The Characteristics of covalent compounds
(i) These exist as gases or liquids under the normal conditions of temperature and pressure. Some of the covalent compounds exist as soft solids
(ii) The components such as Diamond, Carborandum (SiC), Silica (SiO2), AlN etc. have the giant three dimensional network structures; Thus have exceptionally high melting points otherwise these compounds posses relatively low melting and boiling points.
(iii) Generally the covalent substances are bad conductor of electricity. The Polar covalent compounds such as HCl in solution conduct electricity. Graphite can also conduct electricity in the solid state since electrons can pass from one layer to the other easily.
(iv) These compounds are usually insoluble in the polar solvent like water but soluble in the non-polar solvents like benzene etc. some covalent compounds such as alcohol, dissolve in water cause of hydrogen bonding.
(v) The covalent bond is rigid and directional and nature. These compounds, therefore show isomerism (structural and space).
(vi) The Covalent substances show molecular reactions. The reaction rates are generally low.
(vii) Number of electrons contributed by the atom of the element for sharing with other atoms is called as covalency of the element. The Covalency = 8 - [Number of group to which the element initially belongs]. The variable covalency of the element is equal to total number of the unpaired electrons in s, p and d-orbitals of its valency shell.
The element like P, S, Cl, Br, I have the vacant d-orbitals in their valency shell. These elements show the variable covalency by increasing the number of unpaired electrons under the excited conditions. The electrons from the paired orbitals and get excited to the vacant d-orbitals of the same shell.
The Four elements, H, N, O and F do not have d-orbitals in their valency shell. Therefore, such an excitation is not possible in them and variable valency is not shown by these elements. This is the reason why NCl3 exists while NCl5 does not.
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