The valence bond description of the bonding in [ N i B r 4 ] 2 − (tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined. Concept introduction: In valence bond theory , the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond. The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands. The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals. With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

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Answer 1

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 20, Problem 20.108SP

(b)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [NiBr4]2−(tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(c)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [Fe( CN)6]3− ( low-spin ) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(d)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [MnCl6]3− (high-spin) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

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Please answer the question and provide a detailed drawing of the structure. If there will not be a new C – C bond, then the box under the drawing area will be checked. Will the following reaction make a molecule with a new C – C bond as its major product: Draw the major organic product or products, if the reaction will work. Be sure you use wedge and dash bonds if necessary, for example to distinguish between major products with different stereochemistry.

Answer 2

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Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 20, Problem 20.108SP

(b)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [NiBr4]2−(tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(c)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [Fe( CN)6]3− ( low-spin ) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(d)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [MnCl6]3− (high-spin) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

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Answer 3

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 20, Problem 20.108SP

(b)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [NiBr4]2−(tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(c)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [Fe( CN)6]3− ( low-spin ) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(d)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [MnCl6]3− (high-spin) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

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Answer 4

Question

Definition Definition Theory that explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. VBT gives a quantum mechanical approach to the formation of covalent bonds with the help of wave functions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.

Chapter 20, Problem 20.108SP

(b)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [NiBr4]2−(tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(c)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [Fe( CN)6]3− ( low-spin ) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(d)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [MnCl6]3− (high-spin) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

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Answer 5

Chapter 20, Problem 20.108SP

(b)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [NiBr4]2−(tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(c)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [Fe( CN)6]3− ( low-spin ) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

(d)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [MnCl6]3− (high-spin) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

Answer 6

Chapter 20, Problem 20.108SP

(b)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [NiBr4]2−(tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

Answer 7

Chapter 20, Problem 20.108SP

(b)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [NiBr4]2−(tetrahedral) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

Answer 8

(c)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [Fe( CN)6]3− ( low-spin ) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

Answer 9

(c)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [Fe( CN)6]3− ( low-spin ) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

Answer 10

(d)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [MnCl6]3− (high-spin) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

Answer 11

(d)

Interpretation Introduction

Interpretation:

The valence bond description of the bonding in [MnCl6]3− (high-spin) complex, orbital diagram and which hybrid orbital of the metal ions are used for bonding with a specific number of unpaired electrons should be determined.

Concept introduction:

In valence bond theory, the donation of pairs of electrons by ligands to the central metal atom or ion results in the metal-ligand bond.
The metal ion possesses a requisite number of valence orbitals of almost equal energy in order to accommodate the electrons given by ligands.
The unpaired (n-1) d electrons, pair up as fully as possible prior to hybridization thus making some (n-1) d orbitals vacant. The central metal atom then makes available the number of empty orbitals equal to its coordination number for the formation of coordinate bonds with suitable ligand orbitals.
With the approach of the ligands, metal-ligand bonds are then formed by the overlap of these orbitals with those of the ligands, that is by donation of electron pairs by the ligands to the empty hybridized orbitals.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 20 - Prob. 20.1P Ch. 20 - Prob. 20.2A Ch. 20 - Prob. 20.3P Ch. 20 - Prob. 20.4P Ch. 20 - Prob. 20.5P Ch. 20 - Prob. 20.6P Ch. 20 - Prob. 20.7A Ch. 20 - Prob. 20.8P Ch. 20 - Prob. 20.9P Ch. 20 - Prob. 20.10A

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