Calculate the frequency and the wavelength of the photon with enough energy to e

Question

Calculate the frequency and the wavelength of the photon with enough energy to eject on electron from a metal plate made of Cesium. The first ionization energy for Cesium is 376 kJ/mote. What it the kinetic energy of the electron elected from the surface of Cesium by a photon with o wavelength of 250 nm? Use your answer from W3 in this question. Calculate the wavelength of light that is emitted or absorbed In the following electron transitions In the hydrogen atom. Clearly slate whether energy b being emitted or absorbed. What type of electromagnetic radiation (UV, visible, etc) is being emitted/absorbed lor each? From n=5 to n=2 From n= 2 to n=5 From n= I to n=7 From n= 1 to n=infinity

Explanation / Answer

3. hv = hv0 + k.e

work function = hv0

energy required per molecule = 376*10^3 / (6.023*10^23) = 6.243*10^-19 joule

6.625*10^-34*v = 6.243*10^-19 + 0

v = frequency required = 9.42*10^14 s-1

wavelength required = c/v = (3*10^8 / (9.42*10^14)) = 3.184*10^-7 m

4.

6.625*10^-34*(3*10^8/ (250*10^-9)) = 6.243*10^-19 + x

x = 1.707*10^-19 joule = kinetic energy of ejected electron

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