The chemical according to the Lewis model, valence bond theory, and the molecular orbital theory. Also, indicate the strength and the weakness of each theory. Concept Introduction: As per Lewis model, a chemical bond is the transfer or sharing of electrons represented as dots. The Lewis theory of bonding allows us to make qualitative calculations about bond strengths and bond lengths. According to valence bond theory, a chemical bond is the overlap of two half-filled atomic orbitals. Valence bond theory defines the formation of covalent bonds as the overlap of atomic orbitals. In molecular orbital theory, atoms will join together (a chemical bond) when the electrons in theatoms can lower energy by occupying the molecular orbitals of the resultant molecule.

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Answer 1

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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 10, Problem 30E

Interpretation Introduction

Interpretation: The chemical according to the Lewis model, valence bond theory, and the molecular orbital theory. Also, indicate the strength and the weakness of each theory.

Concept Introduction:

As per Lewis model, a chemical bond is the transfer or sharing of electrons represented as dots. The Lewis theory of bonding allows us to make qualitative calculations about bond strengths and bond lengths. According to valence bond theory, a chemical bond is the overlap of two half-filled atomic orbitals. Valence bond theory defines the formation of covalent bonds as the overlap of atomic orbitals. In molecular orbital theory, atoms will join together (a chemical bond) when the electrons in theatoms can lower energy by occupying the molecular orbitals of the resultant molecule.

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a) Draw the octahedral mer-[FeCl3(CN)3] complex and determine its point group. Use proper wedges and dashes in order to illustrate 3 dimensional details. Use the point group to determine if the complex has a resulting net dipole moment and describe its allowed direction with respect to its symmetry elements (if applicable). ード M 4- b) Substitute one chlorido ligand in mer-[FeCl3(CN)3] 4 with one fluorido ligand. Determine all possible isomers and their corresponding point groups. Use the point groups to determine if the complexes have resulting net dipole moments and describe their allowed direction with respect to its symmetry elements (if applicable). The number of complex sketches below is not necessarily indicative of the number of isomers. 4- 4- ☐☐☐ c) Substitute two chlorido ligands in mer-[FeCl3 (CN)3] 4 with two fluorido ligands. Determine all possible isomers and their corresponding point groups.. Use the point groups to determine if the complexes have resulting net dipole…

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Differentiate electron spin and electron spin moment.

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 10, Problem 30E

Interpretation Introduction

Interpretation: The chemical according to the Lewis model, valence bond theory, and the molecular orbital theory. Also, indicate the strength and the weakness of each theory.

Concept Introduction:

As per Lewis model, a chemical bond is the transfer or sharing of electrons represented as dots. The Lewis theory of bonding allows us to make qualitative calculations about bond strengths and bond lengths. According to valence bond theory, a chemical bond is the overlap of two half-filled atomic orbitals. Valence bond theory defines the formation of covalent bonds as the overlap of atomic orbitals. In molecular orbital theory, atoms will join together (a chemical bond) when the electrons in theatoms can lower energy by occupying the molecular orbitals of the resultant molecule.

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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 10, Problem 30E

Interpretation Introduction

Interpretation: The chemical according to the Lewis model, valence bond theory, and the molecular orbital theory. Also, indicate the strength and the weakness of each theory.

Concept Introduction:

As per Lewis model, a chemical bond is the transfer or sharing of electrons represented as dots. The Lewis theory of bonding allows us to make qualitative calculations about bond strengths and bond lengths. According to valence bond theory, a chemical bond is the overlap of two half-filled atomic orbitals. Valence bond theory defines the formation of covalent bonds as the overlap of atomic orbitals. In molecular orbital theory, atoms will join together (a chemical bond) when the electrons in theatoms can lower energy by occupying the molecular orbitals of the resultant molecule.

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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 10, Problem 30E

Interpretation Introduction