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  2. Bohr model - Wikipedia

    en.wikipedia.org/wiki/Bohr_model

    In Bohr's theory describing the energies of transitions or quantum jumps between orbital energy levels is able to explain these formula. For the hydrogen atom Bohr starts with his derived formula for the energy released as a free electron moves into a stable circular orbit indexed by : [28] = The energy difference between two such levels is ...

  3. Bohr radius - Wikipedia

    en.wikipedia.org/wiki/Bohr_radius

    The Bohr radius is one of a trio of related units of length, the other two being the Compton wavelength of the electron and the classical electron radius (). Any one of these constants can be written in terms of any of the others using the fine-structure constant α {\displaystyle \alpha } :

  4. Bohr–Sommerfeld model - Wikipedia

    en.wikipedia.org/wiki/Bohr–Sommerfeld_model

    The theory would have correctly explained the Zeeman effect, except for the issue of electron spin. Sommerfeld's model was much closer to the modern quantum mechanical picture than Bohr's. In the 1950s Joseph Keller updated Bohr–Sommerfeld quantization using Einstein's interpretation of 1917, [6] now known as Einstein–Brillouin–Keller method.

  5. Atomic orbital - Wikipedia

    en.wikipedia.org/wiki/Atomic_orbital

    With de Broglie's suggestion of the existence of electron matter waves in 1924, and for a short time before the full 1926 Schrödinger equation treatment of hydrogen-like atoms, a Bohr electron "wavelength" could be seen to be a function of its momentum; so a Bohr orbiting electron was seen to orbit in a circle at a multiple of its half ...

  6. Quantum dot - Wikipedia

    en.wikipedia.org/wiki/Quantum_dot

    where μ is the reduced mass, a is the radius of the quantum dot, m e is the free electron mass, m h is the hole mass, and ε r is the size-dependent dielectric constant. Although the above equations were derived using simplifying assumptions, they imply that the electronic transitions of the quantum dots will depend on their size.

  7. Rydberg formula - Wikipedia

    en.wikipedia.org/wiki/Rydberg_formula

    In Bohr's conception of the atom, the integer Rydberg (and Balmer) n numbers represent electron orbitals at different integral distances from the atom. A frequency (or spectral energy) emitted in a transition from n 1 to n 2 therefore represents the photon energy emitted or absorbed when an electron makes a jump from orbital 1 to orbital 2.

  8. Rydberg constant - Wikipedia

    en.wikipedia.org/wiki/Rydberg_constant

    The last expression in the first equation shows that the wavelength of light needed to ionize a hydrogen atom is 4π/α times the Bohr radius of the atom. The second equation is relevant because its value is the coefficient for the energy of the atomic orbitals of a hydrogen atom: E n = − h c R ∞ / n 2 {\displaystyle E_{n}=-hcR_{\infty }/n ...

  9. Quantum jump - Wikipedia

    en.wikipedia.org/wiki/Quantum_jump

    A quantum jump is the abrupt transition of a quantum system (atom, molecule, atomic nucleus) from one quantum state to another, from one energy level to another. When the system absorbs energy, there is a transition to a higher energy level (); when the system loses energy, there is a transition to a lower energy level.