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Among the following metal carbonyls, the C --- O bond order is lowest in :
a) [ Mn(CO)6]+
b) [ V(CO)6 ]-
c) [ Cr(CO)6]
d) [ Fe(CO)5]
Correct answer is option 'D'. Can you explain this answer?
a) [ Mn(CO)6]+
b) [ V(CO)6 ]-
c) [ Cr(CO)6]
d) [ Fe(CO)5]
Correct answer is option 'D'. Can you explain this answer?
Verified Answer
Among the following metal carbonyls, the C ---O bond order is lowest i...
"Correct option would be b)
Metallic carbonyls involves both sigma and pi-bonding. pi-bonding involves the back donation of metal d-electrons into vacant orbital of CO. Larger the electrons involve in back-bonding, lesser will be the bond order.
CO is strong field ligand. The electronic configuration of metal ion in presence of CO will be as follows:
a) Mn+ = 3d5, 4s1 = 3d6 (in presence of CO)
b)Fe0 = 3d6, 4s2 = 3d8 (in presence of CO)
c) Cr0 = 3d5, 4s1 = 3d6 (in presence of CO)
d) V- = 3d4, 4s2 = 3d6 (in presence of CO)
In Fe(CO)5, 4 lone pairs of electrons are available on metals for back donation hence lowest will be bond order."
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Most Upvoted Answer
Among the following metal carbonyls, the C ---O bond order is lowest i...
Explanation:
Metal carbonyls are compounds in which carbon monoxide (CO) acts as a ligand to a metal center. The carbon monoxide molecule forms a coordinate covalent bond with the metal atom, where the carbon atom donates a lone pair of electrons to the metal atom.
In metal carbonyls, the C---O bond order is a measure of the strength of the bond between carbon and oxygen. The bond order is related to the number of shared electron pairs between the carbon and oxygen atoms. A higher bond order indicates a stronger bond.
Comparison of Metal Carbonyls:
a) [Mn(CO)6]:
- The central metal atom is Mn, which has a d5 electronic configuration.
- The oxidation state of Mn is +1.
- The complex has 6 CO ligands.
- The Mn atom can accept 5 electrons from the CO ligands, leaving one unpaired electron in the d orbital.
- The C---O bond order is 3, indicating a triple bond between carbon and oxygen.
b) [V(CO)6]-:
- The central metal atom is V, which has a d3 electronic configuration.
- The oxidation state of V is -1.
- The complex has 6 CO ligands.
- The V atom can accept 2 electrons from the CO ligands, leaving one unpaired electron in the d orbital.
- The C---O bond order is 2, indicating a double bond between carbon and oxygen.
c) [Cr(CO)6]:
- The central metal atom is Cr, which has a d6 electronic configuration.
- The oxidation state of Cr is 0.
- The complex has 6 CO ligands.
- The Cr atom can accept 4 electrons from the CO ligands, leaving two unpaired electrons in the d orbitals.
- The C---O bond order is 3, indicating a triple bond between carbon and oxygen.
d) [Fe(CO)5]:
- The central metal atom is Fe, which has a d6 electronic configuration.
- The oxidation state of Fe is 0.
- The complex has 5 CO ligands.
- The Fe atom can accept 5 electrons from the CO ligands, leaving one unpaired electron in the d orbital.
- The C---O bond order is 2, indicating a double bond between carbon and oxygen.
Conclusion:
Among the given metal carbonyls, the C---O bond order is lowest in [Fe(CO)5]. This is because the Fe atom in [Fe(CO)5] can accept 5 electrons from the CO ligands, resulting in a double bond between carbon and oxygen. In contrast, the other metal carbonyls have a higher C---O bond order, indicating a triple bond between carbon and oxygen.
Metal carbonyls are compounds in which carbon monoxide (CO) acts as a ligand to a metal center. The carbon monoxide molecule forms a coordinate covalent bond with the metal atom, where the carbon atom donates a lone pair of electrons to the metal atom.
In metal carbonyls, the C---O bond order is a measure of the strength of the bond between carbon and oxygen. The bond order is related to the number of shared electron pairs between the carbon and oxygen atoms. A higher bond order indicates a stronger bond.
Comparison of Metal Carbonyls:
a) [Mn(CO)6]:
- The central metal atom is Mn, which has a d5 electronic configuration.
- The oxidation state of Mn is +1.
- The complex has 6 CO ligands.
- The Mn atom can accept 5 electrons from the CO ligands, leaving one unpaired electron in the d orbital.
- The C---O bond order is 3, indicating a triple bond between carbon and oxygen.
b) [V(CO)6]-:
- The central metal atom is V, which has a d3 electronic configuration.
- The oxidation state of V is -1.
- The complex has 6 CO ligands.
- The V atom can accept 2 electrons from the CO ligands, leaving one unpaired electron in the d orbital.
- The C---O bond order is 2, indicating a double bond between carbon and oxygen.
c) [Cr(CO)6]:
- The central metal atom is Cr, which has a d6 electronic configuration.
- The oxidation state of Cr is 0.
- The complex has 6 CO ligands.
- The Cr atom can accept 4 electrons from the CO ligands, leaving two unpaired electrons in the d orbitals.
- The C---O bond order is 3, indicating a triple bond between carbon and oxygen.
d) [Fe(CO)5]:
- The central metal atom is Fe, which has a d6 electronic configuration.
- The oxidation state of Fe is 0.
- The complex has 5 CO ligands.
- The Fe atom can accept 5 electrons from the CO ligands, leaving one unpaired electron in the d orbital.
- The C---O bond order is 2, indicating a double bond between carbon and oxygen.
Conclusion:
Among the given metal carbonyls, the C---O bond order is lowest in [Fe(CO)5]. This is because the Fe atom in [Fe(CO)5] can accept 5 electrons from the CO ligands, resulting in a double bond between carbon and oxygen. In contrast, the other metal carbonyls have a higher C---O bond order, indicating a triple bond between carbon and oxygen.
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Among the following metal carbonyls, the C ---O bond order is lowest i...
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Among the following metal carbonyls, the C ---O bond order is lowest in :a) [ Mn(CO)6]+b) [ V(CO)6]- c) [ Cr(CO)6]d) [ Fe(CO)5]Correct answer is option 'D'. Can you explain this answer?
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