The correct statements regarding CO and CO2 are

In CO2, C is bonded with two oxygen atoms (electronegative atoms). It is a polar molecule that has a positive center on the carbon atom and can attract (and accept) lone electron pairs. Therefore, it acts as Lewis acid.In CO, C is bonded with one O atom through double bond, C=O and it acts as a Lewis acid in exactly the way your CO 2 molecule did.As partial positive character is more on C in CO2 compared to CO, therefore it is a strong Lewis acid than CO and weaker Lewis base than CO.The sigma bond is formed when a lone pair of electrons of carbonyl carbon is donated to a vacant orbital of metal. To form a pi bond, an electron pair is donated from filled metal d-orbital to vacant anti-bonding pi-orbitals of CO.This weakens the bond between C and O in CO and the bond strength between metal and carbon increases.

The correct statements regarding CO and CO2 are

In CO2, C is bonded with two oxygen atoms (electronegative atoms). It is a polar molecule that has a positive center on the carbon atom and can attract (and accept) lone electron pairs. Therefore, it acts as Lewis acid.In CO, C is bonded with one O atom through double bond, C=O and it acts as a Lewis acid in exactly the way your CO 2 molecule did.As partial positive character is more on C in CO2 compared to CO, therefore it is a strong Lewis acid than CO and weaker Lewis base than CO.The sigma bond is formed when a lone pair of electrons of carbonyl carbon is donated to a vacant orbital of metal. To form a pi bond, an electron pair is donated from filled metal d-orbital to vacant anti-bonding pi-orbitals of CO.This weakens the bond between C and O in CO and the bond strength between metal and carbon increases.

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The correct statements regarding CO and CO₂ are

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Both CO and CO₂ can act as Lewis acids

CO is stronger Lewis base than CO₂

CO₂ is stronger Lewis acid than CO

The back bonding in complex compounds with CO increased the stability of the coordination complexes

answer is A, B, C, D.

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Detailed Solution

In CO₂, C is bonded with two oxygen atoms (electronegative atoms). It is a polar molecule that has a positive center on the carbon atom and can attract (and accept) lone electron pairs. Therefore, it acts as Lewis acid.
In CO, C is bonded with one O atom through double bond, $C = O$ and it acts as a Lewis acid in exactly the way your $C O_{2}$ molecule did.
As partial positive character is more on C in CO₂ compared to CO, therefore it is a strong Lewis acid than CO and weaker Lewis base than CO.
The sigma bond is formed when a lone pair of electrons of carbonyl carbon is donated to a vacant orbital of metal. To form a pi bond, an electron pair is donated from filled metal d-orbital to vacant anti-bonding pi-orbitals of CO.
This weakens the bond between C and O in CO and the bond strength between metal and carbon increases.