(1) Rutherford, the analytical model of classical electromagnetic theory, is based on classical electromagnetic theory, and charged with electromagnetic radiation to accelerate its movement, so the energy is decreasing, so the orbital radius is decreasing, and finally it falls into the nucleus, which is still an unstable atom; According to the classical electromagnetic theory, the electrons of electromagnetic radiation frequency around the nucleus should be equal to those around the nucleus, the electron orbit has a reduced frequency range, and the atomic spectrum should be continuous, but this is not the case in the experiment, and the line spectrum is contradictory.

(2) Bohr's atomic theory:

(1) only in a series of discrete atomic energy states, the atoms in these states are stable. Although this accelerates the movement of electrons, it does not radiate electromagnetic waves.

② An atom transitions from a given state (energy E2) to another stable state (energy E 1). When it absorbs a photon radiation or photons of certain frequencies, the energy Hυ= E2-E 1 is determined by two energy differences.

(3) Moment motion of momentum nuclei around electrons is quantized, and the orbital radius is equal to integer multiple h/2π, that is, the momentum of the product of millivolts R = N, where n is the quantum number. This phenomenon is called quantized orbit.

Calculated by the above theory and classical electromagnetic theory.

Hydrogen energy can be used to calculate the orbital radius and time (including kinetic energy and potential energy) radius RN = N2R 1, energy, where n = 1, 2,3. .......

Under normal circumstances, starting from the lowest energy atom closest to the core orbit, the ground state is called a stable state. When an object is heated or irradiated, some atoms will absorb energy and change from the above-ground state to a higher energy level, so the electrons are far away from the core. These states are called excited states.

Energy h nu = E2-e1,excited state → ground state → excited state absorbs radiation energy h nu = E2-e1.

(3) The success and limitation of Bohr's theory: According to the obtained energy levels of hydrogen atoms and hydrogen atoms, the successful formula of Bohr's theoretical calculation and experimental observation of bright-line spectra is very close to the first Bohr's point of view, that is, classical physical concepts and laws cannot be completely applied to atoms, and the system provides unique concepts and limitations of microscopic quantum, which is more complicated than the explanation of some very difficult spectra in hydrogen atoms, because there is no concept of completely separated classical physical effects.