(a) Interpretation: The formal charge on each atom and the net charge in the given species are to be stated. Concept introduction: Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Question

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Answer 1

Question

Chapter 1, Problem 1.25AP

Interpretation Introduction

(a)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 1.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 1

Figure 1

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ each. The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $4$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−4=3$

Thus, the formal charge on chlorine atom is $3$ .

The total charge on the given species is calculated as follows.

$Total charge=3+(−1)×4=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Interpretation Introduction

(b)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 2.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 2

Figure 2

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of nitrogen atom in given species are $4$ . The group number for nitrogen atom is $5$ . Substitute the values in equation (1) for nitrogen atom as follows.

$Formal charge=Group number−valence electrons=5−4=1$

Thus, the formal charge on nitrogen atom is $3$ .

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon atom as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(c)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 3.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 3

Figure 3

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of left oxygen atom in given species are $6$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−6=0$

Thus, the formal charge on each oxygen atom is $0$ .

The valence electrons of right oxygen atom in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of central oxygen atom in given species are $5$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−5=1$

Thus, the formal charge on each oxygen atom is $1$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(d)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 4.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 4

Figure 4

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(e)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 5.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 5

Figure 5

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The valence electrons of carbon radical in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon radical as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon radical is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(f)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 6.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 6

Figure 6

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $7$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−7=0$

Thus, the formal charge on chlorine atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=0+(−1)=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

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Answer 2

Question

Chapter 1, Problem 1.25AP

Interpretation Introduction

(a)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 1.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 1

Figure 1

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ each. The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $4$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−4=3$

Thus, the formal charge on chlorine atom is $3$ .

The total charge on the given species is calculated as follows.

$Total charge=3+(−1)×4=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Interpretation Introduction

(b)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 2.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 2

Figure 2

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of nitrogen atom in given species are $4$ . The group number for nitrogen atom is $5$ . Substitute the values in equation (1) for nitrogen atom as follows.

$Formal charge=Group number−valence electrons=5−4=1$

Thus, the formal charge on nitrogen atom is $3$ .

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon atom as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(c)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 3.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 3

Figure 3

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of left oxygen atom in given species are $6$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−6=0$

Thus, the formal charge on each oxygen atom is $0$ .

The valence electrons of right oxygen atom in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of central oxygen atom in given species are $5$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−5=1$

Thus, the formal charge on each oxygen atom is $1$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(d)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 4.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 4

Figure 4

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(e)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 5.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 5

Figure 5

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The valence electrons of carbon radical in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon radical as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon radical is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(f)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 6.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 6

Figure 6

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $7$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−7=0$

Thus, the formal charge on chlorine atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=0+(−1)=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

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Answer 3

Question

Chapter 1, Problem 1.25AP

Interpretation Introduction

(a)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 1.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 1

Figure 1

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ each. The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $4$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−4=3$

Thus, the formal charge on chlorine atom is $3$ .

The total charge on the given species is calculated as follows.

$Total charge=3+(−1)×4=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Interpretation Introduction

(b)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 2.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 2

Figure 2

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of nitrogen atom in given species are $4$ . The group number for nitrogen atom is $5$ . Substitute the values in equation (1) for nitrogen atom as follows.

$Formal charge=Group number−valence electrons=5−4=1$

Thus, the formal charge on nitrogen atom is $3$ .

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon atom as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(c)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 3.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 3

Figure 3

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of left oxygen atom in given species are $6$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−6=0$

Thus, the formal charge on each oxygen atom is $0$ .

The valence electrons of right oxygen atom in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of central oxygen atom in given species are $5$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−5=1$

Thus, the formal charge on each oxygen atom is $1$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(d)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 4.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 4

Figure 4

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(e)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 5.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 5

Figure 5

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The valence electrons of carbon radical in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon radical as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon radical is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(f)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 6.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 6

Figure 6

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $7$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−7=0$

Thus, the formal charge on chlorine atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=0+(−1)=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

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Answer 4

Question

Chapter 1, Problem 1.25AP

Interpretation Introduction

(a)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 1.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 1

Figure 1

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ each. The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $4$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−4=3$

Thus, the formal charge on chlorine atom is $3$ .

The total charge on the given species is calculated as follows.

$Total charge=3+(−1)×4=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Interpretation Introduction

(b)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 2.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 2

Figure 2

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of nitrogen atom in given species are $4$ . The group number for nitrogen atom is $5$ . Substitute the values in equation (1) for nitrogen atom as follows.

$Formal charge=Group number−valence electrons=5−4=1$

Thus, the formal charge on nitrogen atom is $3$ .

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon atom as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(c)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 3.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 3

Figure 3

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of left oxygen atom in given species are $6$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−6=0$

Thus, the formal charge on each oxygen atom is $0$ .

The valence electrons of right oxygen atom in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of central oxygen atom in given species are $5$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−5=1$

Thus, the formal charge on each oxygen atom is $1$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(d)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 4.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 4

Figure 4

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(e)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 5.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 5

Figure 5

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The valence electrons of carbon radical in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon radical as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon radical is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(f)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 6.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 6

Figure 6

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $7$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−7=0$

Thus, the formal charge on chlorine atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=0+(−1)=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

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Answer 5

Chapter 1, Problem 1.25AP

Interpretation Introduction

(a)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 1.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 1

Figure 1

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ each. The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $4$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−4=3$

Thus, the formal charge on chlorine atom is $3$ .

The total charge on the given species is calculated as follows.

$Total charge=3+(−1)×4=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Interpretation Introduction

(b)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 2.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 2

Figure 2

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of nitrogen atom in given species are $4$ . The group number for nitrogen atom is $5$ . Substitute the values in equation (1) for nitrogen atom as follows.

$Formal charge=Group number−valence electrons=5−4=1$

Thus, the formal charge on nitrogen atom is $3$ .

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon atom as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(c)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 3.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 3

Figure 3

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of left oxygen atom in given species are $6$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−6=0$

Thus, the formal charge on each oxygen atom is $0$ .

The valence electrons of right oxygen atom in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of central oxygen atom in given species are $5$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−5=1$

Thus, the formal charge on each oxygen atom is $1$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Interpretation Introduction

(d)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 4.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 4

Figure 4

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(e)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 5.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 5

Figure 5

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The valence electrons of carbon radical in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon radical as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon radical is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Interpretation Introduction

(f)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 6.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 6

Figure 6

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $7$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−7=0$

Thus, the formal charge on chlorine atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=0+(−1)=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Answer 6

Chapter 1, Problem 1.25AP

Interpretation Introduction

(a)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 1.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 1

Figure 1

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ each. The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $4$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−4=3$

Thus, the formal charge on chlorine atom is $3$ .

The total charge on the given species is calculated as follows.

$Total charge=3+(−1)×4=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Answer 7

Chapter 1, Problem 1.25AP

Interpretation Introduction

(a)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Answer 8

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

The given structure is shown in figure 1.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 1

Figure 1

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ each. The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $4$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−4=3$

Thus, the formal charge on chlorine atom is $3$ .

The total charge on the given species is calculated as follows.

$Total charge=3+(−1)×4=−1$

Hence, total charge on the species is $−1$ .

Answer 13

Conclusion

The formal charges on oxygen atom and chlorine atom are $−1$ and $3$ respectively. The net charge in the given species is $−1$ .

Answer 14

Interpretation Introduction

(b)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 2.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 2

Figure 2

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of nitrogen atom in given species are $4$ . The group number for nitrogen atom is $5$ . Substitute the values in equation (1) for nitrogen atom as follows.

$Formal charge=Group number−valence electrons=5−4=1$

Thus, the formal charge on nitrogen atom is $3$ .

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon atom as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Answer 15

Interpretation Introduction

(b)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Answer 16

Expert Solution

Answer to Problem 1.25AP

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Expert Solution

Answer 20

Explanation of Solution

The given structure is shown in figure 2.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 2

Figure 2

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of nitrogen atom in given species are $4$ . The group number for nitrogen atom is $5$ . Substitute the values in equation (1) for nitrogen atom as follows.

$Formal charge=Group number−valence electrons=5−4=1$

Thus, the formal charge on nitrogen atom is $3$ .

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon atom as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Answer 21

Conclusion

The formal charges on oxygen atom, nitrogen atom and carbon atom are $−1$ , $1$ and $0$ respectively. The net charge in the given species is $0$ .

Answer 22

Interpretation Introduction

(c)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Explanation of Solution

The given structure is shown in figure 3.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 3

Figure 3

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of left oxygen atom in given species are $6$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−6=0$

Thus, the formal charge on each oxygen atom is $0$ .

The valence electrons of right oxygen atom in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of central oxygen atom in given species are $5$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−5=1$

Thus, the formal charge on each oxygen atom is $1$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Conclusion

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Answer 23

Interpretation Introduction

(c)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Answer 24

Expert Solution

Answer to Problem 1.25AP

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Answer 25

Expert Solution

Answer 26

Expert Solution

Answer 27

Expert Solution

Answer 28

Explanation of Solution

The given structure is shown in figure 3.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 3

Figure 3

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of left oxygen atom in given species are $6$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−6=0$

Thus, the formal charge on each oxygen atom is $0$ .

The valence electrons of right oxygen atom in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of central oxygen atom in given species are $5$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−5=1$

Thus, the formal charge on each oxygen atom is $1$ .

The total charge on the given species is calculated as follows.

$Total charge=1+(−1)+0=0$

Hence, total charge on the species is $0$ .

Answer 29

Conclusion

The formal charges on left oxygen atom, right oxygen atom and central oxygen atom are $0$ , $−1$ and $1$ respectively. The net charge in the given species is $0$ .

Answer 30

Interpretation Introduction

(d)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 4.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 4

Figure 4

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Answer 31

Interpretation Introduction

(d)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Answer 32

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Answer 33

Expert Solution

Answer 34

Expert Solution

Answer 35

Expert Solution

Answer 36

Explanation of Solution

The given structure is shown in figure 4.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 4

Figure 4

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

Hence, total charge on the species is also $0$ .

Answer 37

Conclusion

The formal charge on carbon atom is $0$ . The net charge in the given species is also $0$ .

Answer 38

Interpretation Introduction

(e)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Explanation of Solution

The given structure is shown in figure 5.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 5

Figure 5

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The valence electrons of carbon radical in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon radical as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon radical is $0$ .

Hence, total charge on the species is also $0$ .

Conclusion

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Answer 39

Interpretation Introduction

(e)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Answer 40

Expert Solution

Answer to Problem 1.25AP

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Answer 41

Expert Solution

Answer 42

Expert Solution

Answer 43

Expert Solution

Answer 44

Explanation of Solution

The given structure is shown in figure 5.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 5

Figure 5

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of carbon atom in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon atom is $0$ .

The valence electrons of carbon radical in given species are $4$ . The group number for carbon atom is $4$ . Substitute the values in equation (1) for carbon radical as follows.

$Formal charge=Group number−valence electrons=4−4=0$

Thus, the formal charge on carbon radical is $0$ .

Hence, total charge on the species is also $0$ .

Answer 45

Conclusion

The formal charge on carbon atom and carbon radical is $0$ . The net charge in the given species is also $0$ .

Answer 46

Interpretation Introduction

(f)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Expert Solution

Answer to Problem 1.25AP

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Explanation of Solution

The given structure is shown in figure 6.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 6

Figure 6

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $7$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−7=0$

Thus, the formal charge on chlorine atom is $0$ .

The total charge on the given species is calculated as follows.

$Total charge=0+(−1)=−1$

Hence, total charge on the species is $−1$ .

Conclusion

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Answer 47

Interpretation Introduction

(f)

Interpretation:

The formal charge on each atom and the net charge in the given species are to be stated.

Concept introduction:

Chemical compounds contain two types of bonds. These are known as ionic and covalent bonds. In ionic bonds, the ions are held by the electrostatic interaction between them. In covalent bonds, the atoms are held together by the sharing of electrons. The formal charge is the charge on the constituent atoms in a molecule. It is calculated by using valence electrons of the atom.

Answer 48

Expert Solution

Answer to Problem 1.25AP

The formal charge on oxygen atom and chlorine atom is $−1$ and $0$ respectively. The net charge in the given species is $−1$ .

Answer 49

Expert Solution

Answer 50

Expert Solution

Answer 51

Expert Solution

Answer 52

Explanation of Solution

The given structure is shown in figure 6.

Organic Chemistry, Ebook And Single-course Homework Access, Chapter 1, Problem 1.25AP , additional homework tip 6

Figure 6

The formal charge on atom is calculated by the formula given below as,

$Formal charge=Group number−valence electrons$ …(1)

The valence electrons of oxygen atoms in given species are $7$ . The group number for oxygen atom is $6$ . Substitute the values in equation (1) for oxygen as follows.

$Formal charge=Group number−valence electrons=6−7=−1$

Thus, the formal charge on each oxygen atom is $−1$ .

The valence electrons of chlorine atom in given species are $7$ . The group number for chlorine atom is $7$ . Substitute the values in equation (1) for chlorine atom as follows.

$Formal charge=Group number−valence electrons=7−7=0$