Each of the following species will be encountered at some point in this text. They all have the same number of electrons binding the same number of atoms and the same arrangement of bonds; they are isoelectronic. Specify which atoms, if any, bear a formal charge in the Lewis formula given and the net charge for each species. :N ≡ N: :C ≡ N: :C ≡ C: :N ≡ O: :C ≡ O:

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Answer 1

Textbook Question

Chapter 1, Problem 46P

Each of the following species will be encountered at some point in this text. They all have the same number of electrons binding the same number of atoms and the same arrangement of bonds; they are isoelectronic. Specify which atoms, if any, bear a formal charge in the Lewis formula given and the net charge for each species.

$:N ≡ N:$

$:C ≡ N:$

$:C ≡ C:$

$:N ≡ O:$

$:C ≡ O:$

Expert Solution & Answer

Interpretation Introduction

Interpretation:

For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.

Concept introduction:

Formula to calculate the formal charge on an atom:

$Formal charge=Group number−electron count$

$Electron count = 12( number of bonded electrons) + (number of unshared electrons)$

In a molecule, the charge that is assigned to an atom is called the formal charge.

Answer to Problem 46P

Solution:

The formal charge is $0$ .

The net charge on the species is $0.$

The formal charge on $N$ is $0$ and on $C$ is $−1$ .

The net charge on the species is $−1.$

The formal charge on $C$ is $−1$ .

The net charge on the species is $−2.$

The formal charge on $N$ is $0$ and on $O$ is $+1$ .

The net charge on the species is $+1$ .

The formal charge on $C$ is $−1$ and on $O$ is $+1$ . The net charge on the species is $0$ .

Explanation of Solution

(a) $: N≡N :$

Nitrogen belongs to Group $5A$ elements, thus the group number to be used for calculation is $5$ . Each nitrogen atom has shared six electrons. There is one unshared electron pair on each nitrogen atom.

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.

(b) $: C≡N :$

Carbon belongs to Group $4A$ while nitrogen belongs to Group $5A$ in the periodic table. The carbon and nitrogen atoms both have shared six electrons. There is one unshared electron pair on carbon and nitrogen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

Therefore, the net charge on the species is $−1 + 0 = −1$ .

(c) $: C≡C :$

Carbon belongs to Group $4A$ in the periodic table. Each carbon atom has shared six electrons. There is one unshared electron pair on the carbon atom.

$Electron count = 12(6) + 2= 3 + 2 = 5$

$Formal charge = 4 −5 = −1$

Hence, the formal charge on each carbon atom is $−1$ .

Therefore, the net charge on the species is $−1 + (−1) = −2$ .

(d) $: N≡O :$

Nitrogen belongs to Group $5A$ while oxygen belongs to Group $6A$ in the periodic table. The nitrogen and oxygen atoms have shared six electrons each. There is one unshared electron pair on nitrogen and oxygen atom.

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3+ 2 = 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $0 +(+ 1) = +1$ .

(d) $: C≡O :$

Carbon belongs to Group $4A$ while oxygen belongs to Group $6A$ in the periodic table. The carbon and oxygen atoms have shared six electrons each. There is one unshared electron pair on carbon and oxygen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $-1 + (+1) = 0$ .

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Answer 2

Textbook Question

Chapter 1, Problem 46P

Each of the following species will be encountered at some point in this text. They all have the same number of electrons binding the same number of atoms and the same arrangement of bonds; they are isoelectronic. Specify which atoms, if any, bear a formal charge in the Lewis formula given and the net charge for each species.

$:N ≡ N:$

$:C ≡ N:$

$:C ≡ C:$

$:N ≡ O:$

$:C ≡ O:$

Expert Solution & Answer

Interpretation Introduction

Interpretation:

For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.

Concept introduction:

Formula to calculate the formal charge on an atom:

$Formal charge=Group number−electron count$

$Electron count = 12( number of bonded electrons) + (number of unshared electrons)$

In a molecule, the charge that is assigned to an atom is called the formal charge.

Answer to Problem 46P

Solution:

The formal charge is $0$ .

The net charge on the species is $0.$

The formal charge on $N$ is $0$ and on $C$ is $−1$ .

The net charge on the species is $−1.$

The formal charge on $C$ is $−1$ .

The net charge on the species is $−2.$

The formal charge on $N$ is $0$ and on $O$ is $+1$ .

The net charge on the species is $+1$ .

The formal charge on $C$ is $−1$ and on $O$ is $+1$ . The net charge on the species is $0$ .

Explanation of Solution

(a) $: N≡N :$

Nitrogen belongs to Group $5A$ elements, thus the group number to be used for calculation is $5$ . Each nitrogen atom has shared six electrons. There is one unshared electron pair on each nitrogen atom.

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.

(b) $: C≡N :$

Carbon belongs to Group $4A$ while nitrogen belongs to Group $5A$ in the periodic table. The carbon and nitrogen atoms both have shared six electrons. There is one unshared electron pair on carbon and nitrogen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

Therefore, the net charge on the species is $−1 + 0 = −1$ .

(c) $: C≡C :$

Carbon belongs to Group $4A$ in the periodic table. Each carbon atom has shared six electrons. There is one unshared electron pair on the carbon atom.

$Electron count = 12(6) + 2= 3 + 2 = 5$

$Formal charge = 4 −5 = −1$

Hence, the formal charge on each carbon atom is $−1$ .

Therefore, the net charge on the species is $−1 + (−1) = −2$ .

(d) $: N≡O :$

Nitrogen belongs to Group $5A$ while oxygen belongs to Group $6A$ in the periodic table. The nitrogen and oxygen atoms have shared six electrons each. There is one unshared electron pair on nitrogen and oxygen atom.

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3+ 2 = 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $0 +(+ 1) = +1$ .

(d) $: C≡O :$

Carbon belongs to Group $4A$ while oxygen belongs to Group $6A$ in the periodic table. The carbon and oxygen atoms have shared six electrons each. There is one unshared electron pair on carbon and oxygen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $-1 + (+1) = 0$ .

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Answer 3

Textbook Question

Chapter 1, Problem 46P

Each of the following species will be encountered at some point in this text. They all have the same number of electrons binding the same number of atoms and the same arrangement of bonds; they are isoelectronic. Specify which atoms, if any, bear a formal charge in the Lewis formula given and the net charge for each species.

$:N ≡ N:$

$:C ≡ N:$

$:C ≡ C:$

$:N ≡ O:$

$:C ≡ O:$

Expert Solution & Answer

Interpretation Introduction

Interpretation:

For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.

Concept introduction:

Formula to calculate the formal charge on an atom:

$Formal charge=Group number−electron count$

$Electron count = 12( number of bonded electrons) + (number of unshared electrons)$

In a molecule, the charge that is assigned to an atom is called the formal charge.

Answer to Problem 46P

Solution:

The formal charge is $0$ .

The net charge on the species is $0.$

The formal charge on $N$ is $0$ and on $C$ is $−1$ .

The net charge on the species is $−1.$

The formal charge on $C$ is $−1$ .

The net charge on the species is $−2.$

The formal charge on $N$ is $0$ and on $O$ is $+1$ .

The net charge on the species is $+1$ .

The formal charge on $C$ is $−1$ and on $O$ is $+1$ . The net charge on the species is $0$ .

Explanation of Solution

(a) $: N≡N :$

Nitrogen belongs to Group $5A$ elements, thus the group number to be used for calculation is $5$ . Each nitrogen atom has shared six electrons. There is one unshared electron pair on each nitrogen atom.

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.

(b) $: C≡N :$

Carbon belongs to Group $4A$ while nitrogen belongs to Group $5A$ in the periodic table. The carbon and nitrogen atoms both have shared six electrons. There is one unshared electron pair on carbon and nitrogen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

Therefore, the net charge on the species is $−1 + 0 = −1$ .

(c) $: C≡C :$

Carbon belongs to Group $4A$ in the periodic table. Each carbon atom has shared six electrons. There is one unshared electron pair on the carbon atom.

$Electron count = 12(6) + 2= 3 + 2 = 5$

$Formal charge = 4 −5 = −1$

Hence, the formal charge on each carbon atom is $−1$ .

Therefore, the net charge on the species is $−1 + (−1) = −2$ .

(d) $: N≡O :$

Nitrogen belongs to Group $5A$ while oxygen belongs to Group $6A$ in the periodic table. The nitrogen and oxygen atoms have shared six electrons each. There is one unshared electron pair on nitrogen and oxygen atom.

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3+ 2 = 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $0 +(+ 1) = +1$ .

(d) $: C≡O :$

Carbon belongs to Group $4A$ while oxygen belongs to Group $6A$ in the periodic table. The carbon and oxygen atoms have shared six electrons each. There is one unshared electron pair on carbon and oxygen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $-1 + (+1) = 0$ .

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Answer 4

Textbook Question

Chapter 1, Problem 46P

Each of the following species will be encountered at some point in this text. They all have the same number of electrons binding the same number of atoms and the same arrangement of bonds; they are isoelectronic. Specify which atoms, if any, bear a formal charge in the Lewis formula given and the net charge for each species.

$:N ≡ N:$

$:C ≡ N:$

$:C ≡ C:$

$:N ≡ O:$

$:C ≡ O:$

Expert Solution & Answer

Interpretation Introduction

Interpretation:

For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.

Concept introduction:

Formula to calculate the formal charge on an atom:

$Formal charge=Group number−electron count$

$Electron count = 12( number of bonded electrons) + (number of unshared electrons)$

In a molecule, the charge that is assigned to an atom is called the formal charge.

Answer to Problem 46P

Solution:

The formal charge is $0$ .

The net charge on the species is $0.$

The formal charge on $N$ is $0$ and on $C$ is $−1$ .

The net charge on the species is $−1.$

The formal charge on $C$ is $−1$ .

The net charge on the species is $−2.$

The formal charge on $N$ is $0$ and on $O$ is $+1$ .

The net charge on the species is $+1$ .

The formal charge on $C$ is $−1$ and on $O$ is $+1$ . The net charge on the species is $0$ .

Explanation of Solution

(a) $: N≡N :$

Nitrogen belongs to Group $5A$ elements, thus the group number to be used for calculation is $5$ . Each nitrogen atom has shared six electrons. There is one unshared electron pair on each nitrogen atom.

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.

(b) $: C≡N :$

Carbon belongs to Group $4A$ while nitrogen belongs to Group $5A$ in the periodic table. The carbon and nitrogen atoms both have shared six electrons. There is one unshared electron pair on carbon and nitrogen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

Therefore, the net charge on the species is $−1 + 0 = −1$ .

(c) $: C≡C :$

Carbon belongs to Group $4A$ in the periodic table. Each carbon atom has shared six electrons. There is one unshared electron pair on the carbon atom.

$Electron count = 12(6) + 2= 3 + 2 = 5$

$Formal charge = 4 −5 = −1$

Hence, the formal charge on each carbon atom is $−1$ .

Therefore, the net charge on the species is $−1 + (−1) = −2$ .

(d) $: N≡O :$

Nitrogen belongs to Group $5A$ while oxygen belongs to Group $6A$ in the periodic table. The nitrogen and oxygen atoms have shared six electrons each. There is one unshared electron pair on nitrogen and oxygen atom.

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3+ 2 = 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $0 +(+ 1) = +1$ .

(d) $: C≡O :$

Carbon belongs to Group $4A$ while oxygen belongs to Group $6A$ in the periodic table. The carbon and oxygen atoms have shared six electrons each. There is one unshared electron pair on carbon and oxygen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $-1 + (+1) = 0$ .

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Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

Expert Solution & Answer

Interpretation Introduction

Interpretation:

For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.

Concept introduction:

Formula to calculate the formal charge on an atom:

$Formal charge=Group number−electron count$

$Electron count = 12( number of bonded electrons) + (number of unshared electrons)$

In a molecule, the charge that is assigned to an atom is called the formal charge.

Answer to Problem 46P

Solution:

The formal charge is $0$ .

The net charge on the species is $0.$

The formal charge on $N$ is $0$ and on $C$ is $−1$ .

The net charge on the species is $−1.$

The formal charge on $C$ is $−1$ .

The net charge on the species is $−2.$

The formal charge on $N$ is $0$ and on $O$ is $+1$ .

The net charge on the species is $+1$ .

The formal charge on $C$ is $−1$ and on $O$ is $+1$ . The net charge on the species is $0$ .

Explanation of Solution

(a) $: N≡N :$

Nitrogen belongs to Group $5A$ elements, thus the group number to be used for calculation is $5$ . Each nitrogen atom has shared six electrons. There is one unshared electron pair on each nitrogen atom.

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.

(b) $: C≡N :$

Carbon belongs to Group $4A$ while nitrogen belongs to Group $5A$ in the periodic table. The carbon and nitrogen atoms both have shared six electrons. There is one unshared electron pair on carbon and nitrogen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

Therefore, the net charge on the species is $−1 + 0 = −1$ .

(c) $: C≡C :$

Carbon belongs to Group $4A$ in the periodic table. Each carbon atom has shared six electrons. There is one unshared electron pair on the carbon atom.

$Electron count = 12(6) + 2= 3 + 2 = 5$

$Formal charge = 4 −5 = −1$

Hence, the formal charge on each carbon atom is $−1$ .

Therefore, the net charge on the species is $−1 + (−1) = −2$ .

(d) $: N≡O :$

Nitrogen belongs to Group $5A$ while oxygen belongs to Group $6A$ in the periodic table. The nitrogen and oxygen atoms have shared six electrons each. There is one unshared electron pair on nitrogen and oxygen atom.

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3+ 2 = 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $0 +(+ 1) = +1$ .

(d) $: C≡O :$

Carbon belongs to Group $4A$ while oxygen belongs to Group $6A$ in the periodic table. The carbon and oxygen atoms have shared six electrons each. There is one unshared electron pair on carbon and oxygen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $-1 + (+1) = 0$ .

Answer 8

Expert Solution & Answer

Interpretation Introduction

Interpretation:

For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.

Concept introduction:

Formula to calculate the formal charge on an atom:

$Formal charge=Group number−electron count$

$Electron count = 12( number of bonded electrons) + (number of unshared electrons)$

In a molecule, the charge that is assigned to an atom is called the formal charge.

Answer to Problem 46P

Solution:

The formal charge is $0$ .

The net charge on the species is $0.$

The formal charge on $N$ is $0$ and on $C$ is $−1$ .

The net charge on the species is $−1.$

The formal charge on $C$ is $−1$ .

The net charge on the species is $−2.$

The formal charge on $N$ is $0$ and on $O$ is $+1$ .

The net charge on the species is $+1$ .

The formal charge on $C$ is $−1$ and on $O$ is $+1$ . The net charge on the species is $0$ .

Explanation of Solution

(a) $: N≡N :$

Nitrogen belongs to Group $5A$ elements, thus the group number to be used for calculation is $5$ . Each nitrogen atom has shared six electrons. There is one unshared electron pair on each nitrogen atom.

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.

(b) $: C≡N :$

Carbon belongs to Group $4A$ while nitrogen belongs to Group $5A$ in the periodic table. The carbon and nitrogen atoms both have shared six electrons. There is one unshared electron pair on carbon and nitrogen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

Therefore, the net charge on the species is $−1 + 0 = −1$ .

(c) $: C≡C :$

Carbon belongs to Group $4A$ in the periodic table. Each carbon atom has shared six electrons. There is one unshared electron pair on the carbon atom.

$Electron count = 12(6) + 2= 3 + 2 = 5$

$Formal charge = 4 −5 = −1$

Hence, the formal charge on each carbon atom is $−1$ .

Therefore, the net charge on the species is $−1 + (−1) = −2$ .

(d) $: N≡O :$

Nitrogen belongs to Group $5A$ while oxygen belongs to Group $6A$ in the periodic table. The nitrogen and oxygen atoms have shared six electrons each. There is one unshared electron pair on nitrogen and oxygen atom.

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3+ 2 = 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $0 +(+ 1) = +1$ .

(d) $: C≡O :$

Carbon belongs to Group $4A$ while oxygen belongs to Group $6A$ in the periodic table. The carbon and oxygen atoms have shared six electrons each. There is one unshared electron pair on carbon and oxygen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $-1 + (+1) = 0$ .

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Interpretation Introduction

Interpretation:

For the given isoelectronic species, the formal charge on the atoms and the net charge on each species is to be determined.

Concept introduction:

Formula to calculate the formal charge on an atom:

$Formal charge=Group number−electron count$

$Electron count = 12( number of bonded electrons) + (number of unshared electrons)$

In a molecule, the charge that is assigned to an atom is called the formal charge.

Answer 12

Answer to Problem 46P

Solution:

The formal charge is $0$ .

The net charge on the species is $0.$

The formal charge on $N$ is $0$ and on $C$ is $−1$ .

The net charge on the species is $−1.$

The formal charge on $C$ is $−1$ .

The net charge on the species is $−2.$

The formal charge on $N$ is $0$ and on $O$ is $+1$ .

The net charge on the species is $+1$ .

The formal charge on $C$ is $−1$ and on $O$ is $+1$ . The net charge on the species is $0$ .

Answer 13

Explanation of Solution

(a) $: N≡N :$

Nitrogen belongs to Group $5A$ elements, thus the group number to be used for calculation is $5$ . Each nitrogen atom has shared six electrons. There is one unshared electron pair on each nitrogen atom.

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Since, both the nitrogen atoms have zero formal charge on them, the net charge of the species is also zero.

(b) $: C≡N :$

Carbon belongs to Group $4A$ while nitrogen belongs to Group $5A$ in the periodic table. The carbon and nitrogen atoms both have shared six electrons. There is one unshared electron pair on carbon and nitrogen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$

$Formal charge = 4 − 5 = −1$

Hence, the formal charge on the carbon atom is $−1$ .

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

Therefore, the net charge on the species is $−1 + 0 = −1$ .

(c) $: C≡C :$

Carbon belongs to Group $4A$ in the periodic table. Each carbon atom has shared six electrons. There is one unshared electron pair on the carbon atom.

$Electron count = 12(6) + 2= 3 + 2 = 5$

$Formal charge = 4 −5 = −1$

Hence, the formal charge on each carbon atom is $−1$ .

Therefore, the net charge on the species is $−1 + (−1) = −2$ .

(d) $: N≡O :$

Nitrogen belongs to Group $5A$ while oxygen belongs to Group $6A$ in the periodic table. The nitrogen and oxygen atoms have shared six electrons each. There is one unshared electron pair on nitrogen and oxygen atom.

For nitrogen atom,

$Electron count = 12(6) + 2 = 3 + 2= 5$

$Formal charge = 5 −5 = 0$

Hence, the formal charge on nitrogen is $0$ .

For oxygen atom,

$Electron count = 12(6) + 2 = 3+ 2 = 5$

$Formal charge = 6 −5 = +1$

Hence, the formal charge on oxygen is $+1$ .

Therefore, the net charge on the species is $0 +(+ 1) = +1$ .

(d) $: C≡O :$

Carbon belongs to Group $4A$ while oxygen belongs to Group $6A$ in the periodic table. The carbon and oxygen atoms have shared six electrons each. There is one unshared electron pair on carbon and oxygen atom.

For carbon atom,

$Electron count = 12(6) + 2 = 3 + 2 = 5$