Electronic Configuration of Iron

A chemical element with an atomic number 26 and a symbol Fe represents it, Iron is a very common element that is found. Unlike other elements, iron exists at the oxidation states of -2 to +6. Elementary iron occurs in a low-oxygen environment in spite of being reactive to water and oxygen.

Iron is characterized by its ability to form variable oxidation states which differ in one or two organometallic chemistry. 

All the Compounds of iron are mainly formed at +2 and +3 oxidation states and may also occur at higher oxidation states of a  + 6. A very good example is potassium ferrate. Iron (4) acts as an intermediate to various biochemical oxidation reactions, cannot reach an oxidation state of +8, and is one of the first elements of its group.

Electronic configuration of iron is [Ar] \[3d^{6} 4s^{2}\]. The peculiar crystalline structure and its electronic and electronic configuration make it naturally attractive to metals. These is known as ferromagnetic materials. Iron has various types of allotropic forms in spite of not having a single crystalline structure. Alpha, Delta, and Gamma iron are allotropic forms of Iron.

These three allotropic forms are exhibited at different temperatures when it cools down to the molten form. The electronic configuration of \[Fe^{2+} is - 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{6},\] and \[Fe^{3+} is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{5}\]. \[Fe^{2+}\] contains 2 fewer electrons compared to the electronic configuration of Fe.  

In order to write the Iron Electron Configuration, we need to know the number of electrons for the GFe atom, and once we have the configuration for Fe, the ions are simple. When we write the electronic configuration the first two electrons go to the 1s orbital. This holds only two electrons, hence the next 2 electrons for Iron will go into 2s Orbital. The next six will also go into a 2p orbital, which can hold up to six electrons. Let us put six inside the 2p and put the next 2 in 3s orbital. Now, since 3s is full, we will have to move to 3p in order to put the next six electrons. We will next move to 4s Orbital Where the remaining two will be placed., and once 4s is full, the remaining six electrons will be in the 3rd orbital and will end with \[3d^{6}\].

Electronic Iron configuration will be : \[1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{6}\].

Iron, a chemical substance or element, is a metal generally represented by its symbol Fe. Its symbol is short for Ferrum which is a Latin term. The atomic number of iron is 26. Iron is a member of group 8 and the first transition series of the periodic table. 

By mass, the element ranks top among the most common substances on the surface of the earth as it constitutes a majority of the inner and outer core of the earth. Also, iron ranks fourth among the most common elements on the surface of the earth.

In contrast with various elements, iron occurs at oxidation states ranging from -2 to +6. 

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Iron is known for the capability to create different oxidation states which vary in specific ways. As iron is present in abundant amounts in the surroundings, it is often referred to as a standard for the whole group of transition metals. Iron (III) is referred to as ferric compounds, while iron (II) is referred to as ferrous compounds.

Compounds containing iron are mostly produced at the oxidation states of +3 and +2. The compounds of iron might also exist in a greater +6 oxidation state. Potassium ferrate would be among the suitable instances in this case. In various biochemical oxidation reactions, iron (IV) behaves as an intermediary substance. Furthermore, iron cannot achieve a +8 oxidation state and is among the primary elements of its class.

The electronic configuration of iron is represented as

Ar

Ar \[3d^{6} 4s^{2}\]. The typical crystalline framework and electronic configuration of iron make it usually attractive towards metals. Iron is considered a ferromagnetic material. The element showcases various kinds of allotropic structures although they are devoid of a lone crystalline framework. Delta, alpha, and gamma iron are the allotropic structures of iron.

Iron shows the above-mentioned three allotropic structures at variable temperatures when it turns cold to the fluid state. The electronic configuration of \[Fe^{2+} is - 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{6},\] while that of \[Fe^{3+} is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{5}\]. \[Fe^{2+}\] consists of 2 electrons less in comparison to the Fe’s electronic configuration - \[1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{6} 4s^{2}\].  

Valency of Iron

Before talking about the valency of iron, let us revise what valency actually is. The valency of an element is the number of electrons it obtains or gives away or shares to achieve noble gas or stable configuration. In simple terms, the number of electrons an element can gain, lose or share to achieve a fully filled outermost electron shell.

Now iron, as we know, has an atomic number of 26, that is, it has a total of 26 electrons. And its electronic configuration is depicted as - \[1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{6} 4s^{2}\]. The energy of 3d and 4s orbitals is almost the same. Another thing to note is that the 3d orbital has a lone pair of electrons, while the remaining electrons are unpaired.

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As mentioned earlier, iron displays the two valence states of +3 and +2. So, when it gives away the two 4s electrons, it acquires a valency of +2. In some cases, iron can also give away either of the paired electrons from a 3d orbital. As a result, the whole 3d orbital is filled with unpaired electrons that deliver a more stable configuration. In such a situation, the valency of iron will be +3.

Now you might be asking yourself this question: Why does iron (Fe) have a variable valency?

As a transition element, iron has the same outermost electronic configuration as the remaining metals in its group. This means that the 4s orbitals are the same in all the elements of that particular group, while only the inner 3d orbitals alter among these elements. On the contrary, these 4s and 3d orbitals have energy similar to each other. Hence, in some cases, iron loses two electrons from its outer 4s orbital, while in other cases, it also loses an extra electron from the inner 3d orbital. As a result, the iron ion has either two or three positive charges, that is, variable valencies – \[Fe^{2+} and Fe^{3+}\].

Applications of Iron

Residential uses

We all can believe in the notion: “Iron is everywhere”. It is a universal fact that you can discover iron or any of its forms in any place possible. Some of it might not be visible to the naked eye, yet it still occurs.

Iron is an important aspect of our homes. The chemical element can be discovered in the living room, bathroom, and kitchen area. In other words, iron is present in every nook and corner of your house. It is also present in a majority of items that run it.

Iron alloys exhibit excellent resistance against corrosion and rust creation. It can also be shaped with ease to develop a bunch of shapes. This is the reason why iron is utilized in most of the products that you generally see about the house.

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For instance, wrought iron is finding purpose in various outdoor products that help in increasing the appearance of the garden and terrace. In addition, items such as arbors, trellis, fences, and even highly catchy furniture can be derived from iron. 

Cast iron is another important form of iron that finds application in creating pans, pots, ovens, skillets, and trays. Further, cast iron consists of a heating substance that is highly suitable for cooking items, cookware, and other accessories. 

Meanwhile, stainless steel is a part of the kitchen cutlery and different electrical appliances.

Industrial Applications

Iron is quite popular all around the globe. It can be seen in every corner of the world. Not only is iron a part of the makeup of various transport options, but also it is a part of a majority of diverse items, products, and stuff that operate our new-age world.

The biggest factor as to why iron is used in a lot of ways is due to its characteristics that can be altered as per the requirements of the application by combining it with materials, be it metallic or non-metallic. 

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Different kinds of steel are present as of now. Each kind is derived from iron with a blend of various elements such as, silicon, nickel, and carbon, among others. Moreover, steel is a vital constituent in all structures and in all sorts of construction activities. 

Apart from that, bridges, skyscrapers, buildings, and other sorts of construction projects would be incomplete if they do not consist of iron in their structure. And the same thing applies to ships, aircraft, automobiles, and heavy machine tools and parts.

Eco-friendly Aspect of Steel (An alloy of Fe, C mainly)

As previously mentioned, iron has got loads of uses. But is it recyclable? The answer is yes, iron can be recycled. All the stuff that contains iron can be easily recycled.

By recycling iron-based applications, you are contributing majorly to the environment in the form of reduced carbon footprint, and energy required to create more metal from raw material. That ultimately leads to lesser pollution.