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3. This question is about energy levels and atomic models. (a) Diagram 1 below shows some of the energy levels (measured in electron-volts) of the hydrogen atom. Diagram 2 is a representation of part of the visible spectrum of atomic hydrogen (not to scale). Diagram 1 Diagram 2 0 -0.54 -0.85 -1.5 2 = 660nm 2. = 470nm 1 = 430nm = -3.4 energy / eV red blue violet -13.6
(i) State the value of the ionization energy of hydrogen. (ii) The wavelength corresponding to the red line in the visible spectrum of atomic hydrogen is 660 nm. Deduce that the energy of a photon of wavelength 660 nm is 1.9 eV. (iii) Deduce with an appropriate calculation whether the energy of a photon of wavelength 660 nm on interaction with a nucleus is enough to produce an electron-positron pair. (iv) On diagram 1, draw an arrow to show the electron transition between energy levels that gives rise to a photon of energy 1.9 eV. Label this arrow with the letter R. (v) On diagram 1 and using your answer to (iii), draw arrows to show the electron transitions that give rise to the blue line and to the violet line in the visible spectrum of atomic hydrogen. Label these arrows B and V respectively. (vi) Determine the wavelength emitted by a photon corresponding to a transition from an n= 5 ton = 1 level and state which part of the electro-magnetic spectrum that the emitted photon belongs.