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.

Question

Want to see the full answer?

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

These are in the wrong boxes. Why does the one on the left have a lower molar mass than the one on the right?

SYNTHESIS REACTIONS. For the following reactions, synthesize the given products from the given reactants. Multiple reactions/steps will be needed. For the one of the steps (ie reactions) in each synthesis, write out the mechanism for that reaction and draw an energy diagram showing the correct number of hills and valleys for that step's mechanism. CI b. a. Use acetylene (ethyne) and any alkyl halide as your starting materials Br C. d. "OH OH III. OH

Calculate the pH and the pOH of each of the following solutions at 25 °C for which the substances ionize completely: (a) 0.200 M HCl

Answer 2

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

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

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

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

Concept explainers

Want to see the full answer?

Chapter 20 Solutions