Is ionization a transition? How does the electronic transition happen?

In layman's terms, electrons leave the particle after ionization occurs, while the electron jumps from one atomic orbital to another during the transition without breaking away from the particle.

Ionization is the process in which an uncharged particle becomes an electrically charged particle under the action of a high-voltage electric arc or high-energy rays. This is the case, for example, with particles in the ionosphere in the Earth's atmosphere. Particles in the ionosphere are ionized into charged particles by the action of high-energy rays in the universe.

Physical ionization takes the form of high temperature, electric field, and high-energy radiation.

The transition is when the particle obtains an excitation energy equivalent to the difference between two energy levels due to heating, collision or radiation, etc., it will jump from the initial state with lower energy to the excited state with higher energy, but it is unstable and has a tendency to spontaneously return to the steady state. After releasing the corresponding energy, the particle automatically returns to its original state, and these behaviors are called transitions, which obey strict quantum rules.

It does not belong to ionization after ionization takes place when electrons leave the particle, whereas transitioning when the electrons jump from one atomic orbital to another without detaching from the particle.

The relationship between the two is that they are both caused by energy, to different degrees, and the energy absorbed by the transition is quantized, that is, only a certain energy value can be absorbed, and ionization only needs to be greater than its work of escape.

It doesn't belong. The definition of transition is the transition of an electron from one atomic orbital (AO) to another, such as the D-D transition, etc.

Ionization has nothing to do with this.

<> differences: 1. Transition refers to the change in the energy level of electrons when energy is absorbed or released, when electrons move from one orbital of an atom to another, resulting in the electron layer where electrons outside the nucleus are located.

Different; Ionization is when an electron is separated from the nucleus.

of the Bondage Eye;

2. The energy released or absorbed by the transition must be the energy level difference; Ionization must be greater than maximum energy;

3. The transition is large, the energy level is high to a certain extent, and the tremor can be separated from the control of the atom before it is called, which leads to the ionization of electrons, that is, ionization is a special case of the transition.

For example, there is only one electron outside the nucleus of h atom, and this electron should be in the 1s orbital, and if it is excited and jumps to the 2s orbital, then it is in the excited state.

Energy level: The energy of electrons in the same energy layer may also be different, and it is divided into different energy levels, usually expressed by s, p, d, f, etc., in the same energy layer, the energy of each energy level increases in the order of s, p, d, f, that is: e(s) electron transition:

Ground state excited state.

When the electrons of the ground state atom absorb energy, they will jump from a lower energy level to a higher energy level and become an excited atom.

The excited state is the ground state.

Energy is released when the electrons of an excited atom jump from a higher energy level to a lower energy level.

Atomic ionization and transition are two different processes that occur in the energy level structure of an atom.

First of all, atomic ionization refers to the process by which an atom loses or gains an electron to become a charged ion. When an atom absorbs more energy than the ionization energy of its bound electrons, one or more of its electrons are removed from the atomic orbital and become free electrons, resulting in the formation of a positively charged (positive ion) or negatively charged (negative ion) atom. Ionization can be initiated by a variety of means, such as electron absorption, particle radiation, high temperature, etc.

Whereas, atomic transition refers to the process of electrons inside an atom jumping from one energy level to another. Atoms complete the transition between energy levels by absorbing or emitting electromagnetic radiation. When an atom absorbs external energy, the electrons absorb energy from a lower energy level and jump to a higher energy level.

And when the stimulated electrons return to a lower energy level, energy is released, usually in the form of light. Sensitivity, or this is what we usually call spectral phenomena, such as luminescence, absorption, etc.

The difference between atomic ionization and transition is the change in the energy level of electrons. Ionization refers to the electron leaving the atom to form a charged ion, that is, changing the overall charged state of the atom; The transition, on the other hand, is the mutual conversion between the electron energy levels inside the atom, which does not change the charge state of the atom, but only changes the energy and orbit of the electron.

Both processes have important applications in fields such as physics, chemistry, and astronomy. By studying atomic ionization and transitions, we can gain insight into the energy level structure, energy transfer, and radiation properties of atoms, which have led to the development of many scientific and technological fields. <>

Electron transfer (ET) refers to the movement of electrons between two atoms or other chemical substances (such as molecules, etc.). Electron transfer is a redox reaction that changes the oxidation state of two reactants.

Electron transfer is the most basic chemical behavior in a homogeneous system. It is ubiquitous in life processes such as redox reactions, nucleophilic substitution reactions of free radicals, photosynthesis, and respiration. There are two mechanisms of electron transfer reaction: outer and inner electron transfer.

In the outer mechanism, the coordination layer of metal ions does not move, and there is no cleavage and formation of chemical bonds between metal and ligands, and only simple electronic transitions occur. In the inner shell mechanism, there is a bridge of ligands (Cl, Oh, Oh2, NH3, etc.) that link the two metal ions and provide continuous covering orbitals for electron transfer. In organic chemistry, the outer and inner electron transfer are represented by nonbonding and bonding, respectively.

An electron transition is essentially a change in the energy of an electron in a particle (atom, ion, or molecule) that makes up a substance. According to the principle of conservation of energy, the outer electrons of a particle absorb energy during the transfer from a lower energy level to a higher energy level; Moving from a higher energy level to a lower energy level releases energy. Energy is the absolute value of the difference between the energies of two energy levels.

According to the molecular orbital theory, there are three types of valence electrons in organic compound molecules that are associated with the UV-Vis absorption spectrum: electrons that form single bonds, electrons that form double bonds, and lone pairs that are not bonded in the molecule, called n electrons, also known as p electrons. When an organic compound absorbs ultraviolet or visible light, the valence electrons in the molecule will transition to the excited state, and there are four main types of transitions, that is, n * n * The energy required for each transition is:

n→σ*n→π*

Please click on the graph to enter the graph for the relative magnitude of potential energy between electron levels.

Electron transition refers to the energy absorbed by the outer electrons of the atom beyond the energy level of the orbit in which it is located, and jumps to an orbit farther away from the nucleus, but such electrons are unstable and easy to release energy and return to the original orbit.

Atomic transitions and ionization are two different concepts. Atomic transitions are when one electron in an atom jumps from one energy level to another, and this transition can be caused by light or other electromagnetic radiation. Ionization, on the other hand, is when an atom or molecule loses or gains one or more electrons and thus becomes a charged ion.

The difference between atomic transitions and ionization is that they differ in their physical processes and outcomes. An atomic transition is a process in which an atom emits or absorbs photons, thus changing its energy state. Whereas, ionization is a process by which an atom or molecule loses or gains one or more electrons, through which the atom or molecule becomes a charged ion.

The atomic transitions caused by the jump of electrons from one energy level to another are caused by the light radiation of a certain energy. This light radiation is in the visible or ultraviolet range, and its wavelength determines the precise energy of the transition. Transitions between different energy levels in atoms emit different wavelengths of light, which are called absorption or emission spectra in spectroscopy.

These spectra can provide a lot of information about the properties of atoms, so atomic transitions are an important means to study atomic structure and atomic properties.

On the other hand, ionization is a process by which an atom or molecule loses or gains one or more electrons, and this process can be caused by an electron beam of a certain energy or electromagnetic radiation. When the radiation fiber dissipates high enough energy, it can break the chemical bonds inside an atom or molecule, thus ionizing it. Once atoms or molecules are ionized, they take on a positive or negative charge and become charged ions.

The behavior and properties of these charged ions are different from those of the number of atoms or molecules because they carry an electric charge.

Overall, atomic transitions and ionization are two different physical processes that occur inside atoms and molecules. Atomic transition is a change in the energy level inside an atom and is caused by light radiation, while ionization is the process by which an atom or molecule loses or gains one or more electrons, making them charged ions. <>

Summary. The electrons are moving in their respective energy levels, which is why they "move", and the energy itself does not change.

But the transition, that is, after the electron gains energy, jumps to the electron layer with a higher energy level, and the electron's own energy increases.

The two are different.

Difference Between Electron Transition and Electron Transfer.

Please wait for me for two minutes, and I'll check the information.

The electrons are moving in their respective energy levels, which is the "movement", and the energy itself does not change but the transition, that is, after the electrons obtain energy, they jump to the electron layer of a higher energy level, and the electrons' own energy increases, and the two are different.

There is a big difference between the two <>

Hope it helps.

Is there an electron transition phenomenon in chemical reactions.

I don't think chemistry is directly related to the electron transition. Chemical reactions are accompanied by the transfer of electrons: the electron transition is due to the absorption of light of a particular wavelength from the ground state to the excited state, or from the excited state to the ground state and the emission of light.

Atomic absorption and atomic emission have transitions, and atomic fluorescence has chemical reactions and transitions.

For example, manganese has the most positive 7 valence, will the low-energy electrons jump to the higher energy level and then lose electrons and a chemical reaction will occur?

If you are, this will not happen.

It is the transfer of electrons that occurs directly.

And not electronic transitions.

Doesn't the inner electron go through a high energy level when it is lost, and isn't that a transition?

This interpretation can also be barely said to be a leap <>

However, chemistry directly talks about electron transfer, and it is rare to hear about transitions.

Excessive NaCl solids are added to the tetraammonium sulfate copper solution, and then diluted with water, what is the change in the color of the solution?

Wait for me to look up the information.

The addition of sodium chloride solids is non-reactive.

Diluting with water is equivalent to diluting the color of the solution.

Will it not produce copper tetrachloride ions.

It won't be generated.