Here is a graph I made, and im being asked to explain the trends in the dips and

ID: 918632 • Letter: H

Question

Here is a graph I made, and im being asked to explain the trends in the dips and waves. The exact question being asked is as follows: Explain the dips and peaks you see for each of the primary colors.

I dont understand the relationship between color, absorbtion, and wavelength, and how to interpert this graph - can someone explain this to me?

Also, the color of the solution mixture used during the experiement is labeled in the graphs key. We are also being asked; explain how each mixture corresponds to the primary colors that were used to make it. Does this mean that their is a difference in the color of the solution used and the trends (that ultimately determine what color would be visible) that are present on the graph?

Absorbtion vs Wavelength 2.50 2.00 Solution 1 (purple) Solution 2 (blue) Solution 3 (green) Solution 4 (yellow) Solution S (orange) Solution 6 (red) 1.50 1.50 1.00 0.50 0.00 440 490 540 590 640 690 740 Wavelength (in nm)

Explanation / Answer

Many molecules absorb ultraviolet or visible light. The absorbance of a solution increases as attenuation of the beam increases. Absorbance is directly proportional to the path length, b, and the concentration, c, of the absorbing species. Beer's Law states that

A = ebc, where e is a constant of proportionality, called the absorbtivity.

Different molecules absorb radiation of different wavelengths. An absorption spectrum will show a number of absorption bands corresponding to structural groups within the molecule. For example, the absorption that is observed in the UV region for the carbonyl group in acetone is of the same wavelength as the absorption from the carbonyl group in diethyl ketone.

The absorption of UV or visible radiation corresponds to the excitation of outer electrons. There are three types of electronic transition which can be considered;

solution 1 (purple): Here it shows three absorption bands at 490nm, 540nm and 665 nm. Among these bands, 490 nm is the strong absorption band.

solution 2(blue): Here it shows three bands at 580 nm, 615 nm and 665nm.Among these bands, 580 nm is the strong absorption band.

solution 3 (green): Here it shows only one absorption band at 630 nm.

solution 4 (yellow): Here there is no absorption band seen in the provided spectrum wavelength range.

solution 5(orange):Here it shows only one absorption band at 500 nm.

solution 6(red): Here it shows three bands at 470 nm, 520 nm and 720 nm. Among these bands, 520 nm is the strong absorption band.

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Here is a graph from the original paper with an abbreviated figure legend: Fig 1

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Here is a graph I made, and im being asked to explain the trends in the dips and

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