What is the first electron affinity and second affinity potential of an oxygen atom?

In contrast to the energy required by an atom to lose an electron, the electron affinity potential refers to the energy emitted by an atom to gain an electron.

A gaseous atom of an element is in the ground state.

The energy emitted by a negative valence ion that acquires an electron to become a gaseous state is called the element's first electron affinity potential

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Second, the third electron affinity potential.

The first electron affinity potential of the oxygen atom (also known as the electron affinity energy) refers to the energy emitted by the gaseous oxygen atom when it gets one electron to become a gaseous negative divalent ion, and the second affinity potential refers to the energy emitted by the gaseous oxygen atom when it gets two electrons to become a gaseous negative divalent ion.

In contrast to the energy consumed by an atom to lose an electron, the electron affinity potential refers to the energy emitted by an atom to gain an electron. The energy emitted by a gaseous atom of an element that gains an electron in the ground state and becomes a gaseous negative valence ion is the first electron affinity potential (ea1) of the element, and similarly, the second electron affinity potential (ea2) and the third electron affinity potential (ea3) can be obtained. The greater the affinity of the first electron of an element, the greater the tendency of the element to become a negative ion from the electrons obtained from the gaseous atom, that is, the stronger the non-metallic nature of the element.

The correct one in the combination of four 2p electrons of the oxygen atom is 1235.

Three P tracks, to be filled. So there are two p electrons that occupy one orbital, the spin quantum numbers are opposite to +1 2 and -1 2, respectively, and the other two occupy the other two orbitals.

Oxygen is the most widely distributed in nature, covering the mass of the crust, and is the most abundant element. Oxygen is needed for the oxidation of hydrocarbons, the treatment of wastewater, rocket propellants, and the respiration of animals and humans in aviation, aerospace and diving. Oxygen is consumed by animal respiration, combustion, and all oxidation processes.

But the oxygen in the air is constantly replenished by the photosynthesis of plants. Metallurgical processes are inseparable from oxygen. Oxygen is also needed to intensify the production process of nitric acid and sulphuric acid.

First of all, the principal quantum number of 4 2p electrons is 2, the angular quantum number is 14, and the magnetic quantum number of 2p electrons is 2px2, 2py1, 2pz, and 12px, and the magnetic quantum number of 12px is 0, 2py is -1, and 2pz is 1, and the spin quantum number is +1 2, and the downward one is -1 2, so the combination of four 2p electrons is 1235

If you don't understand, please ask! Hope!

First of all, the primary quantum number of the 4 2p electrons is 2, and the angular quantum number is hungry.

The magnetic quantum number of 14 2p electrons is 2px2, 2py1, 2pz, 12px is 0, 2py is -1, and 2pz is 1

The spin upwards of the electron, the spin quantum number.

+1 2 and -1 2 downward

Therefore, the combination of four 2p electrons is correct 1235

If you don't understand, please ask! Hope!

Because it is a 2p electron, the search stool n=2,l=1;

m can be taken , -1;

MS can take 1 2. But the two electrons should be taken the same as the first value of the world sales brigade.

Haha, you're looking for a rather difficult question.

The outer electron configuration of oxygen is 2s2 2p4, and the second electron shell only allows 8 electrons to stabilize the structure, as a result of which the oxygen molecule forms a unique molecular orbital: two oxygen atoms are hybridized by sp to form two sp orbitals each, and two p orbitals perpendicular to each other, and their electronic configurations are:

Oxygen atom a: sp( )sp(:) py( )pz(:)

Oxygen atom b: sp( )sp(:) py(:)pz( ).

Then the two sp( ) of the two atoms bond with each other; The two sp(:) are still lone pairs, pointing to the axial ends of the molecule.

The py( ) and py(:)pz(:) and pz() of ab overlap laterally to form two two-centered, three-electron bonds, which are equivalent to a special bond, and the bond energy is about half of the general bond.

This particular structure results in a fairly reactive oxygen and paramagnetic nature of the molecules (caused by two two-centered, three-electron bonds).

Two pairs of electrons are shared to form a covalent bond o=o