Final answer:
The absorbance spectrum of common available metal oxides can be found in scientific literature or databases. Transition metal complexes absorb visible light in a manner that depends on the d-orbital configuration, which often permits viewing colors in solution.
Step-by-step explanation:
To find the absorbance spectrum of visible light of common available metal oxides, you would typically refer to published scientific literature or specialized databases that house spectral data for various compounds. However, understanding the principles of how these metal oxides interact with light, particularly in the visible range, is essential.
When transition metal complexes absorb light at the proper frequency, their d-electron configuration allows some visible light to be absorbed due to the energy difference between the d orbitals. The specific wavelengths that are absorbed determine the perceived color of the metal oxide when dissolved in water. This is because the visible light of a given energy level that is not absorbed is what we actually see.
For example, if a compound absorbs light in the green region (around 524 nm), it would appear red to our eyes because green light is being subtracted from the visible spectrum. The absorbance spectrum can be analyzed using a UV-vis spectrophotometer, which records the wavelengths absorbed by a sample.
For a practical application, you can often find UV-vis spectra in online databases such as the Spectral Database for Organic Compounds. These spectra include absorbance peaks, represented as Amax for the maximal light absorbance wavelength, and the absorbance value, which can be used to determine the concentration of the solution using the Beer-Lambert Law.
The Spectrum Explorer tool is another resource that provides insights into how elemental absorption lines change with temperature, though it is more commonly suited to individual elements rather than complex oxides.