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10 Nov 2019

Thisenergy diagram shows the allowed energy levels of an electron in acertain atom.

1)what is the energy of the electron in the ground state?zJ

2)whatis the energy of the electron in the first excited state ?zJ

3)Ifthe electron makes the transition shown by the red arrow from B toC, will a photon be absorbed or emitted ?

4)calculatethe wavelength of the photon that would be absorbed or emitted.Round your answer to 3 sig fig

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2) The average time the electron stays in the excited state before dropping back into the ground state is called its mean lifetime. The fact that the lifetime is not infinite introduces some uncertainty in the energy of the photon, and thus the wavelength. If the lifetime of the donor excited state in this problem is 3 ns, what is the uncertainty in the wavelength? (Hint: use the fact that E â Î»â1 and calculate âE/E. In other words, calculate the percent uncertainty in the energy to determine the wavelength uncertainty.) The fluorescent molecules can be used to determine how close the biomolecules are. To do this, the solution is illuminated by light that will promote the D1 â D2 transition. If the molecules are widely separated (as in Fig. 1a) the electron will decay back to D1 emitting a photon very close to the energy of the absorbed photon. However, if the molecules are close (Fig. 1b) the absorbed energy can transfer from the donor molecule to the acceptor (dotted line). For properly chosen donor and acceptor molecules, this transfer is much faster than the lifetime of the donor excited state. So, when the electron decays back to the ground state the emitted photon corresponds to the A2 â A1 transition. This means that color of the fluorescent light indicates whether the molecules are close together or far apart. This technique is called Fluorescence Resonance Energy Transfer (FRET).

The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3 state. Which of the following statements are true and which are false.

The wavelength of light emitted when the electron drops from n=3 to n=2 is longer than the wavelength of light emitted if the electron falls from n=3 to n=1.

The wavelength of the light emitted when the electron returns to the ground state from n=3 is the same as the wavelength of light absorbed to go from n=1 to n=3.

The electron is farther from the nucleus on average in the n=3 state than in the ground state.

It takes more energy to ionize the electron from n=3 than it does from the ground state.

The first excited state corresponds to n=2.

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