Chapter 12, Problem 34E

Interpretation Introduction

(a)

Interpretation:

The electron dot formula and structural formula for ${\text{Cl}}_{\text{2}}$ molecule, is to be stated.

Concept introduction:

The electron dot formula shows the valence electrons which form the bond between the atoms in a molecule. The electron pairs that are shared by the atoms are known as bonding electrons. The other electrons that are present in order to complete the octet are known as non-bonding electrons. The electron dot formula is also known as the Lewis structure.

Answer to Problem 34E

The electron dot formula for ${\text{Cl}}_{\text{2}}$ molecule is shown below.

The structural formula for ${\text{Cl}}_{\text{2}}$ molecule is shown below.

Explanation of Solution

The total number of valence electron in ${\text{Cl}}_{\text{2}}$ molecule is the sum of valence electron of two chlorine atom. The number of valence electron in each chlorine atom is seven. Therefore, the total number of valence electron in ${\text{Cl}}_{\text{2}}$ molecule is fourteen $\left(14e^{-}\right)$. The number of electron pair is seven $\left(14/2=7\right)$. The electron dot formula for ${\text{Cl}}_{\text{2}}$ molecule is shown below.

Figure 1

Out of seven electron pairs, only one electron pair is involved in bonding. Therefore, there is six lone pair. The structural formula for ${\text{Cl}}_{\text{2}}$ molecule is shown below.

Figure 2

Conclusion

The electron dot formula for ${\text{Cl}}_{\text{2}}$ molecule is shown in figure 1.

The structural formula for ${\text{Cl}}_{\text{2}}$ molecule is shown in figure 2.

Interpretation Introduction

(b)

Interpretation:

The electron dot formula and structural formula for ${\text{O}}_{\text{2}}$ molecule, is to be stated.

Concept introduction:

The electron dot formula shows the valence electrons which form the bond between the atoms in a molecule. The electron pairs that are shared by the atoms are known as bonding electrons. The other electrons that are present in order to complete the octet are known as non-bonding electrons. The electron dot formula is also known as the Lewis structure.

Answer to Problem 34E

The electron dot formula for ${\text{O}}_{\text{2}}$ molecule is shown below.

The structural formula for ${\text{F}}_{\text{2}}$ molecule is shown below.

Explanation of Solution

The total number of valence electron in ${\text{O}}_{\text{2}}$ molecule is the sum of valence electron of two oxygen atom. The number of valence electron in each oxygen atom is six. Therefore, the total number of valence electron in ${\text{O}}_{\text{2}}$ molecule is twelve $\left(12e^{-}\right)$. The number of electron pair is six $\left(12/2=6\right)$. The electron dot formula for ${\text{O}}_{\text{2}}$ molecule is shown below.

Figure 3

Out of six electron pairs, only two electron pair is involved in bonding. Therefore, there is four lone pair. The structural formula for ${\text{O}}_{\text{2}}$ molecule is shown below.

Figure 4

Conclusion

The electron dot formula for ${\text{O}}_{\text{2}}$ molecule is shown in Figure 3.

The structural formula for ${\text{O}}_{\text{2}}$ molecule is shown in Figure 4.

Interpretation Introduction

(c)

Interpretation:

The electron dot formula and structural formula for $\text{HI}$ molecule, is to be stated.

Concept introduction:

The electron dot formula shows the valence electrons which form the bond between the atoms in a molecule. The electron pairs that are shared by the atoms are known as bonding electrons. The other electrons that are present in order to complete the octet are known as non-bonding electrons. The electron dot formula is also known as the Lewis structure.

Answer to Problem 34E

The electron dot formula for $\text{HI}$ molecule is shown below.

The structural formula for $\text{HI}$ molecule is shown below.

Explanation of Solution

The total number of valence electron in $\text{HI}$ molecule is the sum of valence electron of one hydrogen atom and one iodine atom. The number of valence electron in each iodine atom is seven. The number of valence electron in each hydrogen atom is one. Therefore, the total number of valence electron in $\text{HI}$ molecule is eight $\left(8e^{-}\right)$. The number of electron pair is four $\left(8/2=4\right)$. The electron dot formula for $\text{HI}$ molecule is shown below.

Figure 5

Out of four electron pairs, one electron pair is involved in bonding. Therefore, there is three lone pair. The structural formula for $\text{HI}$ molecule is shown below.

Figure 6

Conclusion

The electron dot formula for $\text{HI}$ molecule is shown in Figure 5.

The structural formula for $\text{HI}$ molecule is shown in Figure 6.

Interpretation Introduction

(d)

Interpretation:

The electron dot formula and structural formula for ${\text{PH}}_3$ molecule, is to be stated.

Concept introduction:

The electron dot formula shows the valence electrons which form the bond between the atoms in a molecule. The electron pairs that are shared by the atoms are known as bonding electrons. The other electrons that are present in order to complete the octet are known as non-bonding electrons. The electron dot formula is also known as the Lewis structure.

Answer to Problem 34E

The electron dot formula for ${\text{PH}}_3$ molecule is shown below.

The structural formula for ${\text{PH}}_3$ molecule is shown below.

Explanation of Solution

The total number of valence electron in ${\text{PH}}_3$ molecule is the sum of valence electron of one phosphorous atom and three hydrogen atoms. The number of valence electron in each phosphorous atom is five. The number of valence electron in each hydrogen atom is one. Therefore, the total number of valence electron in ${\text{PH}}_3$ molecule is eight $\left(8e^{-}\right)$. The number of electron pair is four $\left(8/2=4\right)$. The electron dot formula for ${\text{PH}}_3$ molecule is shown below.

Figure 7

Out of four electron pairs, three electron pair is involved in bonding. Therefore, there is one lone pair. The structural formula for ${\text{PH}}_3$ molecule is shown below.

Figure 8

Conclusion

The electron dot formula for ${\text{PH}}_3$ molecule is shown in Figure 7.

The structural formula for ${\text{PH}}_3$ molecule is shown in Figure 8.