The octahedral complex [Ti(H2O)6]3+ has a single d electron. To excite this electron from the ground state t2g orbital to the eg orbital, this complex absorbs light from 450 to 600 nm. The maximum absorbance corresponds to Δoct and occurs at 499 nm. Calculate the value of Δoct in Joules and predict what color the solution will appear.

What is the charge on each of the following complex ions? hexaaquairon(II), [Fe(H2O)6]? tris(carbonato)ferrate(III), [Fe(CO3)3]? diaquatetrachlorovanadate(III), [V(H2O)2Cl4]? Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g., +1,-2,+3).

Write the valence electron configuration for the cobalt ions in the complexes  [Co(H2O)6]2+ and draw labelled crystal field splitting diagram (relative to the spherical ion) and calculate the magnetic moment, µ(spin-only) of the cobalt ion in the complexes and as a free metal ion.

Answer the following questions about the transition metals complexes with the chemical formulas [Co(en)3]3+and [CoCl6]3- Would either the low-spin or high-spin configuration result in a paramagnetic complex? One of the complexes is orange while the other is blue. Which cobalt complex is which color? Justify your answer and identify which color the complex will absorb based on its color.

A) Using a cobalt (III) ion as the central metal atom, and with chloride ions (Cl-) and ammonia (NH3) molecules as the ligands, draw both isomers of the coordination complex that will exhibit fac/mer isomerism. B) Using a platinum (II) ion as the central metal atom, with chloride ions and ammonia molecules as the ligands, draw both isomers of the coordination complex that will exhibit cis/trans isomerism. Platinum (II) forms four coordinate bonds.

In 2001, chemists at SUNY-Stony Brook succeeded in syn-thesizing the complex trans-[Fe(CN)4(CO)2]2-, which could be a model of complexes that may have played a role in the origin of life. Sketch the structure of the complex.