Chapter 1, Problem 1.44P

Interpretation Introduction

(a)

Interpretation:

Lewis structure for the ${\text{CH}}_5\text{N}$ is to be drawn.

Concept introduction:

Lewis structure is a convenient way to convey information such as which atoms are bonded to each other by which type of bond. Only valence electrons take part to draw Lewis structure.

Valence electrons that participate in bond formation are called bonding electron pairs whereas electrons that do not take part in bonding and that remain as non-bonding electrons are termed as lone pair of electrons.

Lewis structure is drawn from the total valence electron count of each atom in the molecule. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom. Electrons that participate in forming the bond are bonding electrons. Remaining electrons are distributed first to outer atoms such that each atom completes its octet other than hydrogen.

Answer to Problem 1.44P

Lewis structure for ${\text{CH}}_5\text{N}$ is as follow

Explanation of Solution

The given molecule ${\text{CH}}_5\text{N}$ has $\text{14}$ valence electron in total, with carbon as the central atom bonded to three hydrogen atoms and one nitrogen atom. Remaining two hydrogen atoms are bonded to a nitrogen atom. Therefore total $\text{12}$ valence electrons participate in the bond formation.

Thus the skeleton structure for $\text{CH5N}$ is:

Remaining two valence electrons are contributed as lone pair of electrons to the outer atom which is nitrogen.

Hence the complete Lewis structure for ${\text{CH}}_5\text{N}$ is as follow

Conclusion

Lewis structure for ${\text{CH}}_5\text{N}$ is drawn from total valence electron count.

Interpretation Introduction

(b)

Interpretation:

Lewis structure for ${\text{CH}}_{\text{3}}{\text{NO}}_{\text{2}}$ molecule is to be drawn.

Concept introduction:

Lewis structure is drawn from the total valence electron count of each atom in the molecule. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom. Electrons that participate in forming the bond are bonding electrons. Remaining electrons are distributed first to outer atoms such that each atom complete its octet other than hydrogen.

Answer to Problem 1.44P

Lewis structure for ${\text{CH}}_{\text{3}}{\text{NO}}_{\text{2}}$ molecule is as follows

Explanation of Solution

In ${\text{CH}}_{\text{3}}{\text{NO}}_{\text{2}}$, carbon is the central atom bonded to three hydrogen and one nitrogen atom with two oxygen atom, therefore there are total $\text{24}$ valence electrons. Also, the structure should contain a bond between carbon and nitrogen but there should be no bonds between carbon and oxygen. Twelve electrons participate in bond formation and form the skeleton structure as:

Remaining $12$ electrons contributed as lone pairs to the outer oxygen atom. One lone pair of electrons from either oxygen atom involved in the bonding to complete octet.

Conclusion

Lewis structure for ${\text{CH}}_{\text{3}}{\text{NO}}_{\text{2}}$ molecule is drawn from the total valence electron count.

Interpretation Introduction

(c)

Interpretation:

Lewis structure for ${\text{CH}}_{\text{2}}\text{O}$ molecule is to be drawn.

Concept introduction:

Lewis structure is drawn from the total valence electron count of each atom in the molecule. Valence electrons participate in bond formation are called bonding electron pairs whereas electrons that do not take part in bonding and that remain as non-bonding electrons are termed as lone pair of electrons. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom.

Lone pair of electrons contributed to outer atoms to complete octet except hydrogen.

Answer to Problem 1.44P

The Lewis structure for ${\text{CH}}_{\text{2}}\text{O}$ molecule is

Explanation of Solution

Carbon is the central atom in ${\text{CH}}_{\text{2}}\text{O}$ molecule bonded to two hydrogen atoms and one oxygen atom. There are total twelve valence electrons, six electrons participates in bond formation. Thus the skeleton structure is as below:

Remaining six electrons are contributed as lone pairs to the outer atom oxygen but one electron is involved in bonding with complete octet of oxygen atom.

Conclusion

Lewis structure is drawn from the total valence electron count.

Interpretation Introduction

(d)

Interpretation:

Lewis structure for ${\text{CH}}_{\text{2}}{\text{Cl}}_{\text{2}}$ molecule is to be drawn.

Concept introduction:

Lewis structure is drawn from the total valence electron count of each atom in the molecule. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom. Electrons that participate in forming the bond are bonding electrons. Remaining electrons are distributed first to outer atoms such that each atom completes its octet other than hydrogen.

Answer to Problem 1.44P

Lewis structure for ${\text{CH}}_{\text{2}}{\text{Cl}}_{\text{2}}$ molecule is shown below:

Explanation of Solution

In ${\text{CH}}_{\text{2}}{\text{Cl}}_{\text{2}}$ molecule, less electronegative carbon is the central atom bonded to two hydrogen and two chlorine atoms. Thus the skeleton structure for ${\text{CH}}_{\text{2}}{\text{Cl}}_{\text{2}}$ molecule is drawn as

Eight electrons from total $20$ valence electrons participate in bonding and remaining $12$ electrons are contributed as lone pair of electrons on outer chlorine atom.

Therefore the Lewis structure for ${\text{CH}}_{\text{2}}{\text{Cl}}_{\text{2}}$ molecule is as follows:

Conclusion

Lewis structure is drawn from total valence electron count.

Interpretation Introduction

(e)

Interpretation:

Lewis structure for $\text{BrCN}$ molecule is to be drawn.

Concept introduction:

Lewis structure is drawn from the total valence electron count of each atom in the molecule. Valence electrons that participate in bond formation are called bonding electron pairs whereas electrons that do not take part in bonding and that remain as non-bonding electrons are termed as lone pair of electrons. Skeleton structure for the given molecule is drawn with atoms bonded with a single bond, the central atom is always less electronegative atom.

Lone pair of electrons contributed to outer atoms to complete octet except hydrogen.

Answer to Problem 1.44P

Lewis structure for $\text{BrCN}$ molecule is as shown below

Explanation of Solution

The given molecule $\text{BrCN}$ carbon is the central bonded to one bromine and one nitrogen atom. Therefore there are total $16$ valence electron in the molecule, four electrons participates in bond formation. Thus the skeleton structure for $\text{BrCN}$ is as follows:

Remaining $12$ electrons are contributed as a lone pair to the outer bromine and nitrogen atom. But to complete the octet of carbon lone pair from nitrogen participates in bond formation between carbon and nitrogen.

Hence the Lewis structure for $\text{BrCN}$ is as follows:

Conclusion

Lewis structure is drawn from total valence electron count.