Chemistry Homework Help: 4 Inorganic Types of Reactions

Are you having trouble grasping the contents of inorganic chemistry? If your answer is yes, then this is an article that you would not want to miss out on. Through thorough research, we have identified a way to help you understand inorganic chemistry and gain mastery in the topic. The method is pretty practical and has worked wonders, so let it work wonders for you too!

Many people stereotype that inorganic chemistry is super hard and that it is only meant for geniuses. However, this is not the case. We have discovered that many students mastery this topic by first changing their mindset:

Mindset change

First, you need to know that inorganic chemistry is not as hard as people assume it is. Drop the assumptions and take a book, read it and make the judgments yourself. You will find that with a bit of effort, the topic and ultimately the subject will seem easier to understand.

After you change your mindset, it is now time to apply the four inorganic types of reaction methods. We found that different compounds and elements create pretty different reactions when merged. It is hence pretty challenging to try and memorize each reaction. However, when using the four inorganic types of reaction concepts, memorizing will be off the table, so do not stress yourself.

The four inorganic types of reaction

Nearly all chemical inorganic reactions fall under 1 of the four inorganic types of reactions. They are like the broad categories of reactions in inorganic chemistry. The four inorganic types of reactions are:

Combination reactions

The first reaction is the combination reaction. It states that 2 or more than 2 reactants create a single product. The product comes as a result of combination reactions. A pretty efficient combination reaction example would be:

When you burn sulfur in the air, it forms sulfur dioxide, ie.

S (s) + O2 (g) -> SO2 (g)

Sulfur (solid) + oxygen (gas) -> sulfur dioxide (gas)

As you can see, sulfur and oxygen combine to form sulfur dioxide.

Decomposition reaction

Just as the name implies, decomposition reactions entail decomposition. In such a reaction, one compound is broken down into several substances according to the reaction. An excellent example of such a reaction would be the decomposition in mercury ii oxide.

2HgO (s) + heat -> 2Hg (l) + O2 (g)

As you can see, mercury ii oxide is heated up, which breaks the compound down to form mercury and oxygen.

Single displacement reaction

Single displacement reactions entail a displacement reaction, this implies that an ion or atom of a compound replaces another element’s atom. Here is a pretty effective example:

Zn (s) + CuSO4 (aq) -> Cu(s) + ZnSO4(aq)

Zinc (solid) + Copper sulfate (aq) -> Zinc sulfate (aq)

Zinc metal is reacted with copper sulfate, which leads to the copper ion displacement in the copper sulfate hence forming the zinc sulfate.

Single displacement can be subdivided further into specific categories such as redox reactions and so much more.

Double displacement reactions

Can also be referred to as metathesis reactions. A displacement reaction occurs between 2 compounds, and they both create new compounds. For example:

CaCl2 (aq) + 2AgNO3 (aq) -> Ca(NO3)2 (aq) + 2AgCl (s)

Silver nitrate is reacted with calcium nitrate hence forming silver chloride and calcium nitrate.

Neutralization reactions can also occur. It is a reaction whereby a base reacts with an acid-producing water and salt in the double displacement category, i.e.:

HCl (aq) + NaOH (aq) -> NaCl (aq) + H2O (l)


Inorganic chemistry is pretty easy to master. When you follow all the guidelines provided in this article, you will find the topic easier than before.