Deck 9: Ionic and Covalent Bonding

Question 1

Which one of the following has an enthalpy change that is equal to the lattice energy of SrCl₂?

A)SrCl₂(s)? Sr(g)+ 2Cl(g)
B)SrCl₂(s)? Sr(g)+ Cl₂(g)
C)SrCl₂(s)? Sr²⁺(g)+ 2Cl(g)
D)SrCl₂(s)? Sr(s)+ Cl₂(g)
E)SrCl₂(s)? Sr²⁺(g)+ 2Cl^-(g)

Answer 1

SrCl₂(s)? Sr²⁺(g)+ 2Cl^-(g)

Question 2

The following representation of an atom is called
​

A)a Lewis dot structure.
B)an ion.
C)a structural formula.
D)an electrostatic potential map.
E)an ionic bond.

Answer 2

a Lewis dot structure.

Question 3

Which of the following compounds has the most ionic bonding (has the highest percentage of ionic character)?

A)CaF₂
B)LiI
C)OF₂
D)CsF
E)LiF

Answer 3

CsF

Question 4

In the Born-Haber cycle for LiCl(s),which of the following processes corresponds to the first ionization energy of Li?

A)Li^-(g)→ Li(g)+ e^-
B)Li(s)→ Li(g)
C)Li⁺(g)+ Cl^-(g)→ LiCl(s)
D)Li(g)→ Li⁺(g)+ e^-
E)Li⁺(g)+ e^- → Li(g)

Question 5

In which pair do both compounds exhibit predominantly ionic bonding?

A)RbCl and CaO
B)PCl₅ and HF
C)KI and O₃
D)Na₂SO₃ and BH₃
E)NaF and H₂O

Question 6

All of the following have ground-state noble-gas electron configurations except

A)Ar
B)N^3-
C)P³⁺
D)Mg²⁺
E)Cl^-

Question 7

Atoms of an element X have the ground-state electron configuration 1s²2s²2p⁶3s²3p⁴.What type of ion is X most likely to form?

A)X⁶⁺
B)X^3-
C)X⁴⁺
D)X^-
E)X^2-

Question 8

Which of the following compounds would be expected to have the lowest melting point?

A)AlF₃
B)RbF
C)NaF
D)MgF₂
E)CaF₂

Question 9

When the cations Na⁺,K⁺,Rb⁺,Cs⁺ are combined with chloride ion in the gas phase to form ion pairs,which pair formation releases the greatest amount of energy?

A)KCl
B)All release the same amount of energy.
C)RbCl
D)NaCl
E)CsCl

Question 10

Which of the following is the Lewis dot structure for the fluoride ion?

A)​
B)​
C)​
D)​
E)​

Question 11

Which of the following compounds would be expected to have the highest melting point?

A)CsF
B)LiCl
C)LiF
D)NaBr
E)CsI

Question 12

In the Born-Haber cycle for KI(s),which of the following processes corresponds to the electron affinity of I?

A)I(g)→ I⁺(g)+ e^-
B)KI(s)→ K⁺(g)+ I^-(g)
C)I^-(g)→ I(g)+ e^-
D)I₂(g)→ 2I(g)
E)I(g)+ e^- → I^-(g)

Question 13

Which of the following processes is not exothermic?

A)Rb⁺(g)+ e^- → Rb(g)
B)​Rb⁺(g)+ Cl^-(g)→ RbCl(s)
C)​Cl(g)+ e^- → Cl^-(g)
D)​Rb(g)→ Rb(s)
E)​ Cl₂(g)→ Cl(g)

Question 14

Which of the following is a correct description of lattice energy?

A)The energy change that occurs when electrons are removed from a lattice.
B)The energy change that occurs when a gas condenses to a liquid.
C)The energy change that occurs when a liquid freezes.
D)The energy change that occurs when an ionic solid is separated into its ions in the gas phase.
E)The lattice energy of a substance is identical to the ionic bond energy determined from coulombs law.

Question 15

Which of the following compounds would be expected to have the highest melting point?

A)NCl₃
B)OCl₂
C)MgCl₂
D)LiCl
E)CCl₄

Question 16

Which of the following is the Lewis dot structure for the potassium ion?

A)
B)​
C)​
D)​
E)​

Question 17

Which of the following statements concerning lattice energy is false?

A)MgO has a larger lattice energy than NaF.
B)The lattice energy for a solid with 2+ and 2- ions should be two times that for a solid with 1+ and 1- ions.
C)MgO has a larger lattice energy than LiF.
D)Lattice energy is often defined as the change in energy that occurs when an ionic solid is separated into isolated ions in the gas phase.
E)All of these are true.

Question 18

In the Born-Haber cycle for NaCl(s),which of the following processes corresponds to the enthalpy of formation of NaCl(s)?

A)Na(s)+ Cl₂(g)→ NaCl(s)
B)Na⁺(aq)+ (aq)→ NaCl(s)
C)NaCl(g)→ NaCl(s)
D)2Na(g)+ Cl₂(g)→ 2NaCl(g)
E)NaCl(aq)→ NaCl(s)

Question 19

Which of the following is the Lewis dot structure for one formula unit of calcium sulfide?

A)
B)​
C)​
D)​
E)​

Question 20

All of the following species have ground-state noble-gas electron configurations except

A)Ge⁴⁺
B)K⁺
C)Kr
D)I^-
E)P^3-

Question 21

What is the ground-state electron configuration of the phosphide ion?

A)
B)
C)
D)
E)

Question 22

The following species, ,
,and
,all have the same number of

A)electrons.
B)nucleons.
C)neutrons.
D)protons.
E)isotopes.

Question 23

What is the electron configuration for ? Mn³⁺

A)
B)
C)
D)
E)

Question 24

Which two species are isoelectronic?

A)Na⁺ and K⁺
B)Al³⁺ and Ne
C)P^- and Ca⁺
D)Cl^- and F^-
E)Ca²⁺ and Mg²⁺

Question 25

What is the electron configuration of Mn²⁺?

A)[Ar]3d⁵
B)[Ar]3d³4s²
C)[Ar]3d⁴4s¹
D)[Ar]3d⁵4s²
E)[Ar]3d⁵4s¹

Question 26

All of the following species are isoelectronic except

A)O^-
B)Ne
C)N^3-
D)Mg²⁺
E)F^-

Question 27

All of the following ions have the ground-state electron configuration of a noble gas except which one?

A)Ca²⁺
B)Cl^-
C)Ga³⁺
D)Al³⁺
E)H^-

Question 28

What is the ground-state electron configuration of Fe³⁺?

A)[Ar]3d⁶4s²
B)[Ar]3d³4s²
C)[Ar]3d⁴4s¹
D)[Ar]3d⁵
E)[Ar]3d⁶

Question 29

Which of the following species is isoelectronic with Ar?

A)Na⁺
B)​Ca²⁺
C)​Ga³⁺
D)​O^2-
E)​Ne

Question 30

The Cr²⁺ ion would be expected to have ____ unpaired electrons.

A)4
B)2
C)3
D)0
E)1

Question 31

The formation of which monatomic ion of oxygen is the most energetically favorable?

A)O⁴⁺
B)O^2-
C)O^-
D)O⁶⁺
E)O²⁺

Question 32

All of the following species are isoelectronic except

A)S^2-
B)K⁺
C)Na⁺
D)Ar
E)Cl^-

Question 33

Which pair of species is isoelectronic?

A)Na⁺ and K⁺
B)K⁺ and Cl^-
C)Be²⁺ and Na⁺
D)Ne and Ar
E)Li⁺ and Ne

Question 34

Which set of ions are isoelectronic in their ground-state electron configurations?

A)N,O,F,Ne
B)Na⁺,K⁺,Rb⁺,Cs⁺
C)F^-,Cl^-,Br^-,I^-
D)Mg²⁺,Ca²⁺,Sr²⁺,Ba²⁺
E)N^3-,O^2-,Mg²⁺,Al³⁺

Question 35

What is the ground-state electron configuration of the zinc ion,Zn²⁺?

A)1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p²
B)1s²2s²2p⁶3s²3p⁶3d¹⁰4s²
C)1s²2s²2p⁶3s²3p⁶3d⁸4s²
D)1s²2s²2p⁶3s²3p⁶3d¹⁰
E)1s²2s²2p⁶3s²3p⁶4s²

Question 36

What is the ground-state electron configuration of Co³⁺?

A)[Ar]3d⁵
B)[Ar]3d⁴4s²
C)[Ar]3d⁶
D)[Ar]3d⁶4s¹
E)[Ar]3d⁵4s²

Question 37

All of the following species are isoelectronic except

A)Ar.
B)Ca²⁺.
C)Mg²⁺.
D)Cl^-.
E)S^2-.

Question 38

What is the ground-state electron configuration of Ni²⁺?

A)[Ar]3d⁶4s²
B)[Ar]3d⁷4s²
C)[Ar]3d⁷4s¹
D)[Ar]3d⁶4s¹
E)[Ar]3d⁸

Question 39

What is the ground-state electron configuration of the Mg²⁺ ion?

A)1s²2s²2p⁶3s²3p²
B)​1s²2s²2p³
C)​1s²2s²2p⁶
D)​1s²2s²2p¹
E)​1s²2s²2p⁶3s²

Question 40

Rank the following ions in order of decreasing atomic radii: Os⁴⁺,Os²⁺,Os⁵⁺.

A)Os²⁺ > Os⁴⁺ > Os⁵⁺
B)Os⁵⁺ > Os⁴⁺ > Os²⁺
C)Os⁴⁺ > Os²⁺ > Os⁵⁺
D)Os⁵⁺ > Os²⁺ > Os⁴⁺
E)Os²⁺ > Os⁵⁺ > Os⁴⁺

Question 41

Which of the following atoms is the most electronegative?

A)B
B)N
C)Al
D)Cs
E)Na

Question 42

Which of the following is the best explanation for a covalent bond?

A)electrons simultaneously attracted by more than one nucleus
B)an interaction between outer electrons
C)the overlapping of unoccupied orbitals of two or more atoms
D)the overlapping of two electron-filled orbitals having different energies
E)a positive ion attracting negative ions

Question 43

In which of the following lists do the ions not appear in order of increasing ionic radius?

A)S^2- < Cl^- < K⁺
B)Na⁺ < F^- < O^2-
C)Cl^- < Br^- < I^-
D)Li⁺ < Na⁺ < K⁺
E)Al³⁺ < Mg²⁺ < Na⁺

Question 44

Rank the following ions in order of decreasing ionic radius: S^2-,O^2-,F^-,Na⁺,Mg²⁺.

A)S^2-,O^2-,F^-,Na⁺,Mg²⁺
B)O^2-,F^-,Na⁺,Mg²⁺,S^2-
C)O^2-,S^2-,F^-,Na⁺,Mg²⁺
D)Mg²⁺,Na⁺,F^-,O^2-,S^2-
E)Mg²⁺,S^2-,Na⁺,F^-,O^2-

Question 45

In which of the following species is there the greatest unequal sharing of the bonding electrons?

A)SO₃
B)SO₃^2-
C)H₂S
D)H₂O
E)NH₄⁺

Question 46

Which pair of elements would form a covalent bond that is the least polar?

A)S and Li
B)Al and N
C)O and H
D)O and F
E)S and Cs

Question 47

Which of the following bonds would be the least polar yet still be considered polar covalent?

A)Mg-O
B)C-O
C)Si-O
D)O-O
E)N-O

Question 48

The measure of the attraction that an atom has for the electrons in a chemical bond is called

A)electronegativity.
B)lattice energy.
C)resonance energy.
D)ionization energy.
E)electron affinity.

Question 49

For which of the following pairs of species is the difference in radius the greatest?

A)C and F
B)K⁺ and Br^-
C)Li⁺ and I^-
D)Na and Mg
E)O^2- and F^-

Question 50

Rank the following covalent bonds in order of decreasing polarity: C-H,N-H,O-H,F-H.

A)F-H,O-H,N-H,C-H
B)O-H,F-H,N-H,C-H
C)N-H,F-H,O-H,C-H
D)C-H,N-H,O-H,F-H
E)C-H,F-H,O-H,N-H

Question 51

Rank the following ions in order of decreasing atomic radii: Te^2-,Te⁴⁺,Te⁶⁺.

A)Te^2- > Te⁴⁺ > Te⁶⁺
B)Te⁶⁺ > Te⁴⁺ > Te^2-
C)Te⁴⁺ > Te^2- > Te⁶⁺
D)Te^2- > Te⁶⁺ > Te⁴⁺
E)Te⁴⁺ > Te⁶⁺ > Te^2-

Question 52

An atom of which of the following elements has the highest electronegativity?

A)K
B)As
C)Ba
D)Si
E)Br

Question 53

During the formation of a chemical bond between two hydrogen atoms,which of the following statements is always true?

A)Energy is released during the formation of the bond.
B)A polar covalent bond is formed.
C)Electrons always are between the nuclei of the atoms.
D)One of the hydrogen atoms is ionized.
E)Resonance stabilizes the bond.

Question 54

Rank the following species in order of decreasing radii: Al³⁺,Mg²⁺,Al³⁺,Al³⁺.

A)Al³⁺ > Al³⁺ > Mg²⁺ > Al
B)Al³⁺ > Al³⁺ > Mg²⁺ > Al³⁺
C)Al³⁺> Mg²⁺ > Al³⁺ > Al³⁺
D)Al³⁺ > Mg²⁺ > Al³⁺ > Al³⁺
E)Mg²⁺ > Al³⁺ > Al³⁺ > Al³⁺

Question 55

A bond in which an electron pair is unequally shared by two atoms is

A)polar covalent.
B)coordinate covalent.
C)ionic.
D)nonpolar covalent.
E)metallic.

Question 56

The Lewis formula for phosphine,PH₃,has

A)four lone pairs.
B)four bonding pairs.
C)two bonding pairs and two lone pairs.
D)three bonding pairs and one lone pair.
E)one bonding pair and three lone pairs.

Question 57

Which of the following species would you expect to have the largest radius?

A)S^2-
B)P
C)​Na⁺
D)​Se^2-
E)​Ca²⁺

Question 58

The formulas of many binary covalent compounds can be predicted on the basis

A)that a bond is formed by the overlapping of two filled orbitals.
B)that the number of bonds an atom can have is equal to the number of empty valence orbitals it has.
C)that a bond is formed by the overlapping of atomic orbitals.
D)that the number of bonds an atom can have is equal to the number of half-filled valence orbitals it can have.
E)that bonding electrons are simultaneously attracted by more than one nucleus.

Question 59

A bond in which both electrons of the bond are donated by one atom is called ____.

A)a coordinate covalent bond
B)a polar covalent bond
C)an ionic bond
D)a double bond
E)a triple bond

Question 60

What is the total number of valence electrons in N₂O?

A)16
B)17
C)34
D)11
E)22

Question 61

How many valence electrons are present in the Lewis formula for the chlorate ion,C1O₃^-?

A)32
B)24
C)30
D)26
E)28

Question 62

What is the total number of valence electrons in the monohydrogen phosphate ion,HPO₄^2-?

A)30
B)28
C)32
D)34
E)36

Question 63

How many valence electrons does a carbonate ion have?

A)30
B)28
C)24
D)32
E)22

Question 64

In the Lewis formula for difluorodiazine,N₂F₂,the total number of lone electron pairs around the two nitrogen atoms is

A)4.
B)0.
C)3.
D)1.
E)2.

Question 65

Which of the following is a correct Lewis electron-dot formula for CO?

A)
B)
C)
D)
E)

Question 66

What is the total number of valence electrons in the ammonium ion,NH₄⁺ ?

A)9
B)11
C)8
D)10
E)12

Question 67

What is the total number of valence electrons in the cyanate ion,CNO^- ion,?

A)20
B)12
C)16
D)22
E)18

Question 68

How many valence electrons are there in the tetramethylammonium ion,(CH₃)₄N⁺?

A)32
B)18
C)8
D)33
E)24

Question 69

The Lewis structure for each of the following except ____contains at least one double bond.

A)O₂
B)CS₂
C)C₂H₄
D)NO⁺
E)N₂H₂

Question 70

Which of the following Lewis formulas is incorrect?

A)
B)
C)
D)
E)

Question 71

The total number of valence electrons in a peroxide ion,O₂^2-,is

A)2.
B)12.
C)14.
D)13.
E)15.

Question 72

The number of valence electrons in the nitrite ion is

A)22.
B)16.
C)23.
D)18.
E)24.

Question 73

Which of the following is a correct Lewis electron-dot formula for H₂SO₄?

A)
B)
C)
D)
E)

Question 74

The Lewis structure for each of the following species except ____ contains a triple bond.

A)N₃^-
B)N₂
C)HCCH
D)NO⁺
E)O₂²⁺

Question 75

Which one of the following has a Lewis formula most similar to that of NO^-?

A)O₂
B)O₂^2-
C)O₂^-
D)NO⁺
E)NO

Question 76

What is the total number of valence electrons in the sulfite ion?

A)30
B)26
C)24
D)8
E)32

Question 77

How many valence electrons are there in the trifluoroacetate ion,CF₃COO^-?

A)41
B)42
C)54
D)56
E)40

Question 78

The number of valence electrons in the propionate ion,CH₃CH₂COO^-,is

A)30.
B)32.
C)36.
D)50.
E)28.

Question 79

The total number of valence electrons in the tetrathionate ion,S₄O₆^2-,is

A)58.
B)60.
C)56.
D)54.
E)62.

Question 80

The total number of valence electrons in the phosphate ion is

A)32.
B)30.
C)24.
D)28.
E)26.