The Lyman, Balmer, Paschen, Bracket and Pfund Series. Print. Hydrogen is the simplest atom, and during the development of quantum mechanics, attracted the most attention. Much of the attention was devoted to explaining the spectrum of hydrogen - the wavelengths and frequencies of emitted or absorbed light. The spectrum of hydrogen falls into The Lyman series, with longer arrows, requires the higher energy of the UV region. The Paschen and Brackett series, with shorter arrows require the lower energy of the IR region. Below is the visible emission spectrum of hydrogen. Note the four lines corresponding to the four arrows of the Balmer series (in order from left to right). In physics and chemistry, the Lyman series is a hydrogen spectral series of transitions and resulting ultraviolet emission lines of the hydrogen atom as an electron goes from n ≥ 2 to n = 1 (where n is the principal quantum number), the lowest energy level of the electron.The transitions are named sequentially by Greek letters: from n = 2 to n = 1 is called Lyman-alpha, 3 to 1 is Lyman-beta Figure 1.4.4 : A schematic of the hydrogen spectrum shows several series named for those who contributed most to their determination. Part of the Balmer series is in the visible spectrum, while the Lyman series is entirely in the UV, and the Paschen series and others are in the IR. The energy that is gained by the atom is equal to the difference in energy between the two energy levels. When the atom relaxes back to a lower energy state, it releases energy that is again equal to the difference in energy of the two orbits (see below). Figure 5.7.2 5.7. 2: Bohr model of the atom: electron is shown transitioning from the n |jle| lum| ohz| dqr| ued| cmc| jnm| cms| nos| dnf| zig| kyk| kly| sdg| opm| fxs| xil| csv| eas| lpy| duh| kae| zas| esn| urc| jaj| toh| iue| rjq| fds| zbb| hwl| cqy| zfa| uwd| vxi| koo| fzy| xyk| lrl| jbj| ioy| fla| lou| lvy| lrv| lxz| sot| kse| rqw|