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प्रश्न
What are the high-spin complexes?
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उत्तर
When crystal field splitting energy is smaller than electron pairing energy, the complexes formed are high-spin complexes.
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संबंधित प्रश्न
On the basis of CFT predict the number of unpaired electrons in [CrF6]3-.
Answer in brief.
[CoCl4]2− is a tetrahedral complex. Draw its box orbital diagram. State which orbitals participate in hybridization.
Answer in brief.
[CoCl4]2- is a tetrahedral complex. Draw its box orbital diagram. State which orbitals participate in hybridization.
Answer in brief.
With the help of the crystal field, the energy-level diagram explains why the complex [Cr(en)3]3⊕ is coloured.
Answer the following question.
Give valence bond description for the bonding in the complex [VCl4]-. Draw box diagrams for the free metal ion. Which hybrid orbitals are used by the metal? State the number of unpaired electrons.
Answer the following question.
Draw a qualitatively energy-level diagram showing d-orbital splitting in the octahedral environment. Predict the number of unpaired electrons in the complex [Fe(CN)6]4-. Is the complex diamagnetic or paramagnetic? Is it coloured? Explain.
Explain, why [Co(NH3)6]3+ ion is low spin? Calculate number of unpaired electrons and write the geometry of [Co(NH3)6]3+.
Identify the number of donor groups present in EDTA.
Chlorophyll and haemoglobin are complexes of ____________ respectively.
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Identify the CORRECT statements regarding [Co(NH3)6]3+.
I. Oxidation state of metal ion = +3
II. It is a high spin complex.
III. It is paramagnetic.
IV. Metal ion undergoes d2sp3 hybridization.
Which one of the following complexes can exhibit geometrical isomerism?
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[Fe (Z = 26), Co (Z = 27), Ni (Z = 28), Cu (Z = 29)]
Explain the formation of [CoF6]3Θ complex with respect to
- Hybridisation
- Magnetic properties
- Inner/outer complex
- Geometry
Describe the bonding in the tetrahedral complex Ni(CO)4 on the basis of valence bond theory. Give the orbital diagrams of metal atoms in free state and in the complex. Mention the number of unpaired electrons in the complex.
A compound forms a hep structure. Calculate the number of octahedral voids in 0.4 mol. (NA = 6.022 × 1023).
Octahedral complex have ______ hybridisation.
Give the limitations of VBT.
A compound forms hexagonal close packed (hcp) structure. What is the number of (i) Octahedral voids, (ii) Tetrahedral voids, (iii) Total voids formed in 0.7 mol of it.
Mention the number of unpaired electrons and geometry of the following complex:
\[\ce{[Ni(CN)4]^2-}\]
