Q11.1-5E - Chemistry (OpenStax)

Question

Indicate the most important types of intermolecular attractions in each of the following solutions: 

 

1. The solution in Figure 

         

1. NO (g) in CO (l) 
2. \({\bf{C}}{{\bf{l}}_{\bf{2}}}\) (g) in \({\bf{B}}{{\bf{r}}_{\bf{2}}}\) (l) 
3. HCl(g) in benzene \({{\bf{C}}_{\bf{6}}}{{\bf{H}}_{\bf{6}}}\) (l) 
4. Methanol \({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\) (l) in \({{\bf{H}}_{\bf{2}}}{\bf{O}}\) (l)

Step-by-Step Solution

Answer

1. Ion-dipole forces 
2. Induced Dipole - induced dipole forces
3. Dispersion forces
4. Dispersion forces

      5. Hydrogen bonding

Step 1: (a) Electrostatic forces

As in figure 11.2, \({\bf{K2Cr2O7}}\) solution in water. After the dissociation of \({\bf{K2Cr2O7}}\) we have \({{\bf{K}}^{\bf{ + }}}\) and \({\bf{Cr2O}}{{\bf{7}}^{{\bf{2 - }}}}\)ions in solutions.

The attraction between the \({{\bf{K}}^{\bf{ + }}}\) and \({\bf{Cr2O}}{{\bf{7}}^{{\bf{2 - }}}}\) ions have electrostatic forces of attraction. As in potassium dichromate solution both ions are present

Step 2: (b) Dipole-dipole Forces

An dipole-dipole forces is an attractive force as NO and CO both electronegative atom present (oxygen). Hence both the component of solution have dipole. So, NO (g) in CO(l)   have dipole-dipole intermolecular forces of attractions. 

Step 3: (c) Induced Dipole-Induced dipole forces

Induced dipole-induced dipole interaction is an intermolecular forces between non -polar molecules. Both components (\({\rm{Cl2 and Br2}}\) ) are non-polar in nature. These forces of attractions are also termed as London dispersion forces.

Step 4: (d) Dipole – Induced dipole Forces

In Ion-dipole forces, in which one component is polar and another component is non-polar in nature. As HCl is polar in nature and \({\rm{C6H6}}\)is non-polar in nature. So, in HCl (g) in \({\rm{C6H6}}\)(l) we have dipole –induced dipole forces of attractions.

Step 4: (e) Hydrogen Bonding

A hydrogen bond is a kind of bonding that is present between an atom of hydrogen and a pair of other atoms having a high electronegativity (Oxygen and nitrogen). Hydrogen bonding used to be competitively weaker than ionic bonding or covalent bonding, but it is stronger than van der Waals forces. So, \({\rm{CH3OH}}\) (l) in \({\rm{H2O (l)}}\) have hydrogen bonding present in them.