(C) The carbonate ion,$CO_3^{2-}$,exhibits resonance. In the resonance hybrid,the carbon-oxygen bonds are equivalent due to delocalization of electron

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(C) The carbonate ion,$CO_3^{2-}$,exhibits resonance. In the resonance hybrid,the carbon-oxygen bonds are equivalent due to delocalization of electrons. The structure is trigonal planar with a bond angle of $120^o$. All $C-O$ bond lengths are identical due to the resonance effect,which averages the single and double bond characteristics.

Class 11 Chemistry Chemical Bonding and Molecular Structure Resonance

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Which of the following species has all bond angles equal to $120^o$ and all bond lengths equal?

A
$S_2O_3^{2-}$
B
$HCO_3^{-}$
C
$CO_3^{2-}$
D
$N_2O_5$

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

Chemical Bonding and Molecular Structure

Subtopic

Resonance

$(i)$ Identify the less stable resonance structure and $(ii)$ give its reason for the following pairs.

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Although $ClO_2$ is an odd-electron molecule,it does not dimerize because...

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Explain the important aspects of resonance with reference to the $CO_{3}^{2-}$ ion.

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In $PO_4^{3-}$ ion,the formal charge on each oxygen atom and $P-O$ bond order respectively are

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The increasing order of stability of the resonance structures is:

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Which of the following species has all bond angles equal to $120^o$ and all bond lengths equal?

Similar Questions

$(i)$ Identify the less stable resonance structure and $(ii)$ give its reason for the following pairs.

Although $ClO_2$ is an odd-electron molecule,it does not dimerize because...

Explain the important aspects of resonance with reference to the $CO_{3}^{2-}$ ion.

In $PO_4^{3-}$ ion,the formal charge on each oxygen atom and $P-O$ bond order respectively are

The increasing order of stability of the resonance structures is:

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