Question

write briefly the pauling's rules for transition of covalent to ionic bond​

Answer 1

Answer:

For a given cation, Pauling defined[2] the electrostatic bond strength to each coordinated anion as {\displaystyle s={\frac {z}{\nu }}}s={\frac {z}{\nu }}, where z is the cation charge and ν is the cation coordination number. A stable ionic structure is arranged to preserve local electroneutrality, so that the sum of the strengths of the electrostatic bonds to an anion equals the charge on that anion.

{\displaystyle \xi =\sum _{i}s_{i}}\xi =\sum _{{i}}s_{i}

where {\displaystyle \xi }\xi is the anion charge and the summation is over the adjacent cations. For simple solids, the {\displaystyle s_{i}}s_{i} are equal for all cations coordinated to a given anion, so that the anion coordination number is the anion charge divided by each electrostatic bond strength. Some examples are given in the table.