A molecule with the formula AX4E uses _________ to form its bonds.

A) sp2 hybrid orbitals B) sp3 hybrid orbitals C) sp3d hybrid orbitals D) sp3d2 hybrid orbitals E) none of the above A) sp2 hybrid orbitals B) sp3 hybrid orbitals C) sp3d hybrid orbitals D) sp3d2 hybrid orbitals E) none of the above

Exam 11: Theories of Covalent Bonding

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.

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Question 1

Correct Answer:

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The carbon atoms are sp² hybridized, leaving the 2p_z orbital on each carbon unhybridized. Overlap of one sp² hybrid on each carbon and occupation of this region by an electron pair produces a C-C  bond. Overlap of the remaining four hybrid orbitals with 1s orbitals of four hydrogen atoms, produces four C-H  bonds. The unhybridized 2p_z orbitals overlap laterally to produce a  bond which has two regions of electron density, above and below the C-C  bond. (Diagram needed.)

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.

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Question 2

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a. Place a sample of the substance near a magnet; if it is attracted to the magnet, it is paramagnetic.
b. The substance must have unpaired electrons in order to be paramagnetic.
c. Yes, they will necessarily be paramagnetic since each will have an odd number of electrons.

In the valence bond treatment, overlap of an s orbital on one atom with an sp³ orbital on another atom can give rise to a  bond.

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(True/False)

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Question 3

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True

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

(Short Answer)

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Question 4

Atoms of period 3 and beyond can undergo sp³d ² hybridization, but atoms of period 2 cannot.

(True/False)

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Question 5

The angles between sp² hybrid orbitals are 109.5°.

(True/False)

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Question 6

In the valence bond treatment, a  bond is formed when two 2p orbitals overlap side to side.

(True/False)

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Question 7

A molecule with the formula AX₄E uses _________ to form its bonds.

(Multiple Choice)

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Question 8

Sketch the shapes of the ₁_s and ₁_s* molecular orbitals formed by the overlap of two hydrogen 1s atomic orbitals.

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Question 9

Which of the following statements relating to molecular orbital (MO) theory is incorrect?

(Multiple Choice)

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Question 10

Explain what is meant by the term "bond order" and describe how it can be calculated using the information in a molecular orbital energy level diagram.

(Essay)

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Question 11

In applying molecular orbital theory, the bond order is calculated in the same way as with Lewis structures.

(True/False)

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Question 12

According to valence bond theory, which orbitals on N and H overlap in the NH₃molecule?

(Multiple Choice)

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Question 13

Explain what is meant by a node (or nodal plane) in a molecular orbital and draw sketches of the following orbitals, indicating at least one nodal plane in each one. a. a * orbital b. a * orbital

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Question 14

When PCl₅solidifies it forms PCl₄⁺ cations and PCl₆^-anions. According to valence bond theory, what hybrid orbitals are used by phosphorus in the PCl₄⁺ cations?

(Multiple Choice)

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Question 15

According to molecular orbital theory, what is the bond order in the O₂⁺ ion?

(Multiple Choice)

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Question 16

Hybrid orbitals of the sp³d type occur in sets of four.

(True/False)

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Question 17

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

(True/False)

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Question 18

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

(True/False)

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Question 19

Valence bond theory predicts that xenon will use _____ hybrid orbitals in XeOF₄.

(Multiple Choice)

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Question 20

Showing 1 - 20 of 58

Exam 11: Theories of Covalent Bonding

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. 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.

In the valence bond treatment, overlap of an s orbital on one atom with an sp3 orbital on another atom can give rise to a  bond.

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

Atoms of period 3 and beyond can undergo sp3d 2 hybridization, but atoms of period 2 cannot.

The angles between sp2 hybrid orbitals are 109.5°.

In the valence bond treatment, a  bond is formed when two 2p orbitals overlap side to side.

A molecule with the formula AX4E uses _________ to form its bonds.

Sketch the shapes of the 1s and 1s* molecular orbitals formed by the overlap of two hydrogen 1s atomic orbitals.

Which of the following statements relating to molecular orbital (MO) theory is incorrect?

Explain what is meant by the term "bond order" and describe how it can be calculated using the information in a molecular orbital energy level diagram.

In applying molecular orbital theory, the bond order is calculated in the same way as with Lewis structures.

According to valence bond theory, which orbitals on N and H overlap in the NH3 molecule?

Explain what is meant by a node (or nodal plane) in a molecular orbital and draw sketches of the following orbitals, indicating at least one nodal plane in each one. a. a * orbital b. a * orbital

When PCl5 solidifies it forms PCl4+ cations and PCl6- anions. According to valence bond theory, what hybrid orbitals are used by phosphorus in the PCl4+ cations?

According to molecular orbital theory, what is the bond order in the O2+ ion?

Hybrid orbitals of the sp3d type occur in sets of four.

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

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

Valence bond theory predicts that xenon will use _____ hybrid orbitals in XeOF4.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The 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: Bonding, Structure, and Reactivity

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

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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. 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.

In the valence bond treatment, overlap of an s orbital on one atom with an sp³ orbital on another atom can give rise to a  bond.

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

Atoms of period 3 and beyond can undergo sp³d ² hybridization, but atoms of period 2 cannot.

The angles between sp² hybrid orbitals are 109.5°.

A molecule with the formula AX₄E uses _________ to form its bonds.

Sketch the shapes of the ₁_s and ₁_s* molecular orbitals formed by the overlap of two hydrogen 1s atomic orbitals.

According to valence bond theory, which orbitals on N and H overlap in the NH₃molecule?

When PCl₅solidifies it forms PCl₄⁺ cations and PCl₆^-anions. According to valence bond theory, what hybrid orbitals are used by phosphorus in the PCl₄⁺ cations?

According to molecular orbital theory, what is the bond order in the O₂⁺ ion?

Hybrid orbitals of the sp³d type occur in sets of four.

Valence bond theory predicts that xenon will use _____ hybrid orbitals in XeOF₄.