Chapter 11, Problem 43E

a)

Interpretation Introduction

Interpretation: The dissolution of the following in water or ${\text{CCl}}_{\text{4}}$ has to be predicted.

Concept Introduction:

The bonds involving the atoms with various electronegativites having a large dipole moment are called as polar solvents. Example of polar solvent is Water.

The bonds involving the atoms with same electronegativites are called as non polar solvents. Examples of non polar solvents are Gasoline, Carbon tetrachloride etc

Water is a polar solvent as well as dissolves polar solutes and ionic solutes. Carbon tetrachloride

( ${\text{CCl}}_{\text{4}}$) is a non-polar solvent and dissolves non-polar solutes. To predict the split of the subsequent molecules, draw the correct Lewis structure and then determine if the entity bond dipoles cancel or not. But the bond dipoles are approved in such a manner that they cancel each other out, then the molecule is non-polar. If the bond dipoles do not withdraw each extra out, then the molecule is polar.

Answer to Problem 43E

Answer

${\text{KrF}}_{\text{2}}$ dissolves in ${\text{CCl}}_{\text{4}}$

Explanation of Solution

${\text{KrF}}_{\text{2}}$

${\text{8+2(7)=22e}}^{\text{-}}$

${\text{KrF}}_{\text{2}}$ is dissolves in ${\text{CCl}}_{\text{4}}$. ${\text{KrF}}_{\text{2}}$ is non-polar molecule that makes it soluble in non polar solvent

b)

Interpretation Introduction

Interpretation: The dissolution of the following in water or ${\text{CCl}}_{\text{4}}$ has to be predicted.

Concept Introduction:

The bonds involving the atoms with various electronegativites having a large dipole moment are called as polar solvents. Example of polar solvent is Water.

The bonds involving the atoms with same electronegativites are called as non polar solvents. Examples of non polar solvents are Gasoline, Carbon tetrachloride etc

Water is a polar solvent as well as dissolves polar solutes and ionic solutes. Carbon tetrachloride

( ${\text{CCl}}_{\text{4}}$) is a non-polar solvent and dissolves non-polar solutes. To predict the split of the subsequent molecules, draw the correct Lewis structure and then determine if the entity bond dipoles cancel or not. But the bond dipoles are approved in such a manner that they cancel each other out, then the molecule is non-polar. If the bond dipoles do not withdraw each extra out, then the molecule is polar.

Answer to Problem 43E

Answer

${\text{SF}}_{\text{2}}$ dissolves in Water

Explanation of Solution

${\text{SF}}_{\text{2}}$

${\text{6+2(7)=20e}}^{\text{-}}$

${\text{SF}}_{\text{2}}$ is dissolves in Water. ${\text{SF}}_{\text{2}}$ is polar molecule; therefore it is soluble in Water.

c)

Interpretation Introduction

Interpretation: The dissolution of the following in water or ${\text{CCl}}_{\text{4}}$ has to be predicted.

Concept Introduction:

The bonds involving the atoms with various electronegativites having a large dipole moment are called as polar solvents. Example of polar solvent is Water.

The bonds involving the atoms with same electronegativites are called as non polar solvents. Examples of non polar solvents are Gasoline, Carbon tetrachloride etc

Water is a polar solvent as well as dissolves polar solutes and ionic solutes. Carbon tetrachloride

( ${\text{CCl}}_{\text{4}}$) is a non-polar solvent and dissolves non-polar solutes. To predict the split of the subsequent molecules, draw the correct Lewis structure and then determine if the entity bond dipoles cancel or not. But the bond dipoles are approved in such a manner that they cancel each other out, then the molecule is non-polar. If the bond dipoles do not withdraw each extra out, then the molecule is polar.

Answer to Problem 43E

Answer

${\text{SO}}_{\text{2}}$ dissolves in Water

Explanation of Solution

${\text{SO}}_{\text{2}}$

${\text{6+2(6)=18e}}^{\text{-}}$

${\text{SO}}_{\text{2}}$ is dissolves in Water. ${\text{SO}}_{\text{2}}$ is polar molecule; therefore it is soluble in Water.

d).

Interpretation Introduction

Interpretation: The dissolution of the following in water or ${\text{CCl}}_{\text{4}}$ has to be predicted.

Concept Introduction:

The bonds involving the atoms with various electronegativites having a large dipole moment are called as polar solvents. Example of polar solvent is Water.

The bonds involving the atoms with same electronegativites are called as non polar solvents. Examples of non polar solvents are Gasoline, Carbon tetrachloride etc

Water is a polar solvent as well as dissolves polar solutes and ionic solutes. Carbon tetrachloride

( ${\text{CCl}}_{\text{4}}$) is a non-polar solvent and dissolves non-polar solutes. To predict the split of the subsequent molecules, draw the correct Lewis structure and then determine if the entity bond dipoles cancel or not. But the bond dipoles are approved in such a manner that they cancel each other out, then the molecule is non-polar. If the bond dipoles do not withdraw each extra out, then the molecule is polar.

Answer to Problem 43E

Answer

${\text{CO}}_{\text{2}}$ dissolves in ${\text{CCl}}_{\text{4}}$

Explanation of Solution

${\text{CO}}_{\text{2}}$

${\text{4+2(6)=16e}}^{\text{-}}$

${\text{CO}}_{\text{2}}$ is dissolves in ${\text{CCl}}_{\text{4}}$. ${\text{CO}}_{\text{2}}$ is non polar molecule that makes it soluble in non polar solvent

e)

Interpretation Introduction

Interpretation: The dissolution of the following in water or ${\text{CCl}}_{\text{4}}$ has to be predicted.

Concept Introduction:

The bonds involving the atoms with various electronegativites having a large dipole moment are called as polar solvents. Example of polar solvent is Water.

The bonds involving the atoms with same electronegativites are called as non polar solvents. Examples of non polar solvents are Gasoline, Carbon tetrachloride etc

Water is a polar solvent as well as dissolves polar solutes and ionic solutes. Carbon tetrachloride

( ${\text{CCl}}_{\text{4}}$) is a non-polar solvent and dissolves non-polar solutes. To predict the split of the subsequent molecules, draw the correct Lewis structure and then determine if the entity bond dipoles cancel or not. But the bond dipoles are approved in such a manner that they cancel each other out, then the molecule is non-polar. If the bond dipoles do not withdraw each extra out, then the molecule is polar.

Answer to Problem 43E

Answer

${\text{MgF}}_{\text{2}}$ dissolves in Water

Explanation of Solution

${\text{MgF}}_{\text{2}}$ is an ionic compound so it is soluble in water.

${\text{MgF}}_{\text{2}}$ is dissolves in Water. ${\text{MgF}}_{\text{2}}$ is polar molecule; therefore it is soluble in Water.

f).

Interpretation Introduction

Interpretation: The dissolution of the following in water or ${\text{CCl}}_{\text{4}}$ has to be predicted.

Concept Introduction:

The bonds involving the atoms with various electronegativites having a large dipole moment are called as polar solvents. Example of polar solvent is Water.

The bonds involving the atoms with same electronegativites are called as non polar solvents. Examples of non polar solvents are Gasoline, Carbon tetrachloride etc

Water is a polar solvent as well as dissolves polar solutes and ionic solutes. Carbon tetrachloride

( ${\text{CCl}}_{\text{4}}$) is a non-polar solvent and dissolves non-polar solutes. To predict the split of the subsequent molecules, draw the correct Lewis structure and then determine if the entity bond dipoles cancel or not. But the bond dipoles are approved in such a manner that they cancel each other out, then the molecule is non-polar. If the bond dipoles do not withdraw each extra out, then the molecule is polar.

Answer to Problem 43E

Answer

${\text{CH}}_{\text{2}}\text{O}$ dissolves in Water

Explanation of Solution

${\text{CH}}_{\text{2}}\text{O}$

${\text{4+2(1)+6=12e}}^{\text{-}}$

${\text{CH}}_{\text{2}}\text{O}$ is dissolves in Water. ${\text{CH}}_{\text{2}}\text{O}$ is polar molecule; therefore it is soluble in Water.

g)

Interpretation Introduction

Interpretation: The dissolution of the following in water or ${\text{CCl}}_{\text{4}}$ has to be predicted.

Concept Introduction:

The bonds involving the atoms with various electronegativites having a large dipole moment are called as polar solvents. Example of polar solvent is Water.

The bonds involving the atoms with same electronegativites are called as non polar solvents. Examples of non polar solvents are Gasoline, Carbon tetrachloride etc

Water is a polar solvent as well as dissolves polar solutes and ionic solutes. Carbon tetrachloride

( ${\text{CCl}}_{\text{4}}$) is a non-polar solvent and dissolves non-polar solutes. To predict the split of the subsequent molecules, draw the correct Lewis structure and then determine if the entity bond dipoles cancel or not. But the bond dipoles are approved in such a manner that they cancel each other out, then the molecule is non-polar. If the bond dipoles do not withdraw each extra out, then the molecule is polar.

Answer to Problem 43E

Answer

${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}$ dissolves in ${\text{CCl}}_{\text{4}}$

Explanation of Solution

${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}$

${\text{2(4)+4(1)=20e}}^{\text{-}}$

${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}$ is dissolves in ${\text{CCl}}_{\text{4}}$. ${\text{C}}_{\text{2}}{\text{H}}_{\text{4}}$ is non polar molecule that makes it soluble in non polar solvent