Deck 8: Basic Concepts of Chemical Bonding

Question 1

The electron configuration [Kr]4d¹⁰ represents __________.

A)Sr⁺²
B)Sn⁺²
C)Te⁺²
D)Ag⁺¹
E)Rb⁺¹

Answer 1

Ag⁺¹

Question 2

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10^-30 coulomb-meters; e=1.6 × 10^-19 coulombs)

A)1.6 × 10^-19
B)0.057
C)9.1
D)1
E)0.22

Answer 2

0.057

Question 3

In which of the molecules below is the carbon-carbon distance the shortest?

A)H₂C-CH₂
B)H-C≡C-H
C)H₃C-CH₃
D)H₂C-C-CH₂
E)H₃C-CH₂-C H₃

Answer 3

H-C≡C-H

Question 4

Of the atoms below, __________ is the most electronegative.

A)Si
B)Cl
C)Rb
D)Ca
E)S

Question 5

There are __________ valence electrons in the Lewis structure of CH₃CH₂Cl.

A)14
B)12
C)18
D)20
E)10

Question 6

Which energy change corresponds to the first ionization energy of potassium?

A)2
B)5
C)4
D)3
E)6

Question 7

Which energy change corresponds to the electron affinity of fluorine?

A)2
B)5
C)4
D)1
E)6

Question 8

Which of the following does not have eight valence electrons?

A)Ca⁺
B)Rb⁺
C)Xe
D)Br^-
E)All of the above have eight valence electrons.

Question 9

Using the Born-Haber cycle, the ΔH_f° of KBr is equal to __________.

A)ΔH_f°[K (g)] + ΔH_f°[Br (g)] + I_l(K)+ E(Br)+ ΔH_lattice
B)ΔH_f°[K (g)] - ΔH_f°[Br (g)] - I_l(K)- E(Br)- ΔH_lattice
C)ΔH_f°[K (g)] - ΔH_f°[Br (g)] + I_l(K)- E(Br)+ ΔH_lattice
D)ΔH_f°[K (g)] + ΔH_f°[Br (g)] - I_l - E(Br)+ ΔH_lattice
E)ΔH_f°[K (g)] + ΔH_f°[Br (g)] + I_l(K)+ E(Br)- ΔH_lattice

Question 10

The type of compound that is most likely to contain a covalent bond is __________.

A)one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table
B)a solid metal
C)one that is composed of only nonmetals
D)held together by the electrostatic forces between oppositely charged ions
E)There is no general rule to predict covalency in bonds.

Question 11

Which of the following has eight valence electrons?

A)Ti⁴⁺
B)Kr
C)Cl^-
D)Na⁺
E)all of the above

Question 12

Fe⁺² ions are represented by __________.

A)[Ar]3d¹
B)[Ar]3d⁴
C)[Ar]3d⁶
D)[Ar]3d¹⁰4s¹
E)[Ar]3d³

Question 13

The Lewis structure of N₂H₂ shows __________.

A)a nitrogen-nitrogen triple bond
B)a nitrogen-nitrogen single bond
C)each nitrogen has one nonbonding electron pair
D)each nitrogen has two nonbonding electron pairs
E)each hydrogen has one nonbonding electron pair

Question 14

In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii __________.

A)increases, decrease, increase
B)increases, increase, increase
C)decreases, increase, increase
D)increases, increase, decrease
E)increases, decrease, decrease

Question 15

There are __________ valence electrons in the Lewis structure of CH₃OCH₂CH₃.

A)18
B)20
C)26
D)32
E)36

Question 16

Of the molecules below, the bond in __________ is the most polar.

A)HBr
B)HI
C)HCl
D)HF
E)H₂

Question 17

Of the ions below, only __________ has a noble gas electron configuration.

A)S^3-
B)O²⁺
C)I⁺
D)K^-
E)Cl^-

Question 18

Which of the following has the bonds correctly arranged in order of increasing polarity?

A)Be-F, Mg-F, N-F, O-F
B)O-F, N-F, Be-F, Mg-F
C)O-F, Be-F, Mg-F, N-F
D)N-F, Be-F, Mg-F, O-F
E)Mg-F, Be-F, N-F, O-F

Question 19

Which ion below has a noble gas electron configuration?

A)Li²⁺
B)Be²⁺
C)B²⁺
D)C²⁺
E)N^2-

Question 20

Lattice energy is __________.

A)the energy required to convert a mole of ionic solid into its constituent ions in the gas phase
B)the energy given off when gaseous ions combine to form one mole of an ionic solid
C)the energy required to produce one mole of an ionic compound from its constituent elements in their standard states
D)the sum of ionization energies of the components in an ionic solid
E)the sum of electron affinities of the components in an ionic solid

Question 21

In which of the ions do all X-O bonds (X indicates the central atom)have the same length?

A)none
B)all
C)(i)and (ii)
D)(iii)and (v)
E)(iii), (iv), and (v)

Question 22

The Lewis structure of the COH₃2^- ion is __________.

A)
B)
C)
D)
E)

Question 23

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

A)ClF₃
B)PCl₃
C)SO₃
D)CCl₄
E)CO₂

Question 24

For resonance forms of a molecule or ion, __________.

A)one always corresponds to the observed structure
B)all the resonance structures are observed in various proportions
C)the observed structure is an average of the resonance forms
D)the same atoms need not be bonded to each other in all resonance forms
E)there cannot be more than two resonance structures for a given species

Question 25

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

A)PO₄3^-
B)SiF₄
C)CF₄
D)SeF₄
E)NF₃

Question 26

The oxidation number of phosphorus in PF₃ is __________.

A)-2
B)+1
C)+3
D)+2
E)-3

Question 27

In the nitrite ion (NO₂^-), __________.

A)both bonds are single bonds
B)both bonds are double bonds
C)one bond is a double bond and the other is a single bond
D)both bonds are the same
E)there are 20 valence electrons

Question 28

To convert from one resonance structure to another, __________.

A)only atoms can be moved
B)electrons and atoms can both be moved
C)only electrons can be moved
D)neither electrons nor atoms can be moved
E)electrons must be added

Question 29

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

A)NF₃
B)BeH₂
C)SO₂
D)CF₄
E)SO₃^2-

Question 30

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

A)NF₃
B)IF₃
C)PF₃
D)SbF₃
E)SO₄2^-

Question 31

In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons.

A)2, 2
B)4, 2
C)2, 4
D)0, 6
E)5, 1

Question 32

Resonance structures differ by __________.

A)number and placement of electrons
B)number of electrons only
C)placement of atoms only
D)number of atoms only
E)placement of electrons only

Question 33

Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl₂?

A)That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom.
B)There aren't enough electrons.
C)That would result in more than eight electrons around beryllium.
D)That would result in more than eight electrons around each chlorine atom.
E)That would result in the formal charges not adding up to zero.

Question 34

There can be four equivalent best resonance structures of __________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 35

Which of the following does not have eight valence electrons?

A)Cl^-
B)Xe
C)Ti⁺⁴
D)Rb⁺¹
E)Sr⁺¹

Question 36

The central atom in __________ violates the octet rule.

A)NH₃
B)SeF₂
C)BF₃
D)AsF₃
E)CF₄

Question 37

Based on the octet rule, boron will most likely form a __________ ion.

A)B^3-
B)B¹⁺
C)B³⁺
D)B²⁺
E)B^2-

Question 38

The central atom in __________ does not violate the octet rule.

A)SF₄
B)KrF₂
C)CF₄
D)XeF₄
E)ICl₄^-

Question 39

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

A)NI₃
B)SO₂
C)ICl₅
D)SiF₄
E)CO₂

Question 40

The oxidation number of iron in Fe₂O₃ is __________.

A)-2
B)+1
C)+3
D)+2
E)-3

Question 41

The electron configuration of the phosphide ion (P^3-)is __________.

A)[Ne]3s²
B)[Ne]3s²3_P^l
C)[Ne]3s²3_P³
D)[Ne]3_P²
E)[Ne]3s²3_P⁶

Question 42

Which of the following would have to lose three electrons in order to achieve a noble gas electron configuration? Si Mg Al Cl P

A)Si, P
B)Al
C)P
D)Cl
E)Mg, Al, P

Question 43

Based on the octet rule, phosphorus most likely forms a __________ ion.

A)P³⁺
B)P^3-
C)P⁵⁺
D)P^5-
E)P⁺

Question 44

Bond enthalpy is __________.

A)always positive
B)always negative
C)sometimes positive, sometimes negative
D)always zero
E)unpredictable

Question 45

As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________.

A)increases, increases
B)decreases, decreases
C)increases, decreases
D)decreases, increases
E)is unpredictable

Question 46

Based on the octet rule, aluminum most likely forms an __________ ion.

A)Al³⁺
B)Al⁴⁺
C)Al^4-
D)Al⁺
E)Al^-

Question 47

Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br

A)O, Se
B)Sr
C)Na
D)Br
E)Sr, O, Se

Question 48

The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively.

A)7, 4, and 6
B)1, 5, and 7
C)8, 2, and 3
D)7, 1, and 2
E)2, 7, and 4

Question 49

Dynamite __________.

A)was invented by Alfred Nobel
B)is made of nitroglycerine and an absorbent such as diatomaceous earth
C)is a much safer explosive than pure nitroglycerine
D)is an explosive
E)all of the above

Question 50

Of the bonds C-N, C-N, and C≡N, the C-N bond is __________.

A)strongest/shortest
B)strongest/longest
C)weakest/shortest
D)weakest/longest
E)intermediate in both strength and length

Question 51

Dynamite consists of nitroglycerine mixed with __________.

A)potassium nitrate
B)damp KOH
C)TNT
D)diatomaceous earth or cellulose
E)solid carbon

Question 52

Based on the octet rule, iodine most likely forms an __________ ion.

A)I²⁺
B)I⁴⁺
C)I^4-
D)I⁺
E)I-

Question 53

The only noble gas without eight valence electrons is __________.

A)Ar
B)Ne
C)He
D)Kr
E)All noble gases have eight valence electrons.

Question 54

Most explosives are compounds that decompose rapidly to produce __________ products and a great deal of __________.

A)gaseous, gases
B)liquid, heat
C)soluble, heat
D)solid, gas
E)gaseous, heat

Question 55

Of the bonds C-C, C-C, and C≡C, the C-C bond is __________.

A)strongest/shortest
B)strongest/longest
C)weakest/longest
D)weakest/shortest
E)intermediate in both strength and length

Question 56

Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr₃)is __________ kJ/mol.

A)1241
B)689
C)-689
D)1378
E)-1378

Question 57

The electron configuration of the sulfide ion (S^2-)is __________.

A)[Ne]3s²
B)[Ne]3s²3_P^l
C)[Ne]3s²3_P⁴
D)[Ne]3_P²
E)[Ne]3s²3_P⁶

Question 58

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

A)N
B)C
C)H
D)O
E)B

Question 59

Based on the octet rule, magnesium most likely forms a __________ ion.

A)Mg²⁺
B)Mg^2-
C)Mg^6-
D)Mg⁶⁺
E)Mg^-

Question 60

Of the possible bonds between carbon atoms (single, double, and triple), __________.

A)a triple bond is longer than a single bond
B)a double bond is stronger than a triple bond
C)a single bond is stronger than a triple bond
D)a double bond is longer than a triple bond
E)a single bond is stronger than a double bond

Question 61

For a given arrangement of ions, the lattice energy increases as ionic radius __________ and as ionic charge __________.

A)decreases, increases
B)increases, decreases
C)increases, increases
D)decreases, decreases
E)This cannot be predicted.

Question 62

Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br

A)Br
B)Sr
C)Na
D)O, Se
E)Sr, O, Se

Question 63

For a given arrangement of ions, the lattice energy decreases as ionic radius __________ and as ionic charge __________.

A)decreases, increases
B)increases, decreases
C)increases, increases
D)decreases, decreases
E)This cannot be predicted.

Question 64

What is the maximum number of double bonds that a carbon atom can form?

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

Question 65

What is the maximum number of double bonds that a hydrogen atom can form?

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

Question 66

What is the electron configuration for the Fe³⁺ ion?

A)[Ar]4s¹3d⁶
B)[Ar]4s⁰3d⁷
C)[Ar]4s⁰3d⁵
D)[Ar]4s²3d⁹
E)[Ne]3s²3p¹⁰

Question 67

The electron configuration of the P^3- ion is __________.

A)[Ar]3s²3_P⁶
B)[Ar]3s²3_P²
C)[Ne]3s²3_P⁶
D)[Ne]3s²3_P²
E)[Kr]3s²3_P^-6

Question 68

What is the electron configuration for the Co²⁺ ion?

A)[Ar]4s¹3d⁶
B)[Ar]3d⁷
C)[Ar]3d⁵
D)[Ar]4s²3d⁹
E)[Ne]3s²3p¹⁰

Question 69

Determining lattice energy from Born-Haber cycle data requires the use of __________.

A)the octet rule
B)Coulomb's law
C)Periodic law
D)Hess's law
E)Avogadro's number

Question 70

How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?

A)1
B)2
C)3
D)4
E)5

Question 71

What species has the electron configuration [Ar]3d²?

A)Mn²⁺
B)Cr²⁺
C)V³⁺
D)Fe³⁺
E)K⁺

Question 72

The electron configuration of the S^2- ion is __________.

A)[Ar]3s²3_P⁶
B)[Ar]3s²3_P²
C)[Ne]3s²3_P²
D)[Ne]3s²3_P⁶
E)[Kr]3s²3_P^-6

Question 73

What is the maximum number of triple bonds that a carbon atom can form?

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

Question 74

What species has the electron configuration [Ar]3d⁴?

A)Mn²⁺
B)Cr²⁺
C)V³⁺
D)Fe³⁺
E)K⁺

Question 75

Elements from opposite sides of the periodic table tend to form __________.

A)covalent compounds
B)ionic compounds
C)compounds that are gaseous at room temperature
D)homonuclear diatomic compounds
E)covalent compounds that are gaseous at room temperature

Question 76

A __________ covalent bond between the same two atoms is the longest.

A)single
B)double
C)triple
D)They are all the same length.
E)strong

Question 77

The formula of palladium(IV)sulfide is __________.

A)Pd₂S₄
B)PdS₄
C)Pd4_S
D)PdS₂
E)Pd₂S₂

Question 78

A double bond consists of __________ pairs of electrons shared between two atoms.

A)1
B)2
C)3
D)4
E)6

Question 79

A triple bond consists of __________ pairs of electrons shared between two atoms.

A)1
B)2
C)3
D)4
E)6

Question 80

What is the electron configuration for the Fe²⁺ ion?

A)[Ar]4s⁰3d⁶
B)[Ar]4s²3d⁴
C)[Ar]4s⁰3d⁸
D)[Ar]4s²3d⁸
E)[Ar]4s⁶3d²