Question

Match the following:

$\begin{array}{cc}ColumnI& ColumnII\\ \left(1\right).Non-polarMolecularsolids& \left(i\right)Coulombicorelectrostaticforces\\ \left(2\right).H-BondedMolecularsolids& \left(ii\right).H-bonding\\ \left(3\right).Ionicsolids& \left(iii\right).Metallicbonding\\ \left(4\right).Weakdispersionforces& \left(iv\right).Weakdispersionforces\\ \left(5\right).Metallicsolids& \left(v\right).dipole–dipoleinteraction.\\ & \left(vi\right).covalentBonding.\end{array}$

• A. (1)-(iv), (2)-(ii), (3)-(iv), (4)-(vi), (5)-(iii)
• B. (1)-(iv), (2)-(ii), (3)-(i), (4)-(vi), (5)-(iii)
• C. (1)-(iv), (2)-(ii), (3)-(iv), (4)-(vi), (5)-(iii)
• D. (1)-(v), (2)-(i), (3)-(iv), (4)-(vi), (5)-(ii)

Answer 1

The correct option is B

(1)-(iv), (2)-(ii), (3)-(i), (4)-(vi), (5)-(iii)

Here we have to match the types of solids to their bonding / attractive forces.For this, we need to remember this table:

$\begin{array}{ccccccc}\text{Types of solid}& \text{Constituent particles}& \text{bonding/attractive force}& \text{examples}& \text{physical nature}& \text{Electrical conductivity}& \text{Melting point}\\ \text{1. Molecular solids a. non-polar}& \text{Molecules}& \text{Dispersion or london forces}& Ar,CC{l}_4,H_2,l_2,C{O}_2& \text{soft}& \text{insulator}& \text{very low}\\ \text{b. Polar}& & \text{dipole-dipole interactions}& HCl,S{O}_2& \text{Soft}& \text{Insulator}& \text{Low}\\ \text{c. Hydrogen}& & \text{Hydrogen bonding}& H_{2}O\left(ice\right)& \text{Hard}& \text{Insulator}& \text{Low}\\ \text{2. Metallic solids}& \text{positive ions in a sea of delocalized electrons}& \text{Metallic bonding}& \text{Fe, Cu, Ag, Mg}& \text{Hard but malleable and ductile}& \text{Conductors in solid state as well as in molten state}& \text{Fairly high}\\ \text{3. Covalent or network solids}& \text{Atoms}& \text{Covalent bonding}& Si{O}_2\left(quartz\right),SiC,C\left(diamond\right),AIN,C_{graphite}& \text{Hard Soft}& \text{Insulators (Graphite is exception)}& \text{very high}\\ \text{4. Ionic solids}& \text{Ions}& \text{Coulombic or electrostatic}& \text{NaCl,MgO, ZnS,}Ca{F}_2& \text{Hard but brittle}& \text{Insulators in solid state but conductor in molten state and in aqueous solutions}& \text{High}\end{array}$

In ionic solid, because of presence of ions, there will be electrostatic force.

$\to$ In covalent solids $\to$ covalent bonding

$\to$ Metallic solids $\to$ Metallic bonding

$\to$ H-bonded Molecular solids – In such solids, the molecules contain polar covalent bonds between H and F, O, or N atoms. Hence, the intermolecular forces of attraction in these molecules are the strong hydrogen bonds between H of one molecule and F,O or N of other molecule.

$\to$ Non-polar moleculer solids – In these solids, the particles are held by weak dispersion forces or London forces.