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Q: If the photon has a frequency of 4 x 1015 Hz how did the energy of the electron change?

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The electron lost 4 x 10-19 J of energy.

If the change in energy of electron is totally exhibited as a photon then the energy = h times frequency. h = 6.626 x 10 to -34 J s Simply multiply h and frequency you would get the energy in joule

The energy of a photon whose frequency is 5.8 x 1014 Hz is: 2.4322643592E-11 electron volts.

The light photon (light wave) was emitted by an electron jumping between two energy levels in an atom, the energy of the photon is determined by how large is the difference between these two levels, i.e the frequency of the photon is determined by the energy of the photon

Photon energy = 1.77006248E-12 electron volts.

As a photon. The exact frequency (color) of the photon depends on the specific energy level.

4x 1015 Hz The electron lost 2.6 x 10-18 J of energy.

The energy of a photon is directly proportional to its frequency.The energy of a photon is directly proportional to its frequency.The energy of a photon is directly proportional to its frequency.The energy of a photon is directly proportional to its frequency.

in quantum mechanism the energy of the photon electron vary with the frequency but independent of the intensity of the incident radiation while in classical mechanism the energy of the photon-electron should vary with intensity but should be independent of the frequency.

An atom emits a photon (particle of light) when transitioning from a ground state to its excited state. To obey conservation of energy, the energy gained by the atom when an electron moves to a lower energy level is equal to the energy it loses in emitting the photon. (The energy of a photon is E = hf, where E is the energy, h is Planck's constant, and f is the frequency of the photon.) Conversely, when an atom absorbs a photon (as is the case in absorption spectra), the electron absorbing the photon moves to a higher energy level.

Depending on the energy (frequency) of the specific photon hitting the electron, one of three events happens: nothing, the electron is excited, or the electron leaves the atom. If the energy of the photon very high, the electron can absorb the energy and escape the nucleus' pull. This is called ionization. If the energy of the photon lines up with the energy spacing in the atoms energy levels, the electron will move to a higher energy state, becoming excited. The electron then returns to its original energy level, releasing the energy as light. If the energy of the photon does not fall into one of these categories, the electron does not interact with it. In terms of actually changing the electron, it only changes in energy, not any other property.

Depending on the energy (frequency) of the specific photon hitting the electron, one of three events happens: nothing, the electron is excited, or the electron leaves the atom. If the energy of the photon very high, the electron can absorb the energy and escape the nucleus' pull. This is called ionization. If the energy of the photon lines up with the energy spacing in the atoms energy levels, the electron will move to a higher energy state, becoming excited. The electron then returns to its original energy level, releasing the energy as light. If the energy of the photon does not fall into one of these categories, the electron does not interact with it. In terms of actually changing the electron, it only changes in energy, not any other property.

The photon energy is directly proportional to its frequency: Energy = Planck's constant * frequency.

An electron emits a photon when it lowers its energy, going for a lower energy orbital. The energy of the photon will be the difference of energy between the orbital where the electron was, and the orbital where the electron went.

what is the energy of a photon that has a frequency of 5.0x1014 Hz?

The energy of the photon is the same as the energy lost by the electron

the frequency of a photon of light , the greater the greater the energy packed into that photon.

The minimum amount of energy per photon necessary for that photon to knock an electron free from the crystal structure of that metal.

Every element has a specific energy describing each of the energy levels that any given electron is able to occupy. In order to occupy a higher energy level the electron must gain some energy, and this energy is derived from a particle of light known as a photon. Since the electron can only exist in specific energy levels it must absorb a photon with the exact amount of energy required. A photon with too much or too little energy will have no effect. The amount of energy in a photon is proportional to the frequency of the light that it came from, so only certain frequencies of light can be used to move electrons from one energy level to another. Similarly, an electron would have to lose energy to drop to a lower energy level, and this energy is released in the form of a photon. If you know the difference in the energy levels, you can actually calculate the energy of such a photon and predict what frequency of light it will produce.

electron lost 3.6 x 10-19 -barbie=]

8.3 x 1017 Hz

4.5 x 1017 Hz

Frequency, color, energy in each photon.

emits a photon of a specific frequency.

Energy is either absorbed or released. If the electron goes from a high energy orbital to a lower energy one, a photon is emitted. When a photon is absorbed, the electron goes from low energy to high.