Match the following:
Column IColumn II(1) HCl(i)Polar Molecular solid(2)Ice(ii)Non−polar Molecular solid(3) CCl4(iii)H−bonded Molecular solid
Match the following:
Column IColumn II(1) HCl(i)Polar Molecular solid(2)Ice(ii)Non−polar Molecular solid(3) CCl4(iii)H−bonded Molecular solid
The correct option is A (1)-(i), (2)-(iii), (3)-(ii)
For this, first we need to know the definitions of polar, non-polar and H-bonded molecular solids.
In some solids, the molecules contain polar covalent bonds between H and F, O, or N atoms.
There is electronegativity difference between H and F,O or N. So there is strong electrostatic force of attraction between Hydrogen from one molecule with O,N or F of another molecule. This is known as hydrogen bond.
Hence, the intermolecular forces of attraction in these molecules are the strong hydrogen bonds.
Polar molecular solids: The intra – molecular forces of attraction are formed by polar covalent bonds. The molecules are held by relatively stronger dipole-dipole interactions.
Dipole-dipole force of attraction
Non-polar molecular solids: They are formed by either atoms (e.g., He and Ar) or molecules formed by non polar covalent bonds (e.g., H2, Cl2, and I2). The atoms or molecules are held by weak dispersion forces or London forces.
Here in HCl, There is dipole dipole interaction between molecules of HCl. Therefore, it is a polar molecular solid.
You might be wondering why dipole-dipole interaction?
The electronegativity difference is very high between H and Cl. Therefore a partial charge exists in H and Cl which leads to dipole-dipole interaction between these molecules.
Now, if we look at Ice, we know that if there is bonding between H and F, O or N atoms, it leads to hydrogen bonding. This is the case in ice too. There is intermolecular H-bonding between H2O molecules.
In case of CCl4, since it is non-polar. These molecules will be held by weak dispersion forces.
(1)-(i), (2)-(iii), (3)-(ii)
For this, first we need to know the definitions of polar, non-polar and H-bonded molecular solids.
In some solids, the molecules contain polar covalent bonds between H and F, O, or N atoms.
There is electronegativity difference between H and F,O or N. So there is strong electrostatic force of attraction between Hydrogen from one molecule with O,N or F of another molecule. This is known as hydrogen bond.
Hence, the intermolecular forces of attraction in these molecules are the strong hydrogen bonds.
Polar molecular solids: The intra – molecular forces of attraction are formed by polar covalent bonds. The molecules are held by relatively stronger dipole-dipole interactions.
Dipole-dipole force of attraction
Non-polar molecular solids: They are formed by either atoms (e.g., He and Ar) or molecules formed by non polar covalent bonds (e.g., H2, Cl2, and I2). The atoms or molecules are held by weak dispersion forces or London forces.
Here in HCl, There is dipole dipole interaction between molecules of HCl. Therefore, it is a polar molecular solid.
You might be wondering why dipole-dipole interaction?
The electronegativity difference is very high between H and Cl. Therefore a partial charge exists in H and Cl which leads to dipole-dipole interaction between these molecules.
Now, if we look at Ice, we know that if there is bonding between H and F, O or N atoms, it leads to hydrogen bonding. This is the case in ice too. There is intermolecular H-bonding between H2O molecules.
In case of CCl4, since it is non-polar. These molecules will be held by weak dispersion forces.
