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Really have no clue what to do on this one..?
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 0 J, at which point the electron has essentially been removed from the nucleus; thus the atom is ionized.
How much energy will it take to ionize a hydrogen atom in its ground state? What is the wavelength of light that would be required to effect this ionization? What are the series of spectral lines to which this wavelength belongs?
The Rydberg formula is used in atomic physics for describing the wavelengths of spectral lines of many chemical elements. For hydrogen:
1/λ = Rh*(1/n1^2-1/n2^2)
Where λ is the wavelength of the light emitted in vacuum, Rh is the Rydberg constant for hydrogen: Rh = 1.0967758341x10^7/m, and n1 and n2 are integers such that n1 < n2.
By setting n1 to 1 and letting n2 approaching infinity(such that 1/n2^2 = 0), the spectral lines known as the Lyman series converging to 91 nm are obtained.
To convert frequency or wavelength to energy, we have to use the following formula:
E = h•ν = h•c/λ
where E is the energy in joule, h the Plank constant 6.626x10^-34 J•s, ν the frequency in 1/s, c the speed of light 2.998x10^8m/s, and λ the wavelength in m (1nm = 10^-9m). Now please do the math.
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