Chapter 12, Problem 19QAP

Which brand in each of the following pairs has the greater ionic character?

msp;  $\begin{array}{l}\text{a}.\text{ Na}—\text{F or Na}—\text{I} \text{b}.\text{ Li}——\text{Cl or Cs}—\text{Cl}\\ \text{c}.\text{ Ca}-\text{S or C}—0 \text{d}.\text{ Mg}—\text{N or Mg}—\text{P}\end{array}$

Interpretation Introduction

(a)

Interpretation:

Among the given pair of bonds, the bond that possesses the greater ionic character is to be identified.

Concept Introduction:

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

In ionic compounds, the bonding is formed by the complete transfer of the electrons between the atoms to achieve the stable electron configuration like the noble gases. The higher electronegativity difference between two atoms of a compound corresponds to the greater ionic character of the compound.

Answer to Problem 19QAP

Among the given pair of bonds, the bond that possesses the greater ionic character is $\text{Na}-\text{F}$.

Explanation of Solution

The given pair of bonds is $\text{Na}-\text{F}$ and $\text{Na}-\text{I}$.

The electronegativity value of sodium is $0.9$.

The electronegativity value of fluorine is $4.0$.

The electronegativity value of iodine is $2.5$.

The difference in the electronegativity values for $\text{Na}-\text{F}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Na}-\text{F bond}=4.0-0.9\\ =3.1\end{array}$

The difference in the electronegativity values for $\text{Na}-\text{I}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Na}-\text{I bond}=2.5-0.9\\ =1.6\end{array}$

The difference in the electronegativity values for $\text{Na}-\text{F}$ bond is $3.1$ and for $\text{Na}-\text{I}$ bond is $1.6$.

Thus, the difference in the electronegativity values for $\text{Na}-\text{F}$ bond is higher than the difference in the electronegativity values for $\text{Na}-\text{I}$ bond. Hence, $\text{Na}-\text{F}$ bond possesses the greater ionic character than $\text{Na}-\text{I}$ bond.

Interpretation Introduction

(b)

Interpretation:

Among the given pair of bonds, the bond that possesses the greater ionic character is to be identified.

Concept Introduction:

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

In ionic compounds, the bonding is formed by the complete transfer of the electrons between the atoms to achieve the stable electron configuration like the noble gases. The higher electronegativity difference between two atoms of a compound corresponds to the greater ionic character of the compound.

Answer to Problem 19QAP

Among the given pair of bonds, the bond that possesses the greater ionic character is $\text{Ca}-\text{O}$.

Explanation of Solution

The given pair of bonds is $\text{Ca}-\text{S}$ and $\text{Ca}-\text{O}$.

The electronegativity value of calcium is $1.0$.

The electronegativity value of sulfur is $2.5$.

The electronegativity value of oxygen is $3.5$.

The difference in the electronegativity values for $\text{Ca}-\text{S}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Ca}-\text{S bond}=2.5-1.0\\ =1.5\end{array}$

The difference in the electronegativity values for $\text{Ca}-\text{O}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Ca}-\text{O bond}=3.5-1.0\\ =2.5\end{array}$

The difference in the electronegativity values for $\text{Ca}-\text{O}$ bond is $2.5$ and for $\text{Ca}-\text{S}$ bond is $1.5$.

Thus, the difference in the electronegativity values for $\text{Ca}-\text{O}$ bond is higher than the difference in the electronegativity values for $\text{Ca}-\text{S}$ bond. Hence, $\text{Ca}-\text{O}$ bond possesses the greater ionic character than $\text{Ca}-\text{S}$ bond.

Interpretation Introduction

(c)

Interpretation:

Among the given pair of bonds, the bond that possesses the greater ionic character is to be identified.

Concept Introduction:

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

In ionic compounds, the bonding is formed by the complete transfer of the electrons between the atoms to achieve the stable electron configuration like the noble gases. The higher electronegativity difference between two atoms of a compound corresponds to the greater ionic character of the compound.

Answer to Problem 19QAP

Among the given pair of bonds, the bond that possesses the greater ionic character is $\text{Cs}-\text{Cl}$.

Explanation of Solution

The given pair of bonds is $\text{Li}-\text{Cl}$ and $\text{Cs}-\text{Cl}$.

The electronegativity value of chlorine is $3.0$.

The electronegativity value of lithium is $1.0$.

The electronegativity value of cesium is $0.7$.

The difference in the electronegativity values for $\text{Li}-\text{Cl}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Li}-\text{Cl bond}=3.0-1.0\\ =2.0\end{array}$

The difference in the electronegativity values for $\text{Cs}-\text{Cl}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Cs}-\text{Cl bond}=3.0-0.7\\ =2.3\end{array}$

The difference in the electronegativity values for $\text{Li}-\text{Cl}$ bond is $2.0$ and for $\text{Cs}-\text{Cl}$ bond is $2.3$.

Thus, the difference in the electronegativity values for $\text{Cs}-\text{Cl}$ bond is higher than the difference in the electronegativity values for $\text{Li}-\text{Cl}$ bond. Hence, $\text{Cs}-\text{Cl}$ bond possesses the greater ionic character than $\text{Li}-\text{Cl}$ bond.

Interpretation Introduction

(d)

Interpretation:

Among the given pair of bonds, the bond that possesses the greater ionic character is to be predicted.

Concept Introduction:

The ability that is possessed by an atom to attract the bonding pair of electrons towards itself is known as electronegativity. The electronegativity decreases while going down the group and increases while moving left to right in the period.

In ionic compounds, the bonding is formed by the complete transfer of the electrons between the atoms to achieve the stable electron configuration like the noble gases. The higher electronegativity difference between two atoms of a compound corresponds to the greater ionic character of the compound.

Answer to Problem 19QAP

Among the given pair of bonds, the bond that possesses the greater ionic character is $\text{Mg}-\text{N}$.

Explanation of Solution

The given pair of bonds is $\text{Mg}-\text{N}$ and $\text{Mg}-\text{P}$.

The electronegativity value of magnesium is $1.2$.

The electronegativity value of nitrogen is $3.0$.

The electronegativity value of phosphorus is $2.1$.

The difference in the electronegativity values for $\text{Mg}-\text{N}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Mg}-\text{N bond}=3.0-1.2\\ =1.8\end{array}$

The difference in the electronegativity values for $\text{Mg}-\text{P}$ bond is,

$\begin{array}{c}\text{Difference}\text{in}\text{electronegativity for Mg}-\text{P bond}=2.1-1.2\\ =0.9\end{array}$

The difference in the electronegativity values for $\text{Mg}-\text{N}$ bond is $1.8$ and for $\text{Mg}-\text{P}$ bond is $0.9$.

Thus, the difference in the electronegativity values for $\text{Mg}-\text{N}$ bond is higher than the difference in the electronegativity values for $\text{Mg}-\text{P}$ bond. Hence, $\text{Mg}-\text{N}$ bond possesses the greater ionic character than $\text{Mg}-\text{P}$ bond.