What does the emission spectrum of the hydrogen atom reveal about its energy levels? c / λ.When the energy increases the wavelength decreases and vice versa. 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. Niels Bohr proposed a model of the atom that explained with startling accuracy, the appearance of the spectrum of hydrogen. From the frequency of the red light, its energy can be calculated. The energy of a {eq}n^{th} {/eq} level of a hydrogen spectrum is expressed as: It is because the energy levels are proportional to $\frac{1}{n^2}\\$, where n is a non-negative integer. This is the origin of the red line in the hydrogen spectrum. The Paschen series corresponds to the transition to the n 7 – Spectrum of the Hydrogen Atom The energy levels of hydrogen, which are shown in Fig. 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. 1.6, can be obtained by substituting the integer values n = 1,2,3,… into Eq. The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. The energy is expressed as a negative number because it takes that much energy to unbind (ionize) the electron from the nucleus. An energy level diagram shows the amounts of energy that electrons have at each level in an atom. The Lyman series corresponds to the transition to the n 1 energy level. (1.22).For the lowest level with n = 1, the energy is − 13.6 eV/1 2 = −13.6 eV. The energies are measured from a zero equivalent to a single free electron. An example would be singly ionized Helium, which is the lightest hydrogen-like atom, besides hydrogen. A hydrogen spectrum has infinite energy levels. Be sure to compare and contrast the terms energy, energy level, transition, and spectroscopic line. The second level, which corresponds to n = 2 has an energy equal to − 13.6 eV/2 2 = −3.4 eV, and so forth. The Balmer series corresponds to the transition to the n 2 energy level. In this model, energy levels, E n, 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. 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. Spectroscopy of the Hydrogen Atom Transitions between the energy states (levels) of individual atoms give rise to characteristic atomic spectra. 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