   Chapter 8.7, Problem 8.11CYU

Chapter
Section
Textbook Problem

For each of the following pairs of bonds, decide which is more polar. For each polar bond, indicate the positive and negative poles. After making your prediction from the relative atom positions in the periodic table, check your prediction by calculating. ∆X from electronegativity values in Figure 8.11. (a) H—F and H—I (b) B—C and B—F (c) C—Si and C—S

(a)

Interpretation Introduction

Interpretation: The most polar bond from the given pairs should be determined also the positive negative poles and Δx should be determined.

Concept Introduction:

Polarity is the separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multiple moments.

Polar molecule must contain polar bond due to presence of electronegativity difference between the bonded atoms.

Dipole: The positive and negative charges separated by the distance between them.

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.

Explanation

H-F

H and F lie apart from each other in the periodic table, where F belongs to halogen that has more capacity to abstract electrons than hydrogen since electronegativity character increases as we move from left to right of the table.  Hence in H-F-Hydrogen is the positive pole and fluorine is the negative pole.  The Δx value is 1.8 [= 4.0(forF)- 2.2(forH)].

Similarly for H-I,

H and I lie apart from each other in the periodic table, where I belongs to halogen that has more capacity to abstract electrons than hydrogen since electronegativity character increases as we move from left to right of the table

(b)

Interpretation Introduction

Interpretation: The most polar bond from the given pairs should be determined also the positive negative poles and Δx should be determined.

Concept Introduction:

Polarity is the separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multiple moments.

Polar molecule must contain polar bond due to presence of electronegativity difference between the bonded atoms.

Dipole: The positive and negative charges separated by the distance between them.

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.

(c)

Interpretation Introduction

Interpretation: The most polar bond from the given pairs should be determined also the positive negative poles and Δx should be determined.

Concept Introduction:

Polarity is the separation of electric charge leading to a molecule or its chemical groups having an electric dipole or multiple moments.

Polar molecule must contain polar bond due to presence of electronegativity difference between the bonded atoms.

Dipole: The positive and negative charges separated by the distance between them.

Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.

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