Introduction to Basic Concepts of Chemistry

Chemistry can also be referred to as a branch of science which deals with the study of composition, properties and interaction of matter. Chemistry plays an important role in meeting with the day to day needs  of a human starting from food to health care products. It mainly focuses on atoms, molecules and ions that make up the elements and compounds. All these chemical components tend to interact via chemical bonds. 

Importance of Chemistry

Chemistry has a vital role in science and it is also involved with other branches of sciences. Chemistry is applicable in various areas like in weather patterns, brain functioning, computer operations, chemical production in industries, production of acids, alkalis, dyes, polymer, salts, alloys, metals, soaps, drugs, detergents. 

Branches of Chemistry

In this chapter we get to know about the different branches of chemistry they are discussed below as follows:

• Physical Chemistry: it defines the fundamental principles that govern various chemical phenomena. It deals with various laws, theories and principles of different branches of chemistry.

• Organic Chemistry: it refers to the study of various carbon compounds mainly hydrocarbons and their derivatives.

• Inorganic Chemistry: this refers to the study of compounds other than carbon. It mainly focuses on minerals present in the Earth’s crust.

Matter

It refers to any substance which occupies space, possesses mass and provides resistance e.g. book, pencil table, air, all living beings etc.

Properties of Matter

The properties of matter can be divided into two types:

• Physical Properties: these properties are observed or measured without changing the composition of matter e.g. changing colour, melting and boiling points, odour, density etc. 

• Chemical Properties: these properties on the other hand depend upon the characteristic reaction among various materials involving acidity, basicity, combustibility etc. 

Significant Figures

This explains the reliability of a measure given via the number of digits used to express it. It gives the positional information of a digit in a number which is reliable in indicating the quantity of something. There are certain rules used for defining significant figures those are discussed below:

• All non-zero numbers are considered as significant e.g. 7.8 has two significant digits whereas 7.14 has three significant digits. Note that decimal is not considered as a significant figure.

• Zero is considered significant only if it appears between two non-zero numbers e.g. 5.089 has three significant numbers whereas 5.003 has only three significant numbers.

• If in the beginning zero is present then it is not considered as a significant number e.g. 0.048 has two significant numbers and 0.003 has only one significant number.

• Zeros present in the right of a number is considered significant e.g. 15.0 has three significant numbers.

Introduction to some basic concepts

Below discussed are few important definitions which is required in this chapter:

• Atomic Mass Unit: it refers to a mass which is equal to one-twelfth of the mass of carbon atom 1 amu = 1.66056×10-24 g. The “amu” has been changed to “u”, called the unified mass.

• Atomic Mass: it refers to the mass of an atom. Though the SI unit of mass is kilogram, the unit of atomic mass is written as “u” or Dalton “Da”. 

• Gram Atomic Mass: the atomic mass of an element which is expressed in grams refers to the gram atomic mass or gram atom e.g. the mass of oxygen is 16 AMU , thus the gram atomic mass of oxygen is 16g

• Molecular Mass: it refers to the average relative mass of molecules of a substance. This expresses how the molecules of a substance are heavier than 1/12th of a carbon atom.

• Gram Molecular Mass: amount of a substance with a mass in grams is equal to its molecular mass is referred to as the gram molecular mass of that substance e.g. the molecular mass of oxygen is given as 32 AMU and the gram molecular mass is given as 32g.

• Formula Mass: it refers to a summation of all the atomic masses of an element that is present in one formula unit of a compound. It is used in ionic compounds. 

• Molar Mass: it refers to the mass of one mole of a substance in grams.

• Molar Volume: it refers to the volume which is occupied by one mole of a substance, it can be represented as VM. Its unit is litre per moles or millilitre per moles.

• Empirical Formula: this formula represents the simplest whole number ratio of different atoms present in a compound. 

• Molecular Formula: this formula represents the exact number of different types of atoms which is present in a molecular compound e.g. C6 H6 is the molecular formula of benzene. 

Conclusion

So, here we come to the end of this article on some basic concepts of chemistry. We hope that this article helps you in your exams to quickly brush up all the concepts. This is a very important topic from the point of view to gain knowledge on the basics of chemistry. We advise all students to focus more on understanding the topic rather than mugging up the concepts.