The correct statement about the Cu–N bond distance in [Cu(NH3)6]...
Explanation:
- [Cu(NH3)6]2+ is an octahedral complex with Cu2+ ion at the center and six NH3 ligands arranged in an octahedral geometry around it.
- The octahedral geometry has two types of bonds, axial bonds, and equatorial bonds.
Axial bonds:
- The axial bonds are formed between the Cu2+ ion and the two NH3 ligands located along the z-axis.
- These bonds are oriented along the axis of symmetry of the octahedron.
- Due to the presence of the axial ligands, the Cu2+ ion is pushed away from the center of the octahedron, resulting in longer bond distances.
Equatorial bonds:
- The equatorial bonds are formed between the Cu2+ ion and the four NH3 ligands located in the xy-plane.
- These bonds are oriented in the plane of the octahedron.
- The presence of the equatorial ligands does not push the Cu2+ ion away from the center of the octahedron, resulting in shorter bond distances.
Conclusion:
- Therefore, the axial bonds in [Cu(NH3)6]2+ are longer than the equatorial bonds, making option B the correct answer.
The correct statement about the Cu–N bond distance in [Cu(NH3)6]...
Explanation:
- In [Cu(NH3)6]2+, there are six NH3 ligands arranged in an octahedral geometry around the central Cu2+ ion.
- The bond distances are different due to the difference in the orientation of the ligands.
- There are two types of bond distances in this complex: axial and equatorial.
- Axial bonds: These are the bonds that are perpendicular to the plane of the equatorial bonds. There are two axial bonds in this complex.
- Equatorial bonds: These are the bonds that lie in the plane of the complex. There are four equatorial bonds in this complex.
- The repulsion between the lone pairs of electrons on the NH3 ligands causes the axial bonds to be longer than the equatorial bonds.
- Therefore, the correct statement is that the axial bonds are longer than the equatorial ones (option B is correct).