Deck 6: Ionic Bonds and Some Main-Group Chemistry
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Deck 6: Ionic Bonds and Some Main-Group Chemistry
1
How many electrons are in the outermost shell of the In3+ ion in its ground state?
A)2
B)3
C)6
D)18
A)2
B)3
C)6
D)18
18
2
What is the ground-state electron configuration of the ion Hg2+?
A)[Xe]4f145d10
B)[Xe]4f145d86s2
C)[Xe]4f145d106s2
D)[Xe]4f145d106s26p2
A)[Xe]4f145d10
B)[Xe]4f145d86s2
C)[Xe]4f145d106s2
D)[Xe]4f145d106s26p2
[Xe]4f145d10
3
Which ion has the smallest ionic radius?
A)Li+
B)Na+
C)K+
D)Rb+
A)Li+
B)Na+
C)K+
D)Rb+
Li+
4
Which contains both covalent bonds and ionic bonds?
A)HCl
B)NaCl
C)NH3
D)NH4Cl
A)HCl
B)NaCl
C)NH3
D)NH4Cl
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5
Which ion has the same electron configuration as Kr?
A)Rb+
B)Br-
C)Se2-
D)All of these
A)Rb+
B)Br-
C)Se2-
D)All of these
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6
Of the following,which element has the highest first ionization energy?
A)beryllium
B)boron
C)hydrogen
D)lithium
A)beryllium
B)boron
C)hydrogen
D)lithium
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7
Which contains covalent bonds?
A)NaH and HCl
B)only HCl
C)only NaCl
D)only NaH
A)NaH and HCl
B)only HCl
C)only NaCl
D)only NaH
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8
Of the following,which element has the highest first ionization energy?
A)aluminum
B)magnesium
C)silicon
D)sodium
A)aluminum
B)magnesium
C)silicon
D)sodium
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9
Which two ions have the same electron configuration in the ground state?
A)Rb+ and Cs+
B)Ba2+ and I-
C)Se2+ and I-
D)Fe2+ and Fe3+
A)Rb+ and Cs+
B)Ba2+ and I-
C)Se2+ and I-
D)Fe2+ and Fe3+
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10
Which contains ionic bonds?
A)CCl4
B)CaCl2
C)Cl2
D)HCl
A)CCl4
B)CaCl2
C)Cl2
D)HCl
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11
Most of the compounds of the 2+ ions of the first row of the transition metals from Mn to Zn are colored due to absorption of visible light promoting an electron from one 3d orbital to another.Which of these ions should tend to form colorless compounds?
A)Mn2+
B)Co2+
C)Cu2+
D)Zn2+
A)Mn2+
B)Co2+
C)Cu2+
D)Zn2+
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12
What is the ground-state electron configuration of the ion Cu2+?
A)[Ar] 3d9
B)[Ar] 4s1 3d8
C)[Ar] 4s2 3d7
D)[Ar] 4s2 3d10 4p1
A)[Ar] 3d9
B)[Ar] 4s1 3d8
C)[Ar] 4s2 3d7
D)[Ar] 4s2 3d10 4p1
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13
What is the ground-state electron configuration of Se2-?
A)[Ar]3d104s24p2
B)[Ar]3d104s24p4
C)[Ar]3d124s24p4
D)[Ar]3d104s24p6
A)[Ar]3d104s24p2
B)[Ar]3d104s24p4
C)[Ar]3d124s24p4
D)[Ar]3d104s24p6
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14
Arrange the ions N3-,O2-,Mg2+,Na+,and F- in order of increasing ionic radius,starting with the smallest first.
A)Mg2+,Na+,F-,O2-,N3-
B)N3-,Mg2+,O2-,Na+,F-
C)N3-,O2-,Mg2+,F-,Na+
D)N3-,O2-,F-,Na+,Mg2+
A)Mg2+,Na+,F-,O2-,N3-
B)N3-,Mg2+,O2-,Na+,F-
C)N3-,O2-,Mg2+,F-,Na+
D)N3-,O2-,F-,Na+,Mg2+
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15
Which ion does not have a noble gas configuration in its ground state?
A)Sc3+
B)Al3+
C)Ga3+
D)As3-
A)Sc3+
B)Al3+
C)Ga3+
D)As3-
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16
Indicate which is larger in each of the following two sets.
(I)Cr3+ or Cr (II)Se2- or Se
A)Cr3+ is larger than Cr and Se2- is larger than Se.
B)Cr3+ is larger than Cr and Se is larger than Se2-.
C)Cr is larger than Cr3+ and Se2- is larger than Se.
D)Cr is larger than Cr3+ and Se is larger than Se2-.
(I)Cr3+ or Cr (II)Se2- or Se
A)Cr3+ is larger than Cr and Se2- is larger than Se.
B)Cr3+ is larger than Cr and Se is larger than Se2-.
C)Cr is larger than Cr3+ and Se2- is larger than Se.
D)Cr is larger than Cr3+ and Se is larger than Se2-.
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17
Which of the following three sets consist of atoms or ions with the same electron configuration in the ground state?
(I)O2-,Ne,and Mg2+
(II)Ni,Cu+,and Zn2+
(III)Hg,Tl+,and Pb2+
A)all three sets
B)all but (I)
C)all but (II)
D)only (I)
(I)O2-,Ne,and Mg2+
(II)Ni,Cu+,and Zn2+
(III)Hg,Tl+,and Pb2+
A)all three sets
B)all but (I)
C)all but (II)
D)only (I)
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18
Which ion has the smallest ionic radius?
A)F-
B)Cl-
C)Br-
D)I-
A)F-
B)Cl-
C)Br-
D)I-
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19
Consider Li+,F-,and O2-.Which ratio should be the largest?
A)(radius Li+)/(radius F-)
B)(radius Li+)/(radius O2-)
C)(radius F-)/(radius Li+)
D)(radius O2-)/(radius Li+)
A)(radius Li+)/(radius F-)
B)(radius Li+)/(radius O2-)
C)(radius F-)/(radius Li+)
D)(radius O2-)/(radius Li+)
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20
Which of the following most likely represent the atomic radius of a Cr atom,the ionic radius of a Cr2+ ion,and the ionic radius of a Cr3+ ion?
A)128 pm for Cr,167 pm for Cr2+,and 193 pm for Cr3+
B)128 pm for Cr,147 pm for Cr2+,and 193 pm for Cr3+
C)128 pm for Cr,109 pm for Cr2+,and 63 pm for Cr3+
D)128 pm for Cr,89 pm for Cr2+,and 63 pm for Cr3+
A)128 pm for Cr,167 pm for Cr2+,and 193 pm for Cr3+
B)128 pm for Cr,147 pm for Cr2+,and 193 pm for Cr3+
C)128 pm for Cr,109 pm for Cr2+,and 63 pm for Cr3+
D)128 pm for Cr,89 pm for Cr2+,and 63 pm for Cr3+
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21
Which element has the least favorable (least negative)electron affinity?
A)B
B)C
C)N
D)O
A)B
B)C
C)N
D)O
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22
Which period 3 element has successive first through seventh ionization energies (kJ/mol)of
Ei1 = 578;Ei2 = 1,817;Ei3 = 2,745;Ei4 = 11,575;Ei5 = 14,830;Ei6 = 18,376;and Ei7 = 23,293?
A)Mg
B)Al
C)S
D)Cl
Ei1 = 578;Ei2 = 1,817;Ei3 = 2,745;Ei4 = 11,575;Ei5 = 14,830;Ei6 = 18,376;and Ei7 = 23,293?
A)Mg
B)Al
C)S
D)Cl
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23
Which ionization process requires the most energy?
A)S(g)→ S+(g)+ e-
B)S+(g)→ S2+(g)+ e-
C)Cl(g)→ Cl+(g)+ e-
D)Cl+(g)→ Cl2+(g)+ e-
A)S(g)→ S+(g)+ e-
B)S+(g)→ S2+(g)+ e-
C)Cl(g)→ Cl+(g)+ e-
D)Cl+(g)→ Cl2+(g)+ e-
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24
Which liberates the most energy?
A)Li(g)+ e- → Li-(g)
B)Na(g)+ e- → Na-(g)
C)K(g)+ e- → K-(g)
D)Rb(g)+ e- → Rb-(g)
A)Li(g)+ e- → Li-(g)
B)Na(g)+ e- → Na-(g)
C)K(g)+ e- → K-(g)
D)Rb(g)+ e- → Rb-(g)
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25
Which of the following represents the change in electronic configuration that is associated with the first ionization energy of magnesium?
A)[Ne]3s13p1 → [Ne]3s1 + e-
B)[Ne]3s2 → [Ne]3s13p1
C)[Ne]3s2 → [Ne]3s1 + e-
D)[Ne]3s2 + e- → [Ne]3s23p1
A)[Ne]3s13p1 → [Ne]3s1 + e-
B)[Ne]3s2 → [Ne]3s13p1
C)[Ne]3s2 → [Ne]3s1 + e-
D)[Ne]3s2 + e- → [Ne]3s23p1
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26
Which element has the most favorable (most negative)electron affinity?
A)B
B)C
C)Li
D)N
A)B
B)C
C)Li
D)N
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27
Of the following,which element has the highest first ionization energy?
A)Al
B)Cl
C)Na
D)P
A)Al
B)Cl
C)Na
D)P
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28
List the elements Cs,Ca,Ne,Na,Ar in order of decreasing first ionization energy.
A)Ar > Ca > Cs > Na > Ne
B)Ne > Ar > Ca > Na > Cs
C)Ne > Ar > Na > Cs > Ca
D)Ne > Na > Cs > Ca > Ar
A)Ar > Ca > Cs > Na > Ne
B)Ne > Ar > Ca > Na > Cs
C)Ne > Ar > Na > Cs > Ca
D)Ne > Na > Cs > Ca > Ar
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29
Of the following,which element has the highest first ionization energy?
A)Cl
B)F
C)O
D)S
A)Cl
B)F
C)O
D)S
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30
Which period 2 element has successive first through seventh ionization energies (kJ/mol)of
Ei1 = 1,402;Ei2 =2,856;Ei3 =4,578;Ei4 =7,475;Ei5 =9,445;Ei6 =53,267;and Ei7 = 64,360?
A)B
B)C
C)N
D)O
Ei1 = 1,402;Ei2 =2,856;Ei3 =4,578;Ei4 =7,475;Ei5 =9,445;Ei6 =53,267;and Ei7 = 64,360?
A)B
B)C
C)N
D)O
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31
Which element has the most favorable (most negative)electron affinity?
A)Na
B)Mg
C)O
D)Ne
A)Na
B)Mg
C)O
D)Ne
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32
Of the following,which element has the highest first ionization energy?
A)Ca
B)K
C)Li
D)Mg
A)Ca
B)K
C)Li
D)Mg
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33
Which of the following atoms with the specified electronic configurations would have the lowest first ionization energy?
A)[He]2s22p3
B)[Ne]3s23p4
C)[Xe]6s1
D)[Xe]6s24f145d106p1
A)[He]2s22p3
B)[Ne]3s23p4
C)[Xe]6s1
D)[Xe]6s24f145d106p1
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34
Which electron affinity process would liberate the most energy?
A)[He] 2s2 + e- → [He] 2s2 2p1
B)[He] 2s2 2p2 + e- → [He] 2s2 2p3
C)[He] 2s2 2p3 + e- → [He] 2s2 2p4
D)[He] 2s2 2p6 + e- → [He] 2s2 2p6 3s1
A)[He] 2s2 + e- → [He] 2s2 2p1
B)[He] 2s2 2p2 + e- → [He] 2s2 2p3
C)[He] 2s2 2p3 + e- → [He] 2s2 2p4
D)[He] 2s2 2p6 + e- → [He] 2s2 2p6 3s1
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35
Which liberates the most energy?
A)Br(g)+ e⁻ → Br⁻(g)
B)Cl(g)+ e⁻ → Cl⁻(g)
C)F(g)+ e⁻ → F⁻(g)
D)I(g)→ I⁻(g)
A)Br(g)+ e⁻ → Br⁻(g)
B)Cl(g)+ e⁻ → Cl⁻(g)
C)F(g)+ e⁻ → F⁻(g)
D)I(g)→ I⁻(g)
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36
Of the following,which element has the highest first ionization energy?
A)Ca
B)Cl
C)Na
D)Se
A)Ca
B)Cl
C)Na
D)Se
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37
List the elements Na,Ca,Rb,Cl,He in order of decreasing first ionization energy.
A)He > Cl > Ca > Na > Rb
B)He > Na > Ca > Cl > Rb
C)He > Na > Cl > Ca > Rb
D)Rb > Ca > Cl > Na > He
A)He > Cl > Ca > Na > Rb
B)He > Na > Ca > Cl > Rb
C)He > Na > Cl > Ca > Rb
D)Rb > Ca > Cl > Na > He
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38
Which of the following species will have the highest ionization energy?
A)Na+
B)Ne
C)F-
D)O2-
A)Na+
B)Ne
C)F-
D)O2-
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39
Consider the following electron configurations for neutral atoms:
Atom I = 1s22s22p63s2
Atom II = 1s22s22p63s23p4
Atom III = 1s22s22p63s23p6
Which atom would be expected to have the largest third ionization energy?
A)atom I
B)atom II
C)atom III
D)All of these atoms would be expected to have the same third ionization energy.
Atom I = 1s22s22p63s2
Atom II = 1s22s22p63s23p4
Atom III = 1s22s22p63s23p6
Which atom would be expected to have the largest third ionization energy?
A)atom I
B)atom II
C)atom III
D)All of these atoms would be expected to have the same third ionization energy.
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40
Which ionization process requires the most energy?
A)P(g)→ P+(g)+ e-
B)P+(g)→ P2+(g)+ e-
C)P2+(g)→ P3+(g)+ e-
D)P3+(g)→ P4+(g)+ e-
A)P(g)→ P+(g)+ e-
B)P+(g)→ P2+(g)+ e-
C)P2+(g)→ P3+(g)+ e-
D)P3+(g)→ P4+(g)+ e-
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41
An element M reacts with chlorine to form MCl2,with oxygen to form MO,and with nitrogen to form M3N2.The most likely candidate for the element is
A)Li
B)Mg
C)Al
D)Si
A)Li
B)Mg
C)Al
D)Si
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42
Calculate the lattice energy for NaCl(s)using a Born-Haber cycle and the following information: 
A)+34.8 kJ/mol
B)+690.3 kJ/mol
C)+787.2 kJ/mol
D)+1512 kJ/mol

A)+34.8 kJ/mol
B)+690.3 kJ/mol
C)+787.2 kJ/mol
D)+1512 kJ/mol
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43
To reach a noble gas electron configuration how many electrons would sulfur have to adopt?
A)1
B)2
C)6
D)8
A)1
B)2
C)6
D)8
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44
Calculate the energy change for the formation of MgBr2(s)from its elements in their standard states: 
A)-150.8 kJ/mol
B)-286.0 kJ/mol
C)-499.2 kJ/mol
D)-5682 kJ/mol

A)-150.8 kJ/mol
B)-286.0 kJ/mol
C)-499.2 kJ/mol
D)-5682 kJ/mol
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45
Calculate the energy change for the formation of LiCl(s)from its elements in their standard states and the following tabulated information: 
A)+1305.7 kJ/mol
B)+296.9 kJ/mol
C)-400.3 kJ/mol
D)-627.2 kJ/mol

A)+1305.7 kJ/mol
B)+296.9 kJ/mol
C)-400.3 kJ/mol
D)-627.2 kJ/mol
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46
Calculate the energy change for the formation of CaF2(s)from its elements in their standard states and the following information: 
A)+4046 kJ/mol
B)-965 kJ/mol
C)-1214 kJ/mol
D)-3286 kJ/mol

A)+4046 kJ/mol
B)-965 kJ/mol
C)-1214 kJ/mol
D)-3286 kJ/mol
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47
Which of these elements has the most favorable (most negative)electron affinity?
A)Ca
B)N
C)Ne
D)S
A)Ca
B)N
C)Ne
D)S
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48
What is the general trend in ionization energy and electron affinity values?
A)Both decrease as one traverses a period from left to right and both decrease as one descends a group.
B)Both decrease as one traverses a period from left to right and both increase as one descends a group.
C)Both increase as one traverses a period from left to right and both decrease as one descends a group.
D)Both increase as one traverses a period from left to right and both increase as one descends a group.
A)Both decrease as one traverses a period from left to right and both decrease as one descends a group.
B)Both decrease as one traverses a period from left to right and both increase as one descends a group.
C)Both increase as one traverses a period from left to right and both decrease as one descends a group.
D)Both increase as one traverses a period from left to right and both increase as one descends a group.
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49
Calculate the energy change in kJ/mol for the reaction Li+(g)+ F-(g)→ Li(g)+ F(g)using the following information:
Li(g)→ Li+(g)+ e- +520 kJ/mol
F(g)+ e- → F-(g)-328 kJ/mol
A)-848 kJ/mol
B)-192 kJ/mol
C)+192 kJ/mol
D)+848 kJ/mol
Li(g)→ Li+(g)+ e- +520 kJ/mol
F(g)+ e- → F-(g)-328 kJ/mol
A)-848 kJ/mol
B)-192 kJ/mol
C)+192 kJ/mol
D)+848 kJ/mol
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50
An element that has the valence electron configuration 3s23p3 belongs to which period and group?
A)period 3;group 3A
B)period 3;group 5A
C)period 4;group 3A
D)period 4;group 5A
A)period 3;group 3A
B)period 3;group 5A
C)period 4;group 3A
D)period 4;group 5A
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51
How many electrons does magnesium lose and nitrogen need to form Mg3N2?
A)magnesium loses 2 and nitrogen gains 2
B)magnesium loses 2 and nitrogen gains 3
C)magnesium loses 3 and nitrogen gains 2
D)magnesium loses 3 and nitrogen gains 3
A)magnesium loses 2 and nitrogen gains 2
B)magnesium loses 2 and nitrogen gains 3
C)magnesium loses 3 and nitrogen gains 2
D)magnesium loses 3 and nitrogen gains 3
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52
Calculate the electron affinity for the formation of the hydride ion from the following information: 
A)-50.1 kJ/mol
B)-70.1 kJ/mol
C)-816 kJ/mol
D)-1632 kJ/mol

A)-50.1 kJ/mol
B)-70.1 kJ/mol
C)-816 kJ/mol
D)-1632 kJ/mol
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53
The octet rule is most likely to fail occasionally for which of the following elements?
A)C
B)N
C)Na
D)S
A)C
B)N
C)Na
D)S
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54
Which species does not have an octet of electrons for its outer core?
A)C4-
B)P3-
C)O2-
D)Mg+
A)C4-
B)P3-
C)O2-
D)Mg+
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55
Which of the following ionic compounds would be expected to have the highest lattice energy?
A)NaF
B)NaCl
C)NaBr
D)NaI
A)NaF
B)NaCl
C)NaBr
D)NaI
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56
Which chemical process is associated with the lattice energy for sodium chloride?
A)NaCl(s)→ Na+(g)+ Cl-(g)
B)NaCl(g)→ Na+(g)+ Cl-(g)
C)Na(s)+ 1/2 Cl2(g)→ NaCl(s)
D)NaCl(s)+ H2O(l)→ Na+(aq)+ Cl-(aq)
A)NaCl(s)→ Na+(g)+ Cl-(g)
B)NaCl(g)→ Na+(g)+ Cl-(g)
C)Na(s)+ 1/2 Cl2(g)→ NaCl(s)
D)NaCl(s)+ H2O(l)→ Na+(aq)+ Cl-(aq)
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57
In the reaction of sodium metal with chlorine gas which of the following processes releases energy?
A)Cl2(g)→ 2 Cl(g)
B)Cl(g)+ e- → Cl-(g)
C)Na(s)→ Na(g)
D)Na(g)→ Na+(g)+ e-
A)Cl2(g)→ 2 Cl(g)
B)Cl(g)+ e- → Cl-(g)
C)Na(s)→ Na(g)
D)Na(g)→ Na+(g)+ e-
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58
How many valence shell electrons does an atom of aluminum have?
A)1
B)2
C)3
D)13
A)1
B)2
C)3
D)13
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59
Calculate the lattice energy for MgO(s)using a Born-Haber cycle and the following information: 
A)+1842 kJ/mol
B)+2444 kJ/mol
C)+3844 kJ/mol
D)+4108 kJ/mol

A)+1842 kJ/mol
B)+2444 kJ/mol
C)+3844 kJ/mol
D)+4108 kJ/mol
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60
Calculate the lattice energy for MgCl2(s)using a Born-Haber cycle and the following information: 
A)+641.6 kJ/mol
B)+1240.5 kJ/mol
C)+1882.1 kJ/mol
D)+2523.7 kJ/mol

A)+641.6 kJ/mol
B)+1240.5 kJ/mol
C)+1882.1 kJ/mol
D)+2523.7 kJ/mol
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61
Which alkaline earth metal reacts the most vigorously with water at room temperature?
A)Be
B)Ca
C)Ba
D)Sr
A)Be
B)Ca
C)Ba
D)Sr
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62
Which is not a chemical reaction of the alkali metal potassium?
A)K(s)+ O2(g)→ KO2(s)
B)2 K(s)+ 2 H2O(l)→ 2 KOH(aq)+ H2(g)
C)2 K(s)+ H2(g)→ 2 KH(s)
D)6 K(s)+ N2(g)→ 2 K3N(s)
A)K(s)+ O2(g)→ KO2(s)
B)2 K(s)+ 2 H2O(l)→ 2 KOH(aq)+ H2(g)
C)2 K(s)+ H2(g)→ 2 KH(s)
D)6 K(s)+ N2(g)→ 2 K3N(s)
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63
Which is not generally considered to be a chemical reaction of the alkaline earth metal calcium?
A)Ca(s)+ Cl2(g)→ CaCl2(s)
B)2 Ca(s)+ 2 H2O(l)→ 2 Ca(OH)2(aq)+ H2(g)
C)6 Ca(s)+ 2 N2(g)→ 2 Ca3N2(s)
D)Ca(s)+ O2(g)→ CaO2(s)
A)Ca(s)+ Cl2(g)→ CaCl2(s)
B)2 Ca(s)+ 2 H2O(l)→ 2 Ca(OH)2(aq)+ H2(g)
C)6 Ca(s)+ 2 N2(g)→ 2 Ca3N2(s)
D)Ca(s)+ O2(g)→ CaO2(s)
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64
The alkali metals K,Rb,and Cs are commercially produced by
A)chemical reduction of their molten salts.
B)electrolysis of their molten salts.
C)thermal decomposition of their molten metal halides.
D)thermal decomposition of their molten metal oxides.
A)chemical reduction of their molten salts.
B)electrolysis of their molten salts.
C)thermal decomposition of their molten metal halides.
D)thermal decomposition of their molten metal oxides.
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65
Which alkali metal reacts with nitrogen to form a nitride?
A)Li
B)Na
C)K
D)All of these
A)Li
B)Na
C)K
D)All of these
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66
Which alkali metal forms preferentially an oxide rather than a peroxide or superoxide?
A)Li
B)Na
C)K
D)Rb
A)Li
B)Na
C)K
D)Rb
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67
Predict the product(s)when the reactants Be(s)+ Br2(l)are mixed.
A)BeBr(s)
B)BeBr2(s)
C)Be2Br(s)
D)BeBr3(s)
A)BeBr(s)
B)BeBr2(s)
C)Be2Br(s)
D)BeBr3(s)
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68
Which of the following ionic compounds would be expected to have the highest lattice energy?
A)LiCl
B)NaCl
C)KCl
D)RbCl
A)LiCl
B)NaCl
C)KCl
D)RbCl
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69
Which ionic compound would be expected to have the highest lattice energy?
A)NaCl
B)MgO
C)AlF3
D)Al2O3
A)NaCl
B)MgO
C)AlF3
D)Al2O3
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70
Which of the following elements is a solid at room temperature?
A)fluorine
B)chlorine
C)bromine
D)iodine
A)fluorine
B)chlorine
C)bromine
D)iodine
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71
Which ionic compound would be expected to have the highest lattice energy?
A)Li2O
B)Na2O2
C)KO2
D)RbO2
A)Li2O
B)Na2O2
C)KO2
D)RbO2
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72
Which ionic compound would be expected to have the highest lattice energy?
A)Na2O
B)MgO
C)Al2O3
D)CO2
A)Na2O
B)MgO
C)Al2O3
D)CO2
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73
Which alkali metal forms preferentially a peroxide and superoxide?
A)Li
B)Na
C)K
D)Mg
A)Li
B)Na
C)K
D)Mg
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74
Group 2A metals tend to be somewhat less reactive than alkali metals,and the order of their reactivity is
A)Ba > Sr > Ca > Mg > Be.
B)Be > Mg > Ca > Sr > Ba.
C)Ca > Mg > Be > Ba > Sr.
D)Sr > Ca > Mg > Be > Ba.
A)Ba > Sr > Ca > Mg > Be.
B)Be > Mg > Ca > Sr > Ba.
C)Ca > Mg > Be > Ba > Sr.
D)Sr > Ca > Mg > Be > Ba.
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75
The alkali metals Li and Na are commercially produced by
A)chemical reduction of their molten salts.
B)electrolysis of their molten salts.
C)thermal decomposition of their molten metal halides.
D)thermal decomposition of their molten metal oxides.
A)chemical reduction of their molten salts.
B)electrolysis of their molten salts.
C)thermal decomposition of their molten metal halides.
D)thermal decomposition of their molten metal oxides.
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76
An incorrect statement about the alkaline earth metals is:
A)Melting points generally decrease as one descends the group.
B)Densities are less than those of the corresponding alkali elements of the same period.
C)Ionic radii of the M2+ ion increases as one descends the group.
D)The first ionization energy is less than that of the second ionization energy.
A)Melting points generally decrease as one descends the group.
B)Densities are less than those of the corresponding alkali elements of the same period.
C)Ionic radii of the M2+ ion increases as one descends the group.
D)The first ionization energy is less than that of the second ionization energy.
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77
Which of the following elements is a liquid at room temperature?
A)fluorine
B)chlorine
C)bromine
D)iodine
A)fluorine
B)chlorine
C)bromine
D)iodine
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78
Which is not a chemical reaction of the alkali metal sodium?
A)4 Na(s)+ 2 O2(g)→ 2 Na2O(s)+ Na2O2(s)
B)2 Na(s)+ 2 NH3(l)→ 2 NaNH2(sol)+ H2(g)
C)2 Na(s)+ Cl2(g)→ 2 NaCl(s)
D)2 Na(s)+ 2 H2O(l)→ 2 NaOH(aq)+ H2(g)
A)4 Na(s)+ 2 O2(g)→ 2 Na2O(s)+ Na2O2(s)
B)2 Na(s)+ 2 NH3(l)→ 2 NaNH2(sol)+ H2(g)
C)2 Na(s)+ Cl2(g)→ 2 NaCl(s)
D)2 Na(s)+ 2 H2O(l)→ 2 NaOH(aq)+ H2(g)
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79
Calcium,strontium,and barium are all prepared commercially by the same method which is
A)electrolysis of the molten metal oxides.
B)electrolysis of the molten metal halides.
C)chemical reduction of the metal oxides with aluminium.
D)chemical reduction of the metal halides with oxygen.
A)electrolysis of the molten metal oxides.
B)electrolysis of the molten metal halides.
C)chemical reduction of the metal oxides with aluminium.
D)chemical reduction of the metal halides with oxygen.
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80
Which is not generally considered to be a chemical reaction of the alkaline earth metal magnesium?
A)2 Mg(g)+ O2(g)→ 2 MgO(s)at room temperature
B)3 Mg(s)+ N2(g)→ Mg3N2(s)at elevated temperatures
C)Mg(s)+ 2 H2O(l)→ Mg(OH)2(s)+ H2(g)at room temperature
D)Mg(s)+ F2(g)→ MgF2(s)at room temperature
A)2 Mg(g)+ O2(g)→ 2 MgO(s)at room temperature
B)3 Mg(s)+ N2(g)→ Mg3N2(s)at elevated temperatures
C)Mg(s)+ 2 H2O(l)→ Mg(OH)2(s)+ H2(g)at room temperature
D)Mg(s)+ F2(g)→ MgF2(s)at room temperature
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