The bond angle from the unhybridized orbitals and the valence bond theory is agree with the experimentally measured bond angle of 98.2 0 . Concept Introduction: In case of sigma bond, the bonding electron pair shared with atom lies additional from the chief metal atom that has a lone pair of that atom. This is known as lone pair–bond pair repulsion. S F 2 Has hybridization of s p 3 . Thus, it has tetrahedral structure. Angle for a tetrahedral structure is 109.5 degrees. In SF 2 , sulfur has configuration [ Ne ] 3 s 2 3 p 4 .

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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 56E

Interpretation Introduction

Interpretation: The bond angle from the unhybridized orbitals and the valence bond theory is agree with the experimentally measured bond angle of 98.2⁰.

Concept Introduction:

In case of sigma bond, the bonding electron pair shared with atom lies additional from the chief metal atom that has a lone pair of that atom. This is known as lone pair–bond pair repulsion.

SF2 Has hybridization of sp3. Thus, it has tetrahedral structure. Angle for a tetrahedral structure is 109.5 degrees.

In SF2, sulfur has configuration [Ne]3s23p4.

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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 56E

Interpretation Introduction

Interpretation: The bond angle from the unhybridized orbitals and the valence bond theory is agree with the experimentally measured bond angle of 98.2⁰.

Concept Introduction:

In case of sigma bond, the bonding electron pair shared with atom lies additional from the chief metal atom that has a lone pair of that atom. This is known as lone pair–bond pair repulsion.

SF2 Has hybridization of sp3. Thus, it has tetrahedral structure. Angle for a tetrahedral structure is 109.5 degrees.

In SF2, sulfur has configuration [Ne]3s23p4.

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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 56E

Interpretation Introduction

Interpretation: The bond angle from the unhybridized orbitals and the valence bond theory is agree with the experimentally measured bond angle of 98.2⁰.

Concept Introduction:

In case of sigma bond, the bonding electron pair shared with atom lies additional from the chief metal atom that has a lone pair of that atom. This is known as lone pair–bond pair repulsion.

SF2 Has hybridization of sp3. Thus, it has tetrahedral structure. Angle for a tetrahedral structure is 109.5 degrees.

In SF2, sulfur has configuration [Ne]3s23p4.

Expert Solution & Answer

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Check out a sample textbook solution

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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 56E

Interpretation Introduction