Download Periodic Table Name: Practice Review H

Unit 5- Periodic Table
Practice Review
Name: _________________________________
1. Which of the following scientists is credited with developing the
modern periodic table?
A) Le Châtelier
C) Dalton
E) Haber
B) Rutherford
D) Mendeleev
A) atomic masses
C) atomic numbers
E) physical properties
2. In the modern Periodic Table, the elements are arranged
according to
A)
B)
C)
D)
E)
10. The Periodic Law states that the chemical properties of
elements are periodic functions of their
11. The original format of the Periodic Table, as described by
Mendeleev, is based on the arranging the elements
atomic mass
atomic number
most common oxidation number
maximum positive oxidation number
atomic density
A)
B)
C)
D)
E)
3. Which is not a periodic property?
A) color
C) atomic radius
E) electronegativity
B) ionization energy
D) oxidation number
A) sodium
C) neptunium
E) tin
A) protons
C) nucleons
E) energy levels
B) Li and Ne
D) Si and P
B) S
C) Se
D) I
A)
B)
C)
D)
E)
E) Ti
7. Similar properties for chemical elements recur at certain
intervals of atomic number. Therefore, these properties are
referred to as
A) periodic
C) electronegativity
E) atomic number
B) neutrons
D) valence electrons
14. Elements in the same family
6. The element whose properties are most similar to those of
tellurium is
A) O
B) gallium
D) germanium
13. Each of the elements in a Main Group of the Periodic Table has
the same number of
B) neutron charge
D) covalent radius
5. Two elements with similar orbital structures are
A) Li and Ne
C) Na and K
E) Co and Ni
in order of increasing density
according to chemical properties
with reference to nuclear stability
in order of increasing number of neutrons
according to physical properties
12. The Periodic Table, based on an octet pattern, led Mendeleev
to predict the existence of the element referred to as
eka–silicon, now known as
4. The periodic table position and the chemical properties of the
elements arise from their
A) atomic mass
C) nuclear radius
E) electron configuration
B) isotopic masses
D) number of neutrons
are in the same horizontal row
have similar chemical properties
have the same number of protons
have the same number of electrons
have the same phase at room temperature
15. Which pair of atoms is expected to show the greatest chemical
similarities?
A) H and He
C) Sr and Ba
E) O and F
B) shielding effect
D) oxidation number
B) K and Ca
D) Na and Cl
8. Which is used as the basis for the atomic weights in the current
Periodic Table?
A) water
C) oxygen
E) carbon
B) hydrogen
D) nitrogen
9. What determines the order of elements in the Periodic Table?
A) size of ions
C) atomic mass
E) number of protons
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B) size of elements
D) number of neutrons
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Dr. Powell
16. The letters X, Y, and Z stand for three elements whose fluorides
have the formulas XF, YF2 , and ZF3. Where could X, Y, and Z be
located in the periodic table?
21. Consider the electron configurations:
I 1s22s23s2
II 1s22s22p6
III 1s22s22p63s1
IV 1s22s22p63s23p63d84s2
V 1s22s22p63s23p63d104s24p6
A)
The configurations that represent elements of the same Group
of the Periodic Table are
B)
A) I and IV
C) IV and V
E) I, II and V
C)
B) II and V
D) I, II and III
22. What similarity exists for the atoms of the Period 3 elements in
the ground state?
A)
B)
C)
D)
E)
D)
17. Similar chemical properties of families of elements is a result of
similar
A)
B)
C)
D)
E)
nuclear charges
physical properties
outer electron shells
numbers of electron shells
inner electron shells
B) 7
A) 6
D) 12
A)
B)
C)
D)
E)
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D) 4
E) 5
B) diagonal rows
D) vertical columns
B) 2
C) 3
D) 4
E) 5
a noble gas
an alkali metal
the eight element in the row
the eighteenth element in the row
a halogen
26. Which period in the periodic table contains the most
nonmetals ?
E) 19
20. In the periodic table elements with similar properties are
grouped in
A) periods
C) horizontal rows
E) horizontal families
C) 3
25. A new row in the periodic table begins immediately after
B) period 3, group IVA
D) period 6, group IVA
C) 9
B) 2
24. An atom with the outer electron structure
3d104s24p5 would be in which row of the periodic table?
19. An element with atomic number 11 is likely to have similar
chemical properties to the element whose atomic number is
A) 2
23. Which period contains elements which are all gases at standard
temperature and pressure?
A) 1
18. The ground state electronic configuration of the valence
electrons for an element is 3s23p2 .
This element belongs to
A) period 3, group IIA
C) period 4, group IIIA
E) period 6, group VA
3 valence electrons
the 3s sublevel contains 2 electrons
the 3p sublevel contains 6 electrons
3 principal energy levels contain electrons
the 3d sublevel is full
A) 1
B) 2
C) 3
D) 4
E) 5
27. Which period in the Periodic Table contains the most metals?
A) 2
B) 3
C) 4
D) 5
E) 6
28. Which element is correctly identified according to family and
period?
A)
B)
C)
D)
E)
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Element 10 is a halogen in period 2
Element 11 is an alkaline earth metal in period 4
Element 17 is a halogen in period 3
Element 21 is a transition metal in period 3
Element 3 is a alkaline earth metal in period 1
Dr. Powell
29. To which families in the periodic table do the elements belong?
31. Elements X', Y' and Z' have the following atomic radii.
Element M forms an M2+ ion
Element N forms a N2– ion
When atomic radii are correctly arranged, how might these
elements appear in the periodic table?
A) Both elements belong to the oxygen family
B) Both elements belong to the alkaline earth family
C) M belongs to the oxygen family and N belongs to the alkali
metals
D) M belongs to the alkaline earth family and N belongs to
the oxygen family
E) M belongs to the alkaline earth family and N belongs to
the halogen family
A)
B)
30. An element has a ground state electron configuration for its
valence electrons:
C)
The location of this element in the Periodic Table is
A) Period 2, Family IA
C) Period 3, Family IIIA
E) Period 3, Family VIA
B) Period 3, Family IIA
D) Period 3, Family VA
D)
32. Base your answer to the following question on the picture
below.
In which part of the Periodic Table are the elements with the
smallest covalent radius found?
A)
B)
C)
D)
E)
H-Chem
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A
B
C
D
None of the above are necessarily correct.
Dr. Powell
33. Chlorine has a smaller atomic radius than bromine because the
bromine atom has a greater
A)
B)
C)
D)
E)
number of protons
number of neutrons
number of energy levels
number of valence electrons
electronegativity
B) Mg
C) Na
D) Na+
A)
B)
C)
D)
E)
E) Be2+
A)
B)
C)
D)
E)
35. Which element has the largest diameter?
A) Al
B) Si
C) P
D) S
E) Cl
36. The atomic radii of the atoms becomes larger from lithium to
francium going down Group IA primarily as a result of
A)
B)
C)
D)
E)
the shielding effect
increased nuclear charge
the increased mass number
decreased metallic character
increasing number of neutrons
A) Ar; Ca2+; Cl–; Cl.
C) Cl–; Ar; Ca2+; Cl.
E) Ca2+; Ar; Cl–; Cl.
a greater nuclear charge
more unpaired electrons
a smaller atomic number
a smaller oxidation number
more neutrons
38. The variation in the radius of successive atoms in a period is
primarily caused by the
A)
B)
C)
D)
E)
B) Ca2+; Ar; Cl; Cl–.
D) Cl; Cl–; Ar; Ca2+.
43. Which is true regarding elements in the Periodic Table in the
sequence shown?
A)
B)
C)
D)
E)
Si ® P ® Cl shows increasing metallic character
Li ® Na ® K shows decreasing metallic character
C ® N ® O shows decreasing atomic radius
Ti, V, and Cr are nonmetals
Cl ® Br ® F shows decreasing electronegativity
44. The atomic radii decrease from left to right in a period of the
Periodic Table because the
A)
B)
C)
D)
atomic mass increases
number of protons decreases
number of electrons increases
electrostatic force between the nucleus and the electrons
increase
E) size of the nucleus increases
increase in nuclear charge
increase in number of neutrons
change in metallic properties
addition of a principal energy level
increase in nuclear radius
39. Consider the covalent radii of the Nitrogen Family
increases
decreases
stays the same
increases and then decreases
cannot be predicted
42. The atoms and ions in order of increasing radius are
37. An atom of fluorine is smaller than an atom of oxygen because
fluorine has
A)
B)
C)
D)
E)
increase from bottom to top
increase from top to bottom
increase from left to right
do not change in a regular manner
changes according to the number of neutrons
41. Within a Main Group of the Periodic Table, such as the
halogens, how does ionization energy change as atomic radius
increases?
34. Which of the following atoms or ions is the largest?
A) Mg2+
40. In the Periodic Table, the radii of atoms
45. Which of the following statements apply when an atom of
chlorine, Cl, becomes an ion in a chemical reaction?
I
Its charge is generally 1+.
II Its charge is generally 1–.
III The ion is larger than the atom.
IV The ion is smaller than the atom.
A) I and III only
C) II and III only
E) I only
The atomic radius of antimony is approximately
A)
C)
E)
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B)
D)
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B) I and IV only
D) II and IV only
Dr. Powell
46. In which part of the periodic table are the elements with the
largest ionic radius found?
50. Which has the smallest ionic radius?
A) aluminum ion
C) magnesium ion
E) lead ion
B) cesium ion
D) sodium ion
51. The diameter of a sodium atom, Na, is larger than the diameter
of a sodium ion, Na+, because the sodium ion has
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
upper left
lower left
upper right
lower right
upper right or lower left.
47. Which graph best depicts the change in the size of an ion with
increasing atomic number in a Period?
A)
B)
C)
more protons than the Na atom.
fewer protons than the Na atom.
a greater proton:electron ratio than its atom.
a smaller proton:electron ratio than its atom.
more neutrons than the Na atom.
52. Which is the element with the smallest ionic radius?
A) (A)
B) (B)
C) (C)
D) (D)
E) (E)
53. An atom of a nonmetal generally becomes an ion by
A)
B)
C)
D)
E)
D)
losing electrons
gaining electrons
losing protons
gaining neutrons
both losing protons and gaining electrons
54. Which electronic configuration represents atoms of the
element having the highest second ionization potential?
A) 1s2s22p4
C) 1s22s22p63s1
E) 1s22s22p63s23p1
E)
B) 1s22s22p6
D) 1s22s22p63s2
55. The first ionization energy of each successive element
decreases as the alkali metals, Group IA, are considered from
the top to the bottom of the Periodic Table. One reason for this
is that there is a
A)
B)
C)
D)
decrease in the nuclear charge.
increase in the number of neutrons.
decrease in the number of principal energy levels.
increase in the distance between the valence electrons
and the nucleus.
E) decrease in the shielding effect.
48. Four pairs of electrons in the outer level is referred to as a
stable
A) octet
B) nuclear charge
C) shielding effect
D) electronegativity
E) noble gas configuration
49. When an atom is changed to a negatively charged ion,
A)
B)
C)
D)
E)
protons are lost
electrons are lost
the radius increases
the ion is a better electron acceptor
the radius decreases
H-Chem
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Dr. Powell
Base your answers to questions 56 through 59 on the data
below. The data is the first four ionization energies, in kJ•mole
-1, of four elements in the same period.
63. Which of the following elements has the greatest electron
affinity
A) Bismuth
C) Fluorine
E) Carbon
B) Aluminum
D) Nitrogen
64. The strength of an atom’s attraction for the electrons in a
chemical bond is the atom’s
A) electronegativity
C) heat of reaction
E) none of the above
56. Which is from Group IIIA ?
A) A
C) C
E) None of the above
B) B
D) D
65. In which group of elements do the atoms gain electrons most
readily?
A) 1
57. Which is from Group VIIA ?
A) A
C) C
E) None of the above
A)
B)
C)
D)
E)
B) B
D) D
periodic force
gravitational attraction
shielding effect
electromagnetic attraction
weak force
H-Chem
low first ionization energy, low electronegativity
high first ionization energy, low electronegativity
low first ionization energy, high electronegativity
high first ionization energy, high electronegativity
high first ionization energy, zero electronegativity
B) sodium
D) calcium
69. The valence electrons of metals are
A)
B)
C)
D)
E)
the nuclear charge
the number of neutrons in the nucleus
the number of energy levels in the atom
the distance of the electron from the nucleus
the number of filled valence orbitals
loses an electron to form a negative ion
gains an electron to form a negative ion
loses an electron to form a positive ion
gains an electron to form a positive ion
none of the above
B) nonmetals
D) precious metals
A) magnesium
C) potassium
E) lithium
few in number and strongly held
few in number and weakly held
many in number and strongly held
many in number and weakly held
variable in number and strongly held
70. Atom X has 11 protons and 12 neutrons and atom Y has 12
protons and 12 neutrons. They are
A)
B)
C)
D)
E)
62. Electron affinity is a measure of the amount of energy released
when a neutral atom in the gaseous phase
A)
B)
C)
D)
E)
E) 18
68. The most metallic of these elements is
61. Which will not affect the ionization energy?
A)
B)
C)
D)
E)
D) 16
67. Which would correctly characterize a metal ?
B) B
D) D
60. The decreased effect of the attraction of a nucleus for valence
electrons due to the presence of intervening electrons is the
A)
B)
C)
D)
E)
C) 14
A) metals
C) noble gases
E) transition elements
59. Which is from Group IA?
A) A
C) C
E) None of the above
B) 2
66. The electronegativity of elements is generally greater for
B) B
D) D
58. Which is from Group IIA ?
A) A
C) C
E) None of the above
B) ionization energy
D) heat of formation
both metallic in character
isotopes of the same element
both nonmetallic in character
members of the same family in the Periodic Table
members of different periods in the Periodic Table
71. Which neutral element will most easily form a positive ion?
A)
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B)
C)
D)
E)
Dr. Powell
72. Which list consists entirely of diatomic molecules under normal
room conditions?
A)
B)
C)
D)
E)
helium, neon, argon, krypton
hydrogen, helium, fluorine, neon
carbon, oxygen, nitrogen, fluorine
oxygen, sulfur, selenium, tellurium
fluorine, chlorine, bromine, iodine
81. Which metal exists as a liquid at room temperature and
standard pressure?
A) aluminum
C) mercury
E) iodine
82. An oxide of the formula X2O would be formed if oxygen
combined with any element in
73. Which would correctly characterize a nonmetal?
A)
B)
C)
D)
E)
A) Group IA.
C) Group IIIA.
E) Group VIIA.
low first ionization energy and low electronegativity
high first ionization energy and low electronegativity
low first ionization energy and high electronegativity
high first ionization energy and high electronegativity
low first ionization energy and zero electronegativity
Al is the only metal
Cl is the only nonmetal
Cl and O are the only nonmetals
Ca and Na are the only metals
Al is the most reactivie element
A) halogens
C) alkali metals
E) chalcogens
A)
B)
C)
D)
E)
B) iodine
D) fluorine
formation of 2+ ions.
oxides dissolve in water to yield acids.
ionic radius is greater than the atomic radius.
atomic radius decreases with increasing atomic number.
large first ionization energy.
85. Among the elements of Group IA, which orbital provides the
electron most used in bonding?
76. Which element is not a diatomic molecule at STP?
A) iodine
C) oxygen
E) hydrogen
B) noble gases
D) alkaline earths
84. The characteristic typical of the elements in Group IIA of the
Periodic Table is the
75. Which is not a gas at room temperature?
A) xenon
C) oxygen
E) nitrogen
B) Group IIA.
D) Group IVA.
83. In which family (or Group) does the element beryllium, Be,
belong?
74. Based on the properties of Ca, O, Na, Al and Cl, which of the
statements is true?
A)
B)
C)
D)
E)
B) magnesium
D) tin
A) s
B) p
C) sp
D) sp2
E) sp3
Base your answers to questions 86 and 87 on the graph below.
B) carbon
D) nitrogen
77. Chemical elements having both metallic and nonmetallic
characteristics are called
A) atoms
C) metalloids
E) semiconductors
B) bi–metals
D) semi–solids
78. Which group contains two metalloids?
A) Group IIA
C) Group IIB
E) Group IA
B) Group VA
D) Group VB
79. Which element has the highest melting point?
A) Ar
B) Br
C) Hg
D) Si
86. Which are just beginning the pairing of electrons in the
p–orbitals?
E) Kr
80. Which Group of the periodic table contains only solid elements
at room temperature and standard pressure?
A) Group IA
C) Group VA
E) Group 0
H-Chem
A) (A)
B) (B)
C) (C)
D) (D)
E) (E)
87. Which have exactly half–filled p–orbitals?
B) Group IIA
D) Group VIA
A) (A)
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B) (B)
C) (C)
D) (D)
E) (E)
Dr. Powell
88. Which element in the 5th period of the Periodic Table have the
following electron configuration
A) Bi
B) Po
C) Sb
D) Te
95. The neutral atom of an element containing eight electrons in its
outer shell
A)
B)
C)
D)
E)
E) I
89. Which is the element with a possible oxidation number of –2?
A) (A)
B) (B)
C) (C)
D) (D)
96. The Noble gases are characterized by completed outer shells of
electrons. The outer shells of the Noble gases, with the
exception of helium, consist of
E) (E)
A) s and d electrons
C) p and d electrons
E) d and f electrons
90. Which group in the Periodic Table contains solid, liquid and
gaseous elements at room temperature and standard
pressure?
A) 0
B) IIA
C) VA
D) VIA
E) VIIA
91. In which family on the Periodic Table would the element having
an atomic number of 117 be placed?
A) Noble gas
C) Alkali metal
E) Nitrogen group
has a charge of 1+
is chemically inert
is chemically active
loses one electron when chemically reacting
forms many compounds
B) Halogen
D) Alkaline earth metal
B) s and p electrons
D) s, p and d electrons
97. From which sublevel(s) will an atom of Ni in the ground state
lose electrons to form the Ni3+ ion?
A) the 3p, only
C) the 4d, only
E) both the 4s and 4p
B) the 4s, only
D) both the 3d and 4s
98. Which set has elements with atomic radii which are nearly
identical?
92. Consider the melting points of Group VIIA elements.
A) C, P, Se, I
C) Cr, Mn, Fe, Co
E) Ne, Ar, Kr, Xe
B) Be, B, C, N
D) Mg, Ca, Sr, Ba
99. The element with the electron structure [Rn] 7s 2 6d1 5f5 is a
member of the series of elements called the
A) rare earths.
C) lanthinides.
E) chalcogens.
B) noble gases.
D) transuraniums.
100. The most colorful solids are the
Which value would be a reasonable prediction for the melting
point of astatine, 85As?
A) –150°C B) –50°C
C) 50°C
D) 100°C
93. The first ionization energy of 33As is 987
the first ionization energy for 34Se is
A)
B)
C)
D)
E)
kJ•mol–1.
A) iodides
C) chromates
E) chlorides
E) 200°C
The expected
101. The radii of the atoms become smaller when comparing
sodium to chlorine in Period 3. This is primarily as a result of
equal to that of arsenic
larger than that of arsenic
smaller than that of arsenic
unrelated to that of arsenic
undeterminable from the information given
94. An atom in the ground state with eight valence electrons is
most likely classified as a(n)
A) halogen
C) active metal
E) chalcogen
H-Chem
B) bromides
D) phosphates
A)
B)
C)
D)
E)
the shielding effect
increased nuclear charge
decreased metallic character
the increased number of electrons
increased number of filled orbitals
102. Which is a correct periodic trend in properties when
comparing Group IA to Group VIIA elements?
B) noble gas
D) inactive metal
A)
B)
C)
D)
E)
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increase in atomic volume
decrease in electronegativity
decrease in ionization energy
decrease in metallic character
decrease in nuclear charge
Dr. Powell
103. I. An aqueous solution of potassium chromate is colored
107. I. Aluminum and phosphorous exhibit different chemical
properties
BECAUSE
BECAUSE
II. a transition metal is present.
II. they are in the same period.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
104. I. Krypton is more likely than neon to react with fluorine
108. I. It is easier to remove the outermost electron from sodium
than from magnesium
BECAUSE
II. Neon is a Noble gas.
BECAUSE
II. the magnesium atom has a larger radius.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
105. I. Oxygen has a lower first ionization energy than fluorine
BECAUSE
109. I. The second ionization energy is larger than the first for any
given atom
II. oxygen has fewer protons in its nucleus.
BECAUSE
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
II. it is harder to remove a second electron from an atom.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
106. I. A sodium atom becomes a positive ion when it loses an
electron
BECAUSE
110. I. Ionic radii decrease across a period
II. electrons have a positive charge.
BECAUSE
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
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II. atomic radii decrease across a period.
A)
B)
C)
D)
I is TRUE, II is FALSE
I is FALSE, II is TRUE
I and II are BOTH FALSE
I and II are BOTH TRUE but II IS NOT a correct explanation
of I
E) I and II are BOTH TRUE and II IS a correct explanation of I
Dr. Powell