enow.com Web Search

Search results

  1. Results from the WOW.Com Content Network
  2. Atomic orbital - Wikipedia

    en.wikipedia.org/wiki/Atomic_orbital

    The number of electrons orbiting a nucleus can be only an integer. Electrons jump between orbitals like particles. For example, if one photon strikes the electrons, only one electron changes state as a result. Electrons retain particle-like properties such as: each wave state has the same electric charge as its electron particle.

  3. Molecular Hamiltonian - Wikipedia

    en.wikipedia.org/wiki/Molecular_Hamiltonian

    This empirical concept was given a theoretical basis by Paul Dirac when he introduced a relativistically correct (Lorentz covariant) form of the one-particle Schrödinger equation. The Dirac equation predicts that spin and spatial motion of a particle interact via spin–orbit coupling. In analogy spin-other-orbit coupling was introduced.

  4. Quantum number - Wikipedia

    en.wikipedia.org/wiki/Quantum_number

    An electron state has spin number s = ⁠ 1 / 2 ⁠, consequently m s will be + ⁠ 1 / 2 ⁠ ("spin up") or - ⁠ 1 / 2 ⁠ "spin down" states. Since electron are fermions they obey the Pauli exclusion principle: each electron state must have different quantum numbers. Therefore, every orbital will be occupied with at most two electrons, one ...

  5. List of equations in nuclear and particle physics - Wikipedia

    en.wikipedia.org/wiki/List_of_equations_in...

    Defining equation SI units Dimension Number of atoms N = Number of atoms remaining at time t. N 0 = Initial number of atoms at time t = 0 N D = Number of atoms decayed at time t = + dimensionless dimensionless Decay rate, activity of a radioisotope: A = Bq = Hz = s −1 [T] −1: Decay constant: λ

  6. Electron configuration - Wikipedia

    en.wikipedia.org/wiki/Electron_configuration

    This gives two electrons in an s subshell, six electrons in a p subshell, ten electrons in a d subshell and fourteen electrons in an f subshell. The numbers of electrons that can occupy each shell and each subshell arise from the equations of quantum mechanics, [ a ] in particular the Pauli exclusion principle , which states that no two ...

  7. Spin quantum number - Wikipedia

    en.wikipedia.org/wiki/Spin_quantum_number

    During the period between 1916 and 1925, much progress was being made concerning the arrangement of electrons in the periodic table.In order to explain the Zeeman effect in the Bohr atom, Sommerfeld proposed that electrons would be based on three 'quantum numbers', n, k, and m, that described the size of the orbit, the shape of the orbit, and the direction in which the orbit was pointing. [10]

  8. Plum pudding model - Wikipedia

    en.wikipedia.org/wiki/Plum_pudding_model

    The number of electrons depends upon the density of electrons along the particle path times the path length L. The net deflection caused by all the electrons within this arbitrary cylinder of effect around the beta particle's path is = where N 0 is the number of electrons per unit volume and is the volume of this cylinder.

  9. Bohr model - Wikipedia

    en.wikipedia.org/wiki/Bohr_model

    The Bohr model of the hydrogen atom (Z = 1) or a hydrogen-like ion (Z > 1), where the negatively charged electron confined to an atomic shell encircles a small, positively charged atomic nucleus and where an electron jumps between orbits, is accompanied by an emitted or absorbed amount of electromagnetic energy (hν). [1]