Difference Between Compound and Mixture
Chemistry is an interesting but complex subject. There is a fountain of terms that have similar meanings, but it is essential to identify their distinction in order to grasp the more complex concepts. As chemistry deals with potentially hazardous chemicals and processes, it is essential that people working in this field have a basic knowledge of chemical conformations to ensure that chemical synthesis or degradation processes are carried out accurately and correctly.
Two of the most commonly confused terms are compounds and mixtures. What is the difference between compounds and mixtures? If you’re a chemist, you should already know the difference between mixtures and compounds. However, if you are a chemistry or science student who has trouble distinguishing one from the other, or if you are simply curious about what these terms mean, then this article will help you to explain both terms properly. We’ll start by defining each term and then present the advantages and disadvantages of each in a comparison chart.
Definition of Mixtures
A mixture is defined as a material that consists of at least two substances that are combined but not chemically bound to each other. In other words, the combination in this context is only physical. They do not lose their individuality or unique properties and no permanent change is encountered as a result.
When different elements are put together without any chemical alteration, there is usually a high possibility that they can be separated. In some cases, separating them may be difficult, so they stay married, maintaining their unique properties for as long as they exist.
Some of the properties that show the distinction in the compound vs mixture comparison include the following with regards to the latter.
- There is a high possibility of separation of the components involved using physical techniques like filtration, distillation, decantation, etc.
- There is no need for any form of energy in the formation process, and there is little or no energy change after
- It can be formulated with components of varying compositions with no definite formula required
- Contents of a mixture retain their individual properties
Definition of Compounds
A compound is defined as the definite material result of two elements that are combined and bonded to each other by some chemical means. The keywords to take note of in this definition is “chemical means.” Without this means, there is a high possibility that the end result would not meet the standards of a compound.
What are these standards, you may ask? Here are some of the properties expected of every such chemically-bonded material.
- The constituents are of fixed proportion. This means they have to be combined in certain proportions
- It has a homogeneous nature, which means that the components are alike
- Every content loses its individual property and the material formed assumes new properties that may be different from the parent contents
- There is no simple physical process that can separate the components once they are chemically bonded to one another
- There is a need for some sort of energy in the formation process
- Every such material has a fixed boiling and melting point
For more clarification, in the examples of mixture vs compound, we have sand and water, oil and water, mud, cement, salt and water, and gasoline as examples of the former. Examples of the latter include hydrogen peroxide, water, aspirin, methane, salt, baking soda, and so on.
Mixture vs Compound Comparison Table
How do these terms compare? The table with the main differences between the two below should supply more clarity:
|Basis of Comparison||Mixture||Compound|
|Definition||Physically joins two or more bases||Chemically joins two or more elements|
|Separation||Easily done through physical mechanisms||Will require breaking down the compound to its elements|
|Nature||Can be homogeneous or heterogeneous||Homogeneous|
|Melting and boiling points||Not defined||Always defined|
|End result||No new substance or no new properties are formed||A new substance with unique properties is formed|
|Examples||Sand and water, oil and water, baking soda, tea and water||Hydrogen peroxide, octane, smoke, etc.|
|Energy used in the formation||Demands little energy||May demand high levels of energy|
|Structure of the bases||Varies||Fixed|
|Properties after combination||Retained||Transformed|
Several examples of compounds and mixtures can help you better understand. An example of a mixture is a salt solution or a mixture of salt and water. An example of a compound is the salt itself, which is an ionic compound formed by sodium and chlorine ions. Another example of a mixture is air because it combines different types of gaseous elements. On the other hand, rust (or iron oxide) is a combination of iron and oxygen through a redox reaction.
Conclusion of the Main Difference Between Mixtures vs Compounds
It is fairly easy to distinguish the difference between compound and mixture. Just think about the basics of the mixture. Then you have to determine whether the dissociation of these bases will require chemical or physical intervention.
In the examples above, airborne gases can be broken down by fractionation of the air. However, rust can be detached in its oxygen and iron bases by any physical method but by chemical methods such as electrolysis.
Another way to distinguish them from each other is to examine the chemical formula that results from amalgamation. Compounds have a distinct formula because when two or more elements are combined in certain amounts, mixtures do not have a formula because their bases are not chemically bound. As with any scientific curiosity, it will be useful to use critical thinking skills to gain a deeper understanding of complex concepts.