The following questions are case-based questions. Read the case carefully and answer the questions that follow

The nature of bonding structure of the coordination compound can be explained to some extent by valence bond theory, The central metal atom/ion makes available a number of vacant orbital equal to its coordination number. The appropriate atomic orbital (s, p and d) of the metal hybridise to give a set of equivalent orbitals of definite geometry such as square planar,tetrahedral, octahedral and so on. A strong covalent bond is formed only when the orbitals overlap to the maximum extent. The d-orbitals involved in the hybridisation may be either inner d-orbitals i.e (n-1)d or outer d-orbitals i.e. nd. The complexes formed are caned inner orbital complex (low spin complex) and outer orbital complex (high spin complex) respectively. Further, the complexes can be paramagnetic or diamagnetic in nature. The drawbacks Of this theory are that this involves number of assumptions and also does not explain the colour of the complex.

Answer the following questions:

(a) Predict whether [CoF₆]^3- is diamagnetic or paramagnetic and why?
[Atomic number: Co=27]

(b) What is the coordination number of Co in [Co(en)₂Cl₂]⁺
(c) (i) Write the IUPAC name of the given complex:

[Pt(NH₃)₂Cl₂]²⁺

(ii) Explain [Co(NH₃)₆]³⁺ is an inner orbital or outer orbital complex

OR

Using valence bond theory,deduce the shape and hybridisation of [Ni(NH₃)₆]²⁺[Atomic number of Ni=28]

Solution

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