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Chapter Test A
Chapter: The Periodic Law
Use the periodic table below to answer the questions in this Chapter Test.
E
E
1
G
H
A1
Hydrogen
2
1.01
B
C
F
He
Helium
4.00
2
3
4
5
6
7
8
9
10
Li
Be
B
C
N
O
F
Ne
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
9.01
10.81
19.00
20.18
6.94
3
4
5
6
7
12.01
14.01
16.00
11
12
13
14
15
16
17
Na
Mg
Al
Si
P
S
Cl
Ar
Sodium
Magnesium
Aluminum
Silicon
Phosphorus
Sulfur
Chlorine
Argon
22.99
24.30
26.98
28.09
30.97
32.07
35.45
39.95
D
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
39.10
47.88
50.94
52.00
54.94
55.85
58.93
58.69
63.55
65.39
69.72
72.61
74.92
83.80
36
40.08
44.96
78.96
79.90
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Rubidium
Strontium
Yttrium
Zirconium
Niobium
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon
85.47
87.62
88.91
91.22
92.91
101.07
102.91
106.42
107.87
112.41
114.82
118.71
121.76
127.60
126.90
131.29
Molybdenum Technetium
95.94
97.91
54
55
56
57
72
73
74
75
76
77
78
79
80
81
82
83
84
85
Cs
Ba
La
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Cesium
Barium
Lanthanum
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury
Thalium
Lead
Bismuth
Polonium
Astatine
Radon
132.90
137.33
195.08
196.97
200.59
204.38
208.98
209.99
222.02
138.91
178.49
180.95
183.84
186.21
190.23
192.22
87
88
89
104
105
106
107
108
109
Fr
Ra
Ac
261.11
262.11
263.12
262.12
58
59
60
61
Pr
Nd
Pm
Francium
Radium
Actinium
223.02
226.02
227.03
Ce
Cerium
H
Praseodymium Neodymium Promethium
62
63
64
65
66
207.2† 208.98
67
68
69
70
86
71
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Samarium
Europium
Gadolinium
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
174.97
140.12
141.91
144.24
144.91
150.36
151.97
157.25
158.92
162.50
164.93
167.26
168.93
173.04
90
91
92
93
94
95
96
97
98
99
100
101
102
Cf
Es
103
Th
Pa
U
Np
Pu
Am
Cm
Bk
Fm
Md
No
Lr
Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
Berkelium
Californium Einsteinium
Fermium
Mendelevium
Nobelium
Lawrencium
232.04
231.04
238.05
237.05
244.06
243.06
247.07
247.07
251.08
257.10
258.10
259.10
262.11
252.08
In the space provided, write the letter of the term or phrase that best completes each
statement or best answers each question.
______ 1. Mendeleev organized the chemical elements based on their
a. symbols.
b. properties.
c. atomic numbers.
d. charges.
______ 2. A horizontal row in the periodic table is called a(n)
a. family.
b. group.
c. octet.
d. period.
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Chapter Test
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Chapter Test A, continued
______ 3. The periodic law states that
a. no two electrons with the same spin can be found in the same place
in an atom.
b. the physical and chemical properties of the elements are functions
of their atomic number.
c. wave patterns repeat at regular intervals.
d. the chemical properties of elements can be grouped according to
periodicity.
______ 4. An element with the general electron configuration ns2np1 for its
outermost electrons would be in Group
a. 2.
b. 13.
c. 14.
d. 15.
______ 5. When a carbon atom is in its ground state, how many electrons does it
have in its outermost shell?
a. 1
b. 2
c. 3
d. 4
______ 6. Which of the following elements is most similar in behavior to
calcium?
a. magnesium
b. sodium
c. sulfur
d. chlorine
______ 7. Which periodic group or family of elements is not correctly matched
with its common family name?
a. Group 2: alkaline-earth metals
b. Group 3: alkali metals
c. Group 17: halogens
d. Group 18: noble gases
______ 8. The electron configurations of main-group elements end in
a. d and f orbitals.
b. s and p orbitals.
c. s and d orbitals.
d. p and d orbitals.
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Chapter Test A, continued
______ 9. Which of the following elements is a transition metal?
a. calcium
b. iron
c. sodium
d. sulfur
______10. All the alkali metal elements are found on the periodic table in
a. Group 1.
b. Group 2.
c. Period 1.
d. Period 2.
______11. A measure of the ability of an atom in a chemical compound to attract
electrons from another atom in the compound is called
a. electron affinity.
b. electron configuration.
c. electronegativity.
d. ionization potential.
______12. Which of the following elements has the greatest atomic radius?
a. Al
b. S
c. Si
d. C
______13. Which of the following elements has the lowest electronegativity?
a. C
b. F
c. Li
d. O
______14. Which of the following elements has the greatest ionization energy?
a. Ga
b. K
c. Bi
d. As
______15. Which of the following elements has an electron affinity of 0 kJ/m?
a. Br
b. As
c. Ar
d. I
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Chapter Test A, continued
______16. Which of the following elements have full outer energy levels when
they are in the ground state?
a. alkali metals
b. noble gases
c. halogens
d. transition metals
______ 17. In which period is an element that has the electron configuration
1s22s22p63s23p63d104s24p1 when it is in its ground state?
a. Period 1
b. Period 2
c. Period 3
d. Period 4
______18. Which of the following elements is not a metal?
a. H
b. K
c. Na
d. Fr
______19. For atoms of p-block elements, the total number of electrons in the
highest occupied level is equal to the
a. period number.
b. group number.
c. period number minus 10.
d. group number minus 10.
______20. As electrons add to s and p sublevels in the same main energy level,
they are pulled closer to the more highly charged nucleus, causing
a. the electron cloud around the nucleus to expand.
b. atoms to lose electrons more easily.
c. atomic radii to decrease in size.
d. a noble gas configuration.
______21. Which electron configuration would result in the largest negative
electron affinity?
a. [He]2s1
b. [He]2s22p2
c. [He]2s22p3
d. [He]2s22p5
______22. In forming an ion, from which sublevel would an atom of nickel lose
electrons first?
a. 4s
b. 3d
c. 3p
d. 3s
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Chapter Test A, continued
______23. Which one of the following groups contains atoms that, in compounds,
have the lowest attraction for electrons?
a. Group 1
b. Group 2
c. Group 16
d. Group 17
______24. Which ionization energy is generally the largest?
a. first ionization energy
b. second ionization energy
c. third ionization energy
d. fourth ionization energy
______25. The metalloids are located on the periodic table between
a. halogens and noble gases.
b. nonmetals and metals.
c. alkaline-earth metals and other metals.
d. alkali metals and transition metals.
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Chapter Test
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Print RESOURCE PAGE
TEACHER
40. 7.05 1016 Hz
41. 1.28 s
42. 4.58 1019 J
24.
5 The Periodic Law,
pp. 36–45
25.
TEST A
1.
3.
5.
7.
9.
11.
13.
15.
17.
19.
21.
23.
25.
b
b
d
b
b
c
c
c
d
d
d
a
b
2.
4.
6.
8.
10.
12.
14.
16.
18.
20.
22.
24.
d
b
a
b
a
a
d
b
a
c
a
d
26.
27.
TEST B
1.
3.
5.
7.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
a
2. c
d
4. d
a
6. a
c
8. a
lanthanides
2
fourth
transition elements
32
valence electrons
electron affinity
electronegativity
ionization energy
3s23p4
atomic radius
ion
Group 1, Period 7, s block
All three groups of elements are metals. Alkali and alkaline-earth metals
are so reactive that they are not found
in nature as free elements. Transition
elements are generally less reactive.
Some are so unreactive that they do
not form compounds easily and exist
as free elements in nature.
23. Sodium has the largest atomic radius.
All the elements belong to Period 3,
but sodium has the lowest atomic
number and is therefore the first ele-
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
ment in Period 3. Atomic radii
decrease as you move from left to
right across a period.
In general, ionization energies of maingroup elements increase from left to
right across a period and decrease
down a group.
Electron affinity and electronegativity
are related. Electron affinity is a measure of the ease with which an atom
gains electrons. Electronegativity is a
measure of the ability of an atom to
attract electrons. Therefore, atoms
with a high negative electron affinity
are also the most electronegative.
The physical and chemical properties
of the elements are periodic functions
of their atomic numbers.
The ionic radii of cations are always
smaller than the atomic radii of the
neutral atoms from which they are
formed. The ionic radii of anions are
always larger than the atomic radii of
the neutral atoms from which they are
formed.
c
b
e
a
d
Period 5, s block
Period 4, p block
Period 4, d block
3d 54s2
3s23p3
4f 145d106s2
1, helium
2, neon
2, argon
3, neon
6 Chemical Bonding,
pp. 46–55
TEST A
1.
3.
5.
7.
9.
11.
13.
c
c
a
c
c
b
a
2.
4.
6.
8.
10.
12.
14.
b
c
d
b
b
c
a
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Answer Key