Which of the following carbonyls will have the strongest C−O bond? A) Mn(CO)+6 B) Cr(CO)6 C) V (CO)−6 D) Fe(CO)5

The highest occupied molecular orbital in the carbonyl CO molecule contains the lone pair of electrons that are projecting away from the carbon atoms. When CO is used as a ligand, it works as a weak electron donor to metal atoms, forming the M C bond. The CO’s vacant antibonding molecular orbital coincides with the transition metal’s d-orbitals, forming a bond.

This causes a bond to develop between the metal’s filled d-orbitals and the CO ligands’ unoccupied orbitals. This is referred to as back bonding. M C is the symbol for the bond.

A) Mn(CO)6+ :

The central metal Mn has a +1 charge on it.

B) Cr(CO)6 :

The central metal atom Cr has a zero change on it.

C) V (CO)6 :

The central metal atom V has a negative charge −1 on it.

D) Fe(CO)5 :

The central metal atom Fe has a zero charge on it.

The Mn have a positive charge compared to other metals. Thus it is not easy for the manganese to donate its electron density to the antibonding orbitals. Therefore, Mn would form a weak metal –carbonyl bond.

Therefore, the C−O bond is the strongest Mn(CO)6+.

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