In the anion $H C O O^{-}$ , the two $C - O$ bonds are found to be of equal length. What is the reason for it?

Electronic orbitals of carbon atom are hybridised

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The

C = O

bond is weaker than the

C - O

bond

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The anion

H C O O^{-}

has two resonating structures

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The anion is obtained by removal of a proton from the acid molecule

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Solution

The correct option is C The anion $H C O O^{-}$ has two resonating structures
Due to its resonance, two $C - O$ bond lengths are equal and its bond order is 1.5.

$H - O | | C - O^{-} \leftrightarrow H - O^{-} | C = O$

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Similar questions

H C O O^{-}

H C O O^{-}

[C o (a c a c)_{3}]

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

C - O

1.27 ˚ A

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