What is the law of electron affinity energy, and what is the law of change of electron affinity?

In general, electron affinity energy.

The algebraic value of varies with the atomic radius.

, i.e., decreasing from top to bottom in the same family and increasing from left to right in the same period. But it should be noted that VIA and VIIA

The absolute value of electron affinity energy is the largest.

Not the first element of each clan, but the second element.

This anomaly can be explained by the fact that the oxygen sum of the second cycle.

Fluorine has a small atomic radius, a high electron density, and a strong repulsion between electrons, so that when atoms are combined1

electrons form a negative ion.

The energy emitted is smaller, while the second elements, sulfur and chlorine, have a larger radius, and empty d orbitals in the same layer can be accommodated.

Nanoelectrons, electrons have less repulsion and thus form negative ions.

The energy emitted is maximum.

Extended Materials. The first electron affinity energy of an elemental atom is generally.

is positive because the potential energy of the electrons falling into the nuclear field of the neutral atom decreases and the energy of the system decreases. Electron affinity potential, which is the energy of the affinity between electrons. Electron affinity energy is the ground state.

The gaseous atom gets electrons to become gaseous anions.

The energy emitted. The unit is kj mol (SI unit is j mol).

The second electricity of all elemental atoms.

The sub-affinity energy is positive, because the anion itself is a negative electric field, which has a repulsive effect on the added electrons, and the electrons must be added again.

, the environment must also do work on the system.

The general law of electron affinity potential change is that in the same period, with the increase of atomic number, the electron affinity potential of an element generally tends to increase, that is, the tendency of the atom to bind electrons increases, or its ability of the anion to lose electrons decreases.

In the same family, there is no obvious change in the electron affinity potential of an element. When the electronic configuration of the element atoms shows stable S2, P3 and P6 configurations, the EA values tend to decrease, and even the EA values of group A and group zero elements are negative, which indicates that it is very difficult for them to bind electrons.

For example, the fluorine atom f(g)e f-(g), h=-322kj mol. Whereas, the electron affinity potential (EA) of fluorine is defined as 322kJ mol. For this reason, it has been suggested that the electron affinity potential of an element refers to the energy absorbed by separating an electron from its gaseous anion.

Thus, the fluoride ion f-(g) e f(g), h 322kj mol. The symbols used in both tend to be unified.

It can be assumed that the electron affinity potential of an atom is numerically the same as the ionization energy of its anion. Based on the electron affinity potential data, it is possible to determine how easy it is for an atom to gain or lose electrons. Non-metallic elements generally have a large electron affinity, and it is easier to get electrons than metallic elements.

The electron affinity potential is determined experimentally, but it is not possible to accurately measure the electron affinity potential of most elements.

The above content reference: Encyclopedia - Electronic Affinity.

Electron affinity energy is similar to ionization energy, electronegativity but not the same as a measure of the strength of the non-metallic strength of an element, it is defined as a neutral gaseous atom, get an electron, become a gaseous negative valence anion, the energy emitted. The greater the affinity energy of the electronic search Zheng, the stronger the non-metallic nature of the element. Due to its difficulty in measurement, there is less data.

The electromorphic sonson affinity of an element reflects how easily the atoms of the element can get electrons. The smaller the algebraic value of the first electron affinity energy of an elemental atom, the greater the tendency of the elemental atom to get electrons, and the stronger the non-metallic nature of the element. In general, the algebraic value of the electron affinity energy decreases with the increase of the atomic radius, i.e., decreases from top to bottom in the same group and increases from left to right in the same period.

The atomic radius of oxygen and fluorine in the second period is small, the electron density is large, and the repulsion between electrons is strong, so that when the atom combines 1 electron to form a negative ion, the energy released is smaller, while the radius of the second element sulfur and code chlorine is larger, and the empty orbital in the same layer can accommodate electrons, and the repulsion force of electrons is small, so the energy released when forming negative ions is the largest.

The algebraic value of electron affinity energy decreases with the increase of atomic radius, that is, it decreases from top to bottom in the same group and increases from left to right in the same period.

The element with the greatest affinity is: chlorine.

Elemental Affinity Data:

Hydrogen: Lithium: Boron: Carbon: Oxygen: Fluorine: Sodium: Aluminum: Silicon: Phosphorus: Sulfur: .

Chlorine (element with the greatest affinity): 349, potassium: calcium: scandium: 18, titanium: vanadium: 51, chromium: iron: cobalt: nickel: copper: etc.

The energy emitted by a gaseous atom in the ground state of an element when it gets an electron to form a -1 valence gaseous anion is called the first electron affinity energy of the element, which is denoted by e1. The energy emitted by the gaseous anion that becomes -2 valence is called the second electron affinity energy e2, and so on.

Cl Although the electronegativity of fluorine is greater than that of chlorine, here it is because the electronegativity of fluorine is too large, and the nucleus attracts the outer electrons too strongly, so that the atomic radius is too small, so that the shielding effect is much larger than that of chlorine, and it is precisely because the outer electrons are close together that it is not easy for a foreign electron to be added to the orbit of fluorine, because the electrons and electrons are negatively charged, and thus the repulsion force is greater, but chlorine does not have these problems, because its outer electrons are much more sparse than fluorine, so it is easier to add to the orbital than fluorine So in general, fluorine has a smaller electron affinity than chlorine.

The administrative power is constantly expanding, and the scale of the administrative organization is expanding day by day; (2) The nature of management is becoming more and more complex, and the management function is constantly expanding; (3) the trend of specialization and professionalization; (4) the strengthening of inter-organizational interdependence and coordination; (5) legal restrictions and stylization; (6) attaching importance to the purpose of society; (7) International influence and internationalization trend.

Get the energy released by electrons.

Electron affinity energy refers to the energy difference between the free electron energy level of the vacuum and the conduction band bottom energy level, that is, the energy required to take the conduction band bottom electron out of the vacuum and become free electrons.

Electron affinity, as the name suggests, is the affinity with electrons.

The energy emitted by a gaseous atom (ground state) when it acquires one electron and becomes a -1 valence gaseous ion is called electron affinity energy.

In semiconductor physics, it refers to the magnitude of the ability of the centers of each atom to gain electrons. In general, the sum of the energies of gaining an electron and losing an electron can be used as a criterion.

The standard definition of electron affinity energy of an atom refers to the energy released when an atom and an electron react to form a negative ion in the lower gas phase. (electron affinities of atoms)

The energy emitted by a ground state gaseous atom to form a gaseous negative valence ion is called the first electron affinity energy, which is represented by EA1, followed by EA2, EA3, and so on.

a（g）+ e－ →a－ （g） <0

The greater the first electron affinity of the element, the greater the tendency of the element to generate negative ions from gaseous atoms, and the stronger the non-metallicity of the metal. The factors that affect the magnitude of the electron affinity energy are the same as the ionization energy, i.e., the radius of the atom, the effective nuclear charge, and the electron configuration of the atom. Its trend is similar to ionization energy, and elements with large ionization energy generally have a large electron affinity.

In a word, the energy generated by electromagnetic resonance is enough for the elements to fuse or decay.

Compared to other elements in the group, the foreign electrons of fluorine are the closest to the nucleus. Therefore, according to the factors we have considered earlier, fluorine should have the highest electron affinity.

However, since fluorine is a very small atom, the small space occupied by the fluorine atom is crowded with electrons, and these crowded electrons have an unusually strong repulsion effect on foreign electrons. This repulsion weakens the attraction of the nucleus to foreign electrons, and the electron affinity energy decreases.

Oxygen and sulfur in group 6 elements also do not obey the law, and the first electron affinity of oxygen is good.

kjmol)

Specific sulfur (-200

kjmol)

The reason for this phenomenon is exactly the same as the reason why fluorine has a smaller electron affinity than chlorine.

The definition of electron affinity energy can also be extended to molecules. For example, the electron affinity energy of benzene and naphthalene is negative, while anthracene.

The electron affinity energy of phenanthrene and pyrene is positive. Confirmed by computer simulation experiments.

hexacyanobenzene

c6(cn)6

The electron affinity energy is higher than that of fullerenes.

Diatomic molecules. Bromine.

Chlorine. Fluorine. Iodine. Oxygen.

Iodine bromide. Lithium chloride.

Nitric oxide. Triatomic molecules. Nitrogen dioxide.

Sulfur dioxide. Polyatomic molecules. Benzene.

1,4-Benededione.

Boron trifluoride. Nitric acid. Nitromethane.

Phosphorus trichloride. Sulfur hexafluoride.

Tetracyanoethylene. Tungsten hexafluoride. Uranium hexafluoride.