Chapter 1, Problem 40P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge for each of the given atom has to be given.

Concept Introduction:

Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.

Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.

$\begin{array}{l}\text{Formal charge= }\left({\text{number of valence e}}^{\text{-}}\right)\text{-}\left({\text{number of lone pair e}}^{\text{-}}\right)\\ {\text{- 1/}}_{\text{2}}\left(\text{number of bond electrons}\right)\end{array}$

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

(b)

Interpretation Introduction

Interpretation:

The appropriate formal charge for each of the given atom has to be given.

Concept Introduction:

Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.

Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.

$\begin{array}{l}\text{Formal charge= }\left({\text{number of valence e}}^{\text{-}}\right)\text{-}\left({\text{number of lone pair e}}^{\text{-}}\right)\\ {\text{- 1/}}_{\text{2}}\left(\text{number of bond electrons}\right)\end{array}$

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

(c)

Interpretation Introduction

Interpretation:

The appropriate formal charge for each of the given atom has to be given.

Concept Introduction:

Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.

Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.

$\begin{array}{l}\text{Formal charge= }\left({\text{number of valence e}}^{\text{-}}\right)\text{-}\left({\text{number of lone pair e}}^{\text{-}}\right)\\ {\text{- 1/}}_{\text{2}}\left(\text{number of bond electrons}\right)\end{array}$

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.

(d)

Interpretation Introduction

Interpretation:

The appropriate formal charge for each of the given atom has to be given.

Concept Introduction:

Formal charge: The formal charge is defined as the charge carried by an atom in a molecule assuming that, irrespective of the relative electronegativity of the shared atoms, all the chemical bonds are shared equally between the two atoms.

Formal Charge: The formal charge on atoms in the Lewis structure is calculated by the equation below.

$\begin{array}{l}\text{Formal charge= }\left({\text{number of valence e}}^{\text{-}}\right)\text{-}\left({\text{number of lone pair e}}^{\text{-}}\right)\\ {\text{- 1/}}_{\text{2}}\left(\text{number of bond electrons}\right)\end{array}$

Lewis structure: The bonding between atoms in a molecule satisfies the octet rule of valence electrons and the lone pairs also exist in the molecule. The electron is represented as dot.