Chapter 1, Problem 1.24P

Interpretation Introduction

(a)

Interpretation:

For the given species, the complete Lewis structure is to be completed by adding multiple bonds and/or lone pairs.

Concept introduction:

In order to draw a Lewis structure for a molecule, start by counting the total number of valence electrons in a molecule. The number of valence electrons by each atom is the same as its group number. For the given skeleton of the molecule, distribute the remaining electrons as lone pairs. In doing so, start with the outer atoms and work inwards. Try to achieve an octet on each atom other than hydrogen. If there is an atom with less than an octet, increase the atom’s share of electrons by converting lone pairs from neighboring atoms to bonding pairs thereby creating double or triple bonds. For an uncharged atom, carbon atoms will have a maximum of four bonds; Nitrogen will have three bonds and one lone pair, while oxygen will have two bonds and two lone pairs. Hydrogen always contributes to one bond. The number of bonds in case of halogen is one; while there will be three lone pair of electrons on halide atoms.

Answer to Problem 1.24P

The complete Lewis structure for the given species is:

Explanation of Solution

The given species is:

The formula for the species above is ${\text{C}}_{\text{2}}{\text{H}}_{\text{5}}\text{NO}$. The total number of valence electrons for the structure is $\text{24}$. The arrangement of atoms is given which attributes to the distribution of $\text{18}$ valence electrons. Thus, there remain $\text{6}$ electrons which need to be distributed.

The carbon atom on the left side has four bonds, thus, its octet is complete. The carbon atom in the middle has four bonds, hence, its octet is also complete. The nitrogen atom has three bonds, thus, its octet is not complete. There should be one lone pair of electron on nitrogen. The double bonded oxygen atom has got two bonds. Thus, in order to complete its octet, it should possess two lone pair of electrons. Thus, all the $\text{24}$ electrons have been distributed. Thus, the complete Lewis structure for the given species is:

Conclusion

The complete Lewis structure for the given species including multiple bonds and lone pairs is shown in Figure 1 above.

Interpretation Introduction

(b)

Interpretation:

For given species, the complete Lewis structure is to be completed by adding multiple bonds and/or lone pairs.

Concept introduction:

In order to draw a Lewis structure for a molecule, start by counting the total number of valence electrons in a molecule. The number of valence electrons by each atom is the same as its group number. For a charged species, each negative charge increases the number of valence electrons by one while each positive charge decreases the number of valence electrons by one. For the given skeleton of the molecule, distribute the remaining electrons as lone pairs. In doing so, start with the outer atoms and work inwards. Try to achieve an octet on each atom other than hydrogen. If there is an atom with less than an octet, increase the atom’s share of electrons by converting lone pairs from neighboring atoms to bonding pairs thereby creating double or triple bonds. For an uncharged atom, carbon atoms will have maximum of four bonds. Nitrogen will have three bonds and one lone pair, while oxygen will have two bonds and two lone pairs. Hydrogen always contributes to one bond. The number of bond in case of halogen is one, while there will be three lone pair of electrons on halide atoms.

Answer to Problem 1.24P

The complete Lewis structure for the given species is:

Explanation of Solution

The given species is:

The formula for the species above is ${\text{C}}_{\text{2}}{\text{H}}_{\text{6}}{\text{N}}^{-}$. The total number of valence electrons for the structure is $19$. One negative charge adds to the total valence electron, count to make it $20$. The arrangement of atoms is given which attributes to distribution of $16$ valence electrons. Thus, there remain $\text{4}$ electrons which need to be distributed.

The carbon atom on the left as well as on the right has four bonds, thus, their octets are complete. The nitrogen atom has two bonds and a negative formal charge. This suggests that the remaining four electrons should be present on the nitrogen atom so as to complete its octet and have a negative formal charge. Thus, the complete Lewis structure for the given species is:

Conclusion

The complete Lewis structure for the given species including multiple bonds and lone pairs is shown in Figure 2 above.

Interpretation Introduction

(c)

Interpretation:

For given species, the complete Lewis structure is to be completed by adding multiple bonds and/or lone pairs.

Concept introduction:

In order to draw a Lewis structure for a molecule, start by counting the total number of valence electrons in a molecule. The number of valence electrons by each atom is the same as its group number. For a charged species, each negative charge increase the number of valence electrons by one while each positive charge decrease the number of valence electrons by one. For the given skeleton of the molecule, distribute the remaining electrons as lone pairs. In doing so, start with the outer atoms and work inwards. Try to achieve an octet on each atom other than hydrogen. If there is an atom with less than an octet, increase the atom’s share of electrons by converting lone pairs from neighboring atoms to bonding pairs thereby creating double or triple bonds. For an uncharged atom, carbon atoms will have maximum of four bonds. Nitrogen will have three bonds and one lone pair, while oxygen will have two bonds and two lone pairs. Hydrogen always contributes to one bond. The number of bond in case of halogen is one, while there will be three lone pair of electrons on halide atoms.

Answer to Problem 1.24P

The complete Lewis structure for the given species is:

Explanation of Solution

The given species is:

The formula for the species above is ${\text{CH}}_{\text{6}}{\text{N}}^{+}$. The total number of valence electrons for the structure is $15$. One positive charge decreases the total valence electron count to make it $14$. The arrangement of atoms is given which attributes to distribution of $14$ valence electrons. Thus, no electron remains, and all the electrons have been distributed. Thus, the given structure is a complete Lewis structure for the given species is:

Conclusion

The complete Lewis structure for the given species including multiple bonds and lone pairs is shown in Figure 2 above.

Interpretation Introduction

(d)

Interpretation:

For given species, the complete Lewis structure is to be completed by adding multiple bonds and/or lone pairs.

Concept introduction:

In order to draw a Lewis structure for a molecule, start by counting the total number of valence electrons in a molecule. The number of valence electrons by each atom is the same as its group number. For a charged species, each negative charge increase the number of valence electrons by one while each positive charge decrease the number of valence electrons by one. For the given skeleton of the molecule, distribute the remaining electrons as lone pairs. In doing so, start with the outer atoms and work inwards. Try to achieve an octet on each atom other than hydrogen. If there is an atom with less than an octet, increase the atom’s share of electrons by converting lone pairs from neighboring atoms into bonding pairs thereby creating double or triple bonds. For an uncharged atom, carbon atoms will have maximum of four bonds. Nitrogen will have three bonds and one lone pair, while oxygen will have two bonds and two lone pairs. Hydrogen always contributes to one bond. The number of bond in case of halogen is one, while there will be three lone pair of electrons on halide atoms.

Answer to Problem 1.24P

The complete Lewis structure for the given species is:

Explanation of Solution

The given species is:

The formula for the species above is ${\text{C}}_2{\text{H}}_5{}^{+}$. The total number of valence electrons for the structure is $13$. One positive charge decreases the total valence electron, count to make it $12$. The arrangement of atoms is given which attributes to the distribution of $12$ valence electrons. Thus, no electron remains, and all the electrons have been distributed. Thus, the given structure is a complete Lewis structure for the given species:

Conclusion

The complete Lewis structure for the given species including multiple bonds and lone pairs is shown in Figure 4 above.