The complex [Cr(acac)3] (acac = acetylacetonate) was prepared as follows. 1.30g CrCl3·6H2O was dissolved in 30cm3 distilled water in a 100cm3 conical flask with a watch glass. To the solution was added 6 drops of concentrated ammonia, 10g of urea and 4.0cm3 of acetylacetone. The mixture was heated on a steam bath, with occasional stirring; within an hour, dark purple crystals formed on the surface of the liquid. After two hours the mixture was cooled to room temperature and the purple crystalline product collected by filtration, washed with water and air dried. It was then recrystallised from 35cm3 each of acetone and water, filtered and air dried. 1.25g of the purple crystal was obtained. Given that the RMM of CrCl3·6H2O = 266.4g mol-1 and the RMM of [Cr(acac)3] = 349.2g mol-1, 1.30g/266.4g mol-1 = 4.88x10-3mol, so 1.70g of product is expected and this represents a percentage yield of 74%.
The complex [Cr(NH3)6]Cl3 was prepared as follows. A pre-calibrated vacuum trap tube (B29) was half-immersed in an acetone/dry ice mixture (kept cold throughout by the regular addition of CO2) in a Dewar flask and connected to an ammonia cylinder. Liquid ammonia was collected to the 40cm3 mark. A small piece of freshly cut sodium, washed with petroleum spirit, was added to the ammonia and the mixture stirred to obtain a blue-black solution. Several small crystals of ferric nitrate were added and the solution stirred again, forming a dark red-brown colour. 2.5g anhydrous CrCl3 was added in small portions, causing slight effervesence, and the solution stirred for 10 minutes. The vacuum tube was removed from the Dewar and the red-brown contents transferred to a 6"diameter evaporating basin. The basin was left for 45 minutes, by which time the ammonia had evaporated. The red-brown solid was then transferred to a 400cm3 beaker containing 40cm3 1M hydrochloric acid. The solution was stirred for 10 minutes, then filtered by gravity into an ice-cooled beaker. The yellow filtrate was cooled for 15 minutes and 40cm3 ice-cold concentrated hydrochloric acid was added. The solution was cooled in ice for 30 minutes, during which time a bright yellow solid precipitated but then largely dissolved. Vacuum filtration yielded a minuscule quantity of yellow crystals.
The following UV spectra were recorded: [Cr(en)3]Cl3 in water; chrome alum (KCr(SO4)2·12H2O) in water slightly acidified with nitric acid; [Cr(acac)3] in toluene; unknown chromium(III) complex. The unknown complex was prepared by mixing anhydrous CrCl3 with 10cm3 0.1M sulphuric acid in a test tube, expelling oxygen by adding solid CO2, and adding a few drops of 2% zinc/mercury amalgam. All the spectra recorded are shown below.
Measurements
The peaks observed in each spectrum were as follows:
[Cr(en)3]Cl3:
460nm, m
360nm, m
350nm, m
KCr(SO4)2·12H2O:
580nm, w
400nm, w
250nm, s
[Cr(acac)3]:
563nm, s
436nm, s
330nm, s
Unknown complex:
600nm, w
400nm, w
~300nm, s
Additional reference spectra:
K3[Cr(CN)6]:
380nm, s
310nm, s
CrCl3 (anhydrous):
699nm, m
519nm, s
Discussion
The splitting of d orbitals in transition complexes, as described by crystal field theory, is paramount to the understanding of their properties. One of the most immediate consequences of orbital splitting is the striking coloration of most d-metal complexes, owing to the fact that the energies of electron transition between orbitals (the d-d transitions) tend to correspond to radiation in the visible and ultraviolet regions.
In this experiment, UV spectroscopy was used to investigate these d-d transitions in a range of prepared and pre-prepared homoleptic chromium(III) complexes in order to investigate the degree of orbital splitting caused by various ligands. Because chromium(III) is not a d1 system, the spectra of its complexes show more than one d-d transition; however this problem can be more or less overcome by considering the same peak in each spectrum. The ligands investigated by this technique were ethylenediamine (en), acetylacetonate (acac), NH3, Cl- (in the unknown complex and in a reference spectrum for anhydrous CrCl3), H2O (in the unknown complex and in chrome alum, which contains the [Cr(H2O)6]3+ ion), and CN- (in a reference spectrum for K3[Cr(CN)6].
Although various factors affect the degree of orbital splitting caused by a ligand, the most significant is its ability to bond to the metal centre as a π-acceptor. This process involves the donation of electron density from the metal’s t2g orbitals to vacant (usually antibonding) π orbitals on the ligand. This reduces the energy of the t2g orbitals and hence increases ΔO. Measurement of the degree of orbital splitting caused by a ligand is therefore usually a good indicator of its ability to bond as a π-acceptor and, conversely, its inability to bond as a π-donor.
In addition to the homoleptic compounds described above, a mixed octahedral chromium(III) compound containing both water and chloride ligands was prepared, and its composition determined by the law of average environment; this simply states that the crystal field effects of each ligand type are purely additive and hence that the crystal field environment around the metal centre is an average of these effects. It can be expressed mathematically as
υ (MXaYb) = a/a+b υ (MXa+b) + b/a+b υ (MYa+b)
where υ is the absorptional frequency of a mixed compound of composition MXaYb; in this case, a + b = 6.
Problems
The main problem encountered was the difficulty in precipitating [Cr(NH3)6]Cl3 from solution; although precipitation of a bright yellow solid initially occurred, most of it subsequently dissolved, and repeated filtrations yielded only a small quantity of the product, not sufficient for spectroscopic analysis. Immediate filtration on precipitation may have yielded a greater quantity.
A secondary problem was the quality of two of the UV spectra recorded: in that for [Cr(en)3]Cl3 the middle peak is almost completely obscured, while in that for the unknown complex the peak of lowest wavelength is so strong it is difficult to place; however since only the peak of highest wavelength is needed for each compound, this is not a significant problem.
Questions
1. The wavenumber (in units of cm-1) of the lowest peak in the spectrum of each compound is as follows:
[Cr(en)3Cl3]: 21700
KCr(SO4)2·12H2O: 17200
[Cr(acac)3]: 17800
Unknown complex: 16700
K3[Cr(CN)6]: 26300
CrCl3 (anhydrous): 14300
2. A spectrochemical series for chromium(III) can be derived by noting that the energy of the lowest wavenumber transition in each spectrum roughly corresponds to ΔO and hence the spectra show the relative degree of orbital splitting caused by each ligand:
Cl- < H2O and Cl- < H2O < acac < en < CN-
This series is in close agreement with those typically given in the literature. In general it is observed that halide ligands cause the weakest d orbital splitting, followed by oxygen-based ligands (eg water), followed by carbon-oxygen ligands (eg acetylacetonate), followed by carbon-nitrogen ligands (eg cyanide). Ligands containing the same elements tend to appear close to each other in the series, and that is observed in the series above.
3. The rule of average environment states that
υ (MXaYb) = a/a+b υ (MXa+b) + b/a+b υ (MYa+b).
In this case υ (MXaYb) is the highest frequency (or, equivalently, wavenumber) of absorption for the unknown compound, and is 16700cm-1; υ (MXa+b) is that for the chrome alum and is 17200cm-1; υ (MYa+b) is that for CrCl3 and is 14300cm-1. The equation thus gives a = 5 and b = 1, hence the primary coordination sphere in the unknown compound is [Cr(H2O)5Cl]2+.
Conclusion
In this experiment, three homoleptic compounds of chromium(III) were prepared: [Cr(en)3]Cl3·3H2O in reasonable yield, [Cr(acac)3] in good yield, and [Cr(NH3)6]Cl3 in poor yield. UV spectra were recorded for the first two of these compounds, and for chrome alum, KCr(SO4)2·12H2O. Analysis of the lowest energy peak in each spectrum allowed a spectrochemical series of these ligands (including two further ligands provided by reference spectra) to be constructed.
An unknown complex of chromium(III) containing both water and chloride ligands was formed by chromium(II)-catalysed dissolution of CrCl3 in water; UV analysis and the rule of average environment allowed determination of its primary coordination sphere as [Cr(H2O)5Cl]2+.
References
Housecroft, C.E. and Sharpe, A.G. Inorganic Chemistry. Pearson Education, 2001.
Shriver, D.F. and Atkins, P.W. Inorganic Chemistry (3rd edition). OUP, 1999.