I believe it can - the energy of a photon is the product of the frequency and Plank's constant - and as far as I know, the frequency is not quantized.
Yes.
There is no such thing as "long energy" or "short energy". The electromagnetic spectrum is:Radio waves; microwaves; infrared; visible light; ultraviolet; x-rays; gamma rays. In this list, going from left to right: * The energy per photon increases. * The frequency increases. * The wavelength decreases. Thus, for instance, gamma rays have the LARGEST energy per photon; the LARGEST frequency; and the SHORTEST wavelength.
Each photon of blue light has more energy than a photon of any other color, because the blue ones have the highest frequency.
A photon is emitted when an electron falls from a higher to lower orbital. A photon is an elementary particles, the quantum of light and all other forms of electromagnetic radiation.
There are spaces in the atomic spectrum of hydrogen because there are discrete energy levels that the electron in the hydrogen atom can be located in. Generally speaking the further away from the nucleus, the higher the potential energy of the electron. When hydrogen gas is excited, the electron can jump up to higher energy levels. When that electron falls back down to a lower energy level, a photon is emitted with an energy equal to the energy difference between the atomic orbital it jumped from and the one it jumped to. Since excited electrons can make a number of different jumps (ex. 4->3, 4->2, 5->3, 5->2, etc) there are a series of photons given off with discrete energies. Each one of these photons has a distinct wavelength (given by the equation E=hf, where E is the energy of the photon, h is planck's constant and f is the frequency of the photon). Each line you see on the spectrum is a photon produced from a different energy jump, with a different wavelength. We are only able to see the photons that emit a wavelength in the visible spectrum (roughly 400-700 nm).
The electromagnetic waves that have the highest energy PER PHOTON are called gamma rays.
Different types of electromagnetic waves have different frequencies; different wavelengths; and different energies per photon.
To answer this question, let's think about the excitation and relaxation processes involved. In the excitation process inside a deuterium lamp, an electrical arc between an oxide coated filament and an electrode excites D2 to D2*. Next, the D2* dissociates into individual D atoms. Let's call these D' and D''. Also, a photon of light is released. For an individual event, the total energy posssessed by D2* is apportioned between the kinetic energies of D', D'', and the photon. The sum of the kinetic energies of D' and D'' can vary from almost zero to the original energy of D2*. If the kinetic energies of D' and D'' are relatively small, the energy of the photon is large, and a shorter wavelength of light is emitted. If the kinetic energies of D' and D'' are relatively large, the energy of the photon is small, and a longer wavelenght of light is emitted. In a population of D2*, a distribution of kinetic energies of D' and D'' will result, allowing for a continuum spectrum to be emitted from the lamp.
The relationship between electromagnetic energy (photon energy) and wavelength is determined by two constants - the speed of light and Planck's constant. Photon energy (in Joules) is equal to the speed of light (in metres per second) multiplied by Plancks constant (in Joule-seconds) divided by the wavelength (in metres). E = hc/wavelength where: E is photon energy h is Planck's constant = 6.626 x 10-34 Js c is the speed of light = 2.998 x 108 m/s This relationship shows that short wavelengths (e.g. X-rays) have high photon energies while long wavelengths (e.g. Radio waves) have low photon energies.
The line emission spectrum of an atom is caused by the energies released when electrons fall from high energy level. It goes down to a low energy level and the extra energy it had from higher level is released as light.
There is no such thing as "long energy" or "short energy". The electromagnetic spectrum is:Radio waves; microwaves; infrared; visible light; ultraviolet; x-rays; gamma rays. In this list, going from left to right: * The energy per photon increases. * The frequency increases. * The wavelength decreases. Thus, for instance, gamma rays have the LARGEST energy per photon; the LARGEST frequency; and the SHORTEST wavelength.
Each photon of blue light has more energy than a photon of any other color, because the blue ones have the highest frequency.
A photon is emitted when an electron falls from a higher to lower orbital. A photon is an elementary particles, the quantum of light and all other forms of electromagnetic radiation.
There are spaces in the atomic spectrum of hydrogen because there are discrete energy levels that the electron in the hydrogen atom can be located in. Generally speaking the further away from the nucleus, the higher the potential energy of the electron. When hydrogen gas is excited, the electron can jump up to higher energy levels. When that electron falls back down to a lower energy level, a photon is emitted with an energy equal to the energy difference between the atomic orbital it jumped from and the one it jumped to. Since excited electrons can make a number of different jumps (ex. 4->3, 4->2, 5->3, 5->2, etc) there are a series of photons given off with discrete energies. Each one of these photons has a distinct wavelength (given by the equation E=hf, where E is the energy of the photon, h is planck's constant and f is the frequency of the photon). Each line you see on the spectrum is a photon produced from a different energy jump, with a different wavelength. We are only able to see the photons that emit a wavelength in the visible spectrum (roughly 400-700 nm).
178.334kJ/mol.
This is a tricky question because there is more than one form of energy in light. There is the energy that each particle of light (the photon) has and there is group energy which is the sum total of all the photon energy as they travel as a group (like in a laser beam). But the good news is that the answer is FALSE for both the photon and group energies. Photon energy depends on the photon fundamental frequency. And the higher the energy the bluer the color, which can run from red to violet. Those photons in the violet color have higher energy than photons in the red color frequency. And group energy is just the sum of all the photon energies in a group, like a light beam from your flashlight (aka, torch). So for a given mix of photons, the more photons in the group the higher is the group energy level. What we call light intensity (e.g., bright or dim) depends on the group energy with high energy equating to high intensity.
They differ:* By their frequency * By their wavelength, which is inversely proportional to their frequency * By the energy per photon, which is proportional to the frequency
Frequency; wavelength; energy per photon.