Iron is a metal found on earth in abundance, and it also plays an important role in human life. For instance, it is found in our blood in the form of hemoglobin which helps carry oxygen to our cells. Along with this, iron also has various oxidation states, which also have significant importance. Hence, it is imperative to teach students about oxidation states of iron and its corresponding chemical reactions.

What are oxidation states?

Oxidation, in simple terms, refers to the process in which an element loses electrons whereas reduction refers to the opposite process in which an element gains electrons. The oxidation of some elements may lead to different oxidation states, which refer to the number of electrons the element has gained or lost.

Iron and its varying oxidation states

Iron has a varied range of oxidation state which ranges from -2 to +10. The most common states of iron are +2 and +3 (ferrous and ferric states, respectively). It is important to understand these two states for getting clarity on the different chemical reactions of iron.

Some examples of chemical reactions of Iron:

1. Formation of Rust:

Rusting is one of the most common examples of iron’s oxidation state in which it reacts with oxygen (O2) present in the atmosphere to form rust, which is mainly hydrated oxide of iron (III). Therefore, rusting is an oxidation reaction that results in the oxidation of iron from +2 to +3 oxidation state.

2. Acid-base reaction:

When iron reacts with hydrochloric acid (HCl), it produces ferrous chloride (FeCl2) and hydrogen gas (H2). This reaction indicates the +2 oxidation state of iron.

3. Combustion of iron:

Iron reacts with oxygen to form iron oxide. This reaction indicates the +2 oxidation state of iron.

Benefits of teaching students about Iron and its oxidation states

The study of different oxidation states of iron helps students gain a better understanding of how chemical reactions occur and how elements are affected by different conditions. By teaching about the oxidation state of iron, students would also develop an interest in chemistry and scientific methods.

Additionally, when students understand the relationship between the oxidation states of iron and its different reactions, they can thereby gain insight into how compounds can be transformed under varying conditions.

Conclusion

Teaching students about the oxidation states of iron is important not just for understanding chemical processes, but it can also aid in understanding metabolic processes in the human body. It is imperative to impart scientific knowledge to students, especially to promote their interest in science and foster their critical thinking abilities. By providing thorough knowledge about the oxidation states of iron, students can develop an understanding of how different compounds are created by different environmental factors and chemical reactions, thereby creating an essential link between science concepts and real-world applications.