Deck 5: Bonding Theories Explaining Molecular Geometry

Question 1

In VSEPR theory, molecular geometry is determined by _______

A)electron-proton attractive forces.
B)electron-electron attractive forces.
C)electron-electron repulsive forces.
D)proton-proton repulsive forces.
E)electron-nucleus attractive forces.

Answer 1

electron-electron repulsive forces.

Question 2

Which would have the largest effect on a neighboring bond angle?

A)two lone pairs of electrons
B)one lone pair of electrons and a double bond
C)one double bond and a single bond
D)two single bonds
E)two double bonds

Answer 2

two lone pairs of electrons

Question 3

What does a Lewis structure NOT show?

A)the bonding arrangement of atoms
B)three-dimensional molecular shape
C)bonding electrons
D)nonbonding electrons
E)charges when applicable)

Answer 3

three-dimensional molecular shape

Question 4

Determine the molecular geometry of N₂O.

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

Question 5

The electron group geometry of AsH₃ is , and its molecular geometry is

A)trigonal planar; trigonal planar.
B)tetrahedral; trigonal planar.
C)tetrahedral; tetrahedral.
D)tetrahedral; trigonal pyramidal.
E)trigonal pyramidal; trigonal pyramidal.

Question 6

What are the electron group number and molecular geometry of CF₂Cl₂?

A)2, linear
B)2, bent
C)4, tetrahedral
D)4, trigonal pyramidal
E)4, bent

Question 7

The electron group geometry of GaCl₃ is , and its molecular geometry is .Gallium trichloride is an exception to the octet rule.

A)trigonal planar; trigonal planar
B)trigonal planar; bent
C)trigonal bipyramidal; tetrahedral
D)tetrahedral; trigonal pyramidal
E)trigonal pyramidal; trigonal pyramidal

Question 8

What is the steric number of the central sulfur atom in SCl₂?

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

Question 9

The electron group geometry of AsCl₃ is , and its molecular geometry is

A)trigonal bipyramidal; trigonal bipyramidal.
B)octahedral; trigonal bipyramidal.
C)trigonal bipyramidal; tetrahedral.
D)tetrahedral; trigonal pyramidal.
E)tetrahedral; tetrahedral.

Question 10

What are the ideal bond angles around a central atom with a steric number of 3?

A)all 72 $\degree$
B)all 90 $\degree$
C)all 120 $\degree$
D)90 $\degree$ and 109.5 $\degree$
E)90 $\degree$ and 120 $\degree$

Question 11

Which compound below has the same shape as NO₂ ion?

A)SO₂
B)HCN
C)BeH₂
D)OCS
E)CO₂

Question 12

Arrange the interactions between pairs of electrons in order of increasing repulsive strength.

A)bonding pair-bonding pair $\lt$ lone pair-bonding pair $\lt$ lone pair-lone pair
B)bonding pair-bonding pair $\lt$ lone pair-lone pair $\lt$ lone pair-bonding pair
C)lone pair-lone pair $\lt$ lone pair-bonding pair $\lt$ bonding pair-bonding pair
D)lone pair-lone pair $\lt$ bonding pair-bonding pair $\lt$ lone pair-bonding pair
E)lone pair-bonding pair $\lt$ bonding pair-bonding pair $\lt$ lone pair-0lone pair

Question 13

Determine the molecular geometry of SeCl₂.

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

Question 14

Which bond angle is the largest?

A)O - C - S in COS
B)H - Si - H in SiH₄
C)O - C - O in CO 2-
D)Cl - C - Cl in COCl₂
E)F - S - F in SF₆

Question 15

What are the ideal bond angles around carbon in CH₂O?

A)180 $\degree$
B)90 $\degree$
C)120 $\degree$
D)109.5 $\degree$
E)60 $\degree$

Question 16

Which bond angle is the smallest?

A)H - C - H in C₂H₄
B)H - C - H in CH₄
C)H - C - H in H₂CO
D)H - C - C in C₂H₂
E)H - C - O in H₂CO

Question 17

What is the steric number of the central phosphorus atom in PF₃?

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

Question 18

What are the steric number and molecular geometry of SO₃?

A)2, linear
B)3, trigonal planar
C)3, trigonal pyramidal
D)3, bent
E)4, bent

Question 19

Which electron-pair geometry has the lowest electron-electron repulsive forces?

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

Question 20

Determine the molecular geometry of the chlorite ion, ClO₂ ^- .

A)linear
B)bent
C)trigonal bipyramidal
D)tetrahedral
E)trigonal pyramidal

Question 21

Which bond angle is the smallest?

A)O - S - O in SO₂
B)O - S - O in SO₃
C)O - S - O in SO₄2-
D)F - S - F in SF₆
E)Cl - S - Cl in SOCl₂

Question 22

What is the molecular geometry of SF₄?

A)tetrahedral
B)square pyramidal
C)seesaw
D)square planar
E)T-shaped

Question 23

Which molecule below is polar?

A)CF₄
B)SiH₄
C)CH₂Cl₂
D)CS₂
E)CO₂

Question 24

The correct H - N - H bond angle in NH₃ is

A)the same as the H - O - H angle in water.
B)exactly 109.5 $\degree$ .
C)greater than 109.5 $\degree$ .
D)less than 109.5 $\degree$ .
E)120 $\degree$ .

Question 25

What is the molecular geometry of SF₄O?

A)pentagonal
B)tetrahedral
C)trigonal bipyramidal
D)trigonal planar
E)square pyramidal

Question 26

Which molecule or ion below is linear?

A)H₂Se
B)H₂S
C)ICl₃
D)IBr ₂^-
E)SO₂

Question 27

Which molecule below has a square planar molecular geometry?

A)NH₃
B)PCl₅
C)KrF₄
D)CH₃COOH
E)SiH₄

Question 28

Which compound below has a square pyramidal molecular geometry?

A)XeF₄
B)IF₅
C)CCl₄
D)PF₅
E)SF₄

Question 29

Which molecule or ion below has a trigonal pyramidal molecular geometry?

A)KrF₄
B)COCl₂
C)SeO₃^2-
D)NH₄ ⁺
E)O₃

Question 30

Which molecule below is NOT polar?

A)NO₂
B)H₂O
C)SO₂
D)CS₂
E)N₂O

Question 31

Which molecule or ion below has the largest bond angle?

A)CF₄
B)NF₃
C)F₂O
D)NF _2^-
E)NH₃

Question 32

You synthesize a compound by combining one volume of iodine vapor with seven volumes of fluorine gas.What is the steric number of the iodine atom?

A)3
B)4
C)6
D)7
E)8

Question 33

You synthesize a cation with a +1 charge by oxidizing a compound made by combining one volume of iodine vapor with six volumes of fluorine gas.What F - I - F bond angle value(s) would you predict?

A)all 120 $\degree$
B)three 120 $\degree$ and four 90 $\degree$
C)three 90 $\degree$ and four 120 $\degree$
D)all 90 $\degree$
E)none of these

Question 34

Which molecule below is T-shaped molecular geometry?

A)NCl₃
B)PCl₃
C)SOCl₂
D)ICl₃
E)COCl₂

Question 35

For the series methane, ammonia, and water, the bond angle increases in the following order: H₂O $\lt$ NH₃ $\lt$ CH₄.This trend is due to _______

A)a decreasing effective nuclear charge.
B)a decrease in the number of lone pairs.
C)an increase in atomic radius.
D)an increase in the polarity of the molecules.
E)an increasing effective nuclear charge.

Question 36

All homonuclear diatomic molecules

A)have polar bonds.
B)are polar.
C)are nonpolar.
D)cannot vibrate.
E)are liquids.

Question 37

What is the correct molecular geometry of the ClO₃^- ion?

A)square planar
B)square pyramidal
C)trigonal pyramidal
D)tetrahedral
E)seesaw

Question 38

Which compound below has a trigonal bipyramidal molecular geometry?

A)ICl₃
B)BrF₅
C)PCl₅
D)PH₃
E)SiF₄

Question 39

Which molecule or ion below has the same approximate geometry as BCl₃?

A)COCl₂
B)ClO₃-
C)ICl₃
D)NCl₃
E)SO₃ ^2-

Question 40

Which compound below has the same molecular shape as CCl₃H?

A)SF₄
B)KrF₄
C)SiF₄
D)C₂H₄
E)C₂H₂

Question 41

Which compound below has the largest dipole moment?

A)CF₂Cl₂
B)CH₂Cl₂
C)CH₂F₂
D)CF₄
E)CH₂Br₂

Question 42

Which statement regarding $\sigma$ and $\pi$ bonds is TRUE?

A)Both types of bonds can be made by the overlap of unhybridized atomic orbitals.
B)The overlap of sp hybrid orbitals can form either a $\sigma$ or a $\pi$ bond.
C)When two atoms form a multiple bond, $\sigma$ and $\pi$ bonds overlap in space and reinforce each other.
D)Multiple bonds between atoms often involve only $\pi$ bonds, not $\sigma$ bonds.
E)Electron density cannot be localized between two atoms when they participate in $\pi$ bonding.

Question 43

What is the hybridization of carbon in C₂H₂?

A)sp2
B)sp3
C)sp3d
D)sp
E)sp3d 2

Question 44

Which statement regarding a $\pi$ bond between two carbon atoms is TRUE?

A)The region of high electron density lies along the bond axis connecting the nuclei of the two atoms.
B)It can be described by the overlap of sp hybrid orbitals from each atom.
C)It can be described by the overlap of sp² hybrid orbitals from each atom.
D)It can be described by the overlap of a p atomic orbital from one atom with an sp² hybrid orbital from the other atom.
E)It can be described by the overlap of p atomic orbitals from each atom.

Question 45

Which compound below has the largest dipole moment?

A)CH₂Cl₂
B)CH₃Cl
C)CHCl₃
D)CCl₄
E)CH₄

Question 46

Which compound below is the most polar?

A)NH₃
B)PH₃
C)AsH₃
D)SbH₃
E)BiH₃

Question 47

Which compound below has the smallest dipole moment?

A)CF₂Cl₂
B)CF₃Cl
C)CF₄
D)CFCl₃
E)CHFCl₂

Question 48

Which molecule below has a central atom with the same hybridization as the oxygen in water?

A)SO₂
B)OCS
C)CS₂
D)NH₃
E)CO₂

Question 49

Which statement regarding hybrid orbitals and molecular shape is FALSE?

A)Atomic orbitals form hybrid orbitals with regions of electron density at specific angles around the nucleus.
B)Hybrid orbitals are mathematical combinations of the wave functions of atomic orbitals.
C)Hybrid orbitals generally have electron density at angles that minimize electron repulsions and maximize orbital overlap when bonding occurs.
D)Hybridization can involve atomic orbitals that are occupied or unoccupied by electrons.
E)Atomic orbitals on different atoms mix to form hybrid orbitals at angles that minimize repulsions.

Question 50

Which statement regarding a $\sigma$ bond between two carbon atoms linked by a single bond is FALSE?

A)The region of electron density lies along the bond axis connecting the nuclei of the two atoms.
B)The bond can be described by the overlap of sp hybrid orbitals from each atom.
C)The bond can be described by the overlap of sp2 hybrid orbitals from each atom.
D)The bond can be described by the overlap of sp3d hybrid orbitals from each atom.
E)The bond can be described by the overlap of an sp2 hybrid orbital from one atom with an sp3 hybrid orbital from the other atom.

Question 51

What is the hybridization of sulfur in SOCl₂?

A)sp²
B)sp³
C)sp³d
D)sp
E)sp³d²

Question 52

Which statement below best describes the C - O bond in COF₂?

A)sp orbitals form one $\sigma$ bond.
B)sp² orbitals form two $\sigma$ bonds.
C)Unhybridized 2p orbitals form two $\pi$ bonds.
D)sp² hybrid orbitals form one $\pi$ bond, and unhybridized 2p orbitals form one $\pi$ bond.
E)sp² hybrid orbitals form one $\sigma$ bond, and unhybridized 2p orbitals form one $\pi$ bond.

Question 53

Which of these molecules have a dipole moment?

A)PCl₅ and SiCl₄
B)POCl₃, SO₂Cl₂, and SO₃
C)POCl₃ and SO₂Cl₂
D)PCl₅, POCl₃, SOCl₂, SO₃, and SiCl₄
E)PCl₅, SF₆, SO₃, and SiCl₄

Question 54

Which statement below regarding valence bond theory is TRUE?

A)Hybrid orbitals cannot contain lone pairs of electrons.
B)A single bond is a sigma bond with a localized electron pair.
C)A double bond can be described as two $\pi$ bonds occupied by four electrons.
D)The magnetic properties of a molecule are readily explained.
E)There is no provision for atoms with expanded octets.

Question 55

What is the hybridization of selenium in SeCl₄?

A)sp2
B)sp3
C)sp3d
D)sp
E)sp3d 2

Question 56

Which compound below contains polar bonds and has a permanent dipole moment?

A)AsCl₅
B)SiF₄
C)CO₂
D)BeCl₂
E)BF₃

Question 57

Which molecule below has a central atom with the same hybridization as the carbon in formaldehyde (H₂CO)?

A)SO₂
B)OCS
C)ICl₃
D)I₃^-
E)C₂H₂

Question 58

Which molecule below has a carbon atom that is sp3 hybridized?

A)C₂H₂
B)H₂CO
C)CH₃Cl
D)C₂H₄
E)C₂H₂Cl₂

Question 59

Benzene C₆H₆) is a cyclic, nonpolar molecule.By removing one of the hydrogens and replacing it with another atom or group, this substituted benzene becomes polar.Which below substituted benzene is the most polar?

A)(C₆H₅F fluorobenzene)
B)(C₆H₅Br bromobenzene)
C)(C₆H₅Cl chlorobenzene)
D)(C₆H₅I iodobenzene)
E)(C₆H₅CH₃ methylbenzene)

Question 60

Which molecule below has a central atom that is sp3 hybridized?

A)C₂H₂
B)H₂CO
C)H₂S
D)C₂H₄
E)C₂H₂Cl₂

Question 61

Ethanol has the formula CH₃CH₂OH.The central carbon atom has a local molecular geometry and hybridization.

A)trigonal planar; sp
B)tetrahedral; sp3
C)tetrahedral; sp2
D)seesaw; sp2
E)seesaw; sp3

Question 62

What type of hybridization is needed to describe the bonding in a seesaw-shaped molecule?

A)sp2
B)sp3
C)sp3d
D)sp
E)sp3d 2

Question 63

Which statement concerning benzene is NOT correct?

A)The electrons in the double bonds are delocalized over the entire carbon ring.
B)All the $\pi$ bonds originate from p atomic orbitals.
C)Benzene does not have a dipole moment.
D)The carbon atomic orbitals are sp² hybridized.
E)Benzene has both long and short carbon-carbon bonds.

Question 64

What is the hybridization of the central xenon atom in XeF₄ , what is its molecular geometry, and what is the F - Xe - F bond angle?

A)sp³, seesaw, 109.5 $\degree$
B)sp³d², square planar, 90 $\degree$
C)sp³d, seesaw, 120 $\degree$
D)sp³d², square planar, 120 $\degree$
E)sp³d, square planar, 90 $\degree$

Question 65

Which molecule below geometry about a carbon atom that is trigonal planar?

A)CH₃CH₂OH
B)CH₃OH
C)C₂H₄
D)CH₃OCH₃
E)C₂H₂

Question 66

Which molecule or ion below has a central atom with the same hybridization as PCl₅?

A)IF₆⁺
B)SiF₄
C)BrF₅
D)SbF₅
E)XeF₄

Question 67

Ethanol has the formula CH₃CH₂OH.The oxygen atom has a local molecular geometry and hybridization.

A)trigonal planar; sp
B)tetrahedral; sp3
C)bent; sp2
D)trigonal planar; sp2
E)bent; sp3

Question 68

What hybridization is needed to describe the square planar molecular geometry of KrF4 ?

A)sp
B)sp2
C)sp3
D)sp3d
E)sp3d 2

Question 69

What is the hybridization of Xe in XeOF₄, and what is the molecular geometry?

A)sp3d, T-shaped
B)sp3d, seesaw
C)sp3d 2, square pyramidal
D)sp3d 2, square planar
E)sp3d 2, octahedral

Question 70

What is the hybridization of the arsenic atom in AsCl₅?

A)sp3
B)sp3d
C)sp3d 2
D)sp
E)sp2

Question 71

What is the hybridization of the iodine atom in ICl₃?

A)sp2
B)sp3d
C)sp3d 2
D)sp3
E)sp

Question 72

What is the hybridization of Cl in ClF₃, and what is the molecular geometry?

A)sp3d, trigonal pyramidal
B)sp3d, T-shaped
C)sp3d, trigonal planar
D)sp3d 2, square planar
E)sp3d 2, octahedral

Question 73

What is the hybridization of I in IF₄⁺, and what is the molecular geometry of the ion?

A)sp³d, seesaw
B)sp³d, T-shaped
C)sp³d, trigonal bipyramidal
D)sp³d ², trigonal planar
E)sp³d ², octahedral

Question 74

Which molecule below has a carbon atom that is sp3 hybridized?

A)C₂H₂
B)C₂HF₃
C)C₂H₄Cl₂
D)C₂H₄
E)C₂H₂Cl₂

Question 75

What type of hybridization is needed to describe the bonding in a T-shaped molecule?

A)sp2
B)sp3
C)sp3d
D)sp
E)sp3d 2

Question 76

Cyclohexane (C₆H₁₂) contains carbon atoms that form a six-member ring.In a valence bond picture of the C - C bonds, hybrid orbitals would overlap for cyclohexane to form bonds.

A)sp; $\sigma$
B)sp²; $\sigma$
C)sp³; $\sigma$
D)sp²; $\pi$
E)sp³; $\pi$

Question 77

Ethanol has the formula CH₃CH₂OH.The end carbon atom has a local molecular geometry and hybridization.

A)trigonal planar; sp
B)tetrahedral; sp3
C)tetrahedral; sp2
D)seesaw; sp2
E)seesaw; sp3

Question 78

The local molecular geometry and the hybridization around each carbon atom in benzene C₆H₆ with a hexagonal ring structure) is

A)square planar and sp.
B)trigonal planar and sp.
C)tetrahedral and sp3.
D)trigonal planar and sp2.
E)T-shaped and sp2.

Question 79

Which statement below about bonds between two carbon atoms is/are TRUE? I) Bond strength increases as more electrons are shared between the atoms.
II) Bond strength increases as the overlap between atomic orbitals increases.
III) Hybrid orbitals account for the observed geometry and bond angles around each carbon atom.

A)I
B)II
C)III
D)Only two of these are correct statements.
E)All three are correct statements.

Question 80

What is the hybridization of the central iodine atom in I₃^- ?

A)sp
B)sp²
C)sp³
D)sp³d²
E)sp³d