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∙ 14y ago5.10 x 10^14 hz
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∙ 11y agoWiki User
∙ 11y ago588 nm
The energy of a photon is given by 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. Rearranging the formula to solve for λ gives λ = hc / E. Plugging in the values gives λ = (6.626 x 10^-34 J·s) * (3.00 x 10^8 m/s) / 3.8 x 10^-19 J = 523 nm. The wavelength of the photon is 523 nm.
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∙ 14y agoLong way. Energy = Planck's constant * speed of light/lambda in meters
3.8 X 10^-19 J = (6.626 X 10^-34 J*s)(2.998 X 10^8 m/s)/ Lambda in meters
= 5.2 X 10^-7 meters, which is ~ 523 nanometers in wavelength.
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∙ 14y agoEnergy = Planck's constant * speed of light/Lambda(wavelength)
4 X 10^-17 J = (6.626 X 10^-34J*s)(2.998 X 10^8m/s)/Lambda
= 4.97 X 10^-9 meters or, 4.97 nanometers ( short wavelength )
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∙ 14y agoE=hC/λ rearranges to λ=hC/E
λ= (6.63 x 10-34) x (3 x 108) / 3.8 x 10-19
λ= 5.23 x 10-7m
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∙ 8y agoThe wavelength is 609,34 nm.
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∙ 14y ago522 nm
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∙ 12y ago588 nm
440 - 460 nm
The wavelength of the electron can be calculated using the de Broglie wavelength formula, which is λ = h/p, where λ is the wavelength, h is the Planck constant, and p is the momentum of the electron. The momentum of the electron can be calculated using the relation p = sqrt(2mE), where m is the mass of the electron and E is the energy gained by the electron from the potential difference. By substituting the given values into these equations, you can calculate the wavelength of the electron.
The smallest energy drop of an electron produces red light. When an electron transitions to its lowest energy level, it emits a photon with the least energy, corresponding to the red wavelength of light.
Drops to a lower energy level and emits one photon of light.
Electrons will travel fastest when hitting uranium at a specific wavelength corresponding to their maximum kinetic energy, which is determined by the energy of the incoming electrons and the properties of uranium. This wavelength can be calculated using the de Broglie wavelength formula involving the electron's energy and momentum.
450 nm
4.8 - 5.2 nm
440 - 460 nm
The wavelength is w = hc/E = .2E-24/4E-17 = 5E-9 meters.
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.
When an electron falls from n4 to n1, it releases more energy because it is transitioning between high energy states. This higher energy transition corresponds to a shorter wavelength of light being emitted, according to the energy of the photon being inversely proportional to its wavelength. In contrast, when an electron falls from n2 to n1, the energy released is less, resulting in a longer wavelength of light emitted.
Beryllium has a much larger second ionization energy than the first because after losing its first electron, the remaining electron is held more tightly due to increased electrostatic attraction from the positively charged nucleus. This results in a higher energy requirement to remove the second electron.
An electron can be removed from an atom if ionization energy is supplied. Ionization energy is the energy required to remove an electron from an atom, resulting in the formation of a positively charged ion.
Adding electrons to an oxygen atom requires more energy because its electron shells are already filled and adding more electrons would create repulsion due to increased electron-electron interactions. Removing an electron requires more energy because oxygen has a strong attraction to electrons due to its high electronegativity, making it difficult to remove an electron.
an electron
The electron would be removed from the outermost energy level, which is the fourth energy level, for calcium.
The wavelength of the electron can be calculated using the de Broglie wavelength formula, which is λ = h/p, where λ is the wavelength, h is the Planck constant, and p is the momentum of the electron. The momentum of the electron can be calculated using the relation p = sqrt(2mE), where m is the mass of the electron and E is the energy gained by the electron from the potential difference. By substituting the given values into these equations, you can calculate the wavelength of the electron.