The molecular shape of C H C l 3 is to be determined. Concept introduction: In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule. Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model. -Draw the Lewis structure. -Count the number of valence electron pairs (bond pairs and lone pairs). -Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible. -If there are only two valence electron pairs, the molecule is linear. -If there are three valence electron pairs, the molecule is shaped like an equilateral triangle. -If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

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Answer 1

Question

Chapter 4.8, Problem 4.15P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of CHCl3 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Draw the Lewis structure.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

-If there are only two valence electron pairs, the molecule is linear.

-If there are three valence electron pairs, the molecule is shaped like an equilateral triangle.

-If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

(b)

Interpretation Introduction

Interpretation:

The molecular shape of Cl2C=CH2 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

- Multiple bonded atoms located in a plane.

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Answer 2

Question

Chapter 4.8, Problem 4.15P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of CHCl3 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Draw the Lewis structure.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

-If there are only two valence electron pairs, the molecule is linear.

-If there are three valence electron pairs, the molecule is shaped like an equilateral triangle.

-If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

(b)

Interpretation Introduction

Interpretation:

The molecular shape of Cl2C=CH2 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

- Multiple bonded atoms located in a plane.

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Answer 3

Question

Chapter 4.8, Problem 4.15P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of CHCl3 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Draw the Lewis structure.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

-If there are only two valence electron pairs, the molecule is linear.

-If there are three valence electron pairs, the molecule is shaped like an equilateral triangle.

-If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

(b)

Interpretation Introduction

Interpretation:

The molecular shape of Cl2C=CH2 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

- Multiple bonded atoms located in a plane.

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Answer 4

Question

Chapter 4.8, Problem 4.15P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of CHCl3 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Draw the Lewis structure.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

-If there are only two valence electron pairs, the molecule is linear.

-If there are three valence electron pairs, the molecule is shaped like an equilateral triangle.

-If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

(b)

Interpretation Introduction

Interpretation:

The molecular shape of Cl2C=CH2 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

- Multiple bonded atoms located in a plane.

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Answer 5

Chapter 4.8, Problem 4.15P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of CHCl3 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Draw the Lewis structure.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

-If there are only two valence electron pairs, the molecule is linear.

-If there are three valence electron pairs, the molecule is shaped like an equilateral triangle.

-If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

(b)

Interpretation Introduction

Interpretation:

The molecular shape of Cl2C=CH2 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

- Multiple bonded atoms located in a plane.

Answer 6

Chapter 4.8, Problem 4.15P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of CHCl3 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Draw the Lewis structure.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

-If there are only two valence electron pairs, the molecule is linear.

-If there are three valence electron pairs, the molecule is shaped like an equilateral triangle.

-If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

Answer 7

Chapter 4.8, Problem 4.15P

(a)

Interpretation Introduction

Interpretation:

The molecular shape of CHCl3 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Draw the Lewis structure.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

-If there are only two valence electron pairs, the molecule is linear.

-If there are three valence electron pairs, the molecule is shaped like an equilateral triangle.

-If there are four valence electron pairs, the molecule is shaped as a regular tetrahedral.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The molecular shape of Cl2C=CH2 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

- Multiple bonded atoms located in a plane.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The molecular shape of Cl2C=CH2 is to be determined.

Concept introduction:

In a Lewis structure, lines are represented for the bonding between atoms of a molecule and the dots for the lone pairs of electrons that may exist in the molecule.

Molecular shape can be predicted from the Lewis structure by using the valence-shell Electron-pair repulsion (VSEPR) model.

-Count the number of valence electron pairs (bond pairs and lone pairs).

-Assume that the valence electron pairs form a structure that allows them to be as far away from each other as possible.

- Multiple bonded atoms located in a plane.

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 4.1 - Prob. 4.1P Ch. 4.2 - Prob. 4.2P Ch. 4.2 - Prob. 4.3P Ch. 4.3 - Prob. 4.4P Ch. 4.3 - Prob. 4.5P Ch. 4.4 - The BF3 molecule can also react with NH3 by...Ch. 4.5 - Prob. 4.7P Ch. 4.7 - Prob. 4.8P Ch. 4.7 - Add lone pairs where appropriate to the following...Ch. 4.7 - Prob. 4.10P

Solution Summary: The author explains how the molecular shape of CHCl_3 can be predicted using the valence-shell Electron-pair repulsion model.

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