(a) Use valence bond theory to describe the hybridization, number of unpaired electron and magnetic properties of the following compounds: (i) [Zn(OH)4]2( Tetrahedral ) (ii) [Ni(CN)4]2. (low-spin) (b) With the aid of suitable diagram, describe bonding in the complex, [Co(CN)6]3 using: i. Valence Bond theory ii. Crystal Field theory iii. Which of the theory is most suitable to describe the colour and magnetic properties of the compound? Give reason for your answer. (5) (c) Describe four factors that governs the magnitude of ect (2) (d) Draw the crystal field diagrams for [Fe(NO2)6]4 and [FeF6]3. State whether each complex is high spin or low spin, paramagnetic or diamagnetic, and compare ect to P for each complex. QUESTION TWO (a) Sketch a comparative crystal field splitting diagram for transition metal ions in an octahedral and square planar crystal field. (2) (b) Draw the crystal field splitting diagram and use it to explain the origin and differences in the colour of the following complexes. (i) [Co(NH3)6]3+ (ii) [CoF6]3 (iii) [Co(CN)6]3 (c) State with reason whether the following complexes would suffer from a Jahn-Teller distortion: (i) [CuCl6]4 (ii) [Cr(CN)6]3 (iii) [Mn(ox)3]3 (d) For complexes of the same metal ion with no change in oxidation number, the stability increases as the number of electrons in the t2g orbital increases. Which complex in each of the following pairs of complexes is more stable? (i) [Fe(H2O)6]2+ or [Fe(CN)6]4 (ii) [Co(NH3)6]3+ or [CoF6]3 (iii) [Mn(CN)6]4 or [MnCl6]4 (e) Arrange the following complexes [Fe(H2O)6]2+,[Fe(CN)6]3 and Fe(CN)6]4 in increasing order of occ.. Give reasons for your