A stream of laser photons with a frequency of 3.0 times 10^15 Hz excited electro

Question

A stream of laser photons with a frequency of 3.0 times 10^15 Hz excited electrons in the lowest energy of the hydrogen atom shown in the energy level diagram below. Show to what level the photon excited the electron. Show all the possible emission transitions as the electron returns from the n = 3 energy level to the ground state. Calculate Delta E for each line produced in b. What is the wavelength of the photon that would just ionize the ground-state atom to H^+? An energy of 1.09 times 10^3 kJ/mol is required to convert gaseous carbon atoms to gaseous C^+ ions and electrons. What is the maximum wavelength, in nm, of electromagnetic radiation with sufficient energy to cause ionization to a single carbon atom? In what region of the electromagnetic spectrum is this photon found?

Explanation / Answer

d)

1/ = Rh [(1/n1²) - (1/n2²)]

where Rh is Rydberg's Constant for hydrogen, and n1, n2 are the two energy states

This is Rydberg's Formula for hydrogen atom. To find the inonization energy of the hydrogen atom in ground state, we set n1 = 1, and n2 = , so that

= 1/Rh = 91.13 nm

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