This is a good question, and one that is of interest to those concerned with the environment. To understand energy in light, we need to understand waves and wavelengths.
Consider waves on an ocean - each wave has a high peak and a low trough, and the ocean is an endless cycle of peaks and troughs. If we were to measure the distance from one peak to the next peak, that measurement would describe the length of one wave. This measurement is appropriately called the wavelength. On the ocean, we would likely measure wavelengths in feet or meters.
Light travels in waves too, but unlike ocean waves, light waves are so small that we cannot see individual light waves. In fact, light waves are so infinitesimally tiny, we describe light wavelengths in nanometers (a nanometer is one billionth of one meter) or often in Angstroms (1 tenth of a nanometer, or one ten-billionth of one meter).
Visible light ranges in wavelength from approximately 4000 Angstroms (blue) to 7000 Angstroms (red). Blue light is therefore carried by waves that are shorter than red light.
Ultraviolet light has even shorter waves than blue light (100 to 4000 Angstroms), while at the other end of the spectrum, infrared has even longer waves than red (7000 to 10,000,000 Angstroms).
The amount of energy in light is inversely proportional to its wavelength. In other words, as the wavelength of light becomes shorter (more blue), the energy carried by that wave becomes higher. Specifically, the energy calculation for light is:
E (hc)/λ,
Where h is Planks Constant, C is the speed of light, and λ is the wavelength
While we will not concern ourselves with the mathematics here, the following statements help illustrate the relationship between light color and energy:
As an aside, the relationship between light color and energy is what has so many people concerned about the ozone layer. The ozone layer is a very high, very thin layer of ozone (O3), and one interesting property of ozone is that it filters out ultraviolet light. Without the ozone layer, high energy ultraviolet light penetrates the atmosphere, and reaches us on the Earth's surface. Because ultraviolet light carries so much more energy at the same brightness than visible light, it has the potential to cause more damage to our bodies, including cancer.
The frequency of blue light is roughly double the frequency of red light.
Light of is made up of a finite number of photons, or light quanta. The energy of each photon is proportional to the frequency of the light, and hence inversely proportional to the wavelength of the light. Red light has a longer wavelength than blue light, so the quantum of red light has less energy than the quantum of blue light.
red light
Red does as it absorbs photons at blue end of the spectrum( the higher energy) and reflects light at the red end of the spectrum (a lower energy). While the blue light absorbs energy at the red end of the spectrum and reflects blue light
The energy jump of an electron producing blue light is greater than the energy jump of an electron producing red light.
The blue light has longer wavelength, lower frequency, andless energy per photon than the ultraviolet light has.The blue light is also visible to the human eyes, whereas theultraviolet light is not.
If the color (frequency, wavelength) of each is the same, then each photon carries the same amount of energy. Three of them carry three times the energy that one of them carries.
Chlorophyll captures light energy using photosynthesis. Energy is absorbed through wavelengths. It can absorb violet-blue and orange-red light energy easily.
The frequency of blue light is roughly double the frequency of red light.
The red light is lower energy than the blue light.
Blue
Chlorophyll a absorbs energy from most wavelengths of violet/blue and orange/red. Chlorophyll b is more soluble that chlorophyll a in polar solvents and more yellow in color. It absorbs most energy from blue light.
very nice answer.
Light of is made up of a finite number of photons, or light quanta. The energy of each photon is proportional to the frequency of the light, and hence inversely proportional to the wavelength of the light. Red light has a longer wavelength than blue light, so the quantum of red light has less energy than the quantum of blue light.
red light
no red uses more energy
Red does as it absorbs photons at blue end of the spectrum( the higher energy) and reflects light at the red end of the spectrum (a lower energy). While the blue light absorbs energy at the red end of the spectrum and reflects blue light