What are the main properties of covalent compounds with respect to melting and boiling points, solubility, and conductivity?
What are the main properties of covalent compounds with respect to melting and boiling points, solubility, and conductivity?
Covalent compounds are those compounds in which the atoms share one or more pairs of electrons present in their valence shells. The atoms in covalent compounds are held together by covalent bonds.
Melting and boiling points:
(i) The intermolecular force of attraction between the covalent compounds is very weak. So, a little amount of energy is needed to break the bonds between the molecules of covalent compounds.
(ii) The molecules in covalent compounds are electrically neutral. So, they have relatively low melting and boiling points.
Solubility:
(i) Covalent compounds are more soluble in non-polar solvents (ether) and less soluble in a polar solvent (water).
Example: Naphthalene readily dissolves in non-polar solvents like ether but is insoluble in water.
Conductivity:
(i) The conductivity of covalent compounds is very low.
(ii) Covalent compounds do not conduct electricity because they do not contain free ions or electrons.
Example: Glucose and urea are non-conductor of electricity.
Exception: Hydrogen chloride is a polar covalent compound that conducts electricity when it dissolves in water.
Covalent compounds are those compounds in which the atoms share one or more pairs of electrons present in their valence shells. The atoms in covalent compounds are held together by covalent bonds.
Melting and boiling points:
(i) The intermolecular force of attraction between the covalent compounds is very weak. So, a little amount of energy is needed to break the bonds between the molecules of covalent compounds.
(ii) The molecules in covalent compounds are electrically neutral. So, they have relatively low melting and boiling points.
Solubility:
(i) Covalent compounds are more soluble in non-polar solvents (ether) and less soluble in a polar solvent (water).
Example: Naphthalene readily dissolves in non-polar solvents like ether but is insoluble in water.
Conductivity:
(i) The conductivity of covalent compounds is very low.
(ii) Covalent compounds do not conduct electricity because they do not contain free ions or electrons.
Example: Glucose and urea are non-conductor of electricity.
Exception: Hydrogen chloride is a polar covalent compound that conducts electricity when it dissolves in water.
