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In a normal hydrogen atom, when the electron occupies its lowest available energy state, the atom is said to be in its ground state. The maximum potential energy that an atom can have is 0J, at which point the electron has essentially been removed from the nucleus; thus the atom is ionized.
a) How much energy will it take to ionize a hydrogen atom in its ground state?
b) Calculate the wavelength of light that would be required to affect its ionization?
c) Identify the series of spectral lines to which this wavelength belongs.
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