a. What is the oxidation number of the transition metal in each of the following complexes?

i. [Co(NH₃)₆]³⁺

ii. [Ni(CN)₄]^2–

iii. [Cr(OH)₆]^3–

iv. [Co(en)₃]³⁺

v. Cu(OH)₂(H₂O)₄

b. EDTA^4– ions can act as ligands. A single EDTA^4–ion can form six co-ordinate bonds to a central transition metal ion to form an octahedral complex. It is called a hexadentate ligand. Give the formula of such a complex formed between Ni²⁺and EDTA^4–.

c. Which ligands in Table 24.4 are bidentate?

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Example of complex TFe(H,0)P Name of ligand Formula Co-ordination Shape of complex number water H,0 6. octahedral (see Figure 24.4) ammonia NH, [CO(NH,)J* 6. octahedral chloride lon 4 tetrahedral (see Figure 24.5b) cyanide lon INI(CN),F- CN- square planar (see Figure 24.5a) 4 hydroxide lon OH- (Cr(OH)- octahedral 6. thlocyanate lon (FESCNJ2" or (Fe(SCN)(H,0),P [Mn(ox) SCN octahedral ethanedioate lon (abbrevlated as 'ox' In the formulae of complexes) -O0C-C00- octahedral [Co(en),P* octahedral (see Figure 24.6) 1,2-dlaminoethane (abbrevlated as 'en' in the formulae of complexes) NH,CH,CH,NH,