Molecular Formula Vs Empirical Formula
The molecular formula and empirical formula of various compounds are different (in some special cases they can be same). They represent different properties of the compound. The differences between Empirical Formula and the Molecular Formula of the compound are given below in the table.
Empirical Formula |
Molecular Formula |
---|---|
Empirical Formula represent the simplest ratio in which the atoms combined to form a molecule. |
Molecular formula tells us that exactly how many atoms combined to form molecule. |
Example: Empirical Formula for Butane is C2H5 |
Example: Molecular Formula for Butane is C4H10 |
Empirical Formula
Empirical Formula in chemistry is defined as the simplest ratio of the elements present in the compound. It does not take into account that these elements are connected with each other in any manner. This is explained in the formula of Glucose as we know that the formula for Glucose is C6H12O6 here we see that there are 3 atoms in the glucose molecule, they are carbon, hydrogen, and oxygen, Now the ratio of these elements is 1: 2: 1 i.e. for one molecule of hydrogen we have 2 molecules of hydrogen and one molecule of oxygen. So its empirical formula is CH2O. It doesn’t tell us how many elements of each element are there in the Glucose molecule.
In this article, we will learn about the Empirical Formula in Chemistry, Molecular Formula, the Difference between Molecular Formula and Empirical Formula, and others in detail.
Table of Content
- Empirical Formula
- Molecular Formula
- Molecular Formula Vs Empirical Formula
- Empirical Formula of Various Compounds
- How to Find Molecular Formula from Empirical Formula?