Everyone seems to have a favorite color. But, to most scientists, having a favorite color relates to its constituents. Colors are a matter of mathematics and geometry; the intimate language of nature.
When Isaac Newton discovered sunlight constituted a rainbow of colors, he helped us to understand the underpinnings of color.
Our visual perception of blue or red is actually only one part of the many individual units of white light.
Furthermore, each unit of color corresponds to a ‘different unit number (or wavelength)’ within the rainbow (or spectrum of colors).
From red to violet, you can examine the corresponding numbers and you may reach the conclusion life is ordered in a numerically consistent manner.
Colors, Wavelengths, and Our Visual Perception
When examining the colors of different substances, certain hues and shades will correspond to differing numerical units or wavelengths.
One particularly easy example is color red-orange (625 nm) which could correspond to a carrot or shade of tomato.
The principle molecular constituent is beta-carotene, its molecular structure (scaffolding) is a complex system of atoms that is noted to be a linear:
Shortening the molecule by eliminating portions of the chain corresponds to another important, colorful molecule gives Vitamin A (corresponds to yellow or 550 nm).
Another important, colorful molecule is hemoglobin (blood). Everyone is familiar with its scarlet coloration; its responsible unit is heme, also known as haem:
While molecules similar to heme (such as chlorophyll) may induce a different color sensation, the principles behind the sensation of color are under the laws of quantum mechanics. From substances that look red to others that appear green, there must be a light reaction – the same light constituting a rainbow (or spectrum of colors).
Sunlight, Chlorophyll, and Wavelengths
In sun light, chlorophyll will absorb purple light and emit green light. It does this because all matter will absorb light and will emit it at a different wavelengths. In fact, once a molecule absorbs at a certain wavelength it will emit at lower wavelength—it must do so. The ‘energy’ associated with absorbance is re-distributed throughout the molecule. The light energy can go only two places—absorbing the light and emitting it.
When envisioning the absorbance and emission of light, you can come away with the following:
Each substance or material contains molecules that can characterize it unambiguously. The geometry (or scaffolding) of the molecule is unique. The uniqueness conveys a manner by which we may use light to identify it. Vitamin A and beta-carotene are similar substances but they may be identified, in part, by their coloration.
We usually use other forms of light (infrared, ultraviolet or x-ray) in conjunction with the visible (rainbow spectrum) to identify molecular constituents of a material. When presented with a material that we cannot unambiguously identify with one form of light, the other forms of light help piece the puzzle together.
Chemistry, Light, And Structure of Color
Perhaps by understanding that we can identify each material and its unique structure with different forms of light, we may seek to understand nature, as well.