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Question: Calculate the formal charge of atoms \(HCl{O_4},\,CO_3^{2 - }.\)...

Calculate the formal charge of atoms HClO4, CO32−.HCl{O_4},\,CO_3^{2 - }.

Explanation

Solution

The formal charge of HClO4HCl{O_4} and CO32−CO_3^{2 - } can be calculated using this formula: FC=V−L−12SFC = V - L - \dfrac{1}{2}S
Formula used:

Formal  charg⁡e=[ Total⁡  no.  of  valence  electrons]−[Total⁡  no.  of  electrons  of  lone  pairs]                                          −12[Tota l⁡  no.  of  shared  electrons]  Formal\,\,ch\arg e = [\,Tota\operatorname{l} \,\,no.\,\,of\,\,valence\,\,electrons] - [Tota\operatorname{l} \,\,no.\,\,of\,\,electrons\,\,of\,\,lone\,\,pairs] \\\ \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, - \dfrac{1}{2}[Tota\,\operatorname{l} \,\,no.\,\,of\,\,shared\,\,electrons] \\\

Complete step by step answer:
The formal charge on an atom in a molecule or ion is defined as the difference between the number of valence electrons of that atom in the free state and the number of electrons assigned to that atom in the Lewis structure, assuming that in each shared pair of electrons the atom has one electron of its own and the lone pair on it belongs to it completely. Thus, it can be calculated as follows
FC=V−L−12SFC = V - L - \dfrac{1}{2}S

where, FCFC = Formal charge on an atom in a molecule
VV= Total number of valence electrons in free atom
LL = Total number of electrons of lone pair (non-bonding electrons)
SS= Total number of shared electrons (bonding electrons)

The Lewis structure of HClO4HCl{O_4} is:

Thus, Formal charge on ClCl = $$$FC = V - L - \dfrac{1}{2}S\,\, = 7 - 0 - \dfrac{1}{2}(8)\,\,\, = 3$$ Formal charge on single bonded O atom = $$FC = V - L - \dfrac{1}{2}S\,\, = 6 - 6 - \dfrac{1}{2}(2)\,\,\, = - 1$$ Formal charge on O atom bonded to H = $$FC = V - L - \dfrac{1}{2}S\,\, = 6 - 4 - \dfrac{1}{2}(4)\,\,\, = 0$$ Formal charge on H = $FC=V−L−12S,,=1−0−12(2),,,=0FC = V - L - \dfrac{1}{2}S,, = 1 - 0 - \dfrac{1}{2}(2),,, = 0
The Lewis structure of  CO32−.\,CO_3^{2 - }.is:

Formal charge on C = $$$FC = V - L - \dfrac{1}{2}S\,\, = 4 - 0 - \dfrac{1}{2}(8)\,\,\, = 0$$ Formal charge on double bonded O atom = $$$FC = V - L - \dfrac{1}{2}S,, = 6 - 4 - \dfrac{1}{2}(4),,, = 0 Formal charge on single bonded O atom$ = $FC = V - L - \dfrac{1}{2}S,, = 6 - 6 - \dfrac{1}{2}(2),,, = - 1$$

Note:
To calculate formal charge it is necessary to draw a Lewis structure. In a molecule, there is no charge on the molecule as a whole or in a polyatomic ion, although the charge present on the ion is the charge on the ion as a whole and not on the individual atoms, yet for some purposes. It is useful to assign a formal charge to each atom in a molecule or ion. The main advantage of the calculation of formal charges is that it helps to select the most stable structure, the one with least energy out of the different possible Lewis structures. The most stable is the one which has the smallest formal charges on the atoms.