Sophomore elective chemistry semi full what does it mean

For example, 2px 2py 2pz three p orbitals can be filled with 2 electrons per orbital, a total of 6 electrons, and semi-filled is only one electron per orbital, a total of 3.

In the case of the p orbital, there are three orbitals, and each orbital has two electrons in opposite spin directions. Semi-filled means that there is only 1 electron in each orbital, and the electrons in the three orbitals spin in the same direction, which is the most stable.

Semi-filling refers to the presence of single electrons in the orbitals of the energy levels of different energy layers.

For example, the third energy layer has energy levels and its semi-full is S1, P3, D5

Semi-filled means that there are only half of the electrons in the orbital. The s orbital can only discharge a maximum of 2 electrons, and a half-filled is an electron. The p orbital can only row up to 6 electrons, and the semi-filled orbital is 3 electrons.

Each orbital of an atom has a definite number of electrons, and when the number of electrons reaches half, it is called semi-filled! At this point, the electron spin direction is the same! Relatively stable!

Semi-filled is half of the number of electrons that can be held in the atom-filled orbital, which is relatively stable. For example, chromium is 3d5 4s1

According to the principle of lowest energy, when the sublayer is half-full or fully full, the energy of the atom in the ground state is low, for example, the chromium configuration is (n-1)d5ns1 instead of (n-1)d4ns2, which is called the half-full rule.

The outermost number of electrons in an electron orbital is equal to half of the maximum number of electrons it can hold.

It is the arrangement of electrons outside the nucleus. The electrons are arranged in layers outside the nucleus, and the electronic configuration formula of the outer nucleus is 1s22s22p3 in several sublayers on each layer, and the p sublayer on the second layer contains orbitals in three directions, and each orbital occupies an electron, which is the half-full state; If there are 8 electrons on the second electron shell, then both the S and P subshells are full of electrons, which is the full state, and both the full and semi-full states are chemically stable.

The arrangement of electrons in the intelligent electron orbital is as p3 d5

Due to the existence of the Hundt rule. The 3D semi-filled ones include CR (chromium) and manganese Mn, and there are many full-filled ones: Cu (copper), zinc, GA, GE, AS, SE, BR, KR

Well, let Teacher Fu secretly tell you that half full is cr mn full is cu zn next time in class be more serious -

Could it be that the atom is an element with electrons of 8 and 4 in the third shell? Element 14 Silicon Si Element 18 Argon

It should be:

The number of electrons in the outermost shell.

The outermost electron number is fully or half-full, and it is relatively stable.

No, c is 1s2 2s2 2p2, half-full stability is under the premise that the energy levels of the last two orbits are close, and the difference between 2s and 2p orbits is relatively far. For example, 3D and 4S orbits will be 3D5 4S2, not 3D7 (D orbits can hold 10 electrons) High school does not need to dig so deeply, just understand it, and write it down individually.

Hunt half-full is the most stable, but it also follows the principle of lowest energy, that is, electrons can only be discharged after one sublayer has been discharged.

According to the principle of lowest energy, electrons first arrange orbitals with low energy, and the 4s energy level is lower than the 3d energy level. There are textbooks.

It stands to reason that cadmium should be 3(d4)4(s2), but semi-filled and stable, so 4s gives 3d one electron.

He has to satisfy Hunt's rule, but also to satisfy the principle of lowest energy, 3d5 is a semi-full state, and the energy is low. And the 4S energy level is lower than the 3D energy level.

This is Hunt's rule also, the principle of minimum added energy. It's in chemistry textbooks.

Because in order to meet the principle of minimum energy, you should first fill in the 4s orbit, and then fill in the 3D orbital, and colleagues should also meet the 3D5 semi-full state, which has the lowest energy and the most stable.

Exception to the Hunt Rule

When the atomic orbitals with the same energy are in the fully filled, semi-filled and fully empty states, the energy of the system is low, and the atoms are called stable.

Special case of Hunt's rule: For the same electron subplane, it is relatively stable when the electron configuration is fully filled, semi-filled, or fully empty. There are many exceptions to the Hunt rule, such as "in the atomic orbital, the energy of each layer is half full or fully full", that is to say, S1, S2, P3, P6, D5, D10, F7, F14 have the lowest energy and the most stable, which is the general form of the existence of the original lead chain, but as long as you look at the periodic table, you will find that the following rows of several types of elements, especially the lanthanide and actinide good elements, do not conform to the Hunt rule, which is also unexplained by the current theory.

The energy of the electric Zhizi row is higher than that of 3D in 4s, and the lower the energy, the more stable. P2 is considered to be semi-full, but because its energy is similar to that of the adjacent S, it is generally not considered.