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I've been working on this problem and I'm not coming up with a reasonable answer.

If the Bohr model is used, what frequency of light

would be required for ionization of hydrogen?

I know that [tex]\Delta E = h \nu[/tex], where E is energy, h is Planck's constant, and [itex]\nu[/itex] is frequency and that [tex]\nu = \frac{c}{\lambda}[/tex] and I know the first ionization energy of hydrogen is 1312 kJ/mol, but I can't seem to arrive at the answer.

I tried using both 1312kJ and 1.312x10^6J for E but the answer comes out too large. The solution is 3.29 × 10^15 Hz. Any help is appreciated.

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# Homework Help: Ionization and light

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