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The complexes [Pt(CN)4]2– and [NiCl4]2–, respectively, are
- a)paramagnetic, paramagnetic
- b)diamagnetic, diamagnetic
- c)paramagnetic, diamagnetic
- d)diamagnetic, paramagnetic
Correct answer is option 'D'. Can you explain this answer?
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The complexes [Pt(CN)4]2– and [NiCl4]2–, respectively, are...
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- d)diamagnetic, paramagnetic
In presence of strong field CN
-
ions, all the electrons are paired up. The empty 4d, 3s and two 4p orbitals undergo dsp
2
hybridization to make bonds with CN
-
ligands in square planar geometry. Thus
[Ni(CN)4
]2
-
is diamagnetic. Since there is no any unpaired electron therefore its magnetic moment is zero.
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The complexes [Pt(CN)4]2– and [NiCl4]2–, respectively, are...
Diamagnetic and Paramagnetic Complexes
Diamagnetic substances are those that do not contain any unpaired electrons and are not attracted to an external magnetic field. Paramagnetic substances, on the other hand, contain unpaired electrons and are attracted to a magnetic field.
The complexes [Pt(CN)4]2 and [NiCl4]2 can be analyzed to determine whether they are diamagnetic or paramagnetic.
1. [Pt(CN)4]2 Complex:
The central metal atom in the [Pt(CN)4]2 complex is platinum (Pt). To determine the electronic configuration of Pt in this complex, we need to consider the oxidation state of Pt and the number of ligands surrounding it.
- The oxidation state of Pt in this complex is +2 since the overall charge of the complex is 2-.
- Each ligand, cyanide (CN-), is a strong field ligand, which means it forms a strong bond with the metal ion and causes the d orbitals to split into two sets of energy levels, with one set lower in energy and the other higher in energy.
Based on the above information, we can determine the electronic configuration of Pt in the [Pt(CN)4]2 complex. Since the oxidation state of Pt is +2, the electronic configuration is [Xe]4f145d8. This configuration shows that Pt has two unpaired electrons in its d orbitals, making it paramagnetic.
2. [NiCl4]2 Complex:
The central metal atom in the [NiCl4]2 complex is nickel (Ni). To determine the electronic configuration of Ni in this complex, we need to consider the oxidation state of Ni and the number of ligands surrounding it.
- The oxidation state of Ni in this complex is +2 since the overall charge of the complex is 2-.
- Each ligand, chloride (Cl-), is a weak field ligand, which means it forms a weak bond with the metal ion and does not cause significant splitting of the d orbitals.
Based on the above information, we can determine the electronic configuration of Ni in the [NiCl4]2 complex. Since the oxidation state of Ni is +2, the electronic configuration is [Ar]3d8. This configuration shows that Ni does not have any unpaired electrons in its d orbitals, making it diamagnetic.
Therefore, the correct answer is option D: [Pt(CN)4]2 is paramagnetic, and [NiCl4]2 is diamagnetic.
Diamagnetic substances are those that do not contain any unpaired electrons and are not attracted to an external magnetic field. Paramagnetic substances, on the other hand, contain unpaired electrons and are attracted to a magnetic field.
The complexes [Pt(CN)4]2 and [NiCl4]2 can be analyzed to determine whether they are diamagnetic or paramagnetic.
1. [Pt(CN)4]2 Complex:
The central metal atom in the [Pt(CN)4]2 complex is platinum (Pt). To determine the electronic configuration of Pt in this complex, we need to consider the oxidation state of Pt and the number of ligands surrounding it.
- The oxidation state of Pt in this complex is +2 since the overall charge of the complex is 2-.
- Each ligand, cyanide (CN-), is a strong field ligand, which means it forms a strong bond with the metal ion and causes the d orbitals to split into two sets of energy levels, with one set lower in energy and the other higher in energy.
Based on the above information, we can determine the electronic configuration of Pt in the [Pt(CN)4]2 complex. Since the oxidation state of Pt is +2, the electronic configuration is [Xe]4f145d8. This configuration shows that Pt has two unpaired electrons in its d orbitals, making it paramagnetic.
2. [NiCl4]2 Complex:
The central metal atom in the [NiCl4]2 complex is nickel (Ni). To determine the electronic configuration of Ni in this complex, we need to consider the oxidation state of Ni and the number of ligands surrounding it.
- The oxidation state of Ni in this complex is +2 since the overall charge of the complex is 2-.
- Each ligand, chloride (Cl-), is a weak field ligand, which means it forms a weak bond with the metal ion and does not cause significant splitting of the d orbitals.
Based on the above information, we can determine the electronic configuration of Ni in the [NiCl4]2 complex. Since the oxidation state of Ni is +2, the electronic configuration is [Ar]3d8. This configuration shows that Ni does not have any unpaired electrons in its d orbitals, making it diamagnetic.
Therefore, the correct answer is option D: [Pt(CN)4]2 is paramagnetic, and [NiCl4]2 is diamagnetic.
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The complexes [Pt(CN)4]2– and [NiCl4]2–, respectively, area)paramagnetic, paramagneticb)diamagnetic, diamagneticc)paramagnetic, diamagneticd)diamagnetic, paramagneticCorrect answer is option 'D'. Can you explain this answer?
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