Question

Successive ionization energies are not represented in the experimental photoelectron spectra. It’s important to realize that PES simply shows the energies required to photoionize ONE electron from a neutral atom. In the case of the nitrogen PES spectrum you examined in section, the one electron photoionized can be from the 1s, 2s or 2p subshell in its ground state.

In contrast, successive ionization energies correspond to the removal of more than one electron from a given atom. These electrons are removed in a precise sequence, starting with the outermost electrons first, followed by the next outermost, and so on.

What is the total amount of energy needed (in unit of J) to ionize one electron from the outermost subshell of 1 million atoms of X in a photoelectron spectroscopy experiment?

An X-ray photon with wavelength of 5.50 nm is used to ionize a 2s electron from “X” (see Figure 2). Calculate the kinetic energy (in units of MJ/mol) of the photoelectrons.

208 18.7 13.5 1.951.01 IE (MJ/mol) Figure 2. PES spectrum for "X"

Answer 1

ionization energy is defined as the energy required to remove one electron from outermost shell of an atom. here we have to find the ionization energy of nitrogen atom in nitrogen with 7 electrons, ionization energy is calculated by subtracting 1 fron atomic number then square the answer and multiply with 13.6

The frequency of a wave is equal to its speed divided by its wavelength. For light, the speed is 3 x 10^8 meters per second.speed divided by wavelength will gives frequency. we know that Energy =plancks constant multiplied with frequency.so (3 * 10^8 / 5.50*10^-9)*.022*10^-34 gives 3.2847*10^-17