Some Basic Concepts of Chemistry - Notes, Topics, Formula, Books, FAQs

"Some basic concepts of chemistry" is the most fundamental chapter of complete chemistry. It gives information about the atomic number and mass number of elements. In any chemical reaction, it is important for us to know about the amount and number of reactants that will consume and the products that will produce, thus for estimating all these calculations, we use the laws of chemical combinations.

Important Topics of Some Basic Concepts in Chemistry

Nature and Characteristics of Matter

Matter is anything that occupies space and has mass. Matter exists in three physical states—solid, liquid, and gas and can also be classified as pure substances or mixtures based on its composition. The study of nature and characteristics matter forms the foundation of chemistry.

Properties of Matter and Their Measurement

Matter exhibits physical properties, like color, density, and boiling point, and chemical properties, like reactivity and flammability. These properties are measured using SI units, ensuring consistency in scientific communication.

Uncertainty in Measurement

All measurements involve some degree of uncertainty due to limitations in instruments or human error. Significant figures and error analysis help quantify and minimize these uncertainties in measurement in scientific calculations.

Atomic Mass and Molecular Mass

Atomic mass is the weighted average mass of an element’s isotopes, while molecular mass is the sum of the atomic masses of all atoms in a molecule. Atomic mass and molecular mass are crucial for stoichiometric and chemical calculations.

Mole Concept

The mole is a fundamental unit in chemistry that represents 6.022×10²³ (Avogadro's number). Mole concept is used to relate the mass of a substance to the number of particles it contains, enabling easy quantitative analysis.

Percent Composition Formula

Percent composition indicates the percentage by mass of each element in a compound. It helps in determining the compound's empirical and molecular formulas, providing insights into its composition.

Empirical and Molecular Formula

The empirical formula represents the simplest whole-number ratio of atoms in a compound, while the molecular formula shows the actual number of atoms of each element. Empirical and Molecular formulas are derived using percent composition and molecular mass.

Stoichiometric Calculations

Stoichiometry deals with quantitative relationships in chemical reactions. Stoichiometric calculations involve balancing chemical equations and determining the amounts of reactants or products, ensuring the conservation of mass and atoms.

Gravimetric Analysis

Gravimetric analysis is a quantitative technique where the mass of a substance is measured to determine its composition or concentration. It is highly accurate and commonly used in laboratories.

Law of Equivalence

The law of equivalence states that the amount of one substance reacting with or replacing another is proportional to its equivalent masses. This principle simplifies stoichiometric calculations.

Oleum and Its % Labelling

Oleum also known as fuming sulfuric acid, is labelled based on the percentage of free SO₃ it contains. This labelling aids in its safe handling and precise use in industrial applications.

Some Basic Concepts in Chemistry Formula

Some basic concepts in chemistry formulas are related to the mole formula, percent composition, and stoichiometry-related equations, which are integral to solving chemical problems.

Laws of Chemical Combination for Elements and Compounds

Laws of chemical combination for elements and compounds include the law of conservation of mass, the law of definite proportions, and the law of multiple proportions. These laws describe how elements combine to form compounds, emphasizing the fixed and predictable nature of chemical reactions.

Molarity and Mole Fraction

Molarity measures the concentration of a solution in moles per litre, while the mole fraction expresses the ratio of moles of a component to the total moles in the mixture. Molarity and mole fraction are important topics for solution chemistry and reaction kinetics.

Overview of the Chapter

Some basic concepts of chemistry is the most basic chapter of chemistry. It has various important concepts that you need to have greater insights for a better understanding of the whole of the chemistry. This article will help you to give important insights into this chapter and will also guide you in some important tips and guidelines.

Nature of Matter

Everything in the universe that has some mass and occupy some space is known as matter. Matter exists in three different physical forms i.e, solid, liquid and gas.

At the macroscopic level, the matter can be classified into two categories i.e, mixtures and pure compounds as shown in the figure.

Mixtures are those substances in which two or more components are mixed. Mixtures are further classified as homogeneous and heterogeneous mixtures. Homogeneous mixtures are the one in which components are present in a fixed ratio and the properties of this kind of mixture are the same throughout, for example, solution of sugar in water. But heterogeneous mixtures are those in which the components are not mixed in a definite ratio and properties of the mixture vary at different positions of the mixture, for example, sand in water.

Also read,

• Elements and Compounds
• Displacement Reaction
• Mole Concept Basics
• Example Chemical Change
• Pure Substances and Mixtures
• Chemical Formula
• Difference Between Physical and Chemical Change

Laws of Chemical Combination

The combination of elements to form some new product follows three basic laws as shown in the figure

• Law of conservation of mass: This law states that "matter can neither be created nor destroyed". This simply means that the number of reactants that are used in the reaction will be equal to the number of products formed.
• Law of definite proportions: This law states that any compound always contains its components in the fixed ratio by mass irrespective of its source and method of preparation.
• Law of multiple proportions: This law states that when two elements combine to form one or more than one compound, then the masses of one element that combine with the other element are in the ratio of small whole numbers.

Dalton's Atomic Theory

John Dalton proposed a theory about matter and atoms in which he proposed the following postulates:

(i) Matter consists of small individual particles known as 'atoms'.
(ii) All atoms of any particular element have the same properties and same mass but atoms of different elements have different properties and mass.
(iii) Compounds are formed when atoms of different elements are combined in a fixed ratio.
(iv) Chemical reactions involve the reorganization of atoms.

Mole Concept

A mole is the standard unit to measure the number of particles like atoms or molecules in a given sample. Mathematically, one mole is equal to 6.022 x 10²³. In other words, it can be said that it is equal to as many particles as there are atoms in 12g of the carbon-12 isotope. For example, if we have one mole of oxygen gas, that means we have 6.022 x 10²³ molecules of O₂.

Empirical Formula and Molecular formula

The empirical formula is the simplest whole-number ratio of atoms present in any particular molecule and the molecular formula is the actual representation of the number of atoms present in the molecule.

For example glucose i.e. C₆H₁₂O₆, its molecular formula is C₆H₁₂O₆ but its empirical formula is CH₂O.
Mathematically, the relation between empirical formula mass and molecular formula mass is given as follows:

n= Molecular mass empirical formula mass

where n is the simplest ratio.

Limiting Reagent

The reactant is consumed first in the reaction. When we are dealing with the balanced chemical equation, if the number of moles of reactants is not in the ratio of the stoichiometric coefficient of the balanced chemical equation, then there should be one reactant that should be limiting reactant.

% yield

Sometimes, experimentally, the reaction does not undergo 100% completion because of many factors which are involved in the actual industrial processes. So in such cases, we need the concept of % yield.

It is defined as the ratio of actual moles of product(s) formed to the number of moles that should have been theoretically formed assuming 100% completion of the reaction.

% yield = Actual number of moles formed Theoretical moles that should have formed

Stoichiometry and Stoichiometric Calculations

This concept helps us to calculate the mass or amount of reactants and products in the given chemical reaction. For calculations, first, we must have a balanced chemical equation, only then can we predict the mass of reactants and products. For example
The chemical reaction is given as follows:2H₂+O₂→2H₂O
Now, this chemical equation is a balanced equation, thus we are able to predict that one-mole oxygen will combine with 2 moles of hydrogen and form 2 moles of water, and thus accordingly, we can calculate the masses of the respective elements.

In this concept, we also study the "limiting reagent". It is the substance that is present in reactants in a smaller amount. In other words, a limiting reagent is a substance that will be completely finished or react in the given chemical reaction.

Some important Concentration Terms

• Mole fraction: It is the ratio of the moles of any substance present in the solution to the total moles of the solution. Mathematically, it is given as follows:
  Mole fraction of A=n_A+n_B
  where n_A is the moles of component A and n_B is the moles of component B.
• Molarity: It is the concentration of any substance present in the solution. In other words, it is moles of solute per unit volume of solution in litres. Mathematically, it can be given as follows:
  Molarity = Moles of solute Volume of solution in litre.
• Molality: It is the moles of solute dissolved in the given amount of solvent. Mathematically, it can be represented as follows:
  Molality = Moles of solute Mass of solvent (Kg)
• Normality: It is defined as the number of equivalents of solute dissolved in a one-litre volume of solution. Mathematically, it can be represented as follows:
  Normality = Number of equivalents of solute Volume of solution in litre

Related topics

• Gravimetric Analysis
• Percent Composition Formula
• Uncertainty In Measurement
• Law of Equivalence
• Some Basic Concept in Chemistry Formula

How do you prepare for States of matter?

• This chapter is the beginning of chemistry. This chapter is one of the most important chapters of the complete chemistry syllabus. Its concepts, laws, numerical, and graphs all are important both for the basic foundation of chemistry and for scoring good marks in the examination.
• Read this chapter carefully, as it has all the basic concepts like the mole concept, stoichiometry, molarity, normality, etc.
• This chapter is the foundation stone of the whole of the chemistry syllabus.
• Rest this chapter is very simple, just be regular and be consistent in your numerical practice.

Real-life application based on Some Basic Concepts in Chemistry

• In cooking, it is always necessary to know the exact amount of ingredients to be add in the food to get the best and tasty dish. This calculation of ingredients in stoichiometry.
  
• Saturn planet is much larger than earth but still, it is less dense. The specific gravity of Saturn is even less than 1.
  
• The GPS system that we use for finding out the way is related to stoichiometry. All these signals come from satellites. The stoichiometry helps to calculate the fuel and its components of reactions in the complete journey of satellites.
  
  
  

Prescribed Books for the States of Matter

First, you must finish the class XI NCERT textbook and solve each and every example and unsolved question given in it. Then for advanced level preparation like JEE and NEET, you must follow R.C. Mukherjee and O.P. Tandon. You must definitely solve the previous year papers. Meanwhile, in the preparation, you must continuously write the mock tests for the depth of knowledge. Our platform will help you to provide with the variety of questions for deeper knowledge with the help of videos, articles and mock tests.

Also read,

• Difference Between Compound and Mixture
• Law Constant Proportion
• Precipitation Reaction
• Chemical Reactions
• Types of Chemical Reactions
• Physical Change Chemical Change
• Laws of Chemical Combination for Elements and Compounds

Recommended topic video on (Some Basic Concepts of Chemistry)

Some Solved Examples

Example 1:

A sample of KCl is placed in 50 ml of solvent. What should be the mass (in gm) of the sample for the molarity to be 2M ?

1) (correct) 7.45

2) 7.81

3) 6.81

4) 7

Solution

Number of Moles = molarity x volume

= 2 x 0.05 = 0.1

So, mass = (39 + 35.5) x 0.01g = 7.45 g

Hence, the answer is an option (1).

Example 2:

The amount (in g) of sugar (C₁₂H₂₂O₁₁) required to prepare 2L of its 0.1 M aqueous solution is:

1) 17.1

2) (correct) 68.4

3) 136.8

4) 34.2

Solution

Molarity -Molarity (M) = (Number of moles of solute)/(volume of solution in litres)

It is defined as the number of moles of the solute in 1 litre of the solution.

As we have learned in the mole concept.

The formula of molarity =(n)solute Vsolution ( in lit )

0.1=wt3422

wt(C₁₂H₂₂O₁₁) = 68.4 gram

Hence, the answer is the option (2).

Example 3:

Calculate the molality of a solution containing of Acetic acid in Ethanol if the mass of solute = 10g and the density of Ethanol = 0.789 gmL^-1.

1) 0.2112

2) 0.2012

3) 0.1992

4) 0.2002

Solution

We know.

Molality (m) = (number of moles of solute)/(mass of solvent in kg)

Now,

Moles of solute Acetic acid = mass / molar mass

=1060 moles

If Volume of ethanol = 1 L

Formula, Density = mass/volume

So,

Weight of ethanol = 1000 x 0.789 = 789g = 0.789 Kg

Molality = mass of solute mass of solution in kg Molality =1060×7891000=0.2112 m/kg

Hence, the answer is (0.2112 m/kg).