atomic number, and similar chemical
properties but differ in their masses.
E) They possess the same number of electrons, the same atomic number, the same mass, and the
same chemical properties.
Answer: D
Diff: 1
Section: 0.5
24) Which answer below best describes all atoms of a particular element?
A) They possess the same number of electrons, the same atomic number, and the same mass, but
have nothing else in common.
B) They possess the same mass and the same chemical properties but have nothing else in
common.
C) They possess the same number of electrons and the same atomic number but may differ in
mass.
D) They possess the same number of electrons, chemical properties, and mass but have nothing
else in common.
E) They possess the same atomic number and the same mass but have nothing else in common.
Answer: C
Diff: 2
Section: 0.5
25) The species shown below that has 24 neutrons is
A) Cr
B) Mn
C) Mg
D) Sc
E) V
Answer: D
Diff: 2
Section: 0.5
7
, 26) The species shown below that has 24 electrons is
A) Cr
B) Mn
C) Mg
D) Sc
E) V
Answer: A
Diff: 2
Section: 0.5
27) The species V has the same number of neutrons as
A) V
B) Sc
C) Mn
D) Cr
E) Co
Answer: D
Diff: 2
Section: 0.5
28) Consider the atoms of Mg and Al. Both of these species have the same
A) number of neutrons and electrons.
B) number of ions.
C) number of neutrons.
D) number of neutrons and mass number.
E) number of protons and electrons.
Answer: C
Diff: 2
Section: 0.5
8
Nature of Matter 8th Edition Jespersen
Hello all ,
We have all what you need with best price
Our email :
Our website :
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,Chemistry: Molecular Nature of Matter, 8e (Jespersen)
Chapter 0 A Very Brief History of Chemistry
1) Which of the following is the logical progression of elements formed in a star?
A) Hydrogen → Helium → Argon → Carbon
B) Hydrogen → Helium → Carbon → Argon
C) Helium → Hydrogen → Argon → Carbon
D) Helium → Hydrogen → Carbon → Argon
E) Argon → Carbon → Helium → Hydrogen
Answer: B
Diff: 2
Section: 0.2
2) Why is iron the heaviest element formed in a star prior to the formation of a supernova?
A) The formation of iron in a star starts a cooling process of the star, ending nucleosynthesis.
B) Iron reacts with the hydrogen in stars to cause a violet explosion that leads to a super nova.
C) Iron is the heaviest element that is stable at high temperatures; all others are radioactive.
D) The formation of iron in a star causes a reaction with helium that causes nucleosynthesis to
end.
E) When iron is formed in the outer layers of a star, the iron has enough kinetic energy to leave
the gravity of the star.
Answer: A
Diff: 1
Section: 0.2
3) One would expect a fairly even distribution of elements on the earth; instead, the distribution
is uneven. Which of the following best describes why we observe this?
A) The nebula that formed the earth had elements that were not evenly distributed.
B) Winds on the surface of the earth have moved the heavy and light elements into bands.
C) The early earth liquefied, resulting in heavier elements migrating toward the core and lighter
elements moving toward the surface. This migration to the surface was largely by lava flows,
which were inconsistent.
D) Some water-soluble elements were washed by water into pockets on the surface.
E) The magnetic properties of the core caused the metals to pool into certain areas between the
poles on the earth.
Answer: C
Diff: 2
Section: 0.2
4) The relative number of atoms of each element in a particular compound
A) is always l:l.
B) is the same as the density ratio.
C) is the same as the weight ratio.
D) is definite and constant.
E) cannot be determined experimentally.
Answer: D
Diff: 2
Section: 0.3 (was 0.2)
1
,5) Which of the following postulates from Dalton's atomic theory are now considered incorrect?
I. All atoms of a given element are identical.
II. Matter consists of very small particles known as atoms.
III. Atoms are indestructible and indivisible.
A) III only
B) II only
C) I only
D) I and II
E) I and III
Answer: E
Diff: 1
Section: 0.4
6) Which of the following statements is/are consistent with Dalton's atomic theory?
I. The atoms in a given sample of an element do not share any common properties.
II. Matter consists of particles called atoms.
III. In chemical reactions, atoms merely rearrange and do not disintegrate.
A) III only
B) II only
C) I only
D) II and III
E) I and III
Answer: D
Diff: 2
Section: 0.5 (was 0.4)
7) Which of the following statements is/are NOT consistent with Dalton's atomic theory?
I. The atoms in a given sample of an element do not share any common properties.
II. Matter consists of tiny particles called molecular substances.
III. In chemical reactions, atoms merely rearrange and do not disintegrate.
A) III only
B) II only
C) I only
D) II and III
E) I and II
Answer: E
Diff: 2
Section: 0.4
2
,8) Which of the following postulates from Dalton's atomic theory is incorrectly stated?
A) The atoms in a given sample of an element are identical.
B) Matter consists of tiny particles called atoms.
C) In chemical reactions, atoms merely rearrange and do not disintegrate.
D) In a given chemical compound, the atoms can be present in various numerical ratios.
E) The atoms of different elements differ in mass and other properties.
Answer: D
Diff: 2
Section: 0.4
9) Which of the following is consistent with the postulates from Dalton's atomic theory?
A) The atoms in a given sample of an element are not necessarily identical.
B) Matter consists of tiny particles called ions.
C) In chemical reactions, atoms both rearrange and disintegrate in smaller subatomic particles.
D) The atoms of different elements can be identical in mass and other properties.
E) In a given chemical compound, the atoms are always present in the same fixed numerical
ratio.
Answer: E
Diff: 2
Section: 0.4
10) Which one of the statements below is true?
A) When two atoms combine to form a chemical compound, they do so in many different
proportions by mass.
B) When two different compounds combine to form an element, they do so in definite
proportions by mass.
C) When two different elements combine to form a chemical compound, they do so in definite
proportions by mass.
D) When two molecules combine in a chemical reaction, a number of different elements can be
generated depending on the masses used.
E) When two different elements combine to form a mixture, they do so in definite proportions by
atomic number.
Answer: C
Diff: 2
Section: 0.4
11) Which one of the statements below is false?
A) In chemical reactions, atoms are rearranged.
B) In a given compound, the atoms are always present in the same fixed numerical ratio.
C) Matter is made up of tiny particles called atoms.
D) In a sealed reaction flask, the total mass after the reaction is over, is the same as before the
reaction started.
E) When hydrogen and oxygen react to form water, the mass of oxygen atoms is equal to the
mass of hydrogen atoms.
Answer: E
Diff: 1
Section: 0.4
3
,12) Which of the following examples is consistent with the postulates from Dalton's atomic
theory?
Hint: Be sure to keep the definitions of atoms and molecules straight!
A) The atoms in a sample of chlorine are similar to the atoms in a sample of elemental sulfur.
B) Matter consists of extremely tiny particles that are always either positively or negatively
charged.
C) When water is formed from oxygen and hydrogen molecules, the atoms in water are grouped
differently compared to the atoms in molecules of hydrogen and oxygen.
D) A sample of water contains hydrogen and oxygen atoms combined in two different ratios by
mass.
E) There are eight different types of sulfur atoms in any naturally occurring sample of elemental
sulfur.
Answer: C
Diff: 2
Section: 0.4
13) To form hydrogen sulfide, H2S, 4.03 g of molecular hydrogen (H2) are reacted with 62.13 g
of sulfur (S). If all of the hydrogen and sulfur completely react to form hydrogen sulfide, how
many grams of hydrogen sulfide should be formed?
A) 66.16 g
B) 58.10 g
C) 4.03 g
D) 70.19 g
E) 33.03 g
Answer: A
Diff: 3
Section: 0.4
14) Which of these scientists developed the atomic theory?
A) John Dalton
B) J. J. Thomson
C) Robert Millikan
D) Henry Moseley
E) Ernest Rutherford
Answer: A
Diff: 1
Section: 0.4
4
,15) When J. J. Thomson discovered the electron, what physical property of the electron did he
measure?
A) charge
B) charge-to-mass ratio
C) temperature
D) mass
E) atomic number
Answer: B
Diff: 1
Section: 0.4
16) Which one of the following contributes to the charge of an atom, but does NOT contribute
significantly to the mass of an atom?
A) electrons
B) nuclei
C) photons
D) neutrons
E) protons
Answer: A
Diff: 2
Section: 0.5 (was 0.4)
17) Which of the following have roughly the same mass?
A) a proton and an electron
B) a neutron and an electron
C) a neutron and a proton
D) an electron and an alpha particle
E) none of these options
Answer: C
Diff: 1
Section: 0.5
18) Which of the following have opposite electric charges?
A) a proton and an electron
B) a neutron and an electron
C) a neutron and a proton
D) an electron and an alpha particle
E) none of these options
Answer: A
Diff: 1
Section: 0.5
5
,19) Consider the atoms of 65Cu and 65Zn. Both of these atoms have the same
A) number of electrons.
B) atomic mass.
C) number of neutrons.
D) mass number.
E) number of protons.
Answer: D
Diff: 1
Section: 0.5
20) Which of the following particles will not be deflected by charged plates?
A) hydrogen atoms
B) cathode rays
C) alpha particles
D) protons
E) These are all deflected by charged plates.
Answer: A
Diff: 2
Section: 0.5
21) Uranium exists in nature in the form of several isotopes and the different isotopes have
different
A) atomic numbers.
B) charges.
C) numbers of electrons.
D) numbers of neutrons.
E) numbers of protons.
Answer: D
Diff: 2
Section: 0.5
22) Two isotopes of an element differ only in their
A) symbol.
B) atomic number.
C) mass number.
D) number of protons.
E) number of electrons.
Answer: C
Diff: 1
Section: 0.5
6
,23) Which answer below best describes all atoms of a given isotope of a particular element?
A) They possess the same mass but their other properties differ.
B) They possess similar chemical properties and the same mass but have nothing else in
common.
C) They possess the same atomic number but have nothing else in common.
D) They possess the same number of electrons, the same atomic number, and similar chemical
properties but differ in their masses.
E) They possess the same number of electrons, the same atomic number, the same mass, and the
same chemical properties.
Answer: D
Diff: 1
Section: 0.5
24) Which answer below best describes all atoms of a particular element?
A) They possess the same number of electrons, the same atomic number, and the same mass, but
have nothing else in common.
B) They possess the same mass and the same chemical properties but have nothing else in
common.
C) They possess the same number of electrons and the same atomic number but may differ in
mass.
D) They possess the same number of electrons, chemical properties, and mass but have nothing
else in common.
E) They possess the same atomic number and the same mass but have nothing else in common.
Answer: C
Diff: 2
Section: 0.5
25) The species shown below that has 24 neutrons is
A) Cr
B) Mn
C) Mg
D) Sc
E) V
Answer: D
Diff: 2
Section: 0.5
7
, 26) The species shown below that has 24 electrons is
A) Cr
B) Mn
C) Mg
D) Sc
E) V
Answer: A
Diff: 2
Section: 0.5
27) The species V has the same number of neutrons as
A) V
B) Sc
C) Mn
D) Cr
E) Co
Answer: D
Diff: 2
Section: 0.5
28) Consider the atoms of Mg and Al. Both of these species have the same
A) number of neutrons and electrons.
B) number of ions.
C) number of neutrons.
D) number of neutrons and mass number.
E) number of protons and electrons.
Answer: C
Diff: 2
Section: 0.5
8
