Chapter 1.4, Problem 7PTS

(a)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (a)

(b)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (b)

(c)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (c)

(d)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (d)

(e)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (e)

(f)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (f)

(g)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (g)

(h)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (h)

(i)

Interpretation Introduction

Interpretation: For the given set of molecules the presence of formal charge of atom should be identified.

Concept Introduction: Formal charge of an atom can be assigned by assuming the electrons which does not correspond to the valence electrons of the respective atom.

Valence electrons represent the electrons present in the outermost shell of an atom.

Non-bonded electrons are the electrons that do not participate in bonding. These electrons are also termed as lone pair of electrons.

Each atom has a specific number of valence electrons.  If the valence electrons in that atom are reduced by one number, it gets positive charge.  If the valence electrons in that atom are increased by one number, it gets negative charge.

Formal charge of an atom can be identified by drawing the molecules in Lewis structures.

The Lewis structure of small molecules can be drawn by combining the Lewis dot structures of the atoms involved in the formation of that compound.

Formal charge of an atom can be calculated by using the formula given below.

$\text{Formal}\text{charge}\left(\text{FC}\right)\text{=}\left[\text{number}\text{of}\text{valence}\text{electrons}\text{on}\text{atom}\right]\text{-}\left[\text{non}\text{bonded}\text{electrons+}\text{number}\text{of}\text{bonds}\right]$

To find: Establish the total number of valence electrons for each atom in the given molecule (i)