Question 1

A molecule with the formula AX4 uses _________ to form its bonds.

Accepted Answer

A)  sp hybrid orbitals 
B)  sp2 hybrid orbitals 
C)  sp3 hybrid orbitals 
D)  sp3d hybrid orbitals 
E)  sp3d2 hybrid orbitals 
A)  sp hybrid orbitals 
B)  sp2 hybrid orbitals 
C)  sp3 hybrid orbitals 
D)  sp3d hybrid orbitals 
E)  sp3d2 hybrid orbitals

Question 2

Valence bond theory predicts that sulfur will use _____ hybrid orbitals in sulfur dioxide, SO2.

Accepted Answer

A)  sp 
B)  sp2 
C)  sp3 
D)  sp3d 
E)  sp3d2 
A)  sp 
B)  sp2 
C)  sp3 
D)  sp3d 
E)  sp3d2

Question 3

Valence bond theory predicts that iodine will use _____ hybrid orbitals in ICl2-.

Accepted Answer

A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp3d2 
E)  None of these choices are correct. 
A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp3d2 
E)  None of these choices are correct.

Question 4

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF5.

Accepted Answer

A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp3d2 
E)  None of these choices are correct. 
A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp3d2 
E)  None of these choices are correct.

Question 5

Atoms of period 3 and beyond can undergo sp3d2 hybridization, but atoms of period 2 cannot.

Accepted Answer

A) True 
 B)False

Question 6

Select the correct statement about   -bonds in valence bond theory.

Accepted Answer

A)  A   bond is stronger than a sigma bond. 
B)  A   bond can hold 4 electrons, two above and two below the σ-bond axis. 
C)  A   carbon-carbon double bond consists of two bonds. 
D)  A   bond is the same strength as a σ bond. 
E)  A   bond between two carbon atoms restricts rotation about the C-C axis. 
A)  A   bond is stronger than a sigma bond. 
B)  A   bond can hold 4 electrons, two above and two below the σ-bond axis. 
C)  A   carbon-carbon double bond consists of two bonds. 
D)  A   bond is the same strength as a σ bond. 
E)  A   bond between two carbon atoms restricts rotation about the C-C axis.

Question 7

Valence bond theory explains the bonding in diatomic molecules such as HCl without resorting to the use of hybrid orbitals.

Accepted Answer

A) True 
 B)False

Question 8

Valence bond theory is able to explain why molecular oxygen is paramagnetic.

Accepted Answer

A) True 
 B)False

A molecule with the formula AX₄ uses _________ to form its bonds.

Valence bond theory predicts that sulfur will use _____ hybrid orbitals in sulfur dioxide, SO₂.

Valence bond theory predicts that iodine will use _____ hybrid orbitals in ICl₂^-.

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF₅.

Atoms of period 3 and beyond can undergo sp³d² hybridization, but atoms of period 2 cannot.

Select the correct statement about -bonds in valence bond theory.

Valence bond theory explains the bonding in diatomic molecules such as HCl without resorting to the use of hybrid orbitals.

Valence bond theory is able to explain why molecular oxygen is paramagnetic.

Keys to Studying Chemistry Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Intermolecular Forces Liquids, Solids, and Phase Changes

The Properties of Mixtures Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics Rates and Mechanisms of Chemical Reactions

Equilibrium the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics Entropy, Free Energy, and Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 11: Theories of Covalent Bonding

A molecule with the formula AX4 uses _________ to form its bonds.

Valence bond theory predicts that sulfur will use _____ hybrid orbitals in sulfur dioxide, SO2.

Valence bond theory predicts that iodine will use _____ hybrid orbitals in ICl2-.

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF5.

Atoms of period 3 and beyond can undergo sp3d2 hybridization, but atoms of period 2 cannot.

Select the correct statement about -bonds in valence bond theory.

Valence bond theory explains the bonding in diatomic molecules such as HCl without resorting to the use of hybrid orbitals.

Valence bond theory is able to explain why molecular oxygen is paramagnetic.

Keys to Studying Chemistry Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Intermolecular Forces Liquids, Solids, and Phase Changes

The Properties of Mixtures Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics Rates and Mechanisms of Chemical Reactions

Equilibrium the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics Entropy, Free Energy, and Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

A molecule with the formula AX₄ uses _________ to form its bonds.

Valence bond theory predicts that sulfur will use _____ hybrid orbitals in sulfur dioxide, SO₂.

Valence bond theory predicts that iodine will use _____ hybrid orbitals in ICl₂^-.

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF₅.

Atoms of period 3 and beyond can undergo sp³d² hybridization, but atoms of period 2 cannot.