General Chemistry, 11e (Petrucci)
Chapter 9 The Periodic Table and Some Atomic Properties
1) The inner transition elements include the actinides and the lanthanides.
2) Moseley used X-rays to determine the atomic mass of each element.
3) Ions always adopt the electron configuration of a noble gas.
4) The covalent radius, metallic radius, and the ionic radius are all equal.
5) The ionization energy is the energy required for a gaseous atom to lose an electron.
6) The electron affinity is opposite to the ionization energy.
7) The electron affinity is the energy for an atom in its standard state to gain an electron.
8) An atom with an even number of electrons is always diamagnetic.
9) Paramagnetic is not the same as magnetic.
10) Polarizability decreases with the size of the atom.
11) Why was Moseley so sure from his X-ray work that there were no other undiscovered elements
besides the three that he predicted in the range of atomic numbers 13-79?
A) The rows on the periodic table were filled.
B) The columns of the periodic table were full.
C) All of the possible atomic weights were assigned.
D) All of the integer atomic numbers were assigned.
E) Mendeleev didn’t predict any more.
12) Elements in the first two groups are part of the main-group elements along with which of the
following groups?
A) d-block elements
B) s-block elements
C) actinides
D) lanthanides
E) p-block elements
13) The transition elements refer to what group of elements?
A) s-block elements
B) d-block elements
C) actinides
D) lanthanides
E) p-block elements
14) The actinides refer to what group of elements?
A) s-block elements
B) d-block elements
C) f-block elements of atomic number 58 through 71
D) f-block elements of atomic number 90 through 103
E) p-block elements
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15) Plutonium is among a group of elements referred to as:
A) actinides
B) alkalides
C) chalcocides
D) halides
E) lanthanides
16) Which of the following pairs of elements are classified as metalloids?
A) aluminum and silicon
B) argon and neon
C) arsenic and germanium
D) bromine and sulfur
E) copper and silver
17) Which of the following could never be isoelectronic species?
A) anions of two different elements
B) cations of two different elements
C) an anion and a cation
D) an anion and an atom
E) atoms of two different elements
18) Most transition elements form monatomic ions that are not:
A) isoelectronic with any other cations
B) isoelectronic with any noble gas
C) isoelectronic with any neutral atom
D) isoelectronic with any other species
E) isoelectronic with any other transition metal ion
19) The ion represented as Ti4+ has:
A) 22 electrons
B) 48 neutrons
C) 26 protons
D) 4 3d electrons
E) 0 4s electrons
20) The similar chemical behavior of the elements in a given group in the periodic table is best accounted
for by the fact that atoms of these elements have:
A) the same number of isotopes
B) the same number of electrons
C) the same number of electrons in the outermost (valence) shell
D) similar nuclear structures
E) the same number of protons
21) What is the ground state electron configuration for iron(III)?
A) [Ar]3d5
B) [Ar]4s23d3
C) [Ar]4s13d4
D) [Ar]4s24p3
E) [Ar]4p5
22) What is the general valence electronic configuration (where n = principal quantum number) that best
describes the halogens as a group?
A) ns1np6
B) ns2np4
C) ns2np5
D) ns2np6
E) ns2np3
23) Which statement best describes relationships in a modern periodic table?
A) Each transition element is placed in the column of the main group element that it most closely
resembles.
B) The fourteen elements in the “lanthanide” series form a new independent period.
C) Metalloids usually are the cations in ionic compounds.
D) Nonmetallic properties tend to predominate for elements at the far right portion of the table.
E) Elements are always arranged in order of increasing atomic weights.
24) Which ground state electronic configuration will most readily produce an ion with a charge of 2+?
A) 1s22s22p63s23p63d104s2
B) 1s22s22p63s23p64s1
C) 1s22s22p63s23p4
D) 1s22s22p63s23p63d104s24p2
E) 1s2s22p63s23p63d104s24p6
25) Which of the following has the largest radius?
A) Cl–
B) Ar
C) Sc3+
D) K+
E) P3-
26) Which of the following has the largest radius?
A) Se2-
B) Kr
C) Rb+
D) Br–
E) Y3+
27) Which of the following statements is INCORRECT?
A) The atomic radius decreases from left to right through a period of elements.
B) Cations are larger than the atoms from which they are formed.
C) The metallic character of elements decreases from left to right through a period of elements.
D) The ionization energy increases from left to right through a period of elements.
E) The atomic radius increases down the periodic table.
28) Which of the following has the largest atomic radius?
A) Rb
B) Br
C) Mo
D) I
29) A is the sequence Na, Mg, Al, Si, and P. B is the sequence He, Ne, Ar, Kr, and Xe. Which statement
below is true?
A) The members of A are decreasing in size.
B) The members of B have larger radii than those of A, respectively. That is He > Na, Ne > Mg, etc.
C) The members of A have larger radii than those of B, respectively.
D) The members of B are decreasing in size.
E) All the members of A are isoelectronic.
30) Among the alkali metals, cesium reacts more rapidly than sodium because:
A) cesium has more electrons
B) cesium has more neutrons
C) the valence electron of cesium is at a greater average distance from the nucleus
D) cesium has a higher atomic weight
E) cesium has more protons
31) Which of the following isoelectronic species has the largest radius?
A) Ne
B) F–
C) Mg2+
D) Na+
E) O2-
32) Which comparison of atomic and/or ionic radii is correct?
A) K+ > K
B) K+ > Ca2+
C) S > Si
D) Kr > Xe
E) Cl > Cl–
33) Which of the following has the smallest radius?
A) Yb3+
B) Ho3+
C) Nd3+
D) Gd3+
E) Ce3+
34) Which of the following has the largest radius?
A) As3-
B) Br
C) Sr2+
D) Cl–
E) Se2-
35) Which of the following occurs for the representative elements going left to right across the period?
A) Electronegativity decreases.
B) Atomic size increases.
C) Forces of attraction between electron and nucleus increase because the effective nuclear charge
increases.
D) The outer electrons are held more weakly.
E) none of these
36) The effective nuclear charge for sodium is:
A) +10
B) +9
C) +1
D) +11
E) 0
37) Which series of elements shows the smallest difference in atomic radii?
A) Li……F
B) Be……Ra
C) He……Xe
D) C……Pb
E) Sc……Zn
38) The first ionization energy for rubidium is +403.0 kJ/mol. How much energy would be required to
convert 17.1 g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature?
A) 185 kJ
B) 80.6 kJ
C) 68.9 kJ
D) 40.4 kJ
E) 34.5 kJ
39) Choose the INCORRECT statement.
A) Within a given subshell, each orbital is usually occupied by a single electron before any orbital has two
electrons.
B) When a metallic element unites with a nonmetallic element, electrons are lost by atoms of the metal
and gained by atoms of the nonmetals.
C) The noble gas atoms complete the filling of the p orbitals.
D) The ionization energy of Ca+ is greater than that for Ca2+.
E) The radius of Ba2+ is smaller than the radius of Ba+.
40) Choose the species from which one electron could most easily be removed.
A) Cl
B) K+
C) K
D) Ca+
E) Ar
41) Which comparison of ionization energies is correct?
A) Cs > Na
B) Na > Mg
C) Ca > Mg
D) Ca+ > Ca
E) Ar > He
42) The first ionization potential for S is lower than the first ionization potential for P because:
A) Hund’s rule is violated
B) P has a p3 configuration
C) ionization potentials decrease across a representative period
D) P is to the right of S on the periodic table
E) P is below S on the periodic table
43) What is the relationship between ionization energy and atomic radii?
A) Energy increases as radii increase.
B) Energy is negative for all large radii.
C) Energy decreases as radii decrease.
D) Energy decreases as radii increase
E) Energy increases as radii decrease
44) Which of the following elements is likely to have the largest second ionization energy?
A) Na
B) Mg
C) Al
D) Si
45) Which of the following has the smallest second ionization energy?
A) Si
B) Mg
C) Al
D) P
46) Which of the following reactions gives a positive value for the electron affinity?
A) S–(g) + e– → S2-(g)
B) O(g) + e– → O–(g)
C) S(g) + e– → S–(g)
D) Br(g) + e– → Br–(g)
47) Can alkali metal atoms form negative ions in the gaseous state? Explain.
A) No, an electron cannot be added.
B) No, only a liquid can be ionized.
C) Yes, an electron can be added to a Li half-filled 2s orbital.
D) Yes, an electron can be removed from a Li half-filled 2s orbital.
E) No, the 2s orbital is completely filled.
48) Why is the electron affinity so positive for the noble gas elements?
A) The added electron would have to go into a new shell.
B) The added electron would have to be added into the half-filled p subshell.
C) The added electron would have to be added into the p subshell.
D) The noble gas elements are diatomic elements.
E) Electrons can’t be added to gases.
49) Why is the electron affinity slightly positive for some of the group 2 elements?
A) The added electron would have to go into a new shell.
B) The added electron would have to be added into the half-filled p subshell.
C) The added electron would have to be added into the p subshell.
D) The groups 2 elements are diatomic elements.
E) Electrons can’t be added to metals.
50) What is the general relationship between electron affinity and atomic radii for neutral atoms in their
ground electronic states?
A) Electron affinity becomes more negative as radii increases.
B) Electron affinity becomes more negative as radii decreases.
C) Electron affinity becomes positive as radii decreases.
D) Electron affinity becomes positive as radii increases.
E) The two quantities are unrelated.
51) Which of the following species is diamagnetic?
A) F–
B) C
C) Al
D) S–
E) Na
52) Which species is diamagnetic?
A) atomic sodium
B) atomic fluorine
C) iron(III) ion
D) calcium(II) ion
E) cobalt(II) ion
53) Which of the following species is most likely to be diamagnetic?
A) Fe
B) I
C) Mn+
D) W3+
E) Zn2+
54) Which of the following has the greatest number of unpaired electrons?
A) Cr2+
B) Ti3+
C) Co2+
D) Ni
55) List in order of increasing charge of the most common ion:
S, Na, F, Ca, Al
A) S2-, Na–, F+, Ca2+, Al3+
B) Ca2-, F–, Al+, Na2+, S3+
C) F2-, S–, Ca+, Al2+, Na3+
D) S2-, F–, Na+, Ca2+, Al3+
E) Al2-, Ca–, F+, Na2+, S3+
56) The number of valence electrons for atomic potassium is ________.
A) 1
B) 5
C) 6
D) 15
E) 19
57) If the formula of an oxide is X2O3, what is the formula of the chloride of X?
A) XCl
B) X3Cl
C) XCl3
D) XCl6
E) X2Cl3
58) List in order of increasing atomic size: F, Na, K, Mg, Ne.
A) K < Mg < Ne < Na < F
B) Ne < Mg < K < Na < F
C) Ne < F < Mg < Na < K
D) Mg < F < Ne < Na < K
E) K < Na < Mg < F < Ne
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59) Which of the following atoms has the smallest atomic radius: Br, K, Fe, Cu, Bi?
A) Br
B) K
C) Fe
D) Cu
E) Bi
60) List in order of increasing size: Cl–, Ar, K+, S2-, Ca2+.
A) Ca2+ < K+ < Ar < Cl– < S2-
B) S2- < Cl– < Ar < K+ < Ca2+
C) Ca2+ < S2- < K+ < Ar < Cl–
D) Cl– < Ar < K+ < S2- < Ca2+
E) K+ < S2- < Ar < Cl– < Ca2+
61) List in order of increasing atomic size: Sr, Se, Cs, Ga, In.
A) Se < Ga < In < Sr < Cs
B) Ga < In < Se < Cs < Sr
C) Sr < In < Ga < Se < Cs
D) In < Ga < Cs < Se < Sr
E) Cs < Ga < Se < Sr < In
62) List in order of increasing size: K+, Se2-, Cl–, Na+, S2-.
A) Cl– < S2- < K+ < Na+ < Se2-
B) Na+ < K+ < Cl– < S2- < Se2-
C) S2- < Na+ < Cl– < Se2- < K+
D) Cl– < Se2- < K+ < Na+ < S2-
E) K+ < Na+ < Cl– < Se2- < S2-
63) Which main group atom or ion should be included in the following list?
Br–, Se2-, Kr, Sr2+
A) As3-
B) Ar
C) K+
D) S2-
64) List in order of increasing ionization energy: Na, K, F, Mg, Ne.
A) Na < K < F < Ne < Mg
B) K < Na < Mg < F < Ne
C) Ne < Mg < F < K < Na
D) F < Mg < Ne < K < Na
E) Ne < Na < Mg < F < K
65) The energy difference between atomic cesium and its most stable ion, in the gaseous state, is referred
to as ________.
A) atomic energy
B) electron affinity
C) entropy of vaporization
D) ionization energy
E) magnetic moment
66) Which of the following has the highest first ionization potential: K, Ge, Kr, Ca, Br?
A) K
B) Ge
C) Kr
D) Ca
E) Br
67) Which of the following has the highest first ionization potential: Sb, I, In, Xe, Rb?
A) Sb
B) I
C) In
D) Xe
E) Rb
68) Which of the following has the smallest value of the first ionization energy: Ar, Cs, N, Cu, Rb?
A) Ar
B) Cs
C) N
D) Cu
E) Rb
69) List in order of increasing ionization potential: O, Mg, Rb, S, Si.
A) Si < O < Mg < Rb < S
B) Si < S < Rb < Mg < O
C) Mg < O < Rb < S < Si
D) Rb < Mg < Si < S < O
E) S < Si < Mg < O < Rb
70) Arrange the following in order of increasing ionization energy: Li, Cs, K.
A) K < Li < Cs
B) Cs < K < Li
C) Li < Cs < K
D) Cs < Li < K
E) K < Cs < Li
71) Arrange the following elements in order of increasing ionization energy: Cs, Sc, Mn.
A) Sc < Mn < Cs
B) Sc < Cs < Mn
C) Cs < Mn < Sc
D) Cs < Sc < Mn
E) Mn < Cs < Sc
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72) How much energy, in joules, must be absorbed to convert all the atoms present in 1.00 mg of gaseous
Na into Na+? The first ionization energy of Na is 495.8 kJ/mol.
A) 21.6 J
B) 0.0464 J
C) 46.4 J
D) 0.0216 J
E) 1.14 × 104 J
73) List in order of more negative electron affinity: F, Br, Sb, Rb, Se.
(more positive → more negative)
A) Br < Se < Sb < Rb < F
B) Se < Rb < Sb < Br < F
C) Sb < Br < Rb < Se < F
D) Br < F < Rb < Sb < Se
E) Rb < Sb < Se < Br < F
74) Which of the following has the most negative electron affinity: Li, Be, N, O, F?
A) Li
B) Be
C) N
D) O
E) F
75) Choose the paramagnetic atom or ion: Ca, Ne, Sc3+, Cl–, Na.
A) Ca
B) Ne
C) Sc3+
D) Cl–
E) Na
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76) Which of the following has the most unpaired electrons: Na, Mn2+, S, N, Ar?
A) Na
B) Mn2+
C) S
D) N
E) Ar
77) Choose the paramagnetic atom or ion: Zn, Zn2+, Mn2+, Ar, Al3+.
A) Zn
B) Zn2+
C) Mn2+
D) Ar
E) Al3+
78) List in order of increasing number of unpaired electrons: N, Na, Si, Cr, Ar.
A) Cr < Si < Na < N < Ar
B) Ar < Cr < N < Na < Si
C) Ar < Cr < Si < Na < N
D) N < Na < Cr < Si < Ar
E) Ar < Na < Si < N < Cr
79) Which of the following has the largest number of unpaired electrons: S, Cr2+, N, K, Ne?
A) S
B) Cr2+
C) N
D) K
E) Ne
80) Which 1+ ion is isoelectronic with S2-?
81) Of the following, which atom has the largest atomic radius?
A) Rb
B) I
C) Cs
D) At
82) Of the following, which atom has the smallest atomic radius?
A) K
B) As
C) Rb
D) Sb
83) Which atom in each group (I and II) has the smallest atomic radius?
(I) Ba, Hf, At (II) As, Sb, Bi
A) Ba; As
B) Ba; Bi
C) At; As
D) At; Bi
84) Of the following, which element has the highest first ionization energy?
A) beryllium
B) boron
C) carbon
D) lithium
85) Of the following, which element has the highest first ionization energy?
A) Al
B) Cl
C) Na
D) P
86) Of the following, which element has the highest first ionization energy?
A) magnesium
B) potassium
C) aluminum
D) sodium
87) Of the following, which element has the highest first ionization energy?
A) Sr
B) Rb
C) Na
D) Ca
88) Of the following, which element has the highest first ionization energy?
A) Sr
B) Br
C) K
D) Te
89) Which ionization process requires the most energy?
A) W(g) → W+(g) + e–
B) W+(g) → W2+(g) + e–
C) W2+(g) → W3+(g) + e–
D) W3+(g) → W4+(g) + e–
90) Which ionization process requires the most energy?
A) O(g) → O+(g) + e–
B) O+(g) → O2+(g) + e–
C) F(g) → F+(g) + e–
D) F+(g) → F2+(g) + e–
91) Which of the following species will have the highest ionization energy?
A) K+
B) Ar
C) Cl–
D) S2-
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92) Which of the following represents the change in electronic configuration that is associated with the
first ionization energy of strontium?
A) [Kr]5s15p1 → [Kr]5s1 + e–
B) [Kr]5s2 → [Kr]5s15p1
C) [Kr]5s2 → [Kr]5s1 + e–
D) [Kr]5s2 + e– → [Kr]5s25p1
93) Which element has the highest first electron affinity?
A) Na
B) Mg
C) O
D) Ne