One of the resonating structure of $S O_{4}^{- 2}$ is as shown.
Which set formal charge on oxygen and bond order is correct?

- 0.5

and

1.5

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1.5

and

3

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2

and

3

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1.5

and

1.5

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Solution

The correct option is A $- 0.5$ and $1.5$
All resonating structures of $S O_{4}^{2 -}$ are
(Refer to Image)
Formal charge on (1)= $\frac{- 1 + 0 - 1 + 0 - 1 + 0}{6} = - 0.5$
Bond order= $\frac{1 + 2 + 1 + 2 + 1 + 2}{6} = \frac{3}{2} = 1.5$

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The roots of quadratic equation are 2x²+3x-9 = 0 are:

P O_{4}^{3 -}

P - O

\frac{(1.5)^{3} + (4.7)^{3} + (3.8)^{3} - 3 \times 1.5 \times 4.7 \times 3.8}{(1.5)^{2} + (4.7)^{2} + (3.8)^{2} - 1.5 \times 4.7 - 4.7 \times 3.8 - 1.5 \times 3.8}

Question 27

Which of the following statement are correct about $C O_{3}^{- 2}$ ?

(a) The hybridisation of central atom is $s p^{3}$

(b) Its resonance structure has one C - O single bond and two C = 0 double bonds

(d) All C - O bond lengths are equal

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