The relationship between the wavelength (λ) and energy (E) of a photon is described by the equation:
E = h * c / λ
where: E represents the energy of the photon, h is Planck's constant (approximately 6.626 x 10^-34 joule-seconds), c is the speed of light in a vacuum (approximately 3.00 x 10^8 meters per second), and λ is the wavelength of the photon.
According to this equation, the energy of a photon is inversely proportional to its wavelength. In other words, photons with shorter wavelengths have higher energies, while photons with longer wavelengths have lower energies.
This relationship is a fundamental concept in physics known as the wave-particle duality of light. It suggests that electromagnetic radiation, including light, can exhibit both wave-like and particle-like properties. The energy of a photon is quantized, meaning it comes in discrete packets or quanta, which are proportional to the frequency or inversely proportional to the wavelength of the associated wave.
For example, photons of visible light have a wide range of wavelengths, from approximately 400 to 700 nanometers (nm). Photons with shorter wavelengths, such as those in the blue or ultraviolet part of the spectrum, have higher energies. On the other hand, photons with longer wavelengths, such as those in the red or infrared part of the spectrum, have lower energies.
It's important to note that this relationship between wavelength and energy applies specifically to photons and electromagnetic radiation. For other particles, such as electrons or atoms, different equations and concepts are used to describe their energy behavior.