Chapter 10, Problem 117IAE

Interpretation Introduction

(a)

Interpretation:

The percent ionic character for LiBr and NaCl bonds separately needs to be determined.

Concept introduction:

Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic.

In a bond, the dipole moment can be calculated as follows:

$\mu =\delta \times \text{d}$

Here,

µ = Dipole mment

δ = Partial charge

d = Distance

Interpretation Introduction

(b)

Interpretation:

The calculated ionic characters of LiBr and NaCl needs to be compared with given theoretical values of figure based on electronegativity values.

Concept introduction:

Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic.

In a bond, the dipole moment can be calculated as follows:

$\mu =\delta \times \text{d}$

Here,

µ = Dipole mment

δ = Partial charge

d = Distance

Interpretation Introduction

(c)

Interpretation:

The reason for equality of calculated percentage ionic values and given data based on electronegativity needs to be explained.

Concept introduction:

Several empirical equations have been proposed to calculate the percentage ionic character in the bond. It is important to note that no bond (even ionic) in chemistry is 100% ionic.

In a bond, the dipole moment can be calculated as follows:

$\mu =\delta \times \text{d}$

Here,

µ = Dipole mment

δ = Partial charge

d = Distance