The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of − C O 2 − has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified. Concept Introduction Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance. All the possible resonance structures are imaginary whereas the resonance hybrid is real. These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei. Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization. sp 3 hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital. sp 2 hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals. sp hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital. Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis. Pi (π) bonds are 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.

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Answer 1

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Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $−CO2−$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.

All the possible resonance structures are imaginary whereas the resonance hybrid is real.

These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.

$sp3$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

$sp2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$sp$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.

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Answer 2

Question

Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $−CO2−$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.

All the possible resonance structures are imaginary whereas the resonance hybrid is real.

These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.

$sp3$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

$sp2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$sp$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.

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Answer 3

Question

Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $−CO2−$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.

All the possible resonance structures are imaginary whereas the resonance hybrid is real.

These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.

$sp3$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

$sp2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$sp$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.

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Answer 4

Question

Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $−CO2−$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.

All the possible resonance structures are imaginary whereas the resonance hybrid is real.

These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.

$sp3$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

$sp2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$sp$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.

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Answer 5

Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $−CO2−$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.

All the possible resonance structures are imaginary whereas the resonance hybrid is real.

These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.

$sp3$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

$sp2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$sp$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.

Answer 6

Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $−CO2−$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.

All the possible resonance structures are imaginary whereas the resonance hybrid is real.

These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.

$sp3$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

$sp2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$sp$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.

Answer 7

Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $−CO2−$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.

All the possible resonance structures are imaginary whereas the resonance hybrid is real.

These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.

$sp3$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

$sp2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$sp$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 9.1 - Use valence bond theory to describe the bonding in...Ch. 9.1 - Identify the hybridization of each underlined atom...Ch. 9.1 - Use valence bond theory to describe the bonding in...Ch. 9.2 - What is the electron configuration of the H2+ ion?...Ch. 9.2 - Could the anion Li2 exist? What is the ions bond...Ch. 9.2 - The cations O2+ and N2+ are formed when molecules...Ch. 9.3 - Photoelectron spectroscopy is s1milar to the...Ch. 9.3 - What is the energy of a photon with a wavelength...Ch. 9.3 - Using the accompanying figure, state which...Ch. 9.3 - The kinetic energy of an electron ejected from the...

Solution Summary: The author explains the two possible structures of acetate ion: the hybridization of the carbon atoms of -CO_2- and the orbitals that overlap to form bonds

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