What Frequency Photon Ionizes an Atom from n=2 State?

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To ionize an atom from the n=2 state, a photon with sufficient energy must be emitted. The energy required for ionization is identified as 4 eV, which is converted to Joules for calculation. The formula E = hf is applied, but the initial frequency calculation of 9.65e14 Hz is incorrect. Participants discuss the importance of understanding ionization energy and ensure proper unit conversion from eV to Joules. Clarifying the ionization process and energy levels is crucial for solving the problem accurately.
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Homework Statement



The following diagram represents the allowed electronic energy levels of a hypothetical atom. What frequency photon would be required to ionize this atom if it were already in the n = 2 state?

[PLAIN]http://img32.imageshack.us/img32/667/picture2vt.png


Homework Equations



E = hf

The Attempt at a Solution



Ionizing the atom would require emission of a photon. From the picure, E = 4eV for an emission of a photon:

4eV = hf
f= 9.65e14 Hz but this is not the answer. Any suggestions??
 
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You used the correct formula. Did you change eV to J? That is the only way I could see you getting it wrong.
 
yeah I did 4eV*1.6e-19 to convert it to Joules. Then I divided by Planck's constant to get the frequency. This problem seems so easy, but I'm missing something... :\
 
What does ionization mean? What is the energy of the electron when the atom is ionized?

ehild
 
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