Chemistry: The Central Science, 13e (Brown et al.)
Chapter 7 Periodic Properties of the Elements
7.1 Multiple-Choice Questions
1) In which set of elements would all members be expected to have very similar chemical properties?
A) O, S, Se
B) N, O, F
C) Na, Mg, K
D) S, Se, Si
E) Ne, Na, Mg
2) In which set of elements would all members be expected to have very similar chemical properties?
A) P, Se, I
B) Cl, Br, Na
C) Si, As, Te
D) Ne, Na, Mg
E) Br, I, At
3) Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ________
in Ar.
A) nuclear charge
B) paramagnetism
C) diamagnetism
D) Hund’s rule
E) azimuthal quantum number
4) Screening of the nuclear charge by core electrons in atoms is ________.
A) less efficient than that by valence electrons
B) more efficient than that by valence electrons
C) essentially identical to that by valence electrons
D) responsible for a general decrease in atomic radius going down a group
E) both essentially identical to that by valence electrons and responsible for a general decrease in atomic
radius going down a group
5) The effective nuclear charge of an atom is primarily affected by ________.
A) inner electrons
B) outer electrons
C) nuclear charge
D) electron distribution
E) orbital radial probability
6) The atomic radius of main-group elements generally increases down a group because ________.
A) effective nuclear charge increases down a group
B) effective nuclear charge decreases down a group
C) effective nuclear charge zigzags down a group
D) the principal quantum number of the valence orbitals increases
E) both effective nuclear charge increases down a group and the principal quantum number of the
valence orbitals increases
7) Atomic radius generally increases as we move ________.
A) down a group and from right to left across a period
B) up a group and from left to right across a period
C) down a group and from left to right across a period
D) up a group and from right to left across a period
E) down a group; the period position has no effect
8) Atomic radius generally decreases as we move ________.
A) down a group and from right to left across a period
B) up a group and from left to right across a period
C) down a group and from left to right across a period
D) up a group and from right to left across a period
E) down a group; the period position has no effect
9) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?
A) Mg > Na > P > Si > Ar
B) Ar > Si > P > Na > Mg
C) Si > P > Ar > Na > Mg
D) Na > Mg > Si > P > Ar
E) Ar > P > Si > Mg > Na
10) Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr?
A) Ca > K > As > Ge > Kr
B) Kr > Ge > As > K > Ca
C) Ge > As > Kr > K > Ca
D) K > Ca > Ge > As > Kr
E) Kr > As > Ge > Ca > K
11) Of the compounds below, ________ has the smallest ionic separation.
A) KF
B) K2S
C) RbCl
D) SrBr2
E) RbF
12) Which of the following is an isoelectronic series?
A) B5-, Si4-, As3-, Te2-
B) F–, Cl–, Br–, I–
C) S, Cl, Ar, K
D) Si2-, P2-, S2-, Cl2-
E) O2-, F–, Ne, Na+
13) Which isoelectronic series is correctly arranged in order of increasing radius?
A) K+ < Ca2+ < Ar < Cl–
B) < Ar < K+ < Ca2+
C) Ca2+ < Ar < K+ < Cl–
D) Ca2+ < K+ < Ar < Cl–
E) Ca2+ < K+ < Cl– < Ar
14) Of the choices below, which gives the order for first ionization energies?
A) Cl > S > Al > Ar > Si
B) Ar > Cl > S > Si > Al
C) Al > Si > S > Cl > Ar
D) Cl > S > Al > Si > Ar
E) S > Si > Cl > Al > Ar
15) Of the choices below, which gives the order for first ionization energies?
A) Kr > Se > Br > Ga > Ge
B) Kr > Br > Se > Ge > Ga
C) Ga > Br > Ge > Kr > Se
D) Ga > Ge > Se > Br > Kr
E) Br > Se > Ga > Kr > Ge
16) ________ have the lowest first ionization energies of the groups listed.
A) Alkali metals
B) Transition elements
C) Halogens
D) Alkaline earth metals
E) Noble gases
17) Which of the following correctly represents the second ionization of aluminum?
A) Al+ (g) + e– → Al (g)
B) Al (g) → (g) + e–
C) Al– (g) + e– → Al2- (g)
D) Al+ (g) + e– → Al2+ (g)
E) Al+ (g) → Al2+ (g) + e–
18) Which of the following correctly represents the third ionization of aluminum?
A) Al2+ (g) + e– → Al+ (g)
B) Al (g) → Al+ (g) + e–
C) Al2- (g) + e– → Al3- (g)
D) Al2+ (g) + e– → Al3+ (g)
E) Al2+ (g) → Al3+ (g) + e–
19) Which of the following correctly represents the second ionization of phosphorus?
A) P+ (g) + e– → P2+ (g)
B) P (g) → P+ (g) + e–
C) P– (g) + e– → P2- (g)
D) P+ (g) → P2+ (g) + e–
E) P+ (g) + e– → P (g)
20) Which equation correctly represents the first ionization of calcium?
A) Ca (g) → Ca+ (g) + e–
B) Ca (g) → Ca– (g) + e–
C) Ca (g) + e– → Ca– (g)
D) Ca– (g) → Ca (g) + e–
E) Ca+ (g) + e– → Ca (g)
21) Which of the following correctly represents the second ionization of calcium?
A) Ca (g) → Ca+ (g) + e–
B) Ca+ (g) → Ca2+ (g) + e–
C) Ca– (g) + e– → Ca2- (g)
D) Ca+ (g) + e– → Ca2+ (g)
E) Ca+ (g) + e– → Ca (g)
22) Which of the following correctly represents the second ionization of copper?
A) Cu (g) → Cu+ (g) + e–
B) Cu+ (g) → Cu2+ (g) + e–
C) Cu– (g) + e– → Cu2- (g)
D) Cu+ (g) + e– → Cu2+ (g)
E) Cu+ (g) + e– → Cu (g)
23) Which ion below has the largest radius?
A) Cl–
B) K+
C) Br–
D) F–
E) Na+
24) Of the following species, ________ has the largest radius.
A) Rb+
B) Sr2+
C) Br–
D) Kr
E) Ar
Consider the following electron configurations to answer the questions that follow:
(i) 1s2 2s2 2p6 3s1
(ii) 1s2 2s2 2p6 3s2
(iii) 1s2 2s2 2p6 3s2 3p1
(iv) 1s2 2s2 2p6 3s2 3p4
(v) 1s2 2s2 2p6 3s2 3p5
25) The electron configuration belonging to the atom with the highest second ionization energy is
________.
A) (i)
B) (ii)
C) (iii)
D) (iv)
E) (v)
26) The electron configuration that belongs to the atom with the lowest second ionization energy is
________.
A) (i)
B) (ii)
C) (iii)
D) (iv)
E) (v)
27) The electron configuration of the atom with the most negative electron affinity is ________.
A) (i)
B) (ii)
C) (iii)
D) (iv)
E) (v)
28) The electron configuration of the atom that is expected to have a positive electron affinity is ________.
A) (i)
B) (ii)
C) (iii)
D) (iv)
E) (v)
29) Of the following elements, ________ has the most negative electron affinity.
A) S
B) Cl
C) Se
D) Br
E) I
30) Of the following elements, ________ has the most negative electron affinity.
A) P
B) Al
C) Si
D) Cl
E) B
31) Of the following elements, ________ has the most negative electron affinity.
A) O
B) K
C) B
D) Na
E) S
32) Sodium is much more apt to exist as a cation than is chlorine. This is because ________.
A) chlorine is a gas and sodium is a solid
B) chlorine has a greater electron affinity than sodium does
C) chlorine is bigger than sodium
D) chlorine has a greater ionization energy than sodium does
E) chlorine is more metallic than sodium
33) Which equation correctly represents the electron affinity of calcium?
A) Ca (g) + e– → Ca– (g)
B) Ca (g) → Ca+ (g) + e–
C) Ca (g) → Ca– (g) + e–
D) Ca– (g) → Ca (g) + e–
E) Ca+ (g) + e– → Ca (g)
34) Which of the following correctly represents the electron affinity of bromine?
A) Br (g) → Br+ (g) + e–
B) Br (g) + e– → Br– (g)
C) Br2 (g) + e– → Br– (g)
D) Br2 (g) + 2e– → 2Br– (g)
E) Br+ (g) + e– → Br (g)
35) Which of the following correctly represents the electron affinity of phosphorus?
A) P (g) → P+ (g) + e–
B) P (g) + e– → P– (g)
C) P4 (g) + e– → P– (g)
D) P4 (g) + 4e– → 4P– (g)
E) P+ (g) + e– → P (g)
36) In the generation of most anions, the energy change (kJ/mol) that _______ an electron is ________.
A) removes, positive
B) adds, positive
C) removes, negative
D) adds, negative
E) None of the above is correct.
37) Of the elements below, ________ is the most metallic.
A) sodium
B) barium
C) magnesium
D) calcium
E) cesium
38) The list that correctly indicates the order of metallic character is ________.
A) B > N > C
B) F > Cl > S
C) Si > P > S
D) P > S > Se
E) Na > K > Rb
39) The list that correctly indicates the order of metallic character is ________.
A) Sr > Ca > Mg
B) F > Cl > Br
C) C > Ge > Si
D) Li > Na > K
E) O > Se > S
40) Of the elements below, ________ has the highest melting point.
A) Ca
B) K
C) Fe
D) Na
E) Ba
41) Of the following metals, ________ exhibits multiple oxidation states.
A) Al
B) Rb
C) Mg
D) Ni
E) Cs
42) Of the following oxides, ________ is the most acidic.
A) CaO
B) CO2
C) Al2O3
D) Li2O
E) Na2O
43) The acidity of carbonated water is due to the ________.
A) presence of sulfur
B) reaction of CO2 and H2O
C) addition of acid
D) nonmetal oxides
E) none of the above
44) The element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an
electrical semiconductor is ________.
A) Sn
B) B
C) As
D) Si
E) Ge
45) Transition metals within a period differ mainly in the number of ________ electrons.
A) s
B) p
C) d
D) f
E) all of the above
46) Which one of the following compounds would produce an acidic solution when dissolved in water?
A) Na2O
B) CaO
C) MgO
D) CO2
E) SrO
47) Nonmetals can be ________ at room temperature.
A) solid, liquid, or gas
B) solid or liquid
C) solid only
D) liquid only
E) liquid or gas
48) Which of the following is not a characteristic of metals?
A) acidic oxides
B) low ionization energies
C) malleability
D) ductility
E) These are all characteristics of metals.
49) When two elements combine to form a compound, the greater the difference in metallic character
between the two elements, the greater the likelihood that the compound will be ________.
A) a gas at room temperature
B) a solid at room temperature
C) metallic
D) nonmetallic
E) a liquid at room temperature
50) Alkaline earth metals ________.
A) have the smallest atomic radius in a given period
B) form monoanions
C) form basic oxides
D) exist as triatomic molecules
E) form halides with the formula MX
51) Between which two elements is the difference in metallic character the greatest?
A) Rb and O
B) O and I
C) Rb and I
D) Li and O
E) Li and Rb
52) The oxide of which element below can react with hydrochloric acid?
A) sulfur
B) selenium
C) nitrogen
D) sodium
E) carbon
53) Consider the general valence electron configuration of ns2np5 and the following statements:
(i) Elements with this electron configuration are expected to form -1 anions.
(ii) Elements with this electron configuration are expected to have large
positive electron affinities.
(iii) Elements with this electron configuration are nonmetals.
(iv) Elements with this electron configuration form acidic oxides.
Which statements are true?
A) (i) and (ii)
B) (i), (ii), and (iii)
C) (ii) and (iii)
D) (i), (iii,) and (iv)
E) All statements are true.
54) Which of the following traits characterizes the alkali metals?
A) very high melting point
B) existence as diatomic molecules
C) formation of dianions
D) the lowest first ionization energies in a period
E) the smallest atomic radius in a period
55) This element is more reactive than lithium and magnesium but less reactive than potassium. This
element is ________.
A) Na
B) Rb
C) Ca
D) Be
E) Fr
56) Which one of the following is not true about the alkali metals?
A) They are low density solids at room temperature.
B) They all readily form ions with a +1 charge.
C) They all have 2 electrons in their valence shells.
D) They are very reactive elements.
E) They have the lowest first ionization energies of the elements.
57) Consider the following properties of an element:
(i) It is solid at room temperature.
(ii) It easily forms an oxide when exposed to air.
(iii) When it reacts with water, hydrogen gas evolves.
(iv) It must be stored submerged in oil.
Which element fits the above description the best?
A) sulfur
B) copper
C) mercury
D) sodium
E) magnesium
58) Which of the following generalizations cannot be made with regard to reactions of alkali metals? (The
symbol M represents any one of the alkali metals.)
A) M (s) + O2 (g) → MO2 (s)
B) 2M (s) + 2H2O (l) → 2MOH (aq) + H2 (g)
C) 2M (s) + H2 (g) → 2MH (s)
D) 2M (s) + Cl2 (g) → 2MCl (s)
E) 2M (s) + S (s) → M2S (s)
59) The reaction of alkali metals with oxygen produce ________.
A) oxides
B) peroxides
C) superoxides
D) all of the above
E) none of the above
60) Alkali metals tend to be more reactive than alkaline earth metals because ________.
A) alkali metals have lower densities
B) alkali metals have lower melting points
C) alkali metals have greater electron affinities
D) alkali metals have lower ionization energies
E) Alkali metals are not more reactive than alkaline earth metals.
61) The alkali metal that is naturally radioactive is ________.
A) rubidium
B) cesium
C) lithium
D) francium
E) sodium
62) Which one of the following beverages originally contained lithium salts?
A) Coca-Cola®
B) Pepsi-Cola®
C) Gatorade®
D) Kool-Aid®
E) Seven-Up®
63) The alkali metal that is used to treat manic-depressive illness is ________.
A) Na
B) K
C) Li
D) Rb
E) Cs
64) Which alkaline earth metal will not react with liquid water or with steam?
A) Be
B) Mg
C) Ca
D) Ba
E) They all react with liquid water and with steam.
65) Which element is solid at room temperature?
A) Cl2
B) F2
C) Br2
D) I2
E) H2
66) ________ is a unique element and does not truly belong to any family.
A) Nitrogen
B) Radium
C) Hydrogen
D) Uranium
E) Helium
67) Which of the following statements is not true for oxygen?
A) The most stable allotrope of oxygen is O2.
B) The chemical formula of ozone is O3.
C) Dry air is about 79% oxygen.
D) Oxygen forms peroxide and superoxide anions.
E) Oxygen is a colorless gas at room temperature.
68) Which one of the following elements has an allotrope that is produced in the upper atmosphere by
lightning?
A) N
B) O
C) S
D) Cl
E) He
69) In nature, sulfur is most commonly found in ________.
A) pure elemental sulfur
B) sulfur oxides
C) metal sulfides
D) sulfuric acid
E) H2S
70) All of the halogens ________.
A) exist under ambient conditions as diatomic gases
B) tend to form positive ions of several different charges
C) tend to form negative ions of several different charges
D) exhibit metallic character
E) form salts with alkali metals with the formula MX
71) The noble gases were, until relatively recently, thought to be entirely unreactive. Experiments in the
early 1960s showed that Xe could, in fact, form compounds with fluorine. The formation of compounds
consisting of Xe is made possible by ________.
A) the availability of xenon atoms
B) xenon’s noble gas electron configuration
C) the stability of xenon atoms
D) xenon’s relatively low ionization energy
E) xenon’s relatively low electron affinity
72) Of the following elements, which have been shown to form compounds?
helium neon argon krypton xenon
A) xenon and argon
B) xenon only
C) xenon, krypton, and argon
D) xenon and krypton
E) None of the above can form compounds.
73) In nature, the noble gases exist as ________.
A) monatomic gaseous atoms
B) the gaseous fluorides
C) solids in rocks and in minerals
D) alkali metal salts
E) the sulfides
74) Hydrogen is unique among the elements because ________.
1. It is not really a member of any particular group.
2. Its electron is not at all shielded from its nucleus.
3. It is the lightest element.
4. It is the only element to exist at room temperature as a diatomic gas.
5. It exhibits some chemical properties similar to those of groups 1A and 7A.
A) 1, 2, 3, 5
B) 1, 2, 3, 4, 5
C) 1, 4, 5
D) 3, 4
E) 2, 3, 4, 5