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Calculate the value of wavelength of hydrogen electron when it jumps from 5th energy level to 2nd energy level |
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Answer» MATE❤✌The energy transition will be equal to 1.55⋅10−19J .So, you know your energy levels to be n = 5 and n = 3. Rydberg's equation will allow you calculate the WAVELENGTH of the photon EMITTED by the electron during this transition1λ=R⋅(1n2final−1n2 initial) , whereλ - the wavelength of the emitted photon;R - Rydberg's constant - 1.0974⋅107m−1 ;n final - the final energy LEVEL - in your case equal to 3;n initial - the initial energy level - in your case equal to 5.So, you've got all you need to SOLVE for λ , so1λ=1.0974⋅107m−1⋅(132−152)1λ=0.07804.107m−1⇒λ=1.28⋅10−6m Since E=hcλ , to calculate for the energy of this transition you'll have to multiply Rydberg's equation by h⋅c, where - Planck's constant - 6.626⋅10−3J ⋅sc - the speed of light - 299,792,458 m/s So, the transition energy for your particular transition (which is part of the Paschen Series) is E=6.62⋅10−34J⋅s⋅299,792,458m/s1.28⋅10−6m E=1.55⋅10−19J✌❤PIYUSH_SHARMA❤✌ |
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