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The structure of the complexes [Cu(NH3)4] (ClO4) and [Cu(NH3)4]ClO4 in solution respectively are
- a)square planer and tetrahedral
- b)octahedral and square pyramidal
- c)octahedral and trigonal bipyramidal
- d)tetrahedral and square pyramidal
Correct answer is option 'A'. Can you explain this answer?
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The structure of the complexes[Cu(NH3)4](ClO4)and[Cu(NH3)4]ClO4 in sol...
In the complex [Cu(NH3)4](CIO4), copper has dsp2 (square planar) while in complex [Cu(NH3)4]CIO4, copper has sp3 (tetrahedral) hybridisation.
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The structure of the complexes[Cu(NH3)4](ClO4)and[Cu(NH3)4]ClO4 in sol...
Structure of [Cu(NH3)4](ClO4) and [Cu(NH3)4]ClO4 in Solution
Structure of [Cu(NH3)4](ClO4)
Square Planar
When copper(II) ions are dissolved in water, they tend to form complexes with ammonia (NH3) ligands. The complex [Cu(NH3)4](ClO4) has a square planar structure. This means that the copper atom is surrounded by four ammonia ligands in a plane, with the two perchlorate (ClO4-) ions located above and below the plane.
Structure of [Cu(NH3)4]ClO4
Tetrahedral
The complex [Cu(NH3)4]ClO4, on the other hand, has a tetrahedral structure. This means that the copper atom is surrounded by four ammonia ligands, which are arranged at the corners of a tetrahedron. The perchlorate ion is located outside the tetrahedron, not interacting directly with the copper atom or the ammonia ligands.
Explanation
The difference in structure between the two complexes can be explained by the presence or absence of anions that coordinate with the copper(II) ion. In the case of [Cu(NH3)4](ClO4), the perchlorate ions coordinate with the copper atom and force the ammonia ligands into a square planar arrangement. In contrast, [Cu(NH3)4]ClO4 has no coordinating anions, so the ammonia ligands are free to arrange themselves in a tetrahedral shape around the copper atom.
Moreover, the steric effect of the perchlorate ion in [Cu(NH3)4](ClO4) is responsible for the square planar structure. Since the perchlorate ion is larger than the ammonia ligands, it cannot fit into the tetrahedral arrangement. Therefore, the ammonia ligands are forced to arrange themselves in a square planar arrangement.
Structure of [Cu(NH3)4](ClO4)
Square Planar
When copper(II) ions are dissolved in water, they tend to form complexes with ammonia (NH3) ligands. The complex [Cu(NH3)4](ClO4) has a square planar structure. This means that the copper atom is surrounded by four ammonia ligands in a plane, with the two perchlorate (ClO4-) ions located above and below the plane.
Structure of [Cu(NH3)4]ClO4
Tetrahedral
The complex [Cu(NH3)4]ClO4, on the other hand, has a tetrahedral structure. This means that the copper atom is surrounded by four ammonia ligands, which are arranged at the corners of a tetrahedron. The perchlorate ion is located outside the tetrahedron, not interacting directly with the copper atom or the ammonia ligands.
Explanation
The difference in structure between the two complexes can be explained by the presence or absence of anions that coordinate with the copper(II) ion. In the case of [Cu(NH3)4](ClO4), the perchlorate ions coordinate with the copper atom and force the ammonia ligands into a square planar arrangement. In contrast, [Cu(NH3)4]ClO4 has no coordinating anions, so the ammonia ligands are free to arrange themselves in a tetrahedral shape around the copper atom.
Moreover, the steric effect of the perchlorate ion in [Cu(NH3)4](ClO4) is responsible for the square planar structure. Since the perchlorate ion is larger than the ammonia ligands, it cannot fit into the tetrahedral arrangement. Therefore, the ammonia ligands are forced to arrange themselves in a square planar arrangement.
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The structure of the complexes[Cu(NH3)4](ClO4)and[Cu(NH3)4]ClO4 in solution respectively area)square planer and tetrahedralb)octahedral and square pyramidalc)octahedral and trigonal bipyramidald)tetrahedral and square pyramidalCorrect answer is option 'A'. Can you explain this answer?
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