A molecular orbital energy level diagram for O 2 + has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown. The bond order in O 2 + has to be predicted and whether O-O bond is longer or shorter than O 2 should be explained. Concept Introduction: Molecular orbital theory: Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below. Atomic orbital of equal energy combine together to form molecular orbital. Shape of molecular orbital depends on the shapes of combining atomic orbital. Bonding orbitals are denoted by σ , π and δ and antibonding orbital are denoted by σ ∗ , π ∗ and δ ∗ . Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle. A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

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Answer 1

Question

Chapter 18, Problem 18.77SP

(a)

Interpretation Introduction

Interpretation:

A molecular orbital energy level diagram for O2+ has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown.

The bond order in O2+ has to be predicted and whether O-O bond is longer or shorter than O2 should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

(b)

Interpretation Introduction

Interpretation:

Whether O2+ is paramagnetic or diamagnetic should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Paramagnetic and diamagnetic nature:

If all electrons in the molecule are paired, the substance is diamagnetic nature and substance has unpaired electron(s) are called paramagnetic nature.

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Answer 2

Question

Chapter 18, Problem 18.77SP

(a)

Interpretation Introduction

Interpretation:

A molecular orbital energy level diagram for O2+ has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown.

The bond order in O2+ has to be predicted and whether O-O bond is longer or shorter than O2 should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

(b)

Interpretation Introduction

Interpretation:

Whether O2+ is paramagnetic or diamagnetic should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Paramagnetic and diamagnetic nature:

If all electrons in the molecule are paired, the substance is diamagnetic nature and substance has unpaired electron(s) are called paramagnetic nature.

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Answer 3

Question

Chapter 18, Problem 18.77SP

(a)

Interpretation Introduction

Interpretation:

A molecular orbital energy level diagram for O2+ has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown.

The bond order in O2+ has to be predicted and whether O-O bond is longer or shorter than O2 should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

(b)

Interpretation Introduction

Interpretation:

Whether O2+ is paramagnetic or diamagnetic should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Paramagnetic and diamagnetic nature:

If all electrons in the molecule are paired, the substance is diamagnetic nature and substance has unpaired electron(s) are called paramagnetic nature.

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Answer 4

Question

Chapter 18, Problem 18.77SP

(a)

Interpretation Introduction

Interpretation:

A molecular orbital energy level diagram for O2+ has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown.

The bond order in O2+ has to be predicted and whether O-O bond is longer or shorter than O2 should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

(b)

Interpretation Introduction

Interpretation:

Whether O2+ is paramagnetic or diamagnetic should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Paramagnetic and diamagnetic nature:

If all electrons in the molecule are paired, the substance is diamagnetic nature and substance has unpaired electron(s) are called paramagnetic nature.

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Answer 5

Chapter 18, Problem 18.77SP

(a)

Interpretation Introduction

Interpretation:

A molecular orbital energy level diagram for O2+ has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown.

The bond order in O2+ has to be predicted and whether O-O bond is longer or shorter than O2 should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

(b)

Interpretation Introduction

Interpretation:

Whether O2+ is paramagnetic or diamagnetic should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Paramagnetic and diamagnetic nature:

If all electrons in the molecule are paired, the substance is diamagnetic nature and substance has unpaired electron(s) are called paramagnetic nature.

Answer 6

Chapter 18, Problem 18.77SP

(a)

Interpretation Introduction

Interpretation:

A molecular orbital energy level diagram for O2+ has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown.

The bond order in O2+ has to be predicted and whether O-O bond is longer or shorter than O2 should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Answer 7

Chapter 18, Problem 18.77SP

(a)

Interpretation Introduction

Interpretation:

A molecular orbital energy level diagram for O2+ has to be drawn with MOs derived from the Oxygen 2p orbitals. Also the electron population of MOs is to be shown.

The bond order in O2+ has to be predicted and whether O-O bond is longer or shorter than O2 should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Whether O2+ is paramagnetic or diamagnetic should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Paramagnetic and diamagnetic nature:

If all electrons in the molecule are paired, the substance is diamagnetic nature and substance has unpaired electron(s) are called paramagnetic nature.

Answer 9

(b)

Interpretation Introduction

Interpretation:

Whether O2+ is paramagnetic or diamagnetic should be explained.

Concept Introduction:

Molecular orbital theory:

Molecular orbital theory states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbital called molecular orbital. A brief outline of this theory is given below.

Atomic orbital of equal energy combine together to form molecular orbital.

Shape of molecular orbital depends on the shapes of combining atomic orbital.

Bonding orbitals are denoted by σ, π and δ and antibonding orbital are denoted by σ∗, π∗ and δ∗.

Molecular orbital are filled in increasing order of their energies, starting with orbital of least energy. This is called Aufbau principle.

A molecular orbital is filled with only two electrons with opposite spins. This is called Paul’s exclusion principle.

Paramagnetic and diamagnetic nature:

If all electrons in the molecule are paired, the substance is diamagnetic nature and substance has unpaired electron(s) are called paramagnetic nature.

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 18.1 - Prob. 18.1P Ch. 18.1 - Prob. 18.2P Ch. 18.2 - Prob. 18.3P Ch. 18.3 - Write the chemical formula of a compound that...Ch. 18.4 - Prob. 18.5P Ch. 18.4 - Prob. 18.6CP Ch. 18.4 - Prob. 18.7P Ch. 18.8 - Prob. 18.8CP Ch. 18.8 - Prob. 18.9P Ch. 18.9 - Prob. 18.10P

Solution Summary: The author explains Molecular orbital theory, which states that atomic orbitals lose their individuality and electrons of the molecule present in the new orbit.

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Chapter 18 Solutions