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

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Homework Help Overview

The problem involves determining the frequency of a photon required to ionize a hypothetical atom from its n=2 electronic state, based on a provided energy level diagram.

Discussion Character

  • Exploratory, Assumption checking

Approaches and Questions Raised

  • Participants discuss the application of the formula E = hf and the conversion of energy units from eV to Joules. There is uncertainty regarding the correct energy value needed for ionization and the implications of the ionization process itself.

Discussion Status

Some participants have provided guidance on unit conversion and have raised questions about the definition of ionization and the energy state of the electron post-ionization. Multiple interpretations of the problem are being explored.

Contextual Notes

There is a lack of clarity regarding the energy level diagram and the specific energy required for ionization from the n=2 state, which is central to the discussion.

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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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