Question 1

What type of hybridization is needed to explain why ethyne, C2H2, is linear?

Accepted Answer

Question 2

Carbon uses ______ hybrid orbitals in ClCN.

Accepted Answer

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

Question 3

For which one of the following molecules is the indicated type of hybridization not appropriate for the central atom?

Accepted Answer

A)  BeCl2 sp2 
B)  SiH4 sp3 
C)  BF3 sp2 
D)  C2H2 sp 
E)  H2O sp3 
A)  BeCl2 sp2 
B)  SiH4 sp3 
C)  BF3 sp2 
D)  C2H2 sp 
E)  H2O sp3

Question 4

Valence bond theory predicts that carbon will use _____ hybrid orbitals in the carbonate anion, CO32¯.

Accepted Answer

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

Question 5

Determine the shape (geometry) of PCl3 and then decide on the appropriate hybridization of phosphorus in this molecule. (Phosphorus is the central atom.)

Accepted Answer

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

Question 6

In one sentence state the basic principle of valence bond theory.

Accepted Answer

A covalent bond forms when the

Question 7

A) What simple experiment could you perform to show that a substance is paramagnetic?
B) What microscopic (atomic/molecular) feature must a substance possess in order to be paramagnetic?
C) Can it be predicted whether or not all homonuclear diatomic ions, X2+, will be paramagnetic? Explain.

Accepted Answer

a. Place a sample of the substance near

Question 8

The nitrosonium ion, NO+, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which of the following statements about NO+ is correct?

Accepted Answer

A)  NO+ has a bond order of 2 and is paramagnetic. 
B)  NO+ has a bond order of 2 and is diamagnetic. 
C)  NO+ has a bond order of 3 and is paramagnetic. 
D)  NO+ has a bond order of 3 and is diamagnetic. 
E)  None of these choices is correct. 
A)  NO+ has a bond order of 2 and is paramagnetic. 
B)  NO+ has a bond order of 2 and is diamagnetic. 
C)  NO+ has a bond order of 3 and is paramagnetic. 
D)  NO+ has a bond order of 3 and is diamagnetic. 
E)  None of these choices is correct.

Question 9

According to valence bond theory, overlap of bonding orbitals of atoms will weaken a bond, due to electron-electron repulsion.

Accepted Answer

A) True 
 B)False

Question 10

Valence bond theory predicts that tin will use _____ hybrid orbitals in SnF5¯.

Accepted Answer

A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp3d2 
E)  d2sp3 
A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp3d2 
E)  d2sp3

Question 11

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF3.

Accepted Answer

A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp4 
E)  sp3d2 
A)  sp2 
B)  sp3 
C)  sp3d 
D)  sp4 
E)  sp3d2

Question 12

Describe the bonding in ethylene (ethene, C2H4) according to valence bond theory. Be sure to indicate the orbital hybridization on the carbon atoms. Draw a diagram clearly showing at least one bond of each type which occurs in the molecule.

Accepted Answer

The carbon atoms are sp² hybridized, leav

Question 13

In not more than two sentences, explain when and why chemists make use of the concept of hybridization.

Accepted Answer

Chemists postulate hybridizati

Question 14

A molecule with the formula AX2 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 15

A molecule with the formula AX3E uses _________ to form its bonds.

Accepted Answer

A)  s and p atomic orbitals 
B)  sp3 hybrid orbitals 
C)  sp2 hybrid orbitals 
D)  sp hybrid orbitals 
E)  sp3d2 hybrid orbitals 
A)  s and p atomic orbitals 
B)  sp3 hybrid orbitals 
C)  sp2 hybrid orbitals 
D)  sp hybrid orbitals 
E)  sp3d2 hybrid orbitals

Question 16

Which one of the following statements about orbital hybridization is incorrect?

Accepted Answer

A)  The carbon atom in CH4 is sp3 hybridized. 
B)  The carbon atom in CO2 is sp hybridized. 
C)  The nitrogen atom in NH3 is sp2 hybridized. 
D)  sp2 hybrid orbitals are coplanar, and at 120$\degree$ to each other. 
E)  sp hybrid orbitals lie at 180$\degree$to each other. 
A)  The carbon atom in CH4 is sp3 hybridized. 
B)  The carbon atom in CO2 is sp hybridized. 
C)  The nitrogen atom in NH3 is sp2 hybridized. 
D)  sp2 hybrid orbitals are coplanar, and at 120$\degree$ to each other. 
E)  sp hybrid orbitals lie at 180$\degree$to each other.

What type of hybridization is needed to explain why ethyne, C₂H₂, is linear?

Carbon uses ______ hybrid orbitals in ClCN.

For which one of the following molecules is the indicated type of hybridization not appropriate for the central atom?

Valence bond theory predicts that carbon will use _____ hybrid orbitals in the carbonate anion, CO₃^2¯.

Determine the shape (geometry) of PCl₃ and then decide on the appropriate hybridization of phosphorus in this molecule. (Phosphorus is the central atom.)

In one sentence state the basic principle of valence bond theory.

A) What simple experiment could you perform to show that a substance is paramagnetic? B) What microscopic (atomic/molecular) feature must a substance possess in order to be paramagnetic? C) Can it be predicted whether or not all homonuclear diatomic ions, X₂⁺, will be paramagnetic? Explain.

The nitrosonium ion, NO⁺, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which of the following statements about NO⁺ is correct?

According to valence bond theory, overlap of bonding orbitals of atoms will weaken a bond, due to electron-electron repulsion.

Valence bond theory predicts that tin will use _____ hybrid orbitals in SnF₅^¯.

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF₃.

Describe the bonding in ethylene (ethene, C₂H₄) according to valence bond theory. Be sure to indicate the orbital hybridization on the carbon atoms. Draw a diagram clearly showing at least one bond of each type which occurs in the molecule.

In not more than two sentences, explain when and why chemists make use of the concept of hybridization.

A molecule with the formula AX₂ uses _________ to form its bonds.

A molecule with the formula AX₃E uses _________ to form its bonds.

Which one of the following statements about orbital hybridization is incorrect?

Keys to the Study of Chemistry

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 the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 11: Theories of Covalent Bonding

What type of hybridization is needed to explain why ethyne, C2H2, is linear?

Carbon uses ______ hybrid orbitals in ClCN.

For which one of the following molecules is the indicated type of hybridization not appropriate for the central atom?

Valence bond theory predicts that carbon will use _____ hybrid orbitals in the carbonate anion, CO32¯.

Determine the shape (geometry) of PCl3 and then decide on the appropriate hybridization of phosphorus in this molecule. (Phosphorus is the central atom.)

In one sentence state the basic principle of valence bond theory.

A) What simple experiment could you perform to show that a substance is paramagnetic? B) What microscopic (atomic/molecular) feature must a substance possess in order to be paramagnetic? C) Can it be predicted whether or not all homonuclear diatomic ions, X2+, will be paramagnetic? Explain.

The nitrosonium ion, NO+, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which of the following statements about NO+ is correct?

According to valence bond theory, overlap of bonding orbitals of atoms will weaken a bond, due to electron-electron repulsion.

Valence bond theory predicts that tin will use _____ hybrid orbitals in SnF5¯.

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF3.

Describe the bonding in ethylene (ethene, C2H4) according to valence bond theory. Be sure to indicate the orbital hybridization on the carbon atoms. Draw a diagram clearly showing at least one bond of each type which occurs in the molecule.

In not more than two sentences, explain when and why chemists make use of the concept of hybridization.

A molecule with the formula AX2 uses _________ to form its bonds.

A molecule with the formula AX3E uses _________ to form its bonds.

Which one of the following statements about orbital hybridization is incorrect?

Keys to the Study of Chemistry

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 the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

What type of hybridization is needed to explain why ethyne, C₂H₂, is linear?

Valence bond theory predicts that carbon will use _____ hybrid orbitals in the carbonate anion, CO₃^2¯.

Determine the shape (geometry) of PCl₃ and then decide on the appropriate hybridization of phosphorus in this molecule. (Phosphorus is the central atom.)

A) What simple experiment could you perform to show that a substance is paramagnetic? B) What microscopic (atomic/molecular) feature must a substance possess in order to be paramagnetic? C) Can it be predicted whether or not all homonuclear diatomic ions, X₂⁺, will be paramagnetic? Explain.

The nitrosonium ion, NO⁺, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which of the following statements about NO⁺ is correct?

Valence bond theory predicts that tin will use _____ hybrid orbitals in SnF₅^¯.

Valence bond theory predicts that bromine will use _____ hybrid orbitals in BrF₃.

Describe the bonding in ethylene (ethene, C₂H₄) according to valence bond theory. Be sure to indicate the orbital hybridization on the carbon atoms. Draw a diagram clearly showing at least one bond of each type which occurs in the molecule.

A molecule with the formula AX₂ uses _________ to form its bonds.

A molecule with the formula AX₃E uses _________ to form its bonds.