A hydrogen spectrum has infinite energy levels. 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. An energy level diagram shows the amounts of energy that electrons have at each level in an atom. 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. It is because the energy levels are proportional to $\frac{1}{n^2}\\$, where n is a non-negative integer. The energy levels of hydrogen, which are shown in Fig. The diagram shows the energy levels in a hydrogen … The three groups of lines in the hydrogen spectrum correspond to the transition of electrons from higher energy levels to lower energy levels. The Lyman series corresponds to the transition to the n 1 energy level. That energy must be exactly the same as the energy gap between the 3-level and the 2-level in the hydrogen atom. Niels Bohr proposed a model of the atom that explained with startling accuracy, the appearance of the spectrum of hydrogen. Be sure to compare and contrast the terms energy, energy level, transition, and spectroscopic line. c / λ.When the energy increases the wavelength decreases and vice versa. 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 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 The Paschen series corresponds to the transition to the n Sample Problem The energy is expressed as a negative number because it takes that much energy to unbind (ionize) the electron from the nucleus. From the frequency of the red light, its energy can be calculated. 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. Line spectrum are unique for each element, and for each isotope of that element. Spectroscopy of the Hydrogen Atom Transitions between the energy states (levels) of individual atoms give rise to characteristic atomic spectra. The Balmer series corresponds to the transition to the n 2 energy level. If an electron falls from the 3-level to the 2-level, red light is seen. The second level, which corresponds to n = 2 has an energy equal to − 13.6 eV/2 2 = −3.4 eV, and so forth. These spectra can be used as analytical tools to assess composition of matter. 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. 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