Can anyone talk about the successes and failures of the Bohr model of the hydrogen atom?

The Bohr model of the hydrogen atom has been successful in introducing the quantization view of the discontinuity of the energy of the hydrogen atom and the discontinuity of the electron orbital.

The unsuccessful part is that too much of the classical theory Newton's laws of motion are retained.

Circular motion, orbit.

Note: Actually, the electrons in the hydrogen atom have no orbitals, only electron clouds.

There are no orbitals for electrons, whereas Bohr defined the place where the probability of electrons appearing is higher as "orbitals".

The two concepts of quantum mechanics contained in the Bohr atomic model are:

1. Orbital discontinuity is introduced.

2. Energy discontinuity.

Bohr's theory is based on two basic assumptions: (l) that electrons cannot move in an atom along all the orbits of the energy that the classical theory allows for continuous variation, but only along a special set of orbits. The orbit of an electron is stable only if the moment of momentum of the electron's motion is equal to an integer multiple of H2 (h is Planck's constant).

It was the era of the invasion of China by the Eight-Nation Alliance, and in that year Planck proposed quantum theory;

Albert Einstein, a descendant of Jews, won the Nobel Prize for proposing an explanation for the photoelectric effect based on quantum theory;

Bohr, another descendant of Jews, who proposed a model of the hydrogen atom based on quantum theory, also won the Nobel Prize.

At the heart of Bohr's thought was the application of quantum theory to the moment of momentum, which could be derived using simple mathematics.

With Rydberg's empirical formula and the Bohr radius of the hydrogen atom, the various line systems of the hydrogen spectrum can be easily solved.

Bohr's theory, in explaining the hydrogen spectrum, has achieved great success;

But it has only been successful in the hydrogen spectrum, and if it is applied to other spectrums, it is still very unsatisfactory;

Even when it came to interpreting the hydrogen spectrum, it was not a complete success. It does not explain why electron acceleration does not radiate.

So far, it has been difficult to justify.

When we study atomic physics, we are only learning about it with the mentality of watching the excitement, and we are not eager to try it.

Impulsive, without the spirit of not waiting for me, and even once someone questions the ** theory, our teachers and professors are not greatly appreciated, but drunk.

If you don't believe it, the landlord can teach it in front of these middle school teachers and university teachers who rely on people's fat and ointment.

face, when openly questioning, see how angry they will be?

Especially when they introduce a certain theory of reality, you ask after class:

Teacher, what you just said is completely contradictory, haven't you discovered it yourself?

Look at their reactions, there are thousands of questions about this.

Here's the line of thought of Bohr's theory:

For the first time, Bohr's atomic theory introduced the quantum concept into the atomic realm, put forward the concept of stationary state and transition, and successfully explained the experimental laws of the spectrum of hydrogen atoms. But for slightly more complex atoms such as helium, Bohr's theory cannot explain its spectral phenomena. This shows that Bohr's theory has not yet fully revealed the laws of microscopic particle motion.

Its disadvantage is that it retains the concept of classical particles, and still regards the motion of electrons as the orbital motion described by classical mechanics.

Actually, there is no definite value for the coordinates of the electrons in the atom. Therefore, we can only say what is the probability of an electron appearing in a unit volume near a certain point at a certain time, and we cannot regard the motion of an electron as the orbital motion of a particle with definite coordinates. (Uncertainty Principle).

When atoms are in different states, the probability of electrons appearing everywhere is not the same. If you use different points to represent the probability of electrons appearing at various locations, you can draw a diagram like a cloud, and you can call it an electron cloud

Boer's theory applies only to hydrogen atoms and not to other atoms.

When an electron jumps from the outer orbital to the inner orbital, it emits photons. The electric field force does positive work, and the electric potential energy decreases. The inner orbital radius is smaller and the centripetal force is larger, so the electron velocity increases and the kinetic energy increases. So B right.

Electrons jump from the inner orbital to the outer orbital, absorbing photons. The electric field force does negative work, and the electric potential energy increases. The outer radius is larger and the centripetal force is less, so the kinetic energy decreases. D false. Pick B

Bohr. The first theory to apply quantum concepts to atomic phenomena. 1911 eRutherford.

The nuclear model is proposed, which is a sharp contradiction with classical physical theory, and the atom will constantly radiate energy and cannot exist stably; Atoms emit a continuum, staring instead of actually discrete spectral lines. Bohr looked at the stability of the atom and absorbed mPlanck.

a.Einstein.

In 1913, considering the circular orbital motion of electrons in hydrogen atoms, Bohr's theory of atomic structure was proposed. The three basic assumptions of the theory are that atoms can only be in a series of discontinuous states of energy, in which the atoms are stable, and these states are called stationary states.

The different energy states of the atoms correspond to the movement of the electrons around the nucleus along different circular orbits, the stationary state of the atoms is discontinuous, so the distribution of the possible orbitals of the electrons is also discontinuous, and the motion of the electrons in these possible orbits is a vibration in the form of standing waves. The transition of an atomic system from one stationary state to another is accompanied by the emission and absorption of quanta of optical radiation. The energy of the radiated or absorbed photon is determined by the energy difference between these two stationary states, i.e., h = |e-, the electron moves around the nucleus, and its orbital radius is not arbitrary, only the angular momentum of the electron in the orbit.

It is possible to scatter and grind the orbital only if the following conditions are satisfied: mvr=nh (2) n=1,2,3....) where n is a positive integer.

It is called quantum number. <>

The "easy to understand" here refers to high school students who have already mastered some classical mechanics. Or for students who don't need to study the basic theories of quantum mechanics in detail but want to use the relevant conclusions (such as chemistry students who use atomic sail preparation spectroscopy for elemental analysis), it is enough to use the basic spirit of Bohr's model (rather than the model itself).

In addition, my personal opinion is that Bohr's atomic theory does not use the condition that "electrons are wave", Bohr only assumes that "electrons other than hydrogen atoms can only move in a series of discrete orbits with fixed energy values", and as for why this assumption is made, it can only be "because it can conform to the emission spectrum of hydrogen atoms". Of course, in order to explain why this hypothesis was made, the concept of de Broglie wave had to be introduced, but that was not the result of Bohr himself. (See Does God Roll the Dice:.)

A History of Quantum Physics).

Starting from the fact that the atomic emission spectrum of the hydrogen atom is actually separate, as long as the assumption that the electrons outside the hydrogen atom can only move in a series of discrete orbits with fixed energy values, the rest can be completely solved by classical mechanics, and the emission spectrum of the hydrogen atom can be perfectly explained. For senior high school students who have been able to use the kinetic energy theorem and centripetal force formula, under the guidance of teachers, they can achieve a considerable degree of understanding of this model, which can be used as a springboard for learning quantum mechanics in the future. <>