Find the maximum wavelength of the photon that a hydrogen atom in its ground state must absorb in order for the ionization to occur.

Solution Preview

Maximum wavelength means minimum frequency (or minimum energy).

The ionization potential of hydrogen atom is 13.6 eV. That is you must give 13.6 eV to an electron in this atom so that it can come out leaving the atom ionized.

Thus the minimum energy that our photon must have is 13.6eV right ?

We will convert ...

Solution Summary

Answer with all mathematical steps and explanations.

A 0.1mol/L aqueous solution of weak monoprotic acid (contains one ionizable hydrogenatom) has a hydrogen ion concentration of 0.001mol/L. The value of the ionization, Ka, for this acid is:
a) 10^-5 (10 to the power of -5)
b) 10^-2 (10 to the power of -2)

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An electron has a de Broglie wavelenght equal to the diameter of the Hydrogenatom.
What is the kinetic energy of the electron?
How does this energy compare to the ground state of the hydrogenatom?

A Hydrogenatom and a Helium atom each with 4 eV of KE approach a thin barrier 6 MeV high which has the greater probability of tunneling through the barrier? Explain.

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a. n = 3 -> n = 6
b. n = 6 -> n = 3
c. n = 1 ->n = 4
d. n = 6 ->n = 1
e. n = 1 ->n = 6
2) The frequency of elect

Which of the following statements are true about the hydrogenatom's energy levels? Support your answers with explanation.
1. 13.6 eV is enough energy to ionize Hydrogen, which means exciting an electron from n = 1 up to zero energy.
2. The wavelength of a photon emitted from the n=3 to n=2 transition is longer than that emi