Difference Between Ferrous and Ferric

Main Difference – Ferrous vs Ferric

Both these terms, ferrous and ferric, refer to different forms of the existence of the Iron element. Iron is an element in the ‘d block’ of the periodic table, which means it is a transition metal. These metals have a special characteristic of exhibiting multiple valencies. Therefore, transition metals can have several stable oxidation states.  This is possible due to the presence of five hybridize orbitals. The main difference between Ferrous and Ferric is that Ferrous is the+2 oxidation state of Iron while Ferric is the +3 oxidation state of Iron

What is Ferrous

As mentioned above, this is the +2 oxidation state of the Iron element and is considered as a stable ion. Its oxide is green in color, and it is the first step in the formation of rust. As Iron is a metal, it needs to release or give away electrons and form positive ions, in order to gain a stable electron configuration. The general electron configuration for the iron element can be written as 1s22s22p63s2 3p6 4s23d6. When it comes to ferrous, two electrons are released from the 4s orbitals as it is the outermost orbital. However, 3d orbitals are higher in energy than the 4s orbitals. Therefore, discharge of electrons takes place from the 4s orbitals, even though electrons are filled into the 3d orbitals at last.

Therefore, the electron configuration of the ferrous iron would be 1s22s22p63s2 3p6 3d6. Now this ionic form is able to form compounds and complexes with other elements and negatively charged ions. These complexes can also be in ionic form and, in that case, they are generally known as ‘transition metal compounds.’ When naming this kind of inorganic complexes, the term ‘Ferrous’ is often replaced with the names of the element and its valency is given within brackets, such as ‘Iron (ll) oxide’. Some examples for famous ferrous compounds are FeO, FeCl2, FeSO4, etc.

Main Difference - Ferrous vs Ferric

What is Ferric

Ferric is known as the +3 oxidation state of Iron and is the most stable form of Iron in the air. Upon the oxidation of Iron, it turns into ferrous oxide and in the presence of more oxygen the ferrous ion get oxidized to form ferric ions, in this case ‘ferric oxide’ which is rust. It is a brown color flaky material. Getting back to the definition, in order for the ferric ion to form, the elemental form of Iron needs to give away three electrons from its orbitals. The resulting electron configuration of the ferric ion would be: 1s22s22p63s2 3p6 3d5. This configuration has more stability than the ferrous ion and also the elemental form. As this configuration satisfies the partial electron filling.

To explain it more, there are five d’ orbitals. Any configuration where the orbitals are fully-filled or half-filled is considered to be higher in stability than the other forms. In the case of ferric ion, each d orbital contains an electron, making it half-filled as d orbitals contain five electrons. Ferric ions too form other compounds and complexes, and when naming inorganic complexes, it is written as ‘Iron (lll).’ Some of the most common ferric compounds are Fe2O3, FeCl3, Fe2(SO4)3, etc.

Difference Between Ferrous and Ferric

Difference Between Ferrous and Ferric

Definition

Ferrous is the +2 oxidation state of Iron.

Ferric is the +3 oxidation state of Iron.

Stability

Ferrous +2 is relatively less stable.

The ferric ion has its d orbitals half-filled in the outer-most shell, making it more stable than other forms of Iron.

Oxidation/ Reduction

Ferrous can be formed through the reduction of Ferric ions.

Ferric ions are formed through the oxidation of Iron elements beyond the stage of Ferrous ions.

Process of Oxidation

Ferrous ions are formed through the loss of 4s electrons from the Iron element.

Ferric ions are formed through the loss of both 4s and 3d electrons.Difference Between Ferrous and Ferric-infographic

Image Courtesy:

“Iron(II) oxide” by Calvero (Public Domain) via Commons

“Iron(III)-oxide-sample” by Benjah-bmm27 – Own work. (Public Domain) via Commons

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