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. 7 – Spectrum of the Hydrogen Atom The diagram shows the energy levels in a hydrogen … 1.6, can be obtained by substituting the integer values n = 1,2,3,… into Eq. This is the origin of the red line in the hydrogen spectrum. Be sure to compare and contrast the terms energy, energy level, transition, and spectroscopic line. If an electron falls from the 3-level to the 2-level, red light is seen. 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. The Balmer series corresponds to the transition to the n 2 energy level. In this model, energy levels, E n, of hydrogen … Line spectrum are unique for each element, and for each isotope of that element. Niels Bohr proposed a model of the atom that explained with startling accuracy, the appearance of the spectrum of hydrogen. 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. An example would be singly ionized Helium, which is the lightest hydrogen-like atom, besides hydrogen. The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. 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. It is because the energy levels are proportional to $\frac{1}{n^2}\\$, where n is a non-negative integer. From the frequency of the red light, its energy can be calculated. Sample Problem Each energy level has a definite amount of energy. The second level, which corresponds to n = 2 has an energy equal to − 13.6 eV/2 2 = −3.4 eV, and so forth. A hydrogen spectrum has infinite energy levels. The Paschen series corresponds to the transition to the n We see that Bohr’s theory of the hydrogen atom answers the question as to why this previously known formula describes the hydrogen spectrum. The energy is expressed as a negative number because it takes that much energy to unbind (ionize) the electron from the nucleus. That energy must be exactly the same as the energy gap between the 3-level and the 2-level in the hydrogen atom. The energy of a {eq}n^{th} {/eq} level of a hydrogen spectrum is expressed as: 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. 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