The energy levels of hydrogen, which are shown in Fig. The Lyman series corresponds to the transition to the n 1 energy level. If an electron falls from the 3-level to the 2-level, red light is seen. Be sure to compare and contrast the terms energy, energy level, transition, and spectroscopic line. We see that Bohr’s theory of the hydrogen atom answers the question as to why this previously known formula describes the hydrogen spectrum. An energy level diagram shows the amounts of energy that electrons have at each level in an atom. The emission spectrum of hydrogen Energy levels of the hydrogen atom: De-excitation of electron results in emission of photon-13.6 eV 0.0 eV E PHYS 1493/1494/2699: Exp. Each energy level has a definite amount of energy. The energy of a {eq}n^{th} {/eq} level of a hydrogen spectrum is expressed as: This is the origin of the red line in the hydrogen spectrum. 7 – Spectrum of the Hydrogen Atom A hydrogen spectrum has infinite energy levels. Sample Problem 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. c / λ.When the energy increases the wavelength decreases and vice versa. The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. An example would be singly ionized Helium, which is the lightest hydrogen-like atom, besides hydrogen. The energies are measured from a zero equivalent to a single free electron. 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. Niels Bohr proposed a model of the atom that explained with startling accuracy, the appearance of the spectrum of hydrogen. It is because the energy levels are proportional to $\frac{1}{n^2}\\$, where n is a non-negative integer. In this model, energy levels, E n, of hydrogen … The diagram shows the energy levels in a hydrogen … The second level, which corresponds to n = 2 has an energy equal to − 13.6 eV/2 2 = −3.4 eV, and so forth. What does the emission spectrum of the hydrogen atom reveal about its energy levels? (1.22).For the lowest level with n = 1, the energy is − 13.6 eV/1 2 = −13.6 eV. The Paschen series corresponds to the transition to the n The Balmer series corresponds to the transition to the n 2 energy level. Line spectrum are unique for each element, and for each isotope of that element. 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. 1.6, can be obtained by substituting the integer values n = 1,2,3,… into Eq. 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