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mid-term 2011 Chapter 3review
Multiple Choice Identify the choice that best completes the statement or answers the question.
(CAPITAL LETTERS ONLY PLEASE)
____ 1.
Which two compounds are examples of the law of multiple proportions?
a.
FeCl3 and Fe2(SO4)3
c.
CO and CO2
b.
O2 and O3
d.
FeCl2 and Fe(NO3)2
____ 2.
If 3 g of element C combine with 8 g of element D to form compound CD, how many
grams of D are needed to form compound CD2?
a.
8g
c.
11 g
b.
16 g
d.
19 g
____ 3.
According to the law of definite proportions, any two samples of KCl have
a.
the same mass.
c.
the same melting point.
b.
slightly different molecular structures.
d.
the same ratio of elements.
____ 4.
Who was the schoolmaster who studied chemistry and proposed an atomic theory?
a.
John Dalton
c.
Robert Brown
b.
Jons Berzelius
d.
Dmitri Mendeleev
____ 5.
Who first recognized that the ratio of the number of atoms that combine is the same as the
ratio of the masses that combine?
a.
Jons Berzelius
c.
John Dalton
b.
Edward Morley
d.
Jon Newlands
____ 6.
According to Dalton's atomic theory, atoms
a.
are destroyed in chemical reactions.
b.
can be divided.
c.
of each element are identical in size, mass, and other properties.
d.
of different elements cannot combine.
____ 7.
Which of the following is NOT part of Dalton's atomic theory?
a.
Atoms cannot be divided, created, or destroyed.
b.
The number of protons in an atom is its atomic number.
c.
In chemical reactions, atoms are combined, separated, or rearranged.
d.
All matter is composed of extremely small particles called atoms.
____ 8.
Which of the following statements is true?
a.
Atoms of the same element may have different masses.
b.
Atoms may be divided in ordinary chemical reactions.
c.
Atoms can never combine with any other atoms.
d.
Matter is composed of large particles called atoms.
____ 9.
The atomic theory proposed by Dalton
a.
has been totally discarded.
b.
has been expanded and modified.
c.
has been accepted unchanged to the present day.
d.
has been found to be false.
____ 10.
In a glass tube, electrical current passes from the negative electrode, called the ____, to
the other electrode.
a.
cathode
c.
electron
b.
anode
d.
millikan
____ 11.
The rays produced in a cathode tube in early experiments were
a.
unaffected by a magnetic field.
c.
found to carry a positive charge.
b.
deflected away from a negative plate.
d.
striking the cathode.
____ 12.
After measuring the ratio of the charge of a cathode-ray particle to its mass, Thomson
concluded that the particles
a.
had no mass.
c.
had a very large mass.
b.
had a very small mass.
d.
carried a positive charge.
____ 13.
Rutherford fired positively charged particles at metal foil and concluded that most of the
mass of an atom was
a.
in the electrons.
c.
evenly spread throughout the atom.
b.
concentrated in the nucleus.
d.
in rings around the atom.
____ 14.
What did Rutherford conclude about the structure of the atom?
a.
An atom is indivisible.
b.
Electrons make up the center of an atom.
c.
An atom carries a positive charge.
d.
An atom contains a small, dense, positively charged central region.
____ 15.
An atom is electrically neutral because
a.
neutrons balance the protons and electrons.
b.
nuclear forces stabilize the charges.
c.
the numbers of protons and electrons are equal.
d.
the numbers of protons and neutrons are equal.
____ 16.
The charge on the electron cloud
a.
prevents compounds from forming.
b.
balances the charge on the nucleus.
c.
attracts electron clouds in other atoms to form compounds.
d.
does not exist.
____ 17.
The smallest unit of an element that can exist either alone or in combination with other
such particles of the same or different elements is the
a.
electron.
c.
neutron.
b.
proton.
d.
atom.
____ 18.
The radius of an atom extends to the outer edge of the
a.
nucleus.
c.
region occupied by the neutrons.
b.
region occupied by the electrons.
d.
positive charges.
____ 19.
Isotopes are atoms of the same element that have different
a.
principal chemical properties.
c.
numbers of protons.
b.
masses.
d.
numbers of electrons.
____ 20.
Isotopes of an element contain different numbers of
a.
electrons.
c.
neutrons.
b.
protons.
d.
____ 21.
The only radioactive form of hydrogen is
a.
protium.
c.
b.
deuterium.
d.
nuclides.
tritium.
quadrium.
____ 22.
Deuterium differs from tritium in having one
a.
less neutron.
c.
more electron.
b.
more proton.
____ 23.
All isotopes of hydrogen contain
a.
one neutron.
b.
two electrons.
d.
more neutron.
c.
one proton.
d.
two nuclei.
____ 24.
Isotopes of each element differ in
a.
the number of neutrons in the nucleus.
b.
atomic number.
c.
the number of electrons in the highest energy level.
d.
the total number of electrons.
____ 25.
The total number of protons and neutrons in the nucleus of an atom is its
a.
atomic number.
c.
mass number.
b.
Avogadro constant.
d.
number of neutrons.
____ 26.
The average atomic mass of an element depends on both the masses of its isotopes and
each isotope's
a.
atomic number.
c.
relative abundance.
b.
radioactivity.
d.
mass number.
____ 27.
A single atom of an isotope does not have a(n)
a.
relative atomic mass.
c.
mass number.
b.
atomic number.
____ 28.
a.
13
b.
d.
average atomic mass.
What is the atomic number for aluminum from the figure above?
c.
26.98
14
d.
26.9815
____ 29.
Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils, has
a.
6 neutrons.
c.
10 neutrons.
b.
8 neutrons.
d.
14 neutrons.
____ 30.
Phosphorus-33 (atomic number 15) contains
a.
33 protons.
c.
33 neutrons.
b.
18 neutrons.
d.
18 protons.
____ 31.
Silicon-30 contains 14 protons. It also contains
a.
16 electrons.
c.
30 neutrons.
b.
16 neutrons.
d.
44 neutrons.
____ 32.
Neon-22 contains 12 neutrons. It also contains
a.
12 protons.
c.
22 electrons.
b.
22 protons.
d.
____ 33.
Calcium-48 (atomic number 20) contains
a.
20 electrons.
c.
b.
48 protons.
d.
10 protons.
20 neutrons.
28 protons.
____ 34.
An electrically neutral atom of mercury (atomic number 80) has
a.
80 neutrons and 80 electrons.
c.
80 protons and 80 neutrons.
b.
40 protons and 40 electrons.
d.
80 protons and 80 electrons.
____ 35.
The number of atoms in 1 mol of carbon is
a.
6.022 × 1022.
c.
5.022 × 1022.
b.
6.022 × 1023.
d.
5.022 × 1023.
____ 36.
The number of atoms in a mole of any pure substance is called
a.
its atomic number.
c.
its mass number.
b.
Avogadro's constant.
d.
its gram-atomic number.
____ 37.
The atomic number of neon is 10. The atomic number of calcium is 20. Compared with a
mole of neon, a mole of calcium contains
a.
twice as many atoms.
c.
an equal number of atoms.
b.
half as many atoms.
d.
20 times as many atoms.
____ 38.
If samples of two different elements each represent one mole, then
a.
they are equal in mass.
c.
their molar masses are equal.
b.
they contain the same number of atoms.
d.
they have the same atomic mass.
____ 39.
Molar mass
a.
is the mass in grams of one mole of a substance.
b.
is numerically equal to the average atomic mass of the element.
c.
both a and b
d.
neither a nor b
____ 40.
A mass of 6.005 g of carbon (atomic mass 12.010 amu) contains
a.
1 mol C.
c.
0.5000 mol C.
b.
2 atoms C.
d.
1 atom O.
Short Answer
41.
How has Dalton's theory about atomic particles been modified by modern science?
42.
What is the relationship between isotopes, mass number, and neutrons?
43.
Why do chemists work with moles instead of individual atoms?
Problem
44.
How many atoms are present in 8.00 mol of chlorine atoms?
45.
How many atoms are present in 80.0 mol of zirconium?
46.
Determine the mass in grams of 5.00 mol of oxygen. The molar mass of oxygen is 16.00
47.
Determine the number of moles of helium in 10.0 g of helium. The molar mass of helium
g/mol.
is 4.00 g/mol.
48.
39.10 g/mol.
Determine the number of moles in 100. g of potassium. The molar mass of potassium is
49.
Calculate the mass in grams of 9.00 mol of potassium (molar mass 39.10 g/mol).
50.
Calculate the number of atoms in 10.0 g of sulfur (molar mass 32.07 g/mol).
mid-term 2011 c3-4 review
Answer Section
MULTIPLE CHOICE
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C
B
D
A
C
C
B
A
B
A
B
B
B
D
C
B
D
B
B
C
C
A
C
A
C
C
D
A
B
B
B
D
A
D
B
B
C
B
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1
1
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1
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II
III
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I
I
I
I
II
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
III
III
III
III
III
III
III
I
I
III
I
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3-1.1
3-1.1
3-1.1
3-1.2
3-1.2
3-1.2
3-1.2
3-1.3
3-1.3
3-2.1
3-2.1
3-2.1
3-2.2
3-2.2
3-2.4
3-2.4
3-2.4
3-2.4
3-3.1
3-3.1
3-3.1
3-3.1
3-3.1
3-3.1
3-3.2
3-3.2
3-3.2
3-3.2
3-3.3
3-3.3
3-3.3
3-3.3
3-3.3
3-3.3
3-3.4
3-3.4
3-3.4
3-3.4
39.
40.
ANS: C
ANS: C
PTS: 1
PTS: 1
DIF: I
DIF: III
OBJ:
OBJ:
3-3.4
3-3.5
SHORT ANSWER
41.
ANS:
The discovery of subatomic particles proved that atoms are divisible. Dalton believed that atoms were
indivisible.
PTS: 1
DIF: II
OBJ: 3-1.3
42.
ANS:
Isotopes are atoms of the same element with different numbers of neutrons and therefore different mass
numbers.
PTS: 1
DIF: II
OBJ: 3-3.2
43.
ANS:
A mole is a collection of atoms that is large enough to measure in the laboratory. A single atom is too
small.
PTS: 1
DIF: II
OBJ: 3-3.4
PROBLEM
44.
ANS:
4.82 × 1024 atoms Cl
PTS: 1
45.
DIF: III
ANS:
OBJ: 3-3.5
DIF: III
ANS:
OBJ: 3-3.5
DIF: III
ANS:
OBJ: 3-3.5
DIF: III
ANS:
OBJ: 3-3.5
4.82 × 1025 atoms Zr
PTS: 1
46.
80.0 g O
PTS: 1
47.
2.50 mol He
PTS: 1
48.
2.56 mol K
PTS: 1
49.
DIF: III
ANS:
OBJ: 3-3.5
DIF: III
ANS:
OBJ: 3-3.5
DIF: III
OBJ: 3-3.5
352 g K
PTS: 1
50.
1.88 × 1023 atoms S
PTS: 1