Question 1

Which statement regarding aF1F1F1S1F1F1F10 bond between two carbon atoms is not correct?

Accepted Answer

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. 
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 2

Which statement A-D about valence bond theory is not correct?

Accepted Answer

A) Valence bond theory describes a bond as the overlap of atomic orbitals between two atoms. 
B) Enhanced electron density between two positively charged nuclei attracts the nuclei together and forms the bond. 
C) Hybridization of atomic orbitals is necessary to account for the molecular geometry. 
D) In valence bond theory, hybridization determines the molecular shape or geometry. 
E) Statements A-D are all correct. 
A) Valence bond theory describes a bond as the overlap of atomic orbitals between two atoms. 
B) Enhanced electron density between two positively charged nuclei attracts the nuclei together and forms the bond. 
C) Hybridization of atomic orbitals is necessary to account for the molecular geometry. 
D) In valence bond theory, hybridization determines the molecular shape or geometry. 
E) Statements A-D are all correct.

Question 3

Which statement about the shape or geometry of a molecule is not correct?

Accepted Answer

A) Physical properties of a substance are not affected by the shape of the molecules. 
B) The shape of a molecule refers to the three-dimensional arrangement of the atoms in space. 
C) Solubility of a substance in a solvent is affected by the shape of the molecules. 
D) Taste and aroma of a substance are affected by the shape of the molecules. 
E) Biological activity and chemical reactivity of a substance are affected by the shape of the molecules. 
A) Physical properties of a substance are not affected by the shape of the molecules. 
B) The shape of a molecule refers to the three-dimensional arrangement of the atoms in space. 
C) Solubility of a substance in a solvent is affected by the shape of the molecules. 
D) Taste and aroma of a substance are affected by the shape of the molecules. 
E) Biological activity and chemical reactivity of a substance are affected by the shape of the molecules.

Question 4

Why does the seesaw molecular geometry (ss) have a lower energy than the trigonal pyramidal molecular geometry (tp) in an AB4 molecule with a trigonal bipyramidal electron-pair geometry?

Accepted Answer

A) The ss geometry has fewer lone-pair bonding-pair interactions at 90o. 
B) The ss geometry has fewer lone-pair bonding-pair interactions at 120o. 
C) The ss geometry has fewer bonding-pair bonding-pair interactions at 120o. 
D) The ss geometry has fewer bonding-pair bonding-pair interactions at 90o. 
E) The ss geometry has fewer lone-pair lone-pair interactions at 90o. 
A) The ss geometry has fewer lone-pair bonding-pair interactions at 90o. 
B) The ss geometry has fewer lone-pair bonding-pair interactions at 120o. 
C) The ss geometry has fewer bonding-pair bonding-pair interactions at 120o. 
D) The ss geometry has fewer bonding-pair bonding-pair interactions at 90o. 
E) The ss geometry has fewer lone-pair lone-pair interactions at 90o.

Question 5

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

Accepted Answer

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

Question 6

Use the relative energies of the molecular orbitals given below, which are derived from the n = 5 atomic orbitals, to determine the bond orders in I2 , I2F1F1F1S1F1F1F10, and  I2F1F1F1S1F1F1F10, and identify the species that is predicted to be the most stable. The valence molecular orbitals in order of increasing energy are F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10* F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10* F1F1F1S1F1F1F10 F1F1F1S1F1F1F10*.

Accepted Answer

The valence electron configuration of I₂F

Question 7

Both diazene (N2H2) and hydrazine (N2H4) have two nitrogen atoms bonded together. In a valence bond picture of the N-N bonds, ________ hybrid orbitals overlap for diazene and ________ hybrid orbitals overlap for hydrazine.

Accepted Answer

A) sp; sp 
B) sp; sp2 
C) sp2; sp3 
D) sp3; sp2 
E) sp2; sp 
A) sp; sp 
B) sp; sp2 
C) sp2; sp3 
D) sp3; sp2 
E) sp2; sp

Question 8

What is the molecular geometry of SF4O?

Accepted Answer

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

Question 9

What is the hybridization of the central iodine atom in I3F1F1F1S1F1F1F10?

Accepted Answer

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

Question 10

Which of the following can be used to increase the conductivity of any semimetal?
I.adding an element with one additional valence electron
II.adding an element with one fewer valence electron
III.lowering the temperature

Accepted Answer

A) I only 
B) II only 
C) III only 
D) I and II only 
E) I, II, and III 
A) I only 
B) II only 
C) III only 
D) I and II only 
E) I, II, and III

Question 11

Which one of the following species has four electrons in antibonding F1F1F1S1F1F1F10 molecular orbitals?

Accepted Answer

A) C22F1F1F1S1F1F1F10 
B) O2F1F1F1S1F1F1F10 
C) N22F1F1F1S1F1F1F10 
D) Br2F1F1F1S1F1F1F10 
E) Br22F1F1F1S1F1F1F10 
A) C22F1F1F1S1F1F1F10 
B) O2F1F1F1S1F1F1F10 
C) N22F1F1F1S1F1F1F10 
D) Br2F1F1F1S1F1F1F10 
E) Br22F1F1F1S1F1F1F10

Question 12

What is the molecular geometry of the triiodide ion (I3F1F1F1S1F1F1F10)?

Accepted Answer

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

Question 13

In the following molecules, what orbitals are involved in bonding on both of the indicated atoms?

Accepted Answer

Molecule 1: sp³ orbital on carbon overlap

Question 14

Which of the following molecules has a carbon atom that is sp3 hybridized?

Accepted Answer

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

Question 15

When Si is doped with P, it produces a(n) ________-type semiconductor.

Accepted Answer

A) p 
B) n 
C) q 
D) np 
E) No semiconductor will be produced. 
A) p 
B) n 
C) q 
D) np 
E) No semiconductor will be produced.

Question 16

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the bond order of the oxygen molecule O2 and the peroxide anion O22F1F1F1S1F1F1F10.

Accepted Answer

A) oxygen (bond order = 2); peroxide (bond order = 3) 
B) oxygen (bond order = 2); peroxide (bond order = 2) 
C) oxygen (bond order = 4); peroxide (bond order = 4) 
D) oxygen (bond order = 4); peroxide (bond order = 5) 
E) oxygen (bond order = 2); peroxide (bond order = 1) 
A) oxygen (bond order = 2); peroxide (bond order = 3) 
B) oxygen (bond order = 2); peroxide (bond order = 2) 
C) oxygen (bond order = 4); peroxide (bond order = 4) 
D) oxygen (bond order = 4); peroxide (bond order = 5) 
E) oxygen (bond order = 2); peroxide (bond order = 1)

Question 17

Which of the following compounds has the smallest dipole moment?

Accepted Answer

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

Question 18

When silicon is doped with gallium, electrical conduction increases because ________

Accepted Answer

A) gallium has fewer valence electrons than silicon, so holes are created in the valence band of silicon. 
B) gallium has more valence electrons than silicon, so electrons are added to the conduction band of silicon. 
C) gallium causes electrons to be transferred from the valence band of silicon to the conduction band of silicon. 
D) gallium causes electrons to be transferred from the conduction band of silicon to the valence band of silicon. 
E) gallium is a better conductor of electricity than silicon. 
A) gallium has fewer valence electrons than silicon, so holes are created in the valence band of silicon. 
B) gallium has more valence electrons than silicon, so electrons are added to the conduction band of silicon. 
C) gallium causes electrons to be transferred from the valence band of silicon to the conduction band of silicon. 
D) gallium causes electrons to be transferred from the conduction band of silicon to the valence band of silicon. 
E) gallium is a better conductor of electricity than silicon.

Question 19

Which electron-pair geometry corresponds to a steric number of 6?

Accepted Answer

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

Question 20

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

Accepted Answer

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

Exam 9: Molecular Geometry: Shape Determines Function

Which statement regarding a bond between two carbon atoms is not correct?

Which statement A-D about valence bond theory is not correct?

Which statement about the shape or geometry of a molecule is not correct?

Why does the seesaw molecular geometry (ss) have a lower energy than the trigonal pyramidal molecular geometry (tp) in an AB4 molecule with a trigonal bipyramidal electron-pair geometry?

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

Both diazene (N2H2) and hydrazine (N2H4) have two nitrogen atoms bonded together. In a valence bond picture of the N-N bonds, ________ hybrid orbitals overlap for diazene and ________ hybrid orbitals overlap for hydrazine.

What is the molecular geometry of SF4O?

What is the hybridization of the central iodine atom in I3?

Which of the following can be used to increase the conductivity of any semimetal? I.adding an element with one additional valence electron II.adding an element with one fewer valence electron III.lowering the temperature

Which one of the following species has four electrons in antibonding  molecular orbitals?

What is the molecular geometry of the triiodide ion (I3)?

In the following molecules, what orbitals are involved in bonding on both of the indicated atoms?

Which of the following molecules has a carbon atom that is sp3 hybridized?

When Si is doped with P, it produces a(n) ________-type semiconductor.

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the bond order of the oxygen molecule O2 and the peroxide anion O22.

Which of the following compounds has the smallest dipole moment?

When silicon is doped with gallium, electrical conduction increases because ________

Which electron-pair geometry corresponds to a steric number of 6?

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

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Why does the seesaw molecular geometry (ss) have a lower energy than the trigonal pyramidal molecular geometry (tp) in an AB₄ molecule with a trigonal bipyramidal electron-pair geometry?

Both diazene (N₂H₂) and hydrazine (N₂H₄) have two nitrogen atoms bonded together. In a valence bond picture of the N-N bonds, hybrid orbitals overlap for diazene and hybrid orbitals overlap for hydrazine.

What is the molecular geometry of SF₄O?

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

What is the molecular geometry of the triiodide ion (I₃^)?

Which of the following molecules has a carbon atom that is sp³ hybridized?

Use energy levels of diatomic molecules derived from molecular orbital theory to predict the bond order of the oxygen molecule O₂ and the peroxide anion O₂²^.

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