(C) In the formate ion $(HCOO^-)$,the negative charge is delocalized over the two oxygen atoms through resonance. The two resonance structures are equ

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The $HCOO^-$ anion has two resonance structures.

(C) In the formate ion $(HCOO^-)$,the negative charge is delocalized over the two oxygen atoms through resonance. The two resonance structures are equivalent,which results in a bond order of $1.5$ for both $C-O$ bonds. Due to this resonance,both $C-O$ bonds have the same bond length,which is intermediate between a single bond and a double bond.

Class 11 Chemistry Chemical Bonding and Molecular Structure Resonance

Medium

What is the reason for the two carbon-oxygen bonds in the $HCOO^-$ anion having equal length?

A
The electronic orbitals of the carbon atom are hybridized.
B
The $C-O$ bond is weaker than the $C=O$ bond.
C
The $HCOO^-$ anion has two resonance structures.
D
The anion is formed by the removal of a proton from the acid molecule.

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Class 11 Questions

Class 11

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Chapter

Chemical Bonding and Molecular Structure

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Resonance

$H_3PO_3$ can be represented by structures $(1)$ and $(2)$ shown below. Can these two structures be taken as the canonical forms of the resonance hybrid representing $H_3PO_3$? If not,give reasons for the same.

Medium

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Compare the relative stability of the following resonating structures:

Difficult

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During the formation of the dimer $N_2O_4$ from two molecules of $NO_2$,what happens to the unpaired electron on the nitrogen atom of each $NO_2$ molecule?

Easy

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What is resonance energy? Write about its value.

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Which is the most important contributing resonating structure of $[CH_2=N(=O)=O]^-$?

Difficult

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What is the reason for the two carbon-oxygen bonds in the $HCOO^-$ anion having equal length?

Similar Questions

$H_3PO_3$ can be represented by structures $(1)$ and $(2)$ shown below. Can these two structures be taken as the canonical forms of the resonance hybrid representing $H_3PO_3$? If not,give reasons for the same.

Compare the relative stability of the following resonating structures:

During the formation of the dimer $N_2O_4$ from two molecules of $NO_2$,what happens to the unpaired electron on the nitrogen atom of each $NO_2$ molecule?

What is resonance energy? Write about its value.

Which is the most important contributing resonating structure of $[CH_2=N(=O)=O]^-$?

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