1. Mendeleev's periodic table is based on _____.
A) atomic weight
B) atomic number
C) electronic configuration
D) atomic volume
2. Moseley correlated _____ of elements with their _____.
A) frequency x-rays; atomic weight
B) frequency x-rays; atomic number
C) frequency of -rays; atomic weight
D) frequency of -rays; atomic number
3. Which of the following statements is true?
A) elements in a group have the same properties
B) elements in a group have similar properties
C) elements in a period have similar properties
D) elements in a period have the same properties
4. A non-metal of the following is _____.
A) Ba
B) Fe
C) P
D) Cu
5. An example of a metal is _____.
A) I2
B) Br2
C) Hg
D) S
6. Which of the following is a metalloid?
A) Bi
B) Pb
C) Ca
D) As
7. Representative elements are also called _____.
A) sub-group elements
B) main group elements
C) non-metals
D) metals
8. Representative elements are in groups _____.
A) 1 and 2
B) 13 to 17
C) 1,2 and 13 to 17
D) 3 to 12
9. An example of a representative element is _____.
A) Cr
B) Ca
C) Cu
D) Fe
10. Which of the following is not a representative element?
A) Cs
B) Al
C) S
D) Ni
11. An example of an element in group IA is _____.
A) Sr
B) Ru
C) Rb
D) Ra
12. Which of the following is an alkaline earth metal?
A) K
B) Ca
C) La
D) Pb
13. An element in group-13 (3A) of the following is _____.
A) P
B) Ge
C) Al
D) As
14. The element Sn is in group _____.
A) 4A
B) 6A
C) 5A
D) 7A
15. An example of an element in group-5A is _____.
A) Ge
B) S
C) Pb
D) P
16. Which of the following elements is not in group –7A?
A) F
B) At
C) I
D) Hf
17. An example of a transition metal is _____.
A) Fr
B) Pb
C) Pd
D) Po
18. An element existing in the monoatomic state is _____.
A) cesium
B) iodine
C) sulfur
D) oxygen
19. Which of the following is diatomic?
A) neon
B) phosphorus
C) oxygen
D) sodium
20. A monoatomic gas at 1 atm and 29°C is _____.
A) chlorine
B) neon
C) magnesium
D) arsenic
21. An element having an extensive three-dimensional structure is _____.
A) iodine
B) Hg
C) Mg
D) carbon
22. An element in the tetra atomic state is ____.
A) gallium
B) phosphorus
C) silicon
D) cesium
23. The element having three valence electrons is _____.
A) N
B) Ge
C) Al
D) Ca
24. Six valence electrons are present in _____.
A) Si
B) B
C) I
D) S
25. The number of valence electrons in phosphorus is _____.
A) 3
B) 5
C) 2
D) 4
26. The elements having ns1 configuration in their outermost shell are _____.
A) transition metals
B) halogens
C) alkali metals
D) alkaline earth metals
27. Halogens have _____ electrons in their outermost shell.
A) four
B) six
C) seven
D) three
28. Elements having eight electrons in their valence shell are _____.
A) noble gases
B) halogens
C) alkali metals
D) metals
29. The subshell which is gradually filled in the transition metal is _____.
A) s
B) d
C) f
D) p
30. Sc to Zn are called _____ row transition metals.
A) second
B) third
C) fourth
D) first
31. Isoelectronic ions have _____ electronic configuration.
A) similar
B) the same
C) different
D) unequal
32. Which of the following pairs cannot be isoelectronic _____.
A) ion–ion
B) atom–atom
C) cation–cation
D) cation–anion
33. O2– is isoelectronic with _____.
A) F–
B) K+
C) Cl–
D) Ar
34. Which of the following is isoelectronic with Na+?
A) Ar
B) Al3+
C) Cl–
D) Ca2+
35. Which of the following is not isoelectronic with Na+?
A) O2–
B) Ne
C) F–
D) K+
36. Mg2+ is isoelectronic with _____.
A) K+
B) Cl–
C) F–
D) S2–
37. Ti4+ is isoelectronic with _____.
A) Ar
B) Kr
C) Br–
D) Mg2+
38. The transition metal ion which is isoelectronic with Ar is _____.
A) V3+
B) Cr3+
C) Ti3+
D) Sc3+
39. An atom has 17 electrons. The element is a/an _____.
A) alkali metal
B) halogen
C) noble gas
D) transition metal
40. The element with atomic number 17 is placed in the _____ group of the IUPAC periodic
table.
A) 7th
B) 11th
C) 17th
D) 16th
41. The element with atomic number 17 is _____.
A) diatomic
B) halogen
C) non metal
D) all the above
Use the following to answer questions 42-47:
Consider the following elements:
A: 1s22s22p63s2
B: 1s22s22p3
C: [Ar]4s23d104p6
D: 1s22s2
E: 1s22s22p6
F: 1s22s22p63s23p3
42. The alkaline earth metals are _____.
A) C, E
B) B, F
C) A, D
D) E, F
43. The element 'D' will be similar in properties to _____.
A) B
B) E
C) F
D) A
44. Element E is a _____.
A) noble gas
B) halogen
C) 15th group element
D) lanthanide
45. A noble gas of is _____.
A) C
B) D
C) B
D) F
46. Element F belongs to the _____ group.
A) carbon
B) nitrogen
C) boron
D) oxygen
47. Element B will be similar in properties to element _____.
A) C
B) D
C) A
D) F
Use the following to answer questions 48-52:
Consider the following electron configurations:
A. 1s22s22p5
B. 1s22s1
C. 1s22s22p6
D. 1s22s22p63s23p5
E. [Ar] 4s1
F. [Ar]4s23d104p6
48. Which is a halogen?
A) B
B) C
C) A
D) E
49. Element E is a/an _____.
A) alkali metal
B) halogen
C) alkaline earth metal
D) transition metal
50. Which is a noble gas?
A) F
B) D
C) E
D) A
51. Element A will be similar in properties to _____.
A) F
B) E
C) D
D) C
52. Which is not a gas?
A) A
B) C
C) D
D) E
53. An element with atomic number-20 is _____.
A) alkali metal
B) transition metal
C) halogen
D) alkaline earth metal
54. Which of the following atomic numbers represents halogen?
A) 34
B) 55
C) 9
D) 16
55. An element with atomic number-26 is _____.
A) Ca
B) Fe
C) Co
D) Ni
56. The element [Ne]3s1 is in the _____ group.
A) 1st
B) 2nd
C) 13th
D) 17th
57. The element [Ne]3s23p3 is in the _____ group.
A) 13th
B) 2nd
C) 15th
D) 17th
58. The element [Ar]4s23d8 is a/an _____.
A) alkali metal
B) transition metal
C) lanthanide
D) halogen
59. 1s22s22p6 is the electronic configuration of _____.
A) Cl–
B) Al3+
C) Ar
D) K+
60. Which of the following will not have the configuration 1s2?
A) Li+
B) H–
C) Be2+
D) Mg2+
61. The ion having d10 configuration in the outermost shell is _____.
A) K+
B) Zn2+
C) Al3+
D) Mg2+
62. Which of the following does not form a monovalent cation?
A) Au
B) Tl
C) Zn
D) Cu
63. The metal which does not form a trivalent cation is _____.
A) Fe
B) Cr
C) Ti
D) Cd
64. The metal with the electronic configuration [Ar]3d3 is _____.
A) Cr3+
B) Fe3+
C) Ni2+
D) Co2+
65. Mn2+ will be isoelectronic with _____.
A) Ni2+
B) Fe3+
C) Cr3+
D) V2+
66. Cl– will be isoelectronic with _____.
A) Al3+
B) Ne
C) O2–
D) Ar
67. Be2+ will be isoelectronic with _____.
A) Na+
B) He
C) H+
D) Al3+
68. S2– will be isoelectronic with _____.
A) O2–
B) Na+
C) Ne
D) Cl–
69. N3– will be isoelectronic with _____.
A) Cl–
B) Ar
C) F–
D) P3–
70. The correct order of radius of an atom, A, to its ion is _____.
A) A– < A
B) A2+ < A+
C) A2+ > A
D) A+ > A–
71. The atom with the largest atomic radius of the following is _____.
A) Na
B) Br
C) Cs
D) Ca
72. The largest halogen atom of the following is _____.
A) F
B) I
C) Cl
D) Br
73. The correct order of atomic radius of the following is _____.
A) Na > Al > Cl > Mg
B) Na < Al < Cl < Mg
C) Na < Mg < Al < Cl
D) Na > Mg > Al > Cl
74. The largest atom in group 4A is _____.
A) Si
B) Ge
C) Pb
D) C
75. The smallest atom in group 7A is _____.
A) F
B) I
C) Br
D) Cl
76. The correct order of the size of the atom or ion of the following is _____.
A) Cl–< Cl
B) O2– < S2–
C) Na+ > Na
D) Mg2+ < Al3+
77. The correct order of radius of the following is _____.
A) O2– < F– < Na+ < Mg2+
B) F– < O2– < Mg2+ < Na+
C) Mg2+ < Na+ < F– < O2–
D) Mg2+ > Na+ > F– > O2–
78. The liquid in the fourth period is _____.
A) Ca
B) Br
C) As
D) Sc
79. The boiling points of neon and krypton are – 245.9°C and – 152.9°C. The boiling point
of argon could be
A) –90°C
B) –190°C
C) –300°C
D) –70°C
80. Pick out the correct statement from the following:
A) alkali metals have the lowest ionization energy
B) alkali metals have the highest ionization energy
C) halogens metals have the lowest ionization energy
D) inert gases metals have the lowest ionization energy
81. The element having higher ionization energy than magnesium is _____.
A) Na
B) Al
C) K
D) Si
82. The element having much higher third ionization energy is _____.
A) Al
B) Fe
C) Mg
D) Tl
83. Electron affinity is the energy liberated when an atom forms a _____.
A) free radiation
B) cation
C) anion
D) molecule
84. Electron affinity is highest for _____.
A) Cl
B) I
C) S
D) Br
85. Which of the following shows greater tendency towards the formation of an anion?
A) Ba
B) Br
C) Sb
D) As
86. Which of the following elements shows diagonal relation?
A) Be and Na
B) Li and Mg
C) Carbon and aluminium
D) Fluorine and argon
87. An acidic oxide of the following is _____.
A) MgO
B) Na2O
C) N2O5
D) Bi2O3
88. An example of a basic oxide is _____.
A) SO3
B) P2O5
C) BaO
D) P2O3
89. Amphoteric oxide of the following is _____.
A) CO2
B) SO2
C) CaO
D) ZnO
90. The most reactive element of the following is _____.
A) Li
B) Fr
C) Fe
D) Au
91. Which of the following has the highest ionization energy?
A) Cs
B) Xe
C) F
D) He
92. Which of the following statements is true for oxides?
A) acidic property increases from top to bottom in a group
B) basic property increases from top to bottom in a group
C) acidic property decreases from left to right in a period
D) metals form acidic oxides
93. The oxide, which forms acid with water, is _____.
A) Li2O
B) CaO
C) SO3
D) Na2O2
94. The most basic oxide of the following is _____.
A) BaO
B) SrO
C) MgO
D) CaO
95. Which oxide of the following is highly acidic?
A) CO2
B) CaO
C) SO3
D) CO
96. An example of a neutral oxide is _____.
A) P2O5
B) N2O
C) CO2
D) N2O5
97. The property, which increases from left to right in the period, is _____.
A) ionization energy
B) atomic radius
C) metallic character
D) covalent radius
98. The property, which decreases along a group from top to bottom, is _____.
A) atomic radius
B) metallic character
C) ionization energy
D) ionic radius
99. The acidity of oxides _____.
A) increases from left to right in a period
B) decreases from left to right in a period
C) increases from top to bottom in a group
D) is greater if the element forming oxide is highly electro positive
100. The halogen element in the fourth period is _____.
A) Cl
B) Br
C) F
D) I
101. The element in the 5th period in the nitrogen group is _____.
A) Sb
B) P
C) As
D) Bi
102. The most reactive metal in the fifth period is _____.
A) Cs
B) K
C) Ba
D) Rb
103. The element with atomic number less than 20 and similar to strontium is _____.
A) Ca
B) Mg
C) Rb
D) Ba
104. The correct order of ionization energy of the following is _____.
A) Na+ < Mg2+ < F– < O2–
B) O2– < F– < Na+ < Mg2+
C) O2– > F– > Na+ > Mg2+
D) F– < O2– < Na+ < Mg2+
105. The correct order of ionic radii of the following is _____.
A) Mg2+ > Na+ > F– > O2–
B) Mg2+ < O2– < Na+ < F–
C) O2– < F– < Na+ < Mg2+
D) Mg2+ < Na+ < F– < O2–
106. Which of the following is not a binary compound of the third period?
A) AlCl3
B) MgCl2
C) PCl3
D) KCl
107. A dark-red liquid of the following is _____.
A) Hg
B) Br2
C) Ga
D) Fr
108. The correct order of radius of the following is _____.
A) O2– > Mg2+
B) F– > O2–
C) Tl2+ > Tl+
D) Be > Mg
109. Which of the following is not a periodic property?
A) atomic radius
B) ionization energy
C) atomic volume
D) density
110. Carbon dioxide gives milky color with limewater due to the formation of _____.
A) CaO
B) CaCO3
C) Ca(HCO3)2
D) Ca(OH)2
111. The gas that attacks even glass is _____.
A) I2
B) Cl2
C) H2
D) F2
112. The element, which forms a compound with almost all elements, is _____.
A) F
B) O
C) H
D) C
113. Which of the following is the biggest in size?
A) H+
B) H
C) H–
D) proton
114. Which of the following produces carbonic acid upon reaction with water?
A) SO2
B) SO3
C) N2O5
D) CO2
115. The Most basic oxide of the following is _____.
A) Na2O
B) SO3
C) BaO
D) N2O5
116. The oxide of a second period element of the following is _____.
A) Na2O
B) P2O3
C) B2O3
D) SO2
117. Mono atomic gas of the following is _____.
A) chlorine
B) magnesium
C) krypton
D) hydrogen
118. Carbon dioxide will not react with _____.
A) Na2O
B) Na2O2
C) BaO
D) NO2
119. Potassium super oxide is _____.
A) K2O
B) KO2
C) K2O2
D) K2O3
120. Carbon dioxide will react with Na2O2 to yield _____.
A) Na2CO3
B) NaHCO3
C) Na2O
D) NaO2
121. The element having negative electron affinity is _____.
A) Cl
B) Ar
C) Br
D) I
122. The radius of K = 216 pm and that of K+ = 133 pm. The percentage decrease in volume
when an atom of potassium is converted into K+ ion is _____.
A) 43.3
B) 76.7
C) 13.6
D) 32.6
123. Which of the following ions is greater in size compared to the corresponding atoms?
A) Mg2+
B) Na+
C) Cl–
D) Al3+
124. The most abundant noble gas in the earth's atmosphere is _____.
A) Ne
B) Kr
C) Xe
D) Ar
125. The first noble gas discovered on the earth was _____.
A) He
B) Ne
C) Ar
D) Xe
126. Experimentally, the electron affinity of an element can be determined by using a laser
light to ionize the anion of the element in the gas phase:
X-(g) + h  X(g) + eThe electron affinity of chlorine is 349 kJ mol–1. The wavelength of a photon
corresponding to the EA of chlorine is _____ nm.
A) 343
B) 154
C) 454
D) 271
127. Which of the following is most easily oxidized into a trivalent state?
A) Cu2+
B) Fe2+
C) Mn2+
D) Mg2+
128. Which of the following hydrides will react with water?
A) HF
B) LiH
C) CH4
D) HCl
129. Which of the following compounds will not exist?
A) K3TiF6
B) K2Ti2O5
C) TiCl3
D) K2TiO4
130. Which of the following is used in antacid?
A) Mg(OH)2
B) NaOH
C) H3PO4
D) CsOH
131. The coolant used in a nuclear reactor is _____.
A) Cd
B) Na
C) B
D) Ba
132. The metal present in Epsom salt is _____.
A) Ca
B) K
C) Mg
D) Ba
133. Baking powder is _____.
A) Na2CO3
B) Na2C2O4
C) CaCO3
D) NaHCO3
134. The salt present in gunpowder is _____.
A) KNO3
B) NaCl
C) K2SO4
D) MgSO4
135. The oxide of nitrogen with +3 oxidation state is _____.
A) NO2
B) N2O4
C) N2O3
D) NO
136. The trend of the atomic radius is opposite to the trend of the _____.
A) covalent radius
B) ionization energy
C) ionic radius
D) density
137. The element having zero electron affinity of the following is _____.
A) C
B) N
C) O
D) F
138. The ionization energy of sodium is 495.9 kJ mol–1. The wavelength of light required to
ionize a Na atom is _____ nm.
A) 154
B) 471
C) 374
D) 242
139. The simplest hydride of silicon is _____.
A) SiH4
B) Si2H6
C) SiH2
D) SiH6
140. Pale yellow gas is ______.
A) O2
B) I2
C) F2
D) N2
141. An example of a metalloid is _____.
A) B
B) Ba
C) Br
D) Bi
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
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.
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
A
B
B
C
C
D
B
C
B
D
C
B
C
A
D
D
C
A
C
B
D
B
C
D
B
C
C
A
B
D
B
B
A
B
D
C
A
D
B
C
D
C
D
A
A
B
D
C
A
A
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
83.
84.
85.
86.
87.
88.
89.
90.
91.
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
C
D
D
C
B
A
C
B
B
D
B
C
D
A
B
D
B
D
C
B
C
B
D
C
A
B
C
B
B
A
D
C
C
A
B
B
C
C
D
B
D
B
C
A
C
B
A
C
A
B
A
D
103.
104.
105.
106.
107.
108.
109.
110.
111.
112.
113.
114.
115.
116.
117.
118.
119.
120.
121.
122.
123.
124.
125.
126.
127.
128.
129.
130.
131.
132.
133.
134.
135.
136.
137.
138.
139.
140.
141.
B
B
D
D
B
A
D
B
D
A
C
D
A
C
C
D
B
A
B
B
C
D
C
A
B
B
D
A
B
C
D
A
C
B
B
D
A
C
A
Chapter 8 Periodic Relationships Among the Elements
Student: ___________________________________________________________________________
1.
The nineteenth century chemists arranged elements in the periodic table according to increasing
A.
B.
C.
D.
E.
2.
Mendeleev proposed the existence of an unknown element that he called eka-aluminum. This element is
now called
A.
B.
C.
D.
E.
3.
the discovery of the periodic law.
the determination of the charge of the proton.
the measurement of the atomic numbers of the elements.
the determination of the electric charge of the electron.
the discovery of the law of octaves.
The elements in Group 7A are known by what name?
A.
B.
C.
D.
E.
5.
gallium.
silicon.
magnesium.
boron.
germanium.
The chief contribution of physicist Henry Moseley to atomic theory was
A.
B.
C.
D.
E.
4.
atomic number.
number of electrons.
atomic mass.
number of neutrons.
nuclear binding energy.
transition metals
halogens
alkali metals
alkaline earth metals
noble gases
The elements in Group 2A are known by what name?
A.
B.
C.
D.
E.
transition metals
halogens
alkali metals
alkaline earth metals
noble gases
6.
The alkali metal elements are found in _______ of the periodic table.
A.
B.
C.
D.
E.
7.
Which one of these elements is a transition element?
A.
B.
C.
D.
E.
8.
Sr
Pb
As
Fe
H
Which one of these elements is a transition element?
A.
B.
C.
D.
E.
9.
Group 1A
Group 2A
Group 3A
Period 7
Period 1
Nickel
Tin
Sodium
Sulfur
Calcium
The general electron configuration for atoms of all elements in Group 5A is
A.
B.
C.
D.
E.
ns2np6.
ns2np5.
ns2np4.
ns2np3.
ns2np1.
10. Which of these choices is the general electron configuration for the outermost electrons of elements in the
alkaline earth group?
A.
B.
C.
D.
E.
ns1
ns2
ns2np4
ns2np5
ns2np6(n -1)d6
11. The general electron configuration for atoms of the halogen group is
A.
B.
C.
D.
E.
ns2np6.
ns2np5.
ns2np6(n -1)d7.
ns1.
ns2np7.
12. The general electron configuration for noble gas atoms is
A.
B.
C.
D.
E.
ns2np6.
ns2np5.
ns2np4.
ns2np3.
ns2.
13. An element with the general electron configuration for its outermost electrons of ns2np1 would be in which
element group?
A.
B.
C.
D.
E.
2A
3A
4A
5A
8A
14. In what group of the periodic table is the element with the electron configuration
[Ar]4s23d104p3?
A.
B.
C.
D.
E.
1A
2A
3A
4A
5A
15. Consider the element with the electron configuration [Kr]5s24d7. This element is
A.
B.
C.
D.
E.
a representative element.
a transition metal.
a nonmetal.
an actinide element.
a noble gas.
16. Consider the element with the electron configuration [Kr]5s24d105p5. This element is
A.
B.
C.
D.
E.
a representative element.
a transition metal.
an alkali metal.
an actinide element.
a noble gas.
17. Consider the element with the electron configuration [Xe]6s24f7. This element is
A.
B.
C.
D.
E.
a representative element.
a lanthanide element.
a nonmetal.
an actinide element .
a noble gas.
18. The representative elements are those with unfilled energy levels in which the "last electron" was added to
A.
B.
C.
D.
E.
an s orbital.
an s or p orbital.
a d orbital.
a p or d orbital.
an f orbital.
19. How many valence electrons does a carbon atom have?
A.
B.
C.
D.
E.
1
2
3
4
6
20. How many valence electrons does a tin (Sn) atom have?
A.
B.
C.
D.
E.
2
4
14
36
50
21. How many electrons are in the 4p orbitals of selenium?
A.
B.
C.
D.
E.
0
2
4
5
6
22. How many electrons are in the 4p orbitals of vanadium?
A.
B.
C.
D.
E.
0
2
4
5
6
23. How many electrons are in the 4d orbitals of Tc?
A.
B.
C.
D.
E.
1
2
3
4
5
24. What is the charge on the monatomic ion that calcium forms in its compounds?
A.
B.
C.
D.
E.
+2
+1
-1
-2
-3
25. What is the charge on the monatomic ion of nitrogen, the nitride ion?
A.
B.
C.
D.
E.
+2
+1
-1
-2
-3
26. What is the charge on the stable ion formed by selenium?
A.
B.
C.
D.
E.
+2
+1
-1
-2
-3
27. Which of these elements forms stable +2 cations?
A.
B.
C.
D.
E.
Kr
I
Se
Al
Ba
28. Which two electron configurations represent elements that would have similar chemical properties?
(1) 1s22s22p4
(2) 1s22s22p5
(3) [Ar]4s23d104p3
(4) [Ar]4s23d104p4
A.
B.
C.
D.
E.
(1) and (2)
(1) and (3)
(1) and (4)
(2) and (4)
(2) and (3)
29. Which of these species make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+?
A.
B.
C.
D.
E.
Ca2+ and Fe3+
O2- and F
F and ClCl- and Ca2+
none of these
30. Which of these pairs consists of isoelectronic species?
A.
B.
C.
D.
E.
Mn2+ and Ar
Zn2+ and Cu2+
Na+ and K+
Cl- and S
K+ and Cl-
31. Which ion is isoelectronic with Ar?
A.
B.
C.
D.
E.
Fe2+
FBrGa3+
Ca2+
32. Which one of these ions is not isoelectronic with Kr?
A.
B.
C.
D.
E.
As3+
Se2Rb+
Sr2+
Br-
33. Which of these choices is the electron configuration for the aluminum ion?
A.
B.
C.
D.
E.
1s22s22p63s2
1s22s22p63s23p2
1s22s22p63s23p1
1s22s22p6
1s22s22p63s23p4
34. Which of these choices is the electron configuration for the chloride ion?
A.
B.
C.
D.
E.
[Ne]3s23p4
[Ne]3s23p7
[Ar]
[Ar]4s1
[Ne]3s23p5
35. Which of these choices is the electron configuration of a sulfide ion?
A.
B.
C.
D.
E.
[Ne]3s23p4
[Ne]
[Ne]3s23p1
[Ar]
[Ne]3s23p2
36. Which of these choices is the electron configuration of the iron(III) ion?
A.
B.
C.
D.
E.
[Ar]3d5
[Ar]4s13d5
[Ar]4s23d3
[Ar]3d6
[Ar]4s23d9
37. The electron configuration of a cobalt(III) ion is
A.
B.
C.
D.
E.
[Ar]3d5.
[Ar]4s13d5.
[Ar]4s23d4.
[Ar]3d6.
[Ar]4s23d9.
38. The sulfide ion, S2-, is isoelectronic with which one of the following?
A.
B.
C.
D.
E.
O2FNa+
Al3+
K+
39. Which one of these ions does not have [Kr] as its electronic configuration?
A.
B.
C.
D.
E.
Se2BrRb+
Y3+
Zn2+
40. Which one of these ions does not have [Xe] as its electronic configuration?
A.
B.
C.
D.
E.
Te2ICs+
Ba2+
Sn4+
41. The cobalt(III) ion, Co3+, has how many 3d electrons?
A.
B.
C.
D.
E.
0
7
6
5
4
42. How many 3d electrons does the copper(I) ion, Cu+, have?
A.
B.
C.
D.
E.
10
9
8
7
6
43. How many 3d electrons does an Fe3+ ion have?
A.
B.
C.
D.
E.
9
6
5
4
3
44. Which of these ground-state ions has the largest number of unpaired electrons?
A.
B.
C.
D.
E.
Cr2+
Mn2+
Ni2+
Cu+
Co2+
45. Which of these ground-state ions has unpaired electrons?
A.
B.
C.
D.
E.
P3V5+
Mg2+
Sc2+
S2-
46. Which of these atoms has the smallest radius?
A.
B.
C.
D.
E.
Al
P
As
Te
Na
47. Which of these atoms has the largest radius?
A.
B.
C.
D.
E.
B
Ga
Br
Si
Cl
48. Which of the elements listed below has the greatest atomic radius?
A.
B.
C.
D.
E.
B
Al
S
P
Si
49. Which one of these ions has the largest radius?
A.
B.
C.
D.
E.
ClK+
S2Na+
O2-
50. Arrange these ions in order of increasing ionic radius: K+, P3-, S2-, Cl-.
A.
B.
C.
D.
E.
Row 1
Row 2
Row 3
Row 4
Row 5
51. For which of these reactions is the enthalpy change equal to the second ionization energy of nitrogen?
A.
B.
C.
D.
E.
N2+(g)  N3+(g) + eN2+(g) + e-  N+(g)
N(g)  N2+(g) + 2eN-(g) + e-  N2-(g)
N+(g)  N2+(g) + e-
52. For which of these reactions is the enthalpy change equal to the third ionization energy of vanadium?
A.
B.
C.
D.
E.
V2+(g)  V3+(g) + eV3+(g) + e-  V2+(g)
V(g)  V3+(g) + 3eV2-(g) + e-  V3-(g)
V3+(g)  V4+(g) + e-
53. Which of these elements has the highest first ionization energy?
A.
B.
C.
D.
E.
Cs
Ga
K
Bi
As
54. Which of these elements has the highest first ionization energy?
A.
B.
C.
D.
E.
C
Si
Ge
Sn
Pb
55. Which of these elements has the smallest first ionization energy?
A.
B.
C.
D.
E.
Cl
Na
Be
K
As
56. Which of these elements has the smallest ionization energy?
A.
B.
C.
D.
E.
Li
Na
Be
K
Rb
57. Which of these elements will display an unusually large jump in ionization energy values between I3 and
I4, its third and fourth ionization energies?
A.
B.
C.
D.
E.
Na
Mg
Al
Si
P
58. For silicon atoms, which ionization energy will show an exceptionally large increase over the preceding
ionization energy?
A.
B.
C.
D.
E.
2nd
3rd
4th
5th
6th
59. For phosphorus atoms, which ionization energy will show an exceptionally large increase over the
previous ionization energy?
A.
B.
C.
D.
E.
2nd
3rd
4th
5th
6th
60. Which of these elements has the following pattern for its first six ionization energies? (I1 = first ionization
energy, I2 = second ionization energy, etc.)
A.
B.
C.
D.
E.
Ca
Si
Al
Se
P
61. The successive ionization energies of a certain element are I1 = 589.5 kJ/mol, I2 =1145 kJ/mol, I3= 4900
kJ/mol, I4 = 6500 kJ/mol, and I5 = 8100 kJ/mol. This pattern of ionization energies suggests that the
unknown element is
A.
B.
C.
D.
E.
K.
Si.
As.
Ca.
S.
62. The successive ionization energies of a certain element are I1 = 577.9 kJ/mol, I2 = 1820 kJ/mol, I3= 2750
kJ/mol, I4 = 11,600 kJ/mol, and I5 = 14,800 kJ/mol. This pattern of ionization energies suggests that the
unknown element is
A.
B.
C.
D.
E.
K.
Al.
Cl.
Se.
Kr.
63. Which of these elements has the greatest electron affinity (largest positive value)?
A.
B.
C.
D.
E.
Mg
Al
Si
P
S
64. Which of these elements has the greatest electron affinity (largest positive value)?
A.
B.
C.
D.
E.
K
Br
As
Ar
I
65. Which of these atoms has the greatest electron affinity (largest positive value)?
A.
B.
C.
D.
E.
S
P
Ga
Li
Br
66. The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s)  Na+(g)
+ e- is therefore
A.
B.
C.
D.
E.
495.9 kJ/mol.
less than 495.9 kJ/mol.
greater than 495.9 kJ/mol.
equal to the electron affinity of sodium.
equal to the second ionization energy of sodium.
67. The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l)  Hg+(g)
+ e- is therefore
A.
B.
C.
D.
E.
1006 kJ/mol.
greater than 1006 kJ/mol.
less than 1006 kJ/mol.
equal to the electron affinity of mercury.
equal to the second ionization energy of mercury.
68. The electron affinity of oxygen is equal to
A.
B.
C.
D.
E.
the ionization energy of O-.
the ionization energy of O2-.
the second ionization energy of O.
twice the electron affinity of O+.
none of these.
69. Which pair of elements from different groups resemble each other the most in their chemical properties?
A.
B.
C.
D.
E.
Be and B
Al and Si
Li and Be
Al and Be
Be and C
70. Which of these elements has the greatest metallic character?
A.
B.
C.
D.
E.
Br
F
Ge
Mn
Sc
71. Which of these elements has the greatest metallic character?
A.
B.
C.
D.
E.
Br
Se
Ni
As
Si
72. Which of these elements has the greatest metallic character?
A.
B.
C.
D.
E.
Ca
Mg
Ba
As
Se
73. If the radius of atom X is greater than the radius of atom Y, then it is also likely that
A.
B.
C.
D.
E.
X has a larger electron affinity than Y does.
X has a larger effective nuclear charge than Y does.
X has greater metallic character than Y does.
X has a larger first ionization energy than Y does.
X is a poorer conductor of electricity than Y when in the solid state.
74. Which of these compounds is an amphoteric oxide?
A.
B.
C.
D.
E.
Na2O
MgO
Al2O3
SO2
Cl2O7
75. Which of these compounds is a basic oxide?
A.
B.
C.
D.
E.
CO2
CaO
SO2
H2O
NO2
76. Which of these compounds is an acidic oxide?
A.
B.
C.
D.
E.
P4O10
MgO
Fe2O3
K2O
Cr2O3
77. Which of these compounds is a basic oxide?
A.
B.
C.
D.
E.
CO2
MgO
As2O3
SO2
Cl2O7
78. Which of these compounds is a basic oxide?
A.
B.
C.
D.
E.
NO2
H2O
Na2O
SnO
SO2
79. Since arsenic is a nonmetal, As2O3 is expected to be a/an _____ oxide.
A.
B.
C.
D.
E.
acidic
ionic
amphoteric
neutral
basic
80. Since zirconium is a metal, ZrO2 is expected to be a/an _____ oxide.
A.
B.
C.
D.
E.
acidic
ionic
amphoteric
neutral
basic
81. Which of these elements exhibits chemical behavior similar to that of calcium?
A.
B.
C.
D.
E.
magnesium
sodium
sulfur
chlorine
iron
82. Which of these elements exhibits chemical behavior similar to that of potassium?
A.
B.
C.
D.
E.
magnesium
sodium
beryllium
chlorine
iron
83. Which of these elements exhibits chemical behavior similar to that of oxygen?
A.
B.
C.
D.
E.
F.
magnesium
sodium
sulfur
chlorine
iron
beryllium
84. Which of these elements exhibits chemical behavior similar to that of silver?
A.
B.
C.
D.
E.
F.
nickel
gold
sulfur
chlorine
iron
beryllium
85. The second ionization energy of Mg is ________ than its first ionization energy, and is __________ than
the second ionization energy of Na.
A.
B.
C.
D.
higher, higher
lower, higher
higher, lower
lower, lower
86. Consider the following reaction: 3Li + Z  Li3Z.
What is the formula for the compound if we substitute sodium for lithium?
A.
B.
C.
D.
E.
NaZ
Na2Z
NaZ2
Na3Z
NaZ3
87. Consider the following reaction: 3Li + Z  Li3Z.
What is the formula for the compound if we substitute magnesium for lithium?
A.
B.
C.
D.
E.
MgZ
Mg2Z
MgZ2
Mg3Z
Mg3Z2
88. Consider the following reaction 2A + 3F2  2AF3.
What is the formula for the reaction product if we substitute iodine for fluorine?
A.
B.
C.
D.
E.
A2I3
A3I2
AI3
A3I
AI
89. Consider the following reaction 2A + 3F2  2AF3.
What is the formula for the reaction product if we substitute sulfur for fluorine?
A.
B.
C.
D.
E.
A2S3
A3S2
AS3
A3S
AS
90. Write the ground-state electron configuration for S2-.
91. Write the ground-state electron configuration for Ca2+.
92. Write the ground-state electron configuration for Cr3+.
93. Write the ground-state electron configuration for Ni2+.
94. Write the ground-state electron configuration for Br-.
95. Write the ground-state electron configuration for K+.
96. Write the ground-state electron configuration for Al3+.
97. Write the ground-state electron configuration for O2-.
98. Write the ground-state electron configuration for I-.
99. Write the ground-state electron configuration for Mg2+.
100. Why is the Mg2+ ion smaller than F- even though they are isoelectronic?
101. Which species has the greater radius, an I- ion or an I atom? Briefly explain your choice of answer.
102. Briefly explain why the atomic radius decreases within a period when moving from left to right.
103. The radius of an atom of sodium is 190 picometers. How many nanometers is this?
104. Given the following density data, what is a reasonable estimate of the density of the element gallium?
105. Given the following melting point data, what is a reasonable estimate of the melting point of potassium.
106. What is the difference between a calcium atom and a calcium ion?
107. How do sodium metal and sodium ions differ in their chemical properties?
108. Consider the following reaction: 3Li + Z  Li3Z.
What is a reasonable guess for the identity of element Z?
109. Consider the following reaction 2A + 3F2  2AF3.
What is a reasonable guess for the identity element A?
110. The radii of ions are always smaller than the radii of the corresponding atoms of the same element.
True False
111. Electron affinity is always a positive quantity.
True False
112. The electron configuration of the outermost electrons of atoms of the halogen group is ns2np7.
True False
113. Amphoteric oxides exhibit both acidic and basic properties.
True False
114. For Mg atoms a very large jump in the magnitudes of the ionization energies will occur between the
second and the third ionization energies.
True False
Chapter 8 Periodic Relationships Among the Elements
Key
1.C
2.A
3.C
4.B
5.D
6.A
7.D
8.A
9.D
10.B
11.B
12.A
13.B
14.E
15.B
16.A
17.B
18.B
19.D
20.B
21.C
22.A
23.E
24.A
25.E
Page 1
26.D
27.E
28.C
29.D
30.E
31.E
32.A
33.D
34.C
35.D
36.A
37.D
38.E
39.E
40.E
41.C
42.A
43.C
44.B
45.D
46.B
47.B
48.B
49.C
50.A
51.E
52.A
53.E
54.A
55.D
56.E
Page 2
57.C
58.D
59.E
60.B
61.D
62.B
63.E
64.B
65.E
66.C
67.B
68.A
69.D
70.E
71.C
72.C
73.C
74.C
75.B
76.A
77.B
78.C
79.A
80.E
81.A
82.B
83.C
84.B
85.C
86.D
87.E
Page 3
88.C
89.A
90.[Ar]
91.[Ar]
92.[Ar]3d3
93.[Ar]3d8
94.[Kr]
95.[Ar]
96.[Ne]
97.[Ne]
98.[Xe]
99.[Ne]
100.Mg2+ has a higher nuclear charge than F-.
101.I-; I and I- have the same number of protons, but I- has a greater number of electrons. The additional electron-electron
repulsion in I- causes the radius of the ion to be larger than that of the neutral atom.
102.Effective nuclear charge increases in that direction. As the effective nuclear charge increases, the electrons are pulled closer
to the nucleus and thus the radius of the atom decreases.
103.0.190 nm
104.5-6 g/mL
105.Around 60oC
106.A calcium atom has two more electrons than a calcium ion.
107.Sodium metal is very reactive, whereas sodium ions are stable in solution.
108.Nitrogen (Student answers will vary.)
109.Aluminum
110.FALSE
111.FALSE
112.FALSE
113.TRUE
114.TRUE
Page 4