What is electron configuration?

Electron configuration usually refers to the arrangement of electrons around the atom core in its basic state, a condition in which all atomic electrons exist at the lowest possible energy level. Different energy levels occupied by electrons are often referred to as shells surrounding the nucleus of the atom. Each shell is marked with a whole number, starting 1. The higher the number of shells, the greater its distance from the atom core. Electrons in each shell exist in regions called orbitals or PodShells, which are marked with, P, D and F. The first shell, which is closest to the core, will contain only two electrons, the second eight, third 18, etc. Within the shell, each orbit can be occupied not more than two electrons.

Each shell contains the same type of orbitals found in the previous shell and a new type of orbital. The first shell contains usee orbital orbital, but the second shell contains orbital and three orbitals; Each of these P orbitals can hold two electrons, so the combined p orbitys in the shell can hold up to six electrons. The third shell has orbital, three orbitals P and five orbitals. Seven orbitals F are first found in the fourth shell, which also holds orbital, three orbitals P and five orbitals. Orbitals outside orbitals exist, but rarely discuss them.

The electron configuration table shows the order in which the orbitals are filled inside the shell. For example, the electron configuration for the sodium is 1s ^{2 2S}

2 2p

6

3s 1 , which means that 11 electrons of sodium are found in the first, second and third electron shells. Orbitals The first and second shells contains two electrons and the second has six electrons. The third shell orbit contains only one electricone; His three orbitals and five orbitals are unoccupied.

while writing a napiSU in the electrons configuration cannot be superscript on a letter indicating the type of orbital never higher than the maximum number of electrons that can occupy this type of orbital. Superspis for S, P, D and F will never be higher than 2, 6, 10 and 14, respectively.

Shell and orbitals are filled in front of those with higher energy levels. However, this does not mean that one shell will be completely filled before the electrons start to occupy another shell. The configuration chart shows that 4S orbital will be occupied before 3D orbitals. This occurs because the electrons increase the electrons to interact and create conditions in which the higher orbital is the lowest energy condition for other electrons.

Understanding electrons configuration is particularly important for studying chemistry. This is because chemical reactions generally occur in valence or external shells. The valence shell electron configuration provides important information about how each element reacts with othersi.