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- (a) What is the crystal field splitting energy (Δ)?(b) How does it arise for an octahedral field of ligands?(c) How is it different for a tetrahedral field of ligands?(a) In early studies it was observed that when the complex [Co(NH3)4Br2]Br was placed in water, the electrical conductivityof a 0.05 M solution changed from an initial value of191 ohm-1 to a final value of 374 ohm-1 over a period of anhour or so. Suggest an explanation for the observed results.(b) Write a balanced chemical equation to describe the reaction.(c) A 500-mL solution is made up by dissolving 3.87 g ofthe complex. As soon as the solution is formed, and beforeany change in conductivity has occurred, a 25.00-mLportion of the solution is titrated with 0.0100 M AgNO3solution. What volume of AgNO3 solution do you expectto be required to precipitate the free Br-(aq)? (d) Based onthe response you gave to part (b), what volume of AgNO3 solution would be required to titrate a fresh 25.00-mL sampleof [Co(NH3)4Br2]Br after all conductivity changes haveoccurred?Predict the products of each of the following reactions and then balance the chemical equations.(a) Fe is heated in an atmosphere of steam.(b) NaOH is added to a solution of Fe(NO3)3.(c) FeSO4 is added to an acidic solution of KMnO4.(d) Fe is added to a dilute solution of H2SO4.(e) A solution of Fe(NO3)2 and HNO3 is allowed to stand in air.(f) FeCO3 is added to a solution of HClO4.(g) Fe is heated in air.
- 示 (C) (D) (A) (B) Which is the crystal field energy level diagram for a square pyramidal ML5 complex that contains a single ligand on the z-axis? O (D) O (A) O (B) O (C)Explain the ways in which the elements act: (a) How do you explain that fluoride, a small anion, is responsible for a weak field while water, a neutral molecule, gives rise to a much stronger binding field? (b) Explain why, for the same metallic cation and the same ligands, the energy of the binding field is lower in tetrahedral compounds than in octahedral compounds.Explain the following: (i) Nickel does not form low spin octahedral complexes. (ii) The Tt-complexes are known for the transition metals only. (iii) Co2+ is easily oxidised to Co3+ in the presence of a strbng ligand.
- (i) Draw the geometrical isomers of complex [Pt(NH3)2Cl2].(ii) On the basis of crystal field theory, write the electronic configuration for d4 ion if Δ0 < P.(iii) Write the hybridization and magnetic behaviour of the complex [Ni(CO)4]. (At. no. of Ni = 28)4 a) (i) Draw the structure of [Co(CO)2(NO)(cot)] where cot is cyclooctatriene. (ii) What is the coordination number of the Co ion? (iii) What is the hapticity of the cot ligand? (iv) Briefly describe the bonding between Co and cot.(i) What type of isomerism is shown by the complex [Cr(H2O)6]Cl3?(ii) On the basis of crystal field theory, write the electronic configuration for d4 ion if Δ0 > P.(iii) Write the hybridization and shape of [CoF6]3-.(Atomic number of Co = 27)
- (b) Consider the oxalate (ox) ligand and answer the following questions:(i) Draw the structure of the ox ligand.(ii) Identify all the donor atoms of the ligand.(iii) What is the denticity of the ligand?(iv) What is the charge of the ligand?(v) Draw the structure of a homoleptic octahedral complex with ox as the ligand.Clearly show the geometry at the metal centre.(vi) Identify the stereoisomer in the structure drawn.(a) Give systematic names for the following formulas: - [Co(N3)(NH3)s]SO4 - KĄ[Fe(CN);ONO] - [Pt(en)2][PtCl4] (b) Provide the formula with the given systematic names: - Sodium pentachloronitridoosmate(VI) - Pentaammineisothiocyanatocobalt(III) chloride - Potassium diaquabis(oxalato)manganate(III) (c)Write the formula of possible isomer structure for [Co(NH3)sBr]SO4 complex. Define the type of isomerism and explain how you can differ them?(a) Square planar complexes (of MXJLJ type) with coordination number of 4 exhibit geometrical isomerism, whereas tetrahedral complexes with similar composition do not. Why? (b) Describe the type of hybridization, shape and magnetic property of [CO(NH3)4Cl2]Cl. [Given : At. no. of Co = 27]
