Deck 10: Theories of Bonding and Structure

Question 1

Which of the five basic geometries for molecules and ions has the largest bond angle?

A)linear
B)planar triangular
C)tetrahedral
D)square planar
E)octahedral

Answer 1

linear

Question 2

Which of these examples is not one of the five basic geometries for molecules and ions?

A)planar triangular
B)octahedral
C)tetrahedral
D)square planar
E)trigonal bipyramidal

Answer 2

square planar

Question 3

Two different values, less than 180°, are observed for the bond angles in which of the following basic structures for molecules and ions?

A)linear
B)planar triangular
C)tetrahedral
D)trigonal bipyramidal
E)octahedral

Answer 3

trigonal bipyramidal

Question 4

Which of the five basic geometries for molecules and ions has the smallest bond angle?

A)linear
B)planar triangular
C)tetrahedral
D)octahedral
E)These all have the same bond angles.

Question 5

Where is the central atom located in a trigonal bipyramidal molecule?

A)in the center of the plane shared by the two triangular pyramids, and at the point where the equatorial and axial bonds meet
B)at the end of an axial bond
C)at the end of an equatorial bond
D)on the middle edge of the plane formed by the two triangular pyramids
E)in the central face of any of the two triangular pyramids, where two bonds form a 120° angle

Question 6

The valence shell electron pair repulsion theory is based on the concept that

A)only two electrons can occupy an atomic orbital.
B)the position and speed of the electron are somewhat uncertain.
C)electron pairs tend to stay as far apart as possible to minimize repulsions between them.
D)electronegativity tends to promote the formation of polar bonds.
E)electrons are added to the lowest energy atomic orbitals first.

Question 7

Which basic arrangement would best accommodate two electron domains in the valence shell of a covalently bonded atom?

A)planar triangular
B)octahedral
C)tetrahedral
D)linear
E)trigonal bipyramidal

Question 8

Which basic arrangement would best accommodate three electron domains in the valence shell of a covalently bonded atom?

A)planar triangular
B)octahedral
C)tetrahedral
D)linear
E)trigonal bipyramidal

Question 9

Which basic arrangement would best accommodate four electron domains in the valence shell of a covalently bonded atom?

A)planar triangular
B)octahedral
C)tetrahedral
D)linear
E)trigonal bipyramidal

Question 10

Which basic arrangement would best accommodate five electron domains in the valence shell of a covalently bonded atom?

A)planar triangular
B)octahedral
C)tetrahedral
D)linear
E)trigonal bipyramidal

Question 11

Which basic arrangement would best accommodate six electron domains in the valence shell of a covalently bonded atom?

A)planar triangular
B)octahedral
C)tetrahedral
D)linear
E)trigonal bipyramidal

Question 12

Based on the Lewis structure, the number of electron domains in the valence shell of the boron atom in the BF₃ molecule is

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

Question 13

A molecule has a central atom surrounded by 2 lone pairs and 3 atoms. The best description for the shape of the molecule is

A)trigonal bipyramidal.
B)octahedral.
C)trigonal planar.
D)T-shaped.
E)see-saw.

Question 14

A molecule has a central atom surrounded by 1 lone pair and 3 atoms. The best description for the shape of the molecule is

A)trigonal pyramidal.
B)bent.
C)trigonal planar.
D)T-shaped.
E)see-saw.

Question 15

A molecule has a central atom surrounded by 1 lone pair and 5 atoms. The best description for the shape of the molecule is

A)octahedral.
B)square pyramidal.
C)trigonal planar.
D)square planar.
E)see-saw.

Question 16

Based on the Lewis structure, the number of electron domains in the valence shell of the arsenic atom in the AsCl₃ molecule is

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

Question 17

Based on the Lewis structure, the number of electron domains in the valence shell of the carbon atom in the CO₃^2- ion is

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

Question 18

Based on the Lewis structure, the number of electron domains in the valence shell of the xenon atom in the XeF₂ molecule is

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

Question 19

Based on the Lewis structure, the number of electron domains in the valence shell of the sulfur atom in the SO₂ molecule is

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

Question 20

Application of the concepts of the VSEPR theory, suggests that the shape of the SO₃ molecule is

A)trigonal pyramidal.
B)square planar.
C)regular tetrahedral.
D)triangular planar.
E)distorted tetrahedron.

Question 21

Application of the concepts of VSEPR theory leads to the prediction that the shape of the PCl₃ molecule is

A)bent.
B)linear.
C)regular tetrahedral.
D)triangular planar.
E)trigonal pyramidal.

Question 22

Application of the VSEPR theory suggests that the geometric arrangement of the atoms in the carbonate ion, CO₃², is

A)octahedral.
B)square planar.
C)regular tetrahedral.
D)triangular planar.
E)trigonal pyramidal.

Question 23

The smallest F-P-F bond angle in PF₆^- ion is

A)90 degrees.
B)109.5 degrees.
C)120 degrees.
D)145 degrees.
E)180 degrees.

Question 24

Application of the VSEPR model to the NCl₃ molecule leads to the prediction that

A)the molecule should have trigonal pyramidal geometry.
B)the molecule should have delocalized valence electrons.
C)the molecule should be nonpolar.
D)the formal charge on the center atom is +3.
E)the molecule should have a planar triangular geometry.

Question 25

The molecular geometry of the SeF₄ molecule is best described as

A)trigonal pyramidal.
B)square planar.
C)regular tetrahedral.
D)triangular planar.
E)distorted tetrahedral.

Question 26

Application of the concepts of VSEPR theory leads to the prediction that the shape of the XeOF₄ molecule is

A)bent.
B)linear.
C)regular tetrahedral.
D)triangular planar.
E)square pyramidal.

Question 27

Based on conclusions from application of the VSEPR theory, which one of the following has a linear shape?

A)IF₂⁺
B)HCN
C)H₂CO
D)H₂S
E)SO₂

Question 28

Based on conclusions from application of the VSEPR theory, which one of the following has a linear shape?

A)IF₂^-
B)HCO^-
C)H₂CO
D)H₂S
E)SO₂

Question 29

Based on application of the VSEPR theory, which molecule has a trigonal bipyramidal shape?

A)BrF₅
B)AsF₅
C)SF₄
D)XeOF₄
E)SbCl₅^2-

Question 30

Based on application of the VSEPR theory, which molecule has a bent (v-shaped)geometry?

A)CO₂
B)CS₂
C)KrF₂
D)C₂H₂
E)SO₂

Question 31

Based on application of the VSEPR theory, which molecule or ion has a bent (v-shaped)geometry?

A)Cl₂O
B)CO₂
C)HCN
D)CO
E)NO₂⁺

Question 32

Based on application of the VSEPR theory, which molecule or ion has a regular tetrahedral geometry?

A)IF₄^-
B)CF₄
C)H₃O⁺
D)SF₄
E)XeF₄

Question 33

Based on application of the VSEPR theory, the expected bond angles in the AsF₄ ion should be approximately

A)90 degrees.
B)109.5 degrees.
C)120 degrees.
D)90, 120 and 180 degrees.
E)90 and 180 degrees.

Question 34

Which statement is true for the BrF₅ molecule?

A)There are two lone pairs in the valence shell of the bromine atom.
B)There is an unpaired electron in the valence shell of the bromine atom.
C)Some of the F-Br-F bond angles are close to 90 degrees.
D)At least one of the bond angles, F-Br-F, is about 109.5 degrees.
E)Some of the F-Br-F bond angles are close to 120 degrees.

Question 35

Which best explains the polarity of the PCl₃ molecule?

A)Vector addition yields a net zero dipole moment.
B)The tetragonal shape leads to no overall polarity.
C)The trigonal pyramid shape leads to a nonpolar molecule.
D)The P-Cl dipole moments sum to a net dipole moment.
E)Two nonbonding electron pairs cause an overall polarity.

Question 36

Based on observed periodic trends, arrange the following species, CH₃Br, CH₃Cl, CH₃F, CH₃I, in order of increasing dipole moment.

A)CH₃F < CH₃Cl < CH₃Br < CH₃I
B)CH₃Br < CH₃Cl < CH₃F < CH₃I
C)CH₃I < CH₃F < CH₃Cl < CH₃Br
D)CH₃I < CH₃Br < CH₃Cl < CH₃F
E)CH₃Cl < CH₃Br < CH₃I < CH₃F

Question 37

In the CSe₂ molecule,

A)the bonds are all nonpolar, which makes it polar.
B)the bonds are polar, but their effect on the overall polarity is canceled by the effect of lone pairs in the valence shell of the carbon atom.
C)the bonds are polar, but their effect on the overall polarity is canceled by the fact that they are equal in magnitude and oppositely directed.
D)the bonds are polar, but the polar effect is canceled by the resonance hybrids which distribute the charge evenly.
E)the bonds are slightly polar, and so they will not affect the overall polarity of the molecule.

Question 38

Based on application of the VSEPR theory, which molecule should be nonpolar?

A)CH₃Cl
B)CS₂
C)H₂O
D)NH₃
E)OF₂

Question 39

Which molecule below is polar?

A)CF₄
B)BF₃
C)C₂H₂
D)CSe₂
E)IBr

Question 40

Which molecule below is most likely nonpolar?

A)NCl₃
B)SO₂
C)NO₂
D)SO₃
E)CH₂Cl₂

Question 41

Which of these examples is a polar molecule?

A)XeF₂
B)BrF₅
C)XeF₄
D)CCl₄
E)PBr₅

Question 42

Which of these examples is a nonpolar molecule?

A)CHCl₃
B)BrF₅
C)CO₂
D)SO₂
E)NH₃

Question 43

Predict the molecular geometry and polarity of the SO₂ molecule by applying VSEPR theory.

A)linear, nonpolar
B)linear, polar
C)bent, 109.5° bond angle, polar
D)bent, 120° bond angle, polar
E)bent, 109.5° bond angle, nonpolar

Question 44

Predict the molecular geometry and polarity of the O-C-S molecule.

A)linear, nonpolar
B)bent, nonpolar
C)linear, polar
D)tetrahedral, nonpolar
E)bent, polar

Question 45

Compare the molecules SbCl₅ and IF₅, using VSEPR theory.

A)IF₅ is polar, while SbF₅ is nonpolar.
B)Both molecules have a trigonal bipyramidal geometry and are also nonpolar.
C)SbF₅ is polar and IF₅ is nonpolar.
D)Both molecules are polar and have a trigonal bipyramidal geometry.
E)Both molecules have lone pairs in the valence shell of the central atom.

Question 46

Bonding in the chlorine molecule can be explained by the valence bond theory in terms of an overlap between

A)the 1s orbital of a chlorine atom and the 1s orbital of the other chlorine atom.
B)the 2s orbital of a chlorine atom and the 2s orbital of the other chlorine atom.
C)a 2p orbital of a chlorine atom and a 2p orbital of the other chlorine atom.
D)the 3s orbital of a chlorine atom and the 3s orbital of the other chlorine atom.
E)a 3p orbital of a chlorine atom and a 3p orbital of the other chlorine atom.

Question 47

Bonding in the hydrogen chloride molecule can be explained by the valence bond theory in terms of an overlap between

A)the 1s orbital of the hydrogen atom and the 1s orbital of the chlorine atom.
B)the 1s orbital of the hydrogen atom and the 2s orbital of the chlorine atom.
C)the 1s orbital of the hydrogen atom and a 2p orbital of the chlorine atom.
D)the 1s orbital of the hydrogen atom and the 3s orbital of the chlorine atom.
E)the 1s orbital of the hydrogen atom and a 3p orbital of the chlorine atom.

Question 48

Bonding in the nitrogen trifluoride molecule can be explained by the valence bond theory in terms of an overlap between

A)the 2s orbital of the nitrogen and the 2s orbital of the fluorine.
B)the 2s orbital of the nitrogen and a 2p orbital of the fluorine.
C)a 2p orbital of the nitrogen and a 2p orbital of the fluorine.
D)the 1s orbital of the nitrogen and a 2p orbital of the fluorine.
E)a 2p orbital of the nitrogen and the 3p orbital of the fluorine.

Question 49

What hybrid orbitals are used by the carbon atom in CH₄ for bonding?

A)sp^3d2
B)sp
C)sp^3d
D)sp³
E)sp²

Question 50

What is the hybridization on C in C₂H₂?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 51

What is the hybridization of the nitrogen atom in NH₃?

A)sp^3d2
B)sp
C)sp^3d
D)sp³
E)sp²

Question 52

What type of hybrid orbitals do the carbon atoms have in C₂H₆?

A)sp^3d2
B)sp
C)sp^3d
D)sp³
E)sp²

Question 53

What type of hybrid orbitals do the carbon atoms have in C₂H₄?

A)sp^3d2
B)sp
C)sp^3d
D)sp³
E)sp²

Question 54

What type of hybridization does the nitrogen atom have in H₃CNO₂?

A)sp^3d2
B)sp
C)sp^3d
D)sp³
E)sp²

Question 55

What hybrid orbitals are on the sulfur atom in a sulfur tetrafluoride molecule?

A)sp^3d2
B)sp
C)sp^3d
D)sp³
E)sp²

Question 56

What hybrid orbitals on an As atom in the AsF₄^- ion?

A)sp^3d2
B)sp
C)sp^3d
D)sp³
E)sp²

Question 57

Which of the following molecules or ions does not use sp³d² hybrid orbitals on the central atom for bonding?

A)SF₆
B)PF₆^-
C)IF₄⁺
D)XeF₄
E)BrF₅

Question 58

The central atom in BrF₅ uses sp^3d2 hybridization. It must therefore have ________ ?bonds and ________ lone pair(s)of electrons in the valence shell of the central atom.

A)1, 5
B)3, 3
C)5, 0
D)5, 1
E)6, 0

Question 59

The central atom in SF₄ has ________ ?bonding pair(s)and ________ lone pair(s)of electrons in the valence shell of the central atom.

A)3, 2
B)4, 0
C)4, 1
D)5, 0
E)5, 1

Question 60

What type of hybrid orbitals are used by the central atom for $\sigma$ bonding in the PCl₃ molecule?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 61

What type of hybrid orbitals are used by the central atom for $\sigma$ -bonding in the PCl₄^- ion?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 62

What kind of hybrid orbitals are used by the central atom for $\sigma$ bonding in the SF₆ molecule?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 63

What kind of hybrid orbitals are used by the central atom for $\sigma$ bonding in the AsF₅ molecule?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 64

What kind of hybrid orbitals are used by the central atom for $\sigma$ bonding in the NO₃ ion?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 65

What kind of hybrid orbitals are used by the As atom for $\sigma$ bonding in the AsF₄^- ion?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 66

What kind of hybrid orbitals are used by the central atom for $\sigma$ bonding in the ClO₃^- ion?

A)sp
B)sp²
C)sp³
D)sp^3d
E)sp^3d2

Question 67

In the carbon monoxide molecule, there will be ________ $\pi$ -bond(s)and the ________ hybrid orbitals on the carbon would be used for $\sigma$ -bonding in the molecule.

A)2, sp
B)2, sp²
C)3, sp
D)3, sp²
E)1, sp²

Question 68

How many $\sigma$ -bonds and $\pi$ -bond(s)are in the H₃CNO₂ molecule?

A)7 $\sigma$ -bonds and 0 $\pi$ -bonds
B)6 $\sigma$ -bonds and 1 $\pi$ -bond
C)1 $\sigma$ -bond and 5 $\pi$ -bonds
D)5 $\sigma$ -bonds and 2 $\pi$ -bonds
E)2 $\sigma$ -bonds and 1 $\pi$ -bond

Question 69

How many $\sigma$ -bonds and $\pi$ -bonds are in a CO₂ molecule?

A)1 $\sigma$ -bond and 2 $\pi$ -bonds
B)2 $\sigma$ -bonds and 0 $\pi$ -bonds
C)2 $\sigma$ -bonds and 2 $\pi$ -bonds
D)2 $\sigma$ -bonds and 4 $\pi$ -bonds
E)4 $\sigma$ -bonds and 0 $\pi$ -bonds

Question 70

Which statement about the ammonia molecule, NH₃, is true?

A)The N-H bonds are polar, but the molecule is nonpolar.
B)The molecule has both three ?- and one ?-bond.
C)The nitrogen atom utilizes sp³ hybrid orbitals for ?bonding.
D)The H-N-H bond angles are greater than 109.5 degrees.
E)The molecular geometry is planar triangular.

Question 71

How many $\pi$ -bonds are there in the CN ion?

A)0
B)1
C)1.5
D)2
E)3

Question 72

If formal charge considerations are taken into account, how many $\pi$ -bond(s)is/are in the SO₃^2- ion?

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

Question 73

Which molecule or ion uses an sp² set of hybrid orbitals on the central atom for ?bonding?Hint: Consider formal charge when deciding on the correct structure and remember that sulfur atoms can access d-orbitals.

A)CS₂
B)N₂O
C)SO₂
D)NF₃
E)I₃^-

Question 74

When formal charges are considered, how many ?-bond(s)and ?bonds, respectively, are in the chlorate ion, ClO₃^-?Hint: Remember that chlorine atoms can access d-orbitals.

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

Question 75

Ozone (O₃)is an allotropic form of oxygen. Based on VSEPR and valence bond theory, which statement is true for this molecule?

A)The molecule is linear, and has no lone pairs in the valence shell on the central atom.
B)The molecule is linear, and has two $\pi$ -bonds and one $\sigma$ -bond.
C)The molecule is T-shaped, and has two $\pi$ -bonds and two $\sigma$ -bonds.
D)The molecule is bent, and has two lone pairs in the valence shell on the central atom.
E)The molecule is bent, and has one $\pi$ -bond and two $\sigma$ -bonds.

Question 76

The H₂ ion, according to MO theory, has a bond order of

A)0
B)0.5
C)1.0
D)1.5
E)2.0

Question 77

The H₂⁺ ion, according to MO theory, has a bond order of

A)0
B)0.5
C)1.0
D)1.5
E)2.0

Question 78

The He₂ molecule, according to MO theory, has a bond order of

A)0
B)0.5
C)1.0
D)1.5
E)2.0

Question 79

The restrictions on the placing of electrons in molecular orbitals in molecules and ions

A)must obey the Pauli exclusion principle but not Hund's rule or the Aufbau principle.
B)must obey the Pauli exclusion principle and the Aufbau principle but not Hund's rule.
C)must obey the Aufbau principle but not the Pauli exclusion principle or Hund's rule.
D)are not governed by either the Aufbau principle, Hund's rule, or the Pauli exclusion principle.
E)must obey the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

Question 80

An energy level scheme for the orbitals of second row diatomic molecules O₂ through Ne₂, lists the molecular orbitals in the following order of increasing energy $\sigma$ _2s < $\sigma$ *_2s < $\sigma$ _2p(z)< $\pi$ _2p(y), $\pi$ _2p(x) < $\pi$ *_2p(y), $\pi$ *_2p(x)< $\sigma$ *_2p(z)
Based on this energy level scheme, the bond order for the bond in the O₂⁺ ion in its ground state is

A)1.0
B)1.5
C)2.0
D)2.5
E)3.0