The bond type for each bond in POF 3 has to be determined using Lewis structure and a formal charge. Concept Introduction: Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom. The formula for the formal charge can be written as Formal charge= Valence electrons-lone pair electrons - Bonding electrons 2

Question

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Answer 1

Question

Chapter 6, Problem 47QRT

(a)

Interpretation Introduction

Interpretation:

The bond type for each bond in $POF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

$Formal charge= Valence electrons-lone pair electrons -Bonding electrons2$

(a)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $POF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 1

Draw a chart:

$O N Cl P O F Valence electrons 5 6 7 Lone pair electrons 0 4 6 Bonding electrons 10 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $32.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 2

The phosphorous atom has three single bonds and one double bond; both fluorine and oxygen have a one single bond. All atoms in $POF3$ has zero formal charge.

The bond between $P-F$ is single bond and the bond between $P=O$ is a double bond.

(b)

Interpretation Introduction

Interpretation:

The bond type for each bond in $SOF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Refer part (a).

(b)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $SOF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 3

Draw a chart:

$S O FValence electrons 6 6 7 Lone pair electrons 0 4 6 Bonding electrons 12 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $40.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 4

The sulfur atom has four single bonds and one double bond; all fluorine has a one single bond, oxygen has double bond. All atoms in $SOF3$ has zero formal charge.

The bond between $S-F$ is single bond and the bond between $S=O$ is a double bond.

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Answer 2

Question

Chapter 6, Problem 47QRT

(a)

Interpretation Introduction

Interpretation:

The bond type for each bond in $POF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

$Formal charge= Valence electrons-lone pair electrons -Bonding electrons2$

(a)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $POF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 1

Draw a chart:

$O N Cl P O F Valence electrons 5 6 7 Lone pair electrons 0 4 6 Bonding electrons 10 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $32.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 2

The phosphorous atom has three single bonds and one double bond; both fluorine and oxygen have a one single bond. All atoms in $POF3$ has zero formal charge.

The bond between $P-F$ is single bond and the bond between $P=O$ is a double bond.

(b)

Interpretation Introduction

Interpretation:

The bond type for each bond in $SOF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Refer part (a).

(b)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $SOF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 3

Draw a chart:

$S O FValence electrons 6 6 7 Lone pair electrons 0 4 6 Bonding electrons 12 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $40.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 4

The sulfur atom has four single bonds and one double bond; all fluorine has a one single bond, oxygen has double bond. All atoms in $SOF3$ has zero formal charge.

The bond between $S-F$ is single bond and the bond between $S=O$ is a double bond.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 6, Problem 47QRT

(a)

Interpretation Introduction

Interpretation:

The bond type for each bond in $POF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

$Formal charge= Valence electrons-lone pair electrons -Bonding electrons2$

(a)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $POF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 1

Draw a chart:

$O N Cl P O F Valence electrons 5 6 7 Lone pair electrons 0 4 6 Bonding electrons 10 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $32.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 2

The phosphorous atom has three single bonds and one double bond; both fluorine and oxygen have a one single bond. All atoms in $POF3$ has zero formal charge.

The bond between $P-F$ is single bond and the bond between $P=O$ is a double bond.

(b)

Interpretation Introduction

Interpretation:

The bond type for each bond in $SOF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Refer part (a).

(b)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $SOF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 3

Draw a chart:

$S O FValence electrons 6 6 7 Lone pair electrons 0 4 6 Bonding electrons 12 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $40.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 4

The sulfur atom has four single bonds and one double bond; all fluorine has a one single bond, oxygen has double bond. All atoms in $SOF3$ has zero formal charge.

The bond between $S-F$ is single bond and the bond between $S=O$ is a double bond.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 6, Problem 47QRT

(a)

Interpretation Introduction

Interpretation:

The bond type for each bond in $POF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

$Formal charge= Valence electrons-lone pair electrons -Bonding electrons2$

(a)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $POF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 1

Draw a chart:

$O N Cl P O F Valence electrons 5 6 7 Lone pair electrons 0 4 6 Bonding electrons 10 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $32.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 2

The phosphorous atom has three single bonds and one double bond; both fluorine and oxygen have a one single bond. All atoms in $POF3$ has zero formal charge.

The bond between $P-F$ is single bond and the bond between $P=O$ is a double bond.

(b)

Interpretation Introduction

Interpretation:

The bond type for each bond in $SOF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Refer part (a).

(b)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $SOF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 3

Draw a chart:

$S O FValence electrons 6 6 7 Lone pair electrons 0 4 6 Bonding electrons 12 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $40.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 4

The sulfur atom has four single bonds and one double bond; all fluorine has a one single bond, oxygen has double bond. All atoms in $SOF3$ has zero formal charge.

The bond between $S-F$ is single bond and the bond between $S=O$ is a double bond.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 6, Problem 47QRT

(a)

Interpretation Introduction

Interpretation:

The bond type for each bond in $POF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

$Formal charge= Valence electrons-lone pair electrons -Bonding electrons2$

(a)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $POF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 1

Draw a chart:

$O N Cl P O F Valence electrons 5 6 7 Lone pair electrons 0 4 6 Bonding electrons 10 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $32.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 2

The phosphorous atom has three single bonds and one double bond; both fluorine and oxygen have a one single bond. All atoms in $POF3$ has zero formal charge.

The bond between $P-F$ is single bond and the bond between $P=O$ is a double bond.

(b)

Interpretation Introduction

Interpretation:

The bond type for each bond in $SOF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Refer part (a).

(b)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $SOF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 3

Draw a chart:

$S O FValence electrons 6 6 7 Lone pair electrons 0 4 6 Bonding electrons 12 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $40.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 4

The sulfur atom has four single bonds and one double bond; all fluorine has a one single bond, oxygen has double bond. All atoms in $SOF3$ has zero formal charge.

The bond between $S-F$ is single bond and the bond between $S=O$ is a double bond.

Answer 6

Chapter 6, Problem 47QRT

(a)

Interpretation Introduction

Interpretation:

The bond type for each bond in $POF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

$Formal charge= Valence electrons-lone pair electrons -Bonding electrons2$

(a)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $POF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 1

Draw a chart:

$O N Cl P O F Valence electrons 5 6 7 Lone pair electrons 0 4 6 Bonding electrons 10 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $32.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 2

The phosphorous atom has three single bonds and one double bond; both fluorine and oxygen have a one single bond. All atoms in $POF3$ has zero formal charge.

The bond between $P-F$ is single bond and the bond between $P=O$ is a double bond.

Answer 7

Chapter 6, Problem 47QRT

(a)

Interpretation Introduction

Interpretation:

The bond type for each bond in $POF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Lewis structure is also known as Lewis dot diagrams or electron dot structures. The bond between atoms and lone pairs of electrons that is present in the molecule. Lewis structure represents each atom and their position in structure using the chemical symbol. Excess electrons forms the lone pair are given by pair of dots, and are located next to the atom.

The formula for the formal charge can be written as

$Formal charge= Valence electrons-lone pair electrons -Bonding electrons2$

Answer 8

(a)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $POF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 1

Draw a chart:

$O N Cl P O F Valence electrons 5 6 7 Lone pair electrons 0 4 6 Bonding electrons 10 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $32.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 2

The phosphorous atom has three single bonds and one double bond; both fluorine and oxygen have a one single bond. All atoms in $POF3$ has zero formal charge.

The bond between $P-F$ is single bond and the bond between $P=O$ is a double bond.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

(b)

Interpretation Introduction

Interpretation:

The bond type for each bond in $SOF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Refer part (a).

(b)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $SOF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 3

Draw a chart:

$S O FValence electrons 6 6 7 Lone pair electrons 0 4 6 Bonding electrons 12 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $40.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 4

The sulfur atom has four single bonds and one double bond; all fluorine has a one single bond, oxygen has double bond. All atoms in $SOF3$ has zero formal charge.

The bond between $S-F$ is single bond and the bond between $S=O$ is a double bond.

Answer 13

(b)

Interpretation Introduction

Interpretation:

The bond type for each bond in $SOF3$ has to be determined using Lewis structure and a formal charge.

Concept Introduction:

Refer part (a).

Answer 14

(b)

Expert Solution

Explanation of Solution

The correct Lewis structure of the $SOF3$ can be drawn as,

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 3

Draw a chart:

$S O FValence electrons 6 6 7 Lone pair electrons 0 4 6 Bonding electrons 12 4 2 Formal charge 0 0 0 _ ¯¯$

The total number of valence electron is $40.$

Chemistry: The Molecular Science, Chapter 6, Problem 47QRT , additional homework tip 4

The sulfur atom has four single bonds and one double bond; all fluorine has a one single bond, oxygen has double bond. All atoms in $SOF3$ has zero formal charge.

The bond between $S-F$ is single bond and the bond between $S=O$ is a double bond.