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When an electron in atom changes energy states a photon is emitted If the photon has a wavelength of 550 nm how did the energy of the electron change?
The energy of the electron decreased as it moved to a lower energy state, emitting a photon with a wavelength of 550 nm. This decrease in energy corresponds to the difference in energy levels between the initial and final states of the electron transition. The energy of the photon is inversely proportional to its wavelength, so a longer wavelength photon corresponds to lower energy.
If a photons wavelength is 663 nm what is its energy?
The energy of a photon can be calculated using the formula E=hc/λ, where h is Planck's constant (6.626 x 10^-34 J*s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength in meters. Converting 663 nm to meters (1 nm = 1 x 10^-9 m), we get λ = 663 x 10^-9 m. Plugging in the values, we find the energy of the photon to be approximately 3.00 x 10^-19 Joules.
What wavelength ultraviolet light is best for viewing fluorescent minerals?
Short-wave ultraviolet light (UV-C, 100-280 nm) is best for viewing fluorescent minerals, as it provides the most intense fluorescence. Medium-wave ultraviolet light (UV-B, 280-315 nm) can also be used, but the fluorescence will be less intense. Long-wave ultraviolet light (UV-A, 315-400 nm) is not ideal for viewing fluorescent minerals as it may not excite the fluorescence as effectively.
What colour is light of a wavelength 700nm?
The formula for frequency is f = c/lambda, where c is the speed of light in a vacuum, lambda is the wavelength in meters, and f is frequency in cycles per second. So, if the wavelength is 700.5 nm, the frequency is 4.28 E14 hertz.
What is the wavelength of a photon with an energy of 3.26 10 19 J?
The wavelength is 610 nm.
What is the energy of a 170 nm ultraviolet photon?
The energy of a photon can be calculated using the formula E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon. Plugging in the values for a 170 nm ultraviolet photon gives an energy of approximately 7.3 eV.
What is the wavelength of a photon whose energy is twice that of a photon with a 580 nm wavelength?
Since the energy of a photon is inversely proportional to its wavelength, for a photon with double the energy of a 580 nm photon, its wavelength would be half that of the 580 nm photon. Therefore, the wavelength of the photon with twice the energy would be 290 nm.
What is the energy in joules of an ultraviolet photon with wavelength 130 nm?
The energy of a photon can be calculated using the formula E = hc/λ, where h is Planck's constant (6.626 x 10^-34 J*s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength of the photon in meters. First, convert the wavelength to meters (130 nm = 130 x 10^-9 m), then plug the values into the formula to find the energy. The energy of an ultraviolet photon with a wavelength of 130 nm is approximately 1.52 x 10^-18 Joules.
What is the energy of a 500 nm photon?
The energy of a 500 nm photon is 3.1 eV (electron volts). This is a unit of measure used to represent the energy of a single photon. To put this into perspective, a single photon of visible light has an energy of 1.8 to 3.1 eV, and a single photon of ultraviolet light has an energy of 3.1 to 124 eV. The energy of a 500 nm photon can be calculated by using the following equation: E = hc/ Where: E = energy of the photon (in eV) h = Planck's constant (6.626 * 10-34 Js) c = speed of light (2.998 * 108 m/s) = wavelength of photon (in meters) Therefore, the energy of a 500 nm photon is calculated as follows: Convert the wavelength from nanometers to meters: 500 nm = 0.0005 m Insert the values into the equation: E = (6.626 * 10-34 Js) * (2.998 * 108 m/s) / (0.0005 m) Calculate the energy: E = 3.1 eVTherefore, the energy of a 500 nm photon is 3.1 eV.
What is the energy of a photon with a wavelength of 500 nm in kilo electron volts (keV)?
The energy of a photon with a wavelength of 500 nm is approximately 2.48 keV.
What is the energy of an ultraviolet photon having a wavelength of 1.18?
The energy of a photon is given by E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength of the photon. Plugging in the values, the energy of an ultraviolet photon with a wavelength of 1.18 nm is approximately 10.53 eV.
What is the frequency and energy of a photon with a wavelength of 488.3 nm?
The frequency of a photon with a wavelength of 488.3 nm is approximately 6.15 x 10^14 Hz. The energy of this photon is approximately 2.54 eV.
How do you calculate the energy in joules of a photon of green light having a wavelength of 529 nm?
The energy of this photon is 3,7351.10e-19 joules.
What is the wavelength of a photon with an energy of 3.26 10-19?
610 nm
What is the wavelength of a photon that has three times as much energy as that of a photon whose wavelength is 779 nm?
Photon energy is proportional to frequency ==> inversely proportional to wavelength.3 times the energy ==> 1/3 times the wavelength = 779/3 = 2592/3 nm
Transition A produces light with a wavelength of 400 nm Transition B involves twice as much energy as A What wavelenth light does it produce?
Transition B produces light with half the wavelength of Transition A, so the wavelength is 200 nm. This is due to the inverse relationship between energy and wavelength in the electromagnetic spectrum.
When an electron in atom changes energy states a photon is emitted If the photon has a wavelength of 550 nm how did the energy of the electron change?
The energy of the electron decreased as it moved to a lower energy state, emitting a photon with a wavelength of 550 nm. This decrease in energy corresponds to the difference in energy levels between the initial and final states of the electron transition. The energy of the photon is inversely proportional to its wavelength, so a longer wavelength photon corresponds to lower energy.
