Explaining the experiments on the photoelectric effect. The energy that a photon carries depends on its wavelength.

Explain why the emitted electrons (in the photoelectric effect) have a range of kinetic energies up to a maximum value. E = hc/l, How these experiments led to the idea of light behaving as a particle of energy called a photon. All photons are emitted from atoms . And it manages to happen in just a fraction of a millisecond. Photons of visible light — light with wavelengths of 400 to 700 nanometers, corresponding to the colors violet, indigo, blue, green, yellow, orange and red — simply don't have enough energy to cause this skipping.

They only interact with charged particles, and not with each other. Consequently, photons of visible light travel through glass instead of being absorbed or reflected, making glass transparent.

And it manages to happen in just a fraction of a millisecond.

Photons emitted by electrons “decaying” from a higher-energy orbital to a lower-energy orbital have the same energy as the energy difference from the higher orbital and the lower orbital. The electron must give up energy to make this transition, and that energy appears as a photon. Photons travel at the vacuum speed of light (more commonly just called the speed of light) of c = 2.998 x 10 8 m/s. Photons emitted before turning off the lamp will continue to bounce off objects until objects in the room completely absorb them. Wavelengths are more like streams of photons -- the greater the heat, the more energy given off (radiated), so more photons and higher frequencies/shorter wavelengths. E/h = n * nu -> the term n * nu should have units of photons/second.

Wavelengths are more like streams of photons -- the greater the heat, the more energy given off (radiated), so more photons and higher frequencies/shorter wavelengths. The emission spectrum of a chemical element or chemical compound is the spectrum of frequencies of electromagnetic radiation emitted due to an atom or molecule making a transition from a high energy state to a lower energy state. Since the photons absorbed or emitted by electrons jumping between the n = 1 and n = 2 energy levels must have exactly 10.2 eV of energy, the light absorbed or emitted must have a definite wavelength. Therefore, it is suffice to ask why photons have specific wavelength? The photon energy of the emitted photon is equal to the energy difference between the two states. The energy in a hydrogen atom depends on the energy of the electron.

Higher energy implies high frequency or low wavelength. When the electron changes levels, it decreases energy and the atom emits photons. The photon is emitted with the electron moving from a higher energy level to a lower energy level. This is the number of photons that the light carries each second. Photons of visible light — light with wavelengths of 400 to 700 nanometers, corresponding to the colors violet, indigo, blue, green, yellow, orange and red — simply don't have enough energy to cause this skipping. Consequently, photons of visible light travel through glass instead of being absorbed or reflected, making glass transparent. All photons are ejected out of an atom with a constant velocity of C, but with different energies which they acquired from the atom. How does treating the electron as a wave rather than as a particle solve the riddle of why electron orbits are discrete? Explain why the emitted electrons (in the photoelectric effect) have a range of kinetic energies up to a maximum value. Photons have energy dependent on frequency. The energy difference between orbits is equal to the sum of the energies of photons emitted by an electron going from one orbit to the other. Photons, real and virtual, are emitted and absorbed by charged particles, even though they are not charged themselves.