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  2. Balmer series - Wikipedia

    en.wikipedia.org/wiki/Balmer_series

    The Balmer series is calculated using the Balmer formula, an empirical equation discovered by Johann Balmer in 1885. The visible spectrum of light from hydrogen displays four wavelengths , 410 nm , 434 nm, 486 nm, and 656 nm, that correspond to emissions of photons by electrons in excited states transitioning to the quantum level described by ...

  3. Emission spectrum - Wikipedia

    en.wikipedia.org/wiki/Emission_spectrum

    The fact that only certain colors appear in an element's atomic emission spectrum means that only certain frequencies of light are emitted. Each of these frequencies are related to energy by the formula: E photon = h ν , {\displaystyle E_{\text{photon}}=h\nu ,} where E photon {\displaystyle E_{\text{photon}}} is the energy of the photon, ν ...

  4. Hydrogen spectral series - Wikipedia

    en.wikipedia.org/wiki/Hydrogen_spectral_series

    The four visible hydrogen emission spectrum lines in the Balmer series. H-alpha is the red line at the right. The Balmer series includes the lines due to transitions from an outer orbit n > 2 to the orbit n' = 2. Named after Johann Balmer, who discovered the Balmer formula, an empirical equation to predict

  5. Electromagnetic radiation - Wikipedia

    en.wikipedia.org/wiki/Electromagnetic_radiation

    Together, wave and particle effects fully explain the emission and absorption spectra of EM radiation. The matter-composition of the medium through which the light travels determines the nature of the absorption and emission spectrum. These bands correspond to the allowed energy levels in the atoms.

  6. Photon energy - Wikipedia

    en.wikipedia.org/wiki/Photon_energy

    This equation is known as the Planck relation. Additionally, using equation f = c/λ, = where E is the photon's energy; λ is the photon's wavelength; c is the speed of light in vacuum; h is the Planck constant; The photon energy at 1 Hz is equal to 6.626 070 15 × 10 −34 J, which is equal to 4.135 667 697 × 10 −15 eV.

  7. Planck's law - Wikipedia

    en.wikipedia.org/wiki/Planck's_law

    The equation of radiative transfer states that for a beam of light going through a small distance ds, energy is conserved: The change in the (spectral) radiance of that beam (I ν) is equal to the amount removed by the material medium plus the amount gained from the material medium. If the radiation field is in equilibrium with the material ...

  8. Einstein coefficients - Wikipedia

    en.wikipedia.org/wiki/Einstein_coefficients

    An emission line is formed when an atom or molecule makes a transition from a particular discrete energy level E 2 of an atom, to a lower energy level E 1, emitting a photon of a particular energy and wavelength. A spectrum of many such photons will show an emission spike at the wavelength associated with these photons.

  9. Spontaneous emission - Wikipedia

    en.wikipedia.org/wiki/Spontaneous_emission

    The rate of spontaneous emission (i.e., the radiative rate) can be described by Fermi's golden rule. [17] The rate of emission depends on two factors: an 'atomic part', which describes the internal structure of the light source and a 'field part', which describes the density of electromagnetic modes of the environment.