Electron Configuration of Atomic Species

electron configuration

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The world in which we live in today is fascinating, we must understand that we are blessed to be part of this reality. We should never take anything for granted and try to understand why it is that the earth, was made the way it is today.

In today’s article, we are going to talk about electron configuration of an atomic species, in order to understand the shape and energy of electrons. The bonding ability, magnetism and other chemical properties, are better understood, when we know the electron configuration of an atomic species.

The location of electrons in an atom, are found thanks to the fact that they are written down, a simple way, known as electron configuration. Protons attract electrons to circle around the nucleus of an atom, and electrons repel each other, causing them to spread out around the nucleus, in regular patterns.

A beautiful geometric structure called orbitals, is the shape formed by these electrons; the orbitals represent the different regions around the nucleus, which each electron traces out.

The Pauli Exclusion Principle, is the reason why electrons tend to stay in their separate orbitals, and don’t pile on top of each other. The Pauli Exclusion Principle states that no two electrons can be in the same place, this principle comes from quantum mechanics and from fundamental physical principles that constrain all subatomic particles.

Each electron occupies an orbital, under the orbital approximation, a single wave function can be utilized, in order to place the electrons. We must follow a set of three rules when assigning electrons, these rules are Aufbau Principle, the Pauli-Exclusion Principles and the Hund’s Rule.

The identifiable address for each electron around an atom are the orbitals, which are similar to a block of studio apartment ready for electrons to occupy it. If you look at the periodic table, you’ll notice that as you move down the table, electrons tend to fill up the orbitals nearest to the nucleus quick.

As a result, orbitals and energy levels which are far from the nucleus begin to fill up with electrons, as we move down the periodic table. A scientist should know, how far from the nucleus an electron can be found, this is known as its energy level, to track down where a given electron lives in an atom.

Also, the type of orbital that the electron occupies must be known as well, the energy level could be seen to represent an apartment building and the orbital the apartment number.

The electron configuration is a way for chemists, to keep track of where all the electrons of a given element are found. The electron configuration of oxygen for example would look similar to this: 1s2 2s2 2p4. The number of electrons, that lives in each orbitals, is represented by the superscript number. The orbitals, which are available, is represented by the letters, and the energy level where the orbital are found, is represented by the big number.

An electron configuration table would be utilized, to write down the various orbitals available to electrons. Using an electron configuration table is the easiest way to create an electron configuration for a given element.

Thank you for reading this article!!!