   Chapter 8, Problem 35PS

Chapter
Section
Textbook Problem

Compare the electron dot structures of the hydrogen carbonate ion and nitric acid. (a) Are these species isoelectronic? (b) How many resonance structures does each species have? (c) What are the formal charges of each atom in these species? (d) Compare the two species with respect to their acid-base behavior. (Can either or both species behave as a base and form a bond to H+?)

a)

Interpretation Introduction

Interpretation:

By comparing electron dot structures of the hydrogen carbonate ion and nitric acid, the isoelectronic nature has to be determined.

Concept Introduction:

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

Resonance structures:

A molecule or ion which show more than structure but none of them are accurately correct show the known property of that molecule, and can lie between the canonical structure is known as resonance or canonical or contributing structure.

Explanation

Yes, these species are isoelectronic

HCO3-:_ValenceelectronofHydrogen: 1ValenceelectronofCarbon:4Valence of Oxygen: 6×3=18=(1+4+18)+1=24electrons

(b)

Interpretation Introduction

Interpretation:

Number of Resonance structures do each species have, has to be determined.

Concept Introduction:

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

Resonance structures:

A molecule or ion which show more than structure but none of them are accurately correct show the known property of that molecule, and can lie between the canonical structure is known as resonance or canonical or contributing structure.

(c)

Interpretation Introduction

Interpretation:

The formal charge of each atom in these species has to be determined.

Concept Introduction:

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

Resonance structures:

A molecule or ion which show more than structure but none of them are accurately correct show the known property of that molecule, and can lie between the canonical structure is known as resonance or canonical or contributing structure.

(d)

Interpretation Introduction

Interpretation:

The given two species, the acid-base behaviour has to be compared.

Concept Introduction:

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

Resonance structures:

A molecule or ion which show more than structure but none of them are accurately correct show the known property of that molecule, and can lie between the canonical structure is known as resonance or canonical or contributing structure.

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