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Bohr`s postulates

This small model illustrates discreteness of hydrogen atom spectrum. Quasi-classic approximation of this quantum effect (Bohr's atom model) was used for development of this model. An electron (yellow point) rotates around a proton (red point in box center).Certainly, electron orbit and depicted electron as a point are simulated (in reality, we should speak about electron cloud) but the model instead boasts higher clarity.

Selecting any switch in Orbit group may change electron orbit number. If electron passes to the orbit with smaller number, it emits photon. Otherwise light quantum collides with electron and transfers it to the orbit with higher sequential number.

Hydrogen spectrum is displayed in lower box. Spectral line corresponding to the last transition is slightly blinking. its length in nanometers is indicated to the right. Top right corner displays the diagram of hydrogen atom energy levels. Current level with electron is outlined by yellow. Arrow marks each transition from orbit to orbit is marked. Reset Button returns the model to the initial position.

Hydrogen lines are observed in spectrums of the majority of astronomic objects. These appear upon transition to first energy level. This is Liman series observed in ultraviolet. Separate lines of series are designated Lα (λ = 121,6 nm), Lβ (λ = 102,6 nm), Lγ (λ = 97,2 nm)), etc. Balmer series hydrogen lines are observed in visible region of spectrum. These comprise red Hα (λ = 656,3 nm), light blue Hβ (λ = 486,1 nm), blue Hγ (λ = 434,0 nm) and violet Hδ (λ = 410,2 nm) lines.

Hydrogen lines are also observed in infrared region of spectrum: Paschen series, Brackett series, and other more distant lines.

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