(a) Interpretation: For the given skeleton of an anion having the overall formula C 6 H 6 NO − , a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included. Concept introduction: Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:) . The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

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Answer 1

Question

Chapter 1, Problem 1.52P

Interpretation Introduction

(a)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included.

Concept introduction:

Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:). The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(b)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on O. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(c)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on C atom that is bonded to three other C atoms. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

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(a) Determine the formal charge of oxygen in the following structure. If the atom is formally neutral, indicate a charge of zero. (b) Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge on O 0

Methyl isocyanate, CH3NCO, was made infamous in 1984when an accidental leakage of this compound from a storagetank in Bhopal, India, resulted in the deaths of about3800 people and severe and lasting injury to many thousandsmore. (a) Draw a Lewis structure for methyl isocyanate.(b) Draw a ball-and-stick model of the structure,including estimates of all the bond angles in the compound.(c) Predict all the bond distances in the molecule.(d) Do you predict that the molecule will have a dipolemoment? Explain.

3. (a) Draw a resonance structure for Molecule 1 in Box B, which satisfies the octet for all non- hydrogen atoms. Hint you may want to use curved arrows to move electrons over the skeleton of Molecule 3 to help you find the resonance structure. H H H H Molecule 1 H H 3. (b) Fill in the table below for Molecule 1 Box B: Resonance Structure of Molecule 1 VSEPR electron pair geometry around atom Molecular geometry Approximate bond or shape around atom angles around atom N atom CH3 C atom CH C atoms 3. (c) Given the information that resonating electrons are delocalized and so are not used to determine VSEPR geometry, how will the table you filled in for 3.(b) change?

Answer 2

Question

Chapter 1, Problem 1.52P

Interpretation Introduction

(a)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included.

Concept introduction:

Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:). The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(b)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on O. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(c)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on C atom that is bonded to three other C atoms. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

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Answer 3

Question

Chapter 1, Problem 1.52P

Interpretation Introduction

(a)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included.

Concept introduction:

Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:). The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(b)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on O. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(c)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on C atom that is bonded to three other C atoms. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

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Answer 4

Question

Chapter 1, Problem 1.52P

Interpretation Introduction

(a)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included.

Concept introduction:

Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:). The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(b)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on O. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(c)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on C atom that is bonded to three other C atoms. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

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Answer 5

Chapter 1, Problem 1.52P

Interpretation Introduction

(a)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included.

Concept introduction:

Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:). The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(b)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on O. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Interpretation Introduction

(c)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on C atom that is bonded to three other C atoms. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Answer 6

Chapter 1, Problem 1.52P

Interpretation Introduction

(a)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included.

Concept introduction:

Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:). The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

Answer 7

Chapter 1, Problem 1.52P

Interpretation Introduction

(a)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on N. All H atoms and valence electrons are to be included.

Concept introduction:

Lewis structure takes into account only the valence electrons. In the Lewis structure, each single line represents a shared pair of electrons, that is, a bonding pair of electrons. Nonbonding electrons are indicated by dots and are usually paired (:). The number of valence electrons contributed by each atom is the same as the group number. For an anion, each negative charge increases the number of valence electrons by one. In a molecule or polyatomic ion, the charge of an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear while half the electrons are assigned to each atom involved in the bond.

Answer 8

Interpretation Introduction

(b)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on O. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Answer 9

Interpretation Introduction

(b)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on O. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Answer 10

Interpretation Introduction

(c)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on C atom that is bonded to three other C atoms. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Answer 11

Interpretation Introduction

(c)

Interpretation:

For the given skeleton of an anion having the overall formula C6H6NO−, a complete Lewis structure is to be drawn in which -1 formal charge is on C atom that is bonded to three other C atoms. All H atoms and valence electrons are to be included.

Concept introduction:

In the Lewis structure each bond represents a shared pair of electrons and the non-bonding electrons are shown by dots. In a molecule or polyatomic ion, charge to an individual atom is determined by the difference between the atoms group number and the actual valence electrons it possesses. For the atoms involved in covalent bonds, the formal charge is determined by assigning both electrons of a lone pair to the atom on which they appear, and half the electrons are assigned to each atom involved in the bond.

Answer 12

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Answer 13

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Answer 15

Ch. 1 - Prob. 1.1P Ch. 1 - Prob. 1.2P Ch. 1 - Prob. 1.3P Ch. 1 - Prob. 1.4P Ch. 1 - Prob. 1.5P Ch. 1 - Prob. 1.6P Ch. 1 - Prob. 1.7P Ch. 1 - Prob. 1.8P Ch. 1 - Prob. 1.9P Ch. 1 - Prob. 1.10P

Solution Summary: The author explains that a complete Lewis structure includes all H atoms and valence electrons with -1 formal charge on N.

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