Q. No.[Cr(NH3)6]3+ is paramagnetic ,while is diamagnetic because:
| 1. | Electrons in the 3d orbitals remain unpaired in |
| 2. | Electrons in the 3d orbitals remain unpaired in [Cr(NH3)6]3+ |
| 3. | Electrons in the 3p orbitals remain unpaired in [Cr(NH3)6]3+ |
| 4. | Electrons in the 3p orbitals remain unpaired in |
The correct electronic configuration of the central atom in based on crystal field theory is:
| 1. | \(e^4 ~t_{2 g}^2 \) | 2. | \(t_{2 g}^4 ~e_g^2 \) |
| 3. | \(t_{2 g}^6 ~e_g^0 \) | 4. | \(e^3 ~t^3_{2g}\) |
The correct splitting diagram of d orbitals in an octahedral crystal field is:
| 1. |  |
2. |  |
| 3. |  |
4. | None of these. |
The electronic configuration that represents the maximum magnetic moment is:
1.
2.
3.
4. (high spin)
The low spin complex among the following is:
| 1. | \(\mathrm{Fe}(\mathrm{CN})_6^{3-} \) | 2. | \(\mathrm{Co}\left(\mathrm{NO}_2\right)_6^{3-} \) |
| 3. | \(\mathrm{Mn}(\mathrm{CN})_6^{3-} \) | 4. | All of the above |
For a tetrahedral complex [MCl4]2-, the spin-only magnetic moment is 3.83 B.M. The element M is:
1. Co
2. Cu
3. Mn
4. Fe
The geometry and magnetic properties of [NiCl4]2-, respectively, are :
1. Tetrahedral, Paramagnetic
2. Tetrahedral, Diamagnetic
3. Square planar, Paramagnetic
4. Square planar, Diamagnetic
The complex ion among the following that cannot absorb visible light is:
1. [Ni(CN)4]2-
2. [Cr(NH3)6]3+
3. [Fe(H2O)6]2+
4. [Ni(H2O)6]2+
An ion, among the following, that has a magnetic moment of 2.84 BM is:
(At. no. Ni = 28, Ti = 22, Cr = 24, Co = 27)
1. Ni2+
2. Ti3+
3. Cr2+
4. Co2+
The complex among the following with the highest value of crystal field splitting energy is :
| 1. | \(\left[Fe \left(H_{2} O\right)_{6}\right]^{+ 3}\) | 2. | \(\left[Ru \left( CN \right)_{6}\right]^{3 -}\) |
| 3. | \(\left[Fe \left(H_{2} O\right)_{6}\right]^{+ 2}\) | 4. | \(\left[Fe \left(NH_{3}\right)_{6}\right]^{3 +}\) |
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