n oo n 6 n 5 n 4 n 3 Paschen (infrared) n 2 Balmer (visible) n 1 Lyman (ultraviolet) lonization

When a hydrogen atom absorbs a photon of electromagnetic radiation (EMR), the internal energy of the atom increases and one or more electrons may be energized into an excited state. The release of this extra energy as the excited state electron transitions back to a lower energy state results in the emission of a photon. These energy changes are responsible for the emission spectrum of hydrogen (shown below) and are described by the Bohr equation. delta?=−2.178×10−18 J(1?2final−1?2initial)ΔE=−2.178×10−18 J(1nfinal2−1ninitial2)

*refer to attached image before proceeding*

To ionize a hydrogen atom (forming a hydrogen ion), requires that the energy absorbed is sufficient to send the energized electron an infinite distance away from the nucleus (as shown by the ionization line in the image above). In other words, n_final is equal to infinity.

Calculate the energy required to ionize a ground state hydrogen atom. Report your answer in kilojoules.

delta E= ____kJ

What is the longest wavelength of electromagnetic radiation capable of ionizing a ground state hydrogen atom? Report your answer in nanometers.

? =  ______nm 

Calculate the energy required to ionize a hydrogen atom to an excited state where the electron is initially in the n = 5 energy level. Report your answer in kilojoules.

delta E= ____ kJ

What is the longest wavelength of electromagnetic radiation capable of ionizing this hydrogen atom in an excited state? Report your answer in nanometers.

? =  ______nm