Deck 6: Ionic Compounds: Periodic Trends and Bonding

Question 1

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

Answer 1

[Ar] 3d⁹

Question 2

Which of the following three sets consist of atoms or ions with the same electron configuration in the ground state? (I)O^2-,Ne,and Mg²⁺
(II)Ni,Cu⁺,and Zn²⁺
(III)Hg,Tl⁺,and Pb²⁺

A)all three sets
B)(II)and (III)
C)(I)and (III)
D)(I)

Answer 2

(I)and (III)

Question 3

Arrange the ions N^3-,O^2-,Mg²⁺,Na⁺,and F^- in order of increasing ionic radius,starting with the smallest first.

A)Mg²⁺,Na⁺,F^-,O^2-,N^3-
B)N^3-,Mg²⁺,O^2-,Na⁺,F^-
C)N^3-,O^2-,Mg²⁺,F^-,Na⁺
D)N^3-,O^2-,F^-,Na⁺,Mg²⁺

Answer 3

Mg²⁺,Na⁺,F^-,O^2-,N^3-

Question 4

Consider the following ground state electron configuration: 1s²2s²2p⁴.Which of the ions has this ground state electron configuration?

A)F^-1
B)N⁺¹
C)C^-2
D)O^-2

Question 5

Of the following,which element has the highest first ionization energy?

A)P
B)C
C)Si
D)N

Question 6

Of the following,which element has the highest first ionization energy?

A)P
B)N
C)Sb
D)As

Question 7

Which ion has the smallest ionic radius?

A)Li⁺
B)Na⁺
C)K⁺
D)Rb⁺

Question 8

What is the ground-state electron configuration of Se^2-?

A)[Ar]3d¹⁰4s²4p²
B)[Ar]3d¹⁰4s²4p⁴
C)[Ar]3d¹²4s²4p⁴
D)[Ar]3d¹⁰4s²4p⁶

Question 9

Of the following,which element has the highest first ionization energy?

A)Cl
B)F
C)O
D)S

Question 10

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

Question 11

Of the following,which element has the highest first ionization energy?

A)Li
B)F
C)Cs
D)At

Question 12

What is the ground-state electron configuration of the ion Hg²⁺?

A)[Xe]4f¹⁴5d¹⁰
B)[Xe]4f¹⁴5d⁸6s²
C)[Xe]4f¹⁴5d¹⁰6s²
D)[Xe]4f¹⁴5d¹⁰6s²6p²

Question 13

Of the following,which element has the highest first ionization energy?

A)argon
B)neon
C)helium
D)krypton

Question 14

Of the following,which element has the highest first ionization energy?

A)iodine
B)bromine
C)fluorine
D)chlorine

Question 15

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

Question 16

Which ion has the largest radius? Ca⁺²,Ca⁺¹,Br^-,K⁺

A)Ca⁺²
B)Ca⁺¹
C)Br^-
D)K⁺

Question 17

Which ion has the smallest ionic radius?

A)F^-
B)Cl^-
C)Br^-
D)I^-

Question 18

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⁺

Question 19

Consider Li⁺,F^-,and O^2-.Which ratio should be the largest?

A)(radius Li⁺)/(radius F^-)
B)(radius Li⁺)/(radius O^2-)
C)(radius F^-)/(radius Li⁺)
D)(radius O^2-)/(radius Li⁺)

Question 20

Which ion has the same electron configuration as Kr?

A)Rb⁺
B)Br^-
C)Se^2-
D)All of these

Question 21

Calculate the energy change for the formation of LiCl(s)from its elements in their standard states and the following tabulated information: Li(s)+ 1/2 Cl₂(g)→ LiCl(s)?
Li⁺(g)+ Cl^-(g)→ LiCl(s)-853 kJ/mol
Li(s)→ Li(g)+159.4 kJ/mol
1/2 Cl₂(g)→ Cl(g)+121.7 kJ/mol
Cl(g)+ e^- → Cl^-(g)-348.6 kJ/mol
Li(g)→ Li⁺(g)+ e^- +520.2 kJ/mol

A)+1305.7 kJ/mol
B)+296.9 kJ/mol
C)-400.3 kJ/mol
D)-627.2 kJ/mol

Question 22

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.

Question 23

Calculate the lattice energy for NaCl(s)using a Born-Haber cycle and the following information: NaCl(s)→ Na⁺(g)+ Cl^-(g)?
Na(s)+ 1/2 Cl₂(g)→ NaCl(s)-411.0 kJ/mol
Na(s)→ Na(g)+107.3 kJ/mol
Na(g)→ Na⁺(g)+ e^- +495.8 kJ/mol
1/2 Cl₂(g)→ Cl(g)+121.7 kJ/mol
Cl(g)+ e^- → Cl^-(g)-348.6 kJ/mol

A)+34.8 kJ/mol
B)+690.3 kJ/mol
C)+787.2 kJ/mol
D)+1512 kJ/mol

Question 24

Calculate the lattice energy for MgCl₂(s)using a Born-Haber cycle and the following information: MgCl₂(s)→ Mg²⁺(g)+ 2 Cl^-(g)?
Mg(s)+ Cl₂(g)→ MgCl₂(s)-641.6 kJ/mol
Mg(s)→ Mg(g)+147.1 kJ/mol
Mg(g)→ Mg⁺(g)+ e^- +737.8 kJ/mol
Mg⁺(g)→ Mg²⁺(g)+ e^- +1451.0 kJ/mol
1/2 Cl₂(g)→ Cl(g)+121.7 kJ/mol
Cl(g)+ e^- → Cl^-(g)-348.6 kJ/mol

A)+641.6 kJ/mol
B)+1240.5 kJ/mol
C)+1882.1 kJ/mol
D)+2523.7 kJ/mol

Question 25

An element Y,has the following ionization energies E_i1 = 578 kJ/mol
E_i2 = 1,817 kJ/mol
E_i3 = 2,745 kJ/mol
E_i4 = 11,575 kJ/mol
What is the most likely identity for this element?

A)Na
B)Mg
C)Al
D)Si

Question 26

Which ionization process requires the most energy?

A)Al(g)→ Al⁺(g)+ e^-
B)Al⁺(g)→ Al²⁺(g)+ e^-
C)Al²⁺(g)→ Al³⁺(g)+ e^-
D)Al³⁺(g)→ Al⁴⁺(g)+ e^-

Question 27

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^-

Question 28

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.

Question 29

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

Question 30

Which period 2 element has successive first through seventh ionization energies (kJ/mol)of E_i1 = 1,402;E_i2 = 2,856;E_i3 = 4,578;E_i4 = 7,475;E_i5 = 9,445;E_i6 = 53,267;and E_i7 = 64,360?

A)B
B)C
C)N
D)O

Question 31

Which element has the most favorable (most negative)electron affinity?

A)K
B)Be
C)I
D)Ne

Question 32

Which of these elements has the most favorable (most negative)electron affinity?

A)Ca
B)N
C)Ne
D)S

Question 33

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

Question 34

Which period 3 element has successive first through seventh ionization energies (kJ/mol)of E_i1 = 578;E_i2 = 1,817;E_i3 = 2,745;E_i4 = 11,575;E_i5 = 14,830;E_i6 = 18,376;and E_i7 = 23,293?

A)Mg
B)Al
C)S
D)Cl

Question 35

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)

Question 36

Which of the following represents the change in electronic configuration that is associated with the second ionization energy of magnesium?

A)[Ne]3s² → [Ne]3s¹ + e^-
B)[Ne]3s² → [Ne] + 2 e^-
C)[Ne]3s¹ → [Ne] + e^-
D)[Ne]3s² + e^- → [Ne]3s²3p¹

Question 37

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

Question 38

Element A has a valence shell configuration of ns²np⁴ while Element B has a valence shell configuration of ns²np⁵ where n = energy level.Which of the following statements is true regarding these elements?

A)The ionization energy of A is lower than the ionization energy of B.
B)The electron affinity of A is higher than the electron affinity of B.
C)Element A and B are transition metals.
D)Element A and B have the same I.E.

Question 39

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)

Question 40

Which element has the most favorable (most negative)electron affinity?

A)B
B)C
C)Li
D)N

Question 41

Calculate the electron affinity for the formation of the hydride ion from the following information: H(g)+ e^- → H^-(g)?
1/2 H₂(g)→ H(g)+217.9 kJ/mol
Na(s)→ Na(g)+107.3 kJ/mol
Na(g)→ Na⁺(g)+ e^- +495.8 kJ/mol
Na(s)+ 1/2 H₂(g)→ NaH(s)-60.0 kJ/mol
NaH(s)→ Na⁺(g)+ H^-(g)+810.9 kJ/mol

A)-50.1 kJ/mol
B)-70.1 kJ/mol
C)-816 kJ/mol
D)-1632 kJ/mol

Question 42

The four spheres below represent Na⁺,Mg²⁺,F⁻,and O^2-,not necessarily in that order.
Which sphere most likely represents the Na⁺ ion?

A)A
B)B
C)C
D)D

Question 43

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)

Question 44

The following four spheres represent an Mg atom,an Mg²⁺ ion,a S atom,and a S^2- ion,not necessarily in that order.Use your knowledge about the relative sizes of atoms,cations,and anions to determine which of the following sets of reactions is most consistent with the sizes of the atoms and ions shown below.

A)A → B + 2e⁻ and C → D + 2e⁻
B)A → B + 2e⁻ and D → C + 2e⁻
C)B → A + 2e⁻ and C → D + 2e⁻
D)B → A + 2e⁻ and D → C + 2e⁻

Question 45

Which ionic compound would be expected to have the highest lattice energy?

A)Li₂O
B)Na₂O₂
C)KO₂
D)RbO₂

Question 46

The following four spheres represent a metal atom,a nonmetal atom,a monatomic anion and a monatomic cation,not necessarily in that order.
Which sphere represents the monatomic anion?

A)A
B)B
C)C
D)D

Question 47

The following four spheres represent a metal atom,a nonmetal atom,a monatomic anion and a monatomic cation,not necessarily in that order.
Which sphere represents the metal atom?

A)A
B)B
C)C
D)D

Question 48

Calculate the lattice energy for MgO(s)using a Born-Haber cycle and the following information: MgO(s)→ Mg²⁺(g)+ O^2-(g)?
Mg(s)→ Mg(g)+147.1 kJ/mol
Mg(g)→ Mg⁺(g)+ e^- +737.8 kJ/mol
Mg⁺(g)→ Mg²⁺(g)+ e^- +1451 kJ/mol
1/2 O₂(g)→ O(g)+249.0 kJ/mol
O(g)+ e^- → O^-(g)-141.1 kJ/mol
O^-(g)+ e^- → O^2-(g)+798.0 kJ/mol
Mg(s)+ 1/2 O₂(g)→ MgO(s)-601.8 kJ/mol

A)+1842 kJ/mol
B)+2444 kJ/mol
C)+3844 kJ/mol
D)+4108 kJ/mol

Question 49

Calculate the energy change in kJ/mol for the reaction 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

Question 50

The four spheres below represent Na⁺,Mg²⁺,F⁻,and O^2-,not necessarily in that order.
Which sphere most likely represents the F^- ion?

A)A
B)B
C)C
D)D

Question 51

The following four spheres represent a metal atom,a nonmetal atom,a monatomic anion and a monatomic cation,not necessarily in that order.
Which sphere represents the nonmetal atom?

A)A
B)B
C)C
D)D

Question 52

The following four spheres represent a Na atom,a Na⁺ ion,a Cl atom,and a Cl^- ion,not necessarily in that order.Use your knowledge about the relative sizes of atoms,cations,and anions to determine which of the following sets of reactions is most consistent with the sizes of the atoms and ions shown below.

A)A → B + e^- and C → D + e^-
B)A → B + e^- and D → C + e^-
C)B → A + e^- and C → D + e^-
D)B → A + e^- and D → C + e^-

Question 53

Which element,indicated by letter on the periodic table above,has a 1+ ion with the electron configuration

A)A
B)B
C)C
D)D

Question 54

Which element,indicated by letter on the periodic table above,has a 3+ ion with the electron configuration

A)A
B)B
C)C
D)D

Question 55

Calculate the energy change for the formation of CaF₂(s)from its elements in their standard states and the following information: Ca(s)+ F₂(g)→ CaF₂(s)?
Ca(s)→ Ca(g)+179.3 kJ/mol
Ca(g)→ Ca⁺(g)+ e^- +589.9 kJ/mol
Ca⁺(g)→ Ca²⁺(g)+ e^- +1145 kJ/mol
1/2 F₂(g)→ F(g)+79.0 kJ/mol
F(g)+ e^- → F^-(g)-328.0 kJ/mol
CaF₂(s)→ Ca²⁺(g)+ 2 F^-(g)+2630 kJ/mol

A)+4046 kJ/mol
B)-965 kJ/mol
C)-1214 kJ/mol
D)-3286 kJ/mol

Question 56

The following four spheres represent a metal atom,a nonmetal atom,a monatomic anion and a monatomic cation,not necessarily in that order.
Which sphere represents the monatomic cation?

A)A
B)B
C)C
D)D

Question 57

Which element,indicated by letter on the periodic table above,has a 2+ ion with the electron configuration [Ar]3d¹⁰?

A)A
B)B
C)C
D)D

Question 58

Which element,indicated by letter on the periodic table above,has a 3+ ion with the electron configuration [Kr]4d⁵?

A)A
B)B
C)C
D)D

Question 59

The four spheres below represent Na⁺,Mg²⁺,F⁻,and O^2-,not necessarily in that order.
Which sphere most likely represents the Mg²⁺ ion?

A)A
B)B
C)C
D)D

Question 60

Calculate the energy change for the formation of MgBr₂(s)from its elements in their standard states: Mg(s)+ Br₂(l)→ MgBr₂(s)?
Mg(s)→ Mg(g)+147.1 kJ/mol
Mg(g)→ Mg⁺(g)+ e^- +737.8 kJ/mol
Mg⁺(g)→ Mg²⁺(g)+ e^- +1451 kJ/mol
Br₂(l)→ Br₂(g)+30.9 kJ/mol
1/2 Br₂(g)→ Br(g)+112.0 kJ/mol
Br(g)+ e^- → Br^-(g)-325.0 kJ/mol
MgBr₂(s)→ Mg²⁺(g)+ 2Br^-(g)+2440 kJ/mol

A)-150.8 kJ/mol
B)-286.0 kJ/mol
C)-499.2 kJ/mol
D)-5682 kJ/mol

Question 61

Which of the above pictures best represents a solid ionic compound?

A)picture (a)
B)picture (b)
C)picture (c)
D)picture (d)

Question 62

The four spheres below represent K⁺,Ca²⁺,Cl^-,and S^2-,not necessarily in that order.
Which sphere most likely represents the K⁺ ion?

A)A
B)B
C)A or B
D)C or D

Question 63

Atoms of which element,indicated by letter on the periodic table above,would be expected to have the highest second ionization energy,E_i1?

A)A
B)B
C)C
D)D

Question 64

The four spheres below represent Na⁺,Mg²⁺,F⁻,and O^2-,not necessarily in that order.
Which sphere most likely represents the O^2- ion?

A)A
B)B
C)C
D)D

Question 65

Atoms of which element,indicated by letter on the periodic table,would be expected to have the most negative value of E_ea?

A)A
B)B
C)C
D)D

Question 66

Atoms of which element,indicated by letter on the periodic table above,would be expected to have the lowest second ionization energy,E_i1?

A)A
B)B
C)C
D)D

Question 67

Which of the above pictures are more likely to represent covalent compounds?

A)pictures (a)and (b)
B)pictures (a)and (d)
C)pictures (b)and (c)
D)pictures (b)and (d)

Question 68

The four spheres below represent K⁺,Ca²⁺,Cl^-,and S^2-,not necessarily in that order.
Which sphere most likely represents the Ca²⁺ ion?

A)A
B)B
C)A or B
D)C or D

Question 69

The four spheres below represent K⁺,Ca²⁺,Cl^-,and S^2-,not necessarily in that order.
Which sphere most likely represents the Cl⁻ ion?

A)A
B)B
C)A or B
D)C or D

Question 70

What is the likely formula for the binary compound formed from the elements represented by letters A and D on the periodic table above?

A)AD
B)A₂D
C)AD₂
D)A₂D₃

Question 71

Which of the above pictures best represents a gaseous covalent compound?

A)picture (a)
B)picture (b)
C)picture (c)
D)picture (d)

Question 72

Atoms of which element,indicated by letter on the periodic table above,would be expected to have the highest first ionization energy,E_i1?

A)A
B)B
C)C
D)D

Question 73

What is the likely formula for the binary compound formed from the elements represented by letters A and C on the periodic table above?

A)AC
B)A₂C
C)AC₂
D)A₂C₃

Question 74

The following pictures represent alkali halide salts.
Which salt has the highest lattice energy?

A)picture (a)
B)picture (b)
C)picture (c)
D)picture (d)

Question 75

The four spheres below represent K⁺,Ca²⁺,Cl^-,and S^2-,not necessarily in that order.
Which sphere most likely represents the S^2- ion?

A)A
B)B
C)A or B
D)C or D

Question 76

The following pictures represent alkali halide salts.
Which salt has the lowest lattice energy?

A)picture (a)
B)picture (b)
C)picture (c)
D)picture (d)

Question 77

Which contains ionic bonds?

A)CH₄
B)CaCl₂
C)Cl₂
D)NCl₃

Question 78

Which element,indicated by letter on the periodic table,is able to form compounds that do not obey the octet rule?

A)A
B)B
C)C
D)D

Question 79

Atoms of which element,indicated by letter on the periodic table above,would be expected to have the lowest first ionization energy,E_i1?

A)A
B)B
C)C
D)D

Question 80

Which of the above pictures are more likely to represent ionic compounds?

A)pictures (a)and (b)
B)pictures (a)and (d)
C)pictures (b)and (c)
D)pictures (b)and (d)