How many energy levels does a hydrogen atom have in chemistry and physics?

Physics and chemistry are corresponding.

This problem requires a little bit of quantum mechanics.

knowledge, but you can remember it as some conclusions for now, and then talk about the specific deductions later.

Physically, Bohr.

The atomic model was an important model of the early days of quantum mechanics, the hydrogen atom.

Electrons outside the nucleus move on a series of steady-state energy levels, which are labeled by the principal quantum number n, and the value of n is all positive integers.

Chemically admiral n = 1, 2, 3 ......The corresponding energy level is called the "shell" and is ...... by the letters k, l, mMark. This one corresponds.

And the s you are talking about, the one is chemically called "s orbital", not "s level" (note that this is a lowercase letter, not an uppercase letter, and the uppercase letter indicates the shell). The quantum mechanical essence of the "orbital" is below the principal quantum number n, the angular quantum number.

l can be 0, 1, 2 ......n-1, (note that infinity cannot be taken at this point until n-1). For different values of l, s, p, d, f, g, h ...... are used in chemistryMark. Here, there is a special case, that is, for the case of n=1, l can only take 0, that is, there is only an s orbital, so it can be considered that the energy level of n=1 is the s orbital, but this is only a special case, and it is not true for all shells of n>1.

For example, there are s orbitals and p orbitals under the shell of n=2, s, p, and d orbitals under the shell of n=3, and s, p, d, and f orbitals under the shell of n=4 ......

Simplified in high school chemistry books.

To make the transition from the second to the first, the first thing to remember is that energy must be emitted in the form of photons. Then there is the relationship between energy conversion: the reduced potential energy of the system is converted into a part of the kinetic energy increased by electrons, and the other part is the photon energy just mentioned.

This is the energy level diagram of the hydrogen atom, note that the hydrogen atom transitions from the ground state of n=1 to the excited state of n=2,3,4 after the excitation of the hydrogen atom, which is the energy state of the whole atom, and when the excited state returns to the ground state from n=2, 3, 4, etc., there will be different energy releases, and different four spectral lines can be seen in the visible range.

And 1s, 2s, etc. are the laws of electron configuration outside the nucleus, 1 represents the arrangement of the closest layer of electrons to the nucleus, the first layer only has s orbitals, up to 2, 2s represents the s orbitals of the second layer of electrons, where s refers to suborbitals, there are a total of s, d, p, f four orbitals, respectively, up to 2, 6, 10, 14 electrons.

The photoelectric effect occurs when electrons escape from the metal. The energy energy released by the electrons in the hydrogen atom during the transition process is greater than the work of the metal, which can cause the photoelectric effect of the metal.

The wish is dead. I don't know much about this.

I can take it. In fact, it is the energy level, but the energy band is not exactly equal to the energy level. Let's talk about it slowly, little by little.

According to Rutherford.

A structural model in which an atom consists of a nucleus.

And the composition of extranuclear electrons, different extranuclear electrons (mainly divided according to energy) have their own orbitals, this is the energy level, here, everything is the same as what you learned in high school chemistry, s, p orbitals or something, you can check the book for details.

When two identical atoms are close to each other, such as two hydrogen atoms.

Theoretically, the energy of electrons of the same energy level is the same, and their orbits are exactly the same. For example, an electron on the S-level of hydrogen atom A can move to the S-level of hydrogen atom B, which is known as electron sharing motion.

However, there is also something to be done, and that is the Pauli principle of incompatibility.

The specific elaboration can be checked in the book, or it can be explained in detail, and this principle will not be explained in detail. When two identical hydrogen atoms are close to each other, there will be such a contradiction: the two electrons are exactly the same, so their motion state and orbital must be exactly the same, but this contradicts Pauli's incompatibility principle, so when the electron sharing motion occurs, the two identical electrons will have subtle differences, mainly in the different electron orbitals, one electron's orbit will be slightly higher or slightly lower than the other's electron orbital, and there will be two different energy levels, This is called level differentiation or level expansion.

But these two electrons are dead and dead at the S-level, and they will not transition in the absence of external conditions, so these two slightly different orbitals are simply called the S-level. At this time, the S energy level is not one orbit but two, and these two orbits together are energy bands, so at this time, a concept can be introduced: "S energy band", of course, there is no so-called "S energy belt", here is to facilitate the understanding of the introduction of a Dongdong.

In the same way, if the hydrogen atom is replaced by a silicon atom, several different energy levels will diverge, forming different energy bands. But in semiconductors we focus on the outermost band (or level, but not very accurate), because the change in electrons generally only occurs in the outermost layer!

If we zoom in a little bit from the electronic perspective to the atomic perspective, we will find that the outermost band is not necessarily full, while the subouter band is generally full, so the outermost band is called the conduction band.

Because the electrons here are relatively active! The energy bands of the subouter layer are called valence bands.

Because the electrons here don't usually change much!

Because there is actually a certain interval between the energy levels, when the energy levels form an energy band, this interval still exists, but the size changes slightly, but it has no effect. So it can be realized that there must also be a gap between the conduction band and the valence band, and this interval must have no electrons, analogous to the concept of the conduction band and the valence band, we call this interval the forbidden band (as the name suggests, prohibits the existence of electrons).

This is the thought process or evolutionary process of the energy band.

1. Energy level diagram of hydrogen atom.

2. Emission and absorption of photons.

Atoms are most stable when they are in the ground state, and when they are at a higher energy level, they will spontaneously transition to a lower energy level, and after one or several transitions to the ground state, they will release energy in the form of photons.

The atom has two energy levels, em and en(m>n).

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The frequency of the emitted photon at the transition is , and its magnitude can be determined by the following formula: h = em-en.

If an atom absorbs a photon of a certain frequency, the atom will jump from a lower energy level to a higher energy level after gaining energy.

When an atom is at the nth level, the different wavelength species n that may be observed are: .

The energy of the atom includes the kinetic energy and electric potential energy of the electron (the electric potential energy is shared by the electron and the original slag), that is: the energy of the atom en=ekn+epn. The lower the orbital, the greater the kinetic energy of the electron, but the less potential energy, the energy of the atom becomes less.

Kinetic energy of electrons: , the smaller r it is, the greater the ek.

The energy level of the hydrogen atom in the chemical medium is the energy value of the hydrogen atom in various states, which includes the electric potential energy of the hydrogen atom system and the kinetic energy of the electron moving in the orbit When the electron attacked by the hydrogen atom jumps from the outer orbit to the inner orbit, the atom will release photons, and the kinetic energy of the electron will increase.

The energy level of a hydrogen atom is the energy value of the hydrogen atom when it is in various fixed states, which includes the electric potential energy of the atomic system and the kinetic energy of the electrons moving in orbit.

Hydrogen atomic energy level 1Hydrogen atomic energy level. The energy value of each stationary state of a hydrogen atom is called its energy level. The energy levels of Bihong are divided and leaked, and the state with the lowest energy is called the other states called the hydrogen atomic energy level.

The probable state of the atom is intolerant and continuous, and the energy corresponding to each state is also discontinuous, and these energy values are called energy levels. The hydrogen atom energy sail stage is 5, and the corresponding energy from 1 to 5 is 13·6

The molecule is a compound, the atom is the nucleus and the electrons outside the nucleus, and its energy atomic energy is huge, such as nuclear fission, and the molecule is relatively stable. The internal motion of molecules includes electronic motion, molecular vibration and molecular rotation, and their energies are all quantized, so electronic energy levels, vibrational energy levels and rotational energy levels can be formed. Molecular energy level refers to the energy level structure formed by various motion states within the molecule.

The energy level structure formed by the collapse of the skin formed by various states of motion inside the molecule. The internal motion of molecules includes electronic motion, molecular vibration and molecular rotation, and their energies are all quantized, so electronic energy levels, vibrational energy levels and rotational energy levels can be formed.

The electronic energy level of a molecule is on the order of 10 electron volts (EV), which is about the same as that of an atom; The vibrational energy level of a molecule is about a multiple of the energy level of an electron, and the rotational energy level of a molecule is about m m times the energy level of an eggplant, where m is the mass of the electron and m is the mass of a typical molecule. Since the mass of a typical molecule is thousands to 10,000 times greater than the mass of an electron, the vibrational energy level of the molecule is electron volts (EV) and the rotational energy level is good, so the energy level of the molecule is more complex than that of the atom, which determines that the molecule has a much richer spectrum than the atom.

1. It is two different things, and the energy level of the electron can be independent of the temperature of the object in principle, and then turn over the photoelectric effect. However, the higher the temperature of the object, the higher the probability of the electrons being excited to a higher energy level (the reverse is not true), so heating is only used as a means of stimulating the electron energy level transition.

2. The so-called thermal expansion and contraction stove Tongqi often refers to condensed matter objects, their atoms are affected by the lattice concealment, usually the more intense the thermal movement, the stronger the tendency of the atoms to break free from the lattice, and the bond distance is slightly larger. Some also have special cases, such as the abnormal expansion of water at 0 4 degrees, which is the process from disorder to lattice formation, and the molecular spacing should be increased.

Since the hydrogen atom is a single-electron atom, its energy level is only related to the principal quantum number n: en=-(1 n 2)Although the hydrogen atom also has 2s, 2p; 3s, but the orbits of the same shell are all degenerate.

Since there is also an interaction between electrons and electrons in multi-electron atoms, the energy of each subshell in the same shell is different. After being excited, the electrons can jump to other orbitals at higher energy levels.