Write the resonance structures of $CO_3^{2-}$ and $HCO_3^{-}$.
(N/A) The resonance structures represent the delocalization of electrons within the ion.
$(a)$ For the carbonate ion $(CO_3^{2-})$,there are three equivalent resonance structures where the double bond is shared among the three oxygen atoms.
$(b)$ For the bicarbonate ion $(HCO_3^{-})$,there are two resonance structures where the double bond is shared between the carbon and the two non-protonated oxygen atoms.
$(a)$ For the carbonate ion $(CO_3^{2-})$,there are three equivalent resonance structures where the double bond is shared among the three oxygen atoms.
$(b)$ For the bicarbonate ion $(HCO_3^{-})$,there are two resonance structures where the double bond is shared between the carbon and the two non-protonated oxygen atoms.
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Similar Questions
The correct statement$(s)$ about $O_3$ is (are)
$A$. $O-O$ bond lengths are equal.
$B$. Thermal decomposition of $O_3$ is endothermic.
$C$. $O_3$ is diamagnetic in nature.
$D$. $O_3$ has a bent structure.
$A$. $O-O$ bond lengths are equal.
$B$. Thermal decomposition of $O_3$ is endothermic.
$C$. $O_3$ is diamagnetic in nature.
$D$. $O_3$ has a bent structure.
DifficultIIT 2013
View SolutionThe cause of resonance is....
Medium
View SolutionDraw the resonance structures for the following compounds. Show the electron shift using curved-arrow notation.
$(a)$ $C_{6}H_{5}OH$
$(b)$ $C_{6}H_{5}NO_{2}$
$(c)$ $CH_{3}CH=CH-CHO$
$(d)$ $C_{6}H_{5}CHO$
$(e)$ $C_{6}H_{5}CH_{2}^{+}$
$(f)$ $CH_{3}CH=CH-CH_{2}^{+}$
$(a)$ $C_{6}H_{5}OH$
$(b)$ $C_{6}H_{5}NO_{2}$
$(c)$ $CH_{3}CH=CH-CHO$
$(d)$ $C_{6}H_{5}CHO$
$(e)$ $C_{6}H_{5}CH_{2}^{+}$
$(f)$ $CH_{3}CH=CH-CH_{2}^{+}$
Medium
View SolutionWhat is resonance energy?
Medium
View SolutionThe $C-O$ bond length in $CO$,$CO_2$ and $CO_3^{2-}$ follows the order.
DifficultKVPY 2012
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