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Among the following metal carbonyls,the C—O bond order is lowest in
(2007, Only One Option Correct Type)
- a)[Mn(CO)6]+
- b)[Fe(CO)5]
- c)[Cr(CO)6]
- d)[V(CO)6]-
Correct answer is option 'B'. Can you explain this answer?
Verified Answer
Among the following metal carbonyls,the C—O bond order is lowest...
Greater the extent of dπ-pπ back bonding, smaller will be the bond order of CO bond in metal carbonyls. In Fe(CO)5, there is maximum number of valence shell electrons (d-electrons), greatest chances of pπ-dπ back bonding, lowest bond order of CO bond.
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Among the following metal carbonyls,the C—O bond order is lowest...
Explanation:
To determine the CO bond order in the given metal carbonyls, we need to consider the electronic configuration and bonding in each compound.
[Mn(CO)6]
- Mn has an atomic number of 25, and its electronic configuration is [Ar] 3d5 4s2.
- Each CO ligand donates two electrons to the Mn atom, resulting in a total of 12 electrons from the CO ligands.
- The Mn atom has 5 valence electrons from its electronic configuration.
- The total number of valence electrons in [Mn(CO)6] is 17.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 17/6 = 2.83.
[Fe(CO)5]
- Fe has an atomic number of 26, and its electronic configuration is [Ar] 3d6 4s2.
- Each CO ligand donates two electrons to the Fe atom, resulting in a total of 10 electrons from the CO ligands.
- The Fe atom has 6 valence electrons from its electronic configuration.
- The total number of valence electrons in [Fe(CO)5] is 16.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 16/5 = 3.2.
[Cr(CO)6]
- Cr has an atomic number of 24, and its electronic configuration is [Ar] 3d5 4s1.
- Each CO ligand donates two electrons to the Cr atom, resulting in a total of 12 electrons from the CO ligands.
- The Cr atom has 6 valence electrons from its electronic configuration.
- The total number of valence electrons in [Cr(CO)6] is 18.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 18/6 = 3.
[V(CO)6]-
- V has an atomic number of 23, and its electronic configuration is [Ar] 3d3 4s2.
- Each CO ligand donates two electrons to the V atom, resulting in a total of 12 electrons from the CO ligands.
- The V atom has 5 valence electrons from its electronic configuration.
- The total number of valence electrons in [V(CO)6]- is 17.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 17/6 = 2.83.
Conclusion:
The CO bond order is lowest in [Fe(CO)5] with a value of 3.2. This is because Fe has a higher number of valence electrons (6) compared to the other metal atoms in the given compounds. The higher number of valence electrons allows for stronger bonding interactions with the CO ligands, resulting in a higher CO bond order.
To determine the CO bond order in the given metal carbonyls, we need to consider the electronic configuration and bonding in each compound.
[Mn(CO)6]
- Mn has an atomic number of 25, and its electronic configuration is [Ar] 3d5 4s2.
- Each CO ligand donates two electrons to the Mn atom, resulting in a total of 12 electrons from the CO ligands.
- The Mn atom has 5 valence electrons from its electronic configuration.
- The total number of valence electrons in [Mn(CO)6] is 17.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 17/6 = 2.83.
[Fe(CO)5]
- Fe has an atomic number of 26, and its electronic configuration is [Ar] 3d6 4s2.
- Each CO ligand donates two electrons to the Fe atom, resulting in a total of 10 electrons from the CO ligands.
- The Fe atom has 6 valence electrons from its electronic configuration.
- The total number of valence electrons in [Fe(CO)5] is 16.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 16/5 = 3.2.
[Cr(CO)6]
- Cr has an atomic number of 24, and its electronic configuration is [Ar] 3d5 4s1.
- Each CO ligand donates two electrons to the Cr atom, resulting in a total of 12 electrons from the CO ligands.
- The Cr atom has 6 valence electrons from its electronic configuration.
- The total number of valence electrons in [Cr(CO)6] is 18.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 18/6 = 3.
[V(CO)6]-
- V has an atomic number of 23, and its electronic configuration is [Ar] 3d3 4s2.
- Each CO ligand donates two electrons to the V atom, resulting in a total of 12 electrons from the CO ligands.
- The V atom has 5 valence electrons from its electronic configuration.
- The total number of valence electrons in [V(CO)6]- is 17.
- The CO bond order is calculated by dividing the number of bonding electrons by the number of CO ligands.
- In this case, the CO bond order is 17/6 = 2.83.
Conclusion:
The CO bond order is lowest in [Fe(CO)5] with a value of 3.2. This is because Fe has a higher number of valence electrons (6) compared to the other metal atoms in the given compounds. The higher number of valence electrons allows for stronger bonding interactions with the CO ligands, resulting in a higher CO bond order.
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Among the following metal carbonyls,the C—O bond order is lowest in(2007, Only One Option Correct Type)a)[Mn(CO)6]+b)[Fe(CO)5]c)[Cr(CO)6]d)[V(CO)6]-Correct answer is option 'B'. Can you explain this answer?
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