and Magnetism in Coordination Chemistry; Crystal-Field

Chapter , Problem 52E

(choose chapter or problem)

As shown in Figure 23.26, the 𝑑-𝑑 transition of \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) produces an absorption maximum at a wavelength of about 500 nm. (a) What is the magnitude of  for \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) in kJ/mol? (b) How would the magnitude of  change if the \(\mathrm{H}_{2} \mathrm{O}\) ligands in \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) were replaced with NH3 ligands?

How would this absorbance spectrum change if you decreased the concentration of the \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) in solution?

▲ Figure 23.26 The color of \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) A solution containing the \(\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) ion appears purple because, as its visible absorption spectrum shows, the solution does not absorb light from the violet and red ends of the spectrum. That unabsorbed light is what reaches our eyes.

Equation transcription:

Text transcription:

{H}_{2} {O}

[{Ti}({H}_{2}{O})_{6}]^{3+}