The atoms that need hybrid orbitals to describe in BCl 3 molecule should be determined. Concept introduction: According to valence bond theory , The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms. The each overlapping atomic orbital must be contained with a single unpaired. Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis. Pi (π) bonds: the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule. Double bonds: One sigma bond and one pi bond are together known as a double bond.

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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 7.8, Problem 7.8.2SR

Interpretation Introduction

Interpretation:

The atoms that need hybrid orbitals to describe in BCl3 molecule should be determined.

Concept introduction:

According to valence bond theory,

The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.

The each overlapping atomic orbital must be contained with a single unpaired.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.

Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis.

Pi (π) bonds: the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule.

Double bonds: One sigma bond and one pi bond are together known as a double bond.

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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 7.8, Problem 7.8.2SR

Interpretation Introduction

Interpretation:

The atoms that need hybrid orbitals to describe in BCl3 molecule should be determined.

Concept introduction:

According to valence bond theory,

The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.

The each overlapping atomic orbital must be contained with a single unpaired.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.

Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis.

Pi (π) bonds: the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule.

Double bonds: One sigma bond and one pi bond are together known as a double bond.

Expert Solution & Answer

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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 7.8, Problem 7.8.2SR

Interpretation Introduction

Interpretation:

The atoms that need hybrid orbitals to describe in BCl3 molecule should be determined.

Concept introduction:

According to valence bond theory,

The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.

The each overlapping atomic orbital must be contained with a single unpaired.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.

Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis.

Pi (π) bonds: the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule.

Double bonds: One sigma bond and one pi bond are together known as a double bond.

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 7.8, Problem 7.8.2SR

Interpretation Introduction