An example would be singly ionized Helium, which is the lightest hydrogen-like atom, besides hydrogen. In the hydrogen atom, with Z = 1, the energy of the emitted photon can be found using: E = (13.6 eV) [1/n f 2 - 1/n i 2] Atoms can also absorb photons. The Paschen series corresponds to the transition to the n Niels Bohr proposed a model of the atom that explained with startling accuracy, the appearance of the spectrum of hydrogen. These spectra can be used as analytical tools to assess composition of matter. 7 – Spectrum of the Hydrogen Atom In this model, energy levels, E n, of hydrogen … From the frequency of the red light, its energy can be calculated. The formula defining the energy levels of a Hydrogen atom are given by the equation: E = -E 0 /n 2, where E 0 = 13.6 eV (1 eV = 1.602×10-19 Joules) and n = 1,2,3… and so on. If an electron falls from the 3-level to the 2-level, red light is seen. The energies are measured from a zero equivalent to a single free electron. The Lyman series corresponds to the transition to the n 1 energy level. If a photon with an energy equal to the energy difference between two levels is incident on an atom, the photon can be absorbed, raising the electron up to the higher level. That energy must be exactly the same as the energy gap between the 3-level and the 2-level in the hydrogen atom. Spectroscopy of the Hydrogen Atom Transitions between the energy states (levels) of individual atoms give rise to characteristic atomic spectra. This is the origin of the red line in the hydrogen spectrum. It is because the energy levels are proportional to [latex]\frac{1}{n^2}\\[/latex], where n is a non-negative integer. (1.22).For the lowest level with n = 1, the energy is − 13.6 eV/1 2 = −13.6 eV. A hydrogen spectrum has infinite energy levels. The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. Each energy level has a definite amount of energy. An energy level diagram shows the amounts of energy that electrons have at each level in an atom. 1.6, can be obtained by substituting the integer values n = 1,2,3,… into Eq. Line spectrum are unique for each element, and for each isotope of that element. c / λ.When the energy increases the wavelength decreases and vice versa. The energy of a {eq}n^{th} {/eq} level of a hydrogen spectrum is expressed as: The energy is expressed as a negative number because it takes that much energy to unbind (ionize) the electron from the nucleus. Sample Problem We see that Bohr’s theory of the hydrogen atom answers the question as to why this previously known formula describes the hydrogen spectrum. Be sure to compare and contrast the terms energy, energy level, transition, and spectroscopic line. The Balmer series corresponds to the transition to the n 2 energy level. 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