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CHAPTER 3 TEST
Atoms: The Building Blocks of Matter
MULTIPLE CHOICE On the line at the left of each statement, write the letter of the
choice that best completes the statement or answers the question.
1.
The behavior of cathode rays in a glass tube containing gas at low pressure led scientists to
conclude that the rays were composed of
.
a. energy
b. positive particles
2.
c. negative particles
d. neutral particles
The basic principles of atomic theory that are still recognized today were first conceived
by
.
a. Avogadro
b. Bohr
3.
c. Dalton
d. Rutherford
An example of the law of multiple proportions is the existence of
a. FeCl3 and Fe(SO4)3
b. O2 and O3
4.
5.
c. CO and CO2
d. FeCl2 and Fe(NO3)2
Atoms of the same element can differ in
a.
b.
c.
d.
.
chemical properties
mass number
atomic number
number of protons and electrons
Dalton’s atomic theory helped to explain the law of conservation of mass because it stated
that atoms
.
a. could not combine
b. were invisible
6.
Milliken’s experiments determined
a.
b.
c.
d.
7.
c. all had the same mass
d. could not be created or destroyed
.
that the electron carried no charge
that the electron carried the smallest possible positive charge
the approximate value of the electron’s mass
that the electron had no mass
In Rutherford’s experiment, a small percentage of the positively charged particles
bombarding the metal’s surface
.
a.
b.
c.
d.
8.
.
were slightly deflected as they passed through the metal
were deflected back toward the source from the metal
passed straight through the metal
combined with the metal
Most of the volume of an atom is made up of the
a. nucleus
b. nuclides
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c. electron cloud
d. protons
CHAPTER 3 TEST
9
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CHAPTER 3 TEST continued
FILL IN THE BLANK Write the correct term (or terms) in the space provided.
9. If a particular compound is composed of elements A and B, the ratio of the mass of B to the mass
of A will always be the same. This is a statement of the law of
.
10. The amount of a substance that contains a number of particles equal to the number of atoms in
exactly 12 g of carbon-12 is referred to as a(n)
.
11. Since any metal cathode used in a cathode-ray tube produced the same charged particles, it was
concluded that all atoms contain
.
12. The smallest particle of an element that retains the chemical properties of that element is a(n)
.
13. Atoms of one element that have different masses are called
.
14. The total number of protons and neutrons in the nucleus of an isotope is called its
number.
15. The short-range attractive forces that hold the nuclear particles together are called
.
16. The number of protons in the nucleus of an element is called its
number.
17. If two or more compounds are composed of elements A and B, the ratio of the masses of B combined with 1 g of A make each compound a ratio of small whole numbers. This is a statement
of the law of
.
18. Dalton’s atomic theory agreed with the modern atomic theory EXCEPT for the statement that
all atoms of the same element have the same
.
Complete the following table to compare the types of subatomic particles.
Particle
Mass number
19.
Proton
20.
Neutron
21.
Electron
10
CHAPTER 3 TEST
Relative charge
Location
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CHAPTER 3 TEST continued
SHORT ANSWER
Write the answers to the following questions in the space provided.
22. Give three of the main concepts in Dalton’s atomic theory.
23. What is molar mass? How is it related to atomic mass?
24. Explain why the atomic mass of a particular isotope of an element differs from the average atomic
mass of that element.
PROBLEMS Write the answers to the questions on the line to the left, and show your
work in the space provided.
25.
The atomic number of nickel-60 is 28. How many neutrons does this isotope have?
26.
Carbon-14 has 8 neutrons. What is the atomic number of carbon-14?
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CHAPTER 3 TEST
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CHAPTER 3 TEST continued
27.
An atom of silicon-30 contains 14 protons. How many electrons does it
have?
28.
Oxygen has three naturally occurring isotopes in the following proportions:
oxygen-16, 99.762% (15.994 91 amu); oxygen-17, 0.038000%
(16.999 13 amu); oxygen-18, 0.20000% (17.999 16 amu). What is
the average atomic mass of oxygen?
29.
The average atomic mass of chromium is 52.00 amu. What is the mass of
3.00 mol of chromium?
30.
How many moles are in a sample of 63.658 g of carbon? (The molar mass
of carbon is 12.01 g/mol.)
31.
The mass of a sample of nickel (average atomic mass 58.69 amu) is
11.74 g. How many atoms does it contain?
32.
The atomic mass of sulfur is 32.06 amu. How many atoms are present in
exactly 2 mol sulfur?
12
CHAPTER 3 TEST
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36.
37.
38.
39.
40.
Print
The graph of two quantities that are inversely
proportional is a curve called a hyperbola.
2.20 g/cm3
3%
114 g
8.12 102 L
3.164 g
28.
29.
30.
31.
32.
15.999 amu
156 g
5.300 mol
1.205 1023 atoms
1.204 1024 atoms
4
3
1.
2.
3.
4.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
Atoms: The Building Blocks
of Matter, pp. 9–12
c
5. d
c
6. c
c
7. b
b
8. c
definite proportions
mole
electrons
atom
isotopes
mass
nuclear forces
atomic
multiple proportions
mass
1; 1; in the nucleus
1; 0; in the nucleus
0; 1; outside the nucleus (in the electron cloud)
Answers should include three of the following:
All matter is composed of extremely small
particles called atoms.
All atoms of an element are identical in size,
mass, and other properties; atoms of different
elements differ in size, mass and other properties.
Atoms cannot be subdivided, created, or
destroyed.
Atoms of different elements combine in simple
whole-number ratios to form chemical
compounds.
In chemical reactions, atoms are combined,
separated, or rearranged.
The molar mass of a substance is the mass of one
mole of the substance. A mole of any substance
contains 6.022137 1023 particles, or
Avogadro’s number of particles. The atomic mass
is the mass of one atom.
The atomic mass of a single isotope of an element
is its relative mass compared to the mass of
carbon-12. The average atomic mass of an
element is the weighted average of the masses of
all naturally occurring isotopes of an element.
32
6
14
90
CHAPTER TESTS ANSWER KEY
1.
2.
3.
4.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
Arrangement of Electrons
in Atoms, pp. 13–16
c
5. c
d
6. b
d
7. a
b
8. a
noble gas
frequency or wavelength
longer
hertz
wavelength
photoelectric effect
ground state
frequency
line-emission
3.00 108 m/s
red
Heisenburg uncertainty principle
inner-shell electrons
electromagnetic radiation
d
a
b
c
the photoelectric effect and the line-emission
spectrum of hydrogen
A line-emission spectrum is produced when an
electron drops from a higher-energy orbit to one
with lower energy, emitting a photon whose
energy is equal to the difference in energy
between the two orbits.
1s22s22p5
1s22s22p63s23p4
1s22s22p63s23p64s2
1s22s22p63s23p63d64s2
[He] 2s22p2
[He] 2s22p6
[Xe] 6s2
[Ar] 4s1
↑↓ ↑
37. 1s 2s
↑↓ ↑↓ ↑
38. 1s 2s 2px
↑
2py
2pz
↑↓ ↑↓ ↑↓
39. 1s 2s 2px
↑↓
2py
↑↓
2pz
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