The correct statement about the Cu–N bond distance in [Cu(NH3)6]2+ is:a)All the bond distance are equal.b)The axial bonds are longer than the equatorial ones.c)The equatorial bonds are longer than the axial ones.d)All the bond distances are unequal.Correct answer is option 'B'. Can you explain this answer?

Question

The correct statement about the Cu&#8211;N bond distance in [Cu(NH3)6]2+ is:a)All the bond distance are equal.b)The axial bonds are longer than the equatorial ones.c)The equatorial bonds are longer than the axial ones.d)All the bond distances are unequal.Correct answer is option 'B'. Can you explain this answer?

Answer

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.

Answer

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).

Answer

Due to Z out  distortion

Answer

- 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).

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