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 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.

Figure 1

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

$\text{Formal}\text{charge}=\text{Group}\text{number}-\text{valence}\text{electrons}$ …(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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 6-7\\ & =& -1\end{array}$

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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 7-4\\ & =& 3\end{array}$

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

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

$\begin{array}{rll}\text{Total}\text{charge}& =& 3+\left(-1\right)\times 4\\ & =& -1\end{array}$

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.

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.

Figure 2

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

$\text{Formal}\text{charge}=\text{Group}\text{number}-\text{valence}\text{electrons}$ …(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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 6-7\\ & =& -1\end{array}$

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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 5-4\\ & =& 1\end{array}$

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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 4-4\\ & =& 0\end{array}$

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

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

$\begin{array}{rll}\text{Total}\text{charge}& =& 1+\left(-1\right)+0\\ & =& 0\end{array}$

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.

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.

Figure 3

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

$\text{Formal}\text{charge}=\text{Group}\text{number}-\text{valence}\text{electrons}$ …(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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 6-6\\ & =& 0\end{array}$

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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 6-7\\ & =& -1\end{array}$

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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 6-5\\ & =& 1\end{array}$

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

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

$\begin{array}{rll}\text{Total}\text{charge}& =& 1+\left(-1\right)+0\\ & =& 0\end{array}$

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.

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.

Figure 4

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

$\text{Formal}\text{charge}=\text{Group}\text{number}-\text{valence}\text{electrons}$ …(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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 4-4\\ & =& 0\end{array}$

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.

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.

Figure 5

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

$\text{Formal}\text{charge}=\text{Group}\text{number}-\text{valence}\text{electrons}$ …(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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 4-4\\ & =& 0\end{array}$

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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 4-4\\ & =& 0\end{array}$

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.

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.

Figure 6

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

$\text{Formal}\text{charge}=\text{Group}\text{number}-\text{valence}\text{electrons}$ …(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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 6-7\\ & =& -1\end{array}$

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.

$\begin{array}{rll}\text{Formal}\text{charge}& =& \text{Group}\text{number}-\text{valence}\text{electrons}\\ & =& 7-7\\ & =& 0\end{array}$

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

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

$\begin{array}{rll}\text{Total}\text{charge}& =& 0+\left(-1\right)\\ & =& -1\end{array}$

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 $-1$.