What are the 3 basic viewpoints of Bohr s quantum theory?

1. Under the action of Coulomb gravity of the nucleus, the electron moves along a circular orbit according to the laws of classical mechanics, and does not radiate electromagnetic waves outward, so the atom is in a stable state (stationary state), and its energy (called energy level) remains unchanged.

2. When an atom transitions from a stationary state at a higher energy level to a stationary state at a lower energy level, it emits photons, and vice versa, it absorbs photons.

3 Electrons can only move in some specific discrete orbitals.

However, Pol's success seems to have more luck in his work, and he uses the principles and formulas of macroscopic physics to deduce microscopic physical phenomena, which in fact are not applicable at the microscopic level. However, he was lucky that the hydrogen atom matched his reasoning, and his theory did not hold up with other atoms.

It is believed that the center of the atom is a very heavy positively charged nucleus, and there are some negatively charged electron movements outside the nucleus, and the main attraction between them is Coulomb. When an electron moves around the nucleus, the motion is stable only when certain conditions are met, and correspondingly, the desirable value of the energy of the electron can only be some specific discrete value, which is called the energy level. The energy of each energy level of an atom is negative, and its value is inversely proportional to the square of the principal quantum number n, and the 2n2 motion states of the same principal quantum number belong to the same energy level.

I don't know if it's these, it's best to verify the following before admitting it.

If you didn't answer last time, you see if these three theories are:

1. Propose the theory of composite nuclear model of atomic nuclear reactions.

2. Propose the droplet model theory of heavy atomic nucleus fission.

3. Propose a collective model theory of the structure of the atomic nucleus.

1. The Bohr-Sommerfeld quantization condition is that when the quantum number n, the quantized energy level will tend to the classical version of the continuous energy, and the quantization weight theory will tend to the classical theory.

2. The Sommerfeld number is often represented by Greek letters. The Sommerfeld number is the ratio of the velocity of the electron in the first Bohr orbit to the speed of light in a vacuum, and is calculated as =E2 (4 0C) (where e is the charge of the electron, 0 is the vacuum permittivity, is the reduced Planck constant, and c is the speed of light in a vacuum).

i.e. angular momentum quantization, l=mvr=nh(n=1,2,3...) h is the reduced Planck constant. This is the formula that Bohr postulated by which the possible orbitals of electrons can be deduced.

to stabilize orbital conditions.

2.Stable state of movement.

3.Bohr frequency conditions.

Reference material: Introduction to Physics, Chapter 1, Chapter 15, Third Edition, Xiong Zhaoxian Edition, I happened to review this part.

l=nh, h is the approximate Planck constant.

1. The Bohr-Sommerfeld quantization condition is that when the quantum number n, the quantized energy level will tend to be the continuous energy of the classical version, and the quantization weight theory will tend to the classical theory. 2. The Sommerfeld number is often represented by Greek letters. The Sommerfeld number is the ratio of the velocity of the electron in the first Bohr orbit to the speed of light in a vacuum, and is calculated as =E2 (4 0C) (where e is the charge of the electron, 0 is the vacuum permittivity, is the Planck constant, and c is the speed of light in a vacuum).

Bohr postulated that the orbits of electrons outside the nucleus of hydrogen are not continuous, but discrete, and that the electrons orbiting in orbit have a certain angular momentum (l=mvr, where m is the mass of the electron, v is the linear velocity of the electron, and r is the radius of the linear orbit of the electron), which can only be taken by the following formula:

where n=1,2,3,4,5,......This point is called the quantization condition, and it is a revolutionary assumption made by Bohr to come up with his model to explain the spectrum of hydrogen atoms. where n is called the quantum number (principal quantum number).

Hello dear, glad to answer for you. 1. The Bohr-Sommerfeld quantization condition is that when the quantum number n, the quantized energy level will tend to the classical version of the continuous energy, and the quantization weight theory will tend to the classical theory. 2. The Sommerfeld number is often represented by Greek letters.

The Sommerfeld number is the ratio of the velocity of the electron in the first Bohr orbit to the speed of light in a vacuum, and is calculated as =E2 (4 0C) (where e is the charge of the electron, 0 is the vacuum permittivity, is the reduced Planck nucleus, and c is the speed of light in a vacuum). Extended information: 1. Physics (Planck) discovered that the transfer of energy is not continuous, but is transmitted in energy units one by one, and this smallest energy unit is called the energy particle (referred to as quantum).

2. Einstein deduced from the photoelectric effect that light energy is not continuous, and the quantization of light is to think that light exists and propagates in the form of tiny units. It is called a quantum of light (photon for short). 3. The energy carried by a single photon is proportional to the frequency of light, and the proportionality coefficient is the Frank constant, and the total energy of n quanta is multiplied by n

In order to explain the Rutherford experiment, Bohr made a quantization hypothesis about the energy of the electron, the simplest of which is that the energy of the electron can only be some fixed value.

The quantization of the microscopic world was proposed by Max Carl Ernst Ludwig Planck and won the Nobel Prize.

Max Karl Ernst Ludwig Planck (April 23, 1858, October 4, 1947), born in Holstein, Germany, is a famous German physicist and one of the important founders of quantum mechanics.

Planck and Albert Einstein are two of the most important physicists of the 20th century. He made another important contribution to another leap forward in physics with the discovery of the quantization of energy, and was awarded the Nobel Prize in Physics in 1918.

In 1874, Planck entered the University of Munich to study mathematics and later physics. In 1877 he transferred to the University of Berlin, where he listened to Professors Helmholtz and Kirchhoff, and in 1879 he received his doctorate. From 1930 to 1937 he was president of the German Royal Wilhelm Society, which was later renamed the Max Planck Society in honor of Planck.

Since his Ph.D., Planck has been paying attention to and studying the second law of thermodynamics and has published many books. Since about 1894, he began to study the problem of black-body radiation, discovered Planck's law of radiation, and put forward the concept of energy subon and constant h (later called Planck's constant, which is also the standard definition of the kilogram in the International System of Units), which has become the most basic concept and extremely important universal constant in microscopic physics. On December 14, 1900, Planck presented this result at the German Physical Society, which became a great moment for the birth of quantum theory and the beginning of a new revolution in physics.

For this discovery, Planck was awarded the 1918 Nobel Prize in Physics.

Bohr Atomic Model:

1.Stationary assumption: Atoms can only be in a series of discontinuous energy states, in these states, although the electrons in the atom are in variable speed motion, they do not believe in radiating electromagnetic waves outward, so the relatively stable and smooth state is called steady branch rise.

The state with the lowest energy is called the ground state; Other states are called excited states.

2.Energy Level Assumption: Atomic orbitals are quantized. These quantized energy values are called energy levels.

The energy of the ground state is e1, and the energy in the n-order orbital is en=e1 n; The orbital radius of the ground state is r1, and the orbital radius of the n-order orbital is rn=n *r1

For hydrogen atom, e1=, r1=

3.Transition hypothesis: When an electron jumps from one stationary orbit to another, it radiates or absorbs photons of a certain frequency, and the energy is determined by the energy difference between these two stationary states, i.e., h = em-en

An atom emits only one photon in a single transition.

When e h or e h, it cannot be absorbed by atoms.