Taking MgCl2 as an electrovalent compound. CCl4 as a covalent compound, give four differences between electrovalent and covalent compounds.
Taking MgCl2 as an electrovalent compound. CCl4 as a covalent compound, give four differences between electrovalent and covalent compounds.
S.No. Electrovalent compounds Covalent compounds 1 These compounds are formed by the complete transfer of electrons from metal to non-metal atom.
Example: In Magnesium chloride (MgCl2), electrons are transferred from Magnesium (metal) to Chlorine (non-metal)
These compounds are formed by the mutual sharing of electrons between atoms of non-metals.
Example: In Carbon tetrachloride (CCl4), both Carbon and Chlorine are non-metals.
2 These compounds are generally solid in nature.
Example: MgCl2 exists as a white crystalline solid.
These compounds are generally liquid or gaseous in nature.
Example: CCl4 is liquid at room temperature.
3 These compounds conduct electricity because of the presence of free ions.
Example: In MgCl2 , Mg+2 and Cl- ions conduct electricity in aqueous and molten state.
These compounds do not conduct electricity because of the absence of ions. These exist as molecules.
Example: CCl4 do not have ions.
4 These compounds have high melting and boiling points.
Example: MgCl2 has high melting point of 714°C
These compounds have low melting and boiling points.
Example: CCl4 has a boiling point of 76.72°C
| S.No. | Electrovalent compounds | Covalent compounds |
| 1 | These compounds are formed by the complete transfer of electrons from metal to non-metal atom. Example: In Magnesium chloride (MgCl2), electrons are transferred from Magnesium (metal) to Chlorine (non-metal) | These compounds are formed by the mutual sharing of electrons between atoms of non-metals. Example: In Carbon tetrachloride (CCl4), both Carbon and Chlorine are non-metals. |
| 2 | These compounds are generally solid in nature. Example: MgCl2 exists as a white crystalline solid. | These compounds are generally liquid or gaseous in nature. Example: CCl4 is liquid at room temperature. |
| 3 | These compounds conduct electricity because of the presence of free ions. Example: In MgCl2 , Mg+2 and Cl- ions conduct electricity in aqueous and molten state. | These compounds do not conduct electricity because of the absence of ions. These exist as molecules. Example: CCl4 do not have ions. |
| 4 | These compounds have high melting and boiling points. Example: MgCl2 has high melting point of 714°C | These compounds have low melting and boiling points. Example: CCl4 has a boiling point of 76.72°C |
