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CBSE Worksheets for Class 10 Chemistry

CBSE Worksheets for Class 10 Chemistry: One of the best teaching strategies employed in most classrooms today is Worksheets. CBSE Class 10 Chemistry Worksheet for students has been used by teachers & students to develop logical, lingual, analytical, and problem-solving capabilities. So in order to help you with that, we at WorksheetsBuddy have come up with Kendriya Vidyalaya Class 10 Chemistry Worksheets for the students of Class 10. All our CBSE NCERT Class 10 Chemistry practice worksheets are designed for helping students to understand various topics, practice skills and improve their subject knowledge which in turn helps students to improve their academic performance. These chapter wise test papers for Class 10 Chemistry will be useful to test your conceptual understanding.

Board: Central Board of Secondary Education(www.cbse.nic.in) Subject: Class 10 Chemistry Number of Worksheets: 25

CBSE Class 10 Chemistry Worksheets PDF

All the CBSE Worksheets for Class 10 Chemistry provided in this page are provided for free which can be downloaded by students, teachers as well as by parents. We have covered all the Class 10 Chemistry important questions and answers in the worksheets which are included in CBSE NCERT Syllabus. Just click on the following link and download the CBSE Class 10 Chemistry Worksheet. CBSE Worksheets for Class 10 Chemistry can also use like assignments for Class 10 Chemistry students.

• CBSE Worksheets for Class 10 Chemistry Acids, Bases And Salts Assignment 1
• CBSE Worksheets for Class 10 Chemistry Acids, Bases And Salts Assignment 2
• CBSE Worksheets for Class 10 Chemistry All Chapters Assignment
• CBSE Worksheets for Class 10 Chemistry Carbon And Its Compound Assignment
• CBSE Worksheets for Class 10 Chemistry Carbon And Its Compounds Assignment
• CBSE Worksheets for Class 10 Chemistry Chemical Reactions And Equations Assignment 1
• CBSE Worksheets for Class 10 Chemistry Chemical Reactions And Equations Assignment 2
• CBSE Worksheets for Class 10 Chemistry Chemical Reactions And Equations Assignment 3
• CBSE Worksheets for Class 10 Chemistry Metals And Non-Metals Assignment 1
• CBSE Worksheets for Class 10 Chemistry Metals And Non-Metals Assignment 2
• CBSE Worksheets for Class 10 Chemistry Periodic Classification of element Assignment 1
• CBSE Worksheets for Class 10 Chemistry Periodic Classification of element Assignment 2
• CBSE Worksheets for Class 10 Chemistry Metals and Non-Metals
• CBSE Worksheets for Class 10 Chemistry SA1 Assignment 1
• CBSE Worksheets for Class 10 Chemistry SA2 Assignment 2
• CBSE Worksheets for Class 10 Chemistry Assignment 1
• CBSE Worksheets for Class 10 Chemistry Assignment 2
• CBSE Worksheets for Class 10 Chemistry Assignment 3
• CBSE Worksheets for Class 10 Chemistry Assignment 4
• CBSE Worksheets for Class 10 Chemistry Assignment 5
• CBSE Worksheets for Class 10 Chemistry Assignment 6
• CBSE Worksheets for Class 10 Chemistry Assignment 7
• CBSE Worksheets for Class 10 Chemistry Assignment 8
• CBSE Worksheets for Class 10 Chemistry Assignment 9
• CBSE Worksheets for Class 10 Chemistry Assignment 10
• CBSE Worksheets for Class 10 Chemistry Assignment 11

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• CBSE Class 10 Chemistry Workbook Helps to improve subject-knowledge.
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Worksheets of CBSE Class 10 Chemistry are devised by experts of WorksheetsBuddy experts who have great experience and expertise in teaching Maths. So practising these worksheets will promote students problem-solving skills and subject knowledge in an interactive method. Students can also download CBSE Class 10 Chemistry Chapter wise question bank pdf and access it anytime, anywhere for free. Browse further to download free CBSE Class 10 Chemistry Worksheets PDF .

Now that you are provided all the necessary information regarding CBSE Class 10 Chemistry Worksheet and we hope this detailed article is helpful. So Students who are preparing for the exams must need to have great solving skills. And in order to have these skills, one must practice enough of Class 10 Chemistry revision worksheets . And more importantly, students should need to follow through the worksheets after completing their syllabus.  Working on CBSE Class 10 Chemistry Worksheets will be a great help to secure good marks in the examination. So start working on Class 10 Chemistry Worksheets to secure good score.

CBSE Worksheets For Class 10

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10 Classs Chemistry Assignment Solution 2022 – 5th Week

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CBSE Class 10 Chemistry – Study Notes Chapter Wise

CBSE Class 10  Science CBSE Class 10 Social Science CBSE Class 10 Maths

CBSE Class 10  Chemistry Study Materials All Chapters

• Chemical Reactions and Equations
• Acid, Base and Salt
• Metal And Non Metal
• Carbon and It’s Compound
• Periodic Classification Of Elements

Course Overview

Cbse class 10  chemistry syllabus.

Best Reference Books CBSE Class 10 For  Science: –  Chemistry

• Science for 10th Class: Chemistry by Lakhmir Singh and Manjit Kaur

Chemistry: CBSE Class 10 Chemistry, Notes ,Test Papers, Sample Papers, NCERT, NCERT Exemplar and Lakhmir Singh Solution and Help from Ex- IITian for Chemistry

Ncert solutions for class 10 chemistry.

Get 100 percent accurate NCERT Solutions for Class 10 Chemistry  explained by expert Chemistry teachers. We provide step by step solutions for the questions given in Class 10 Chemistry textbook as per CBSE Board guidelines from the latest NCERT book for Class 10 Chemistry.

CBSE Class 10 Chemistry  Notes

Get Notes prepared by Ex-IITIan for CBSE Class 10 Chemistry

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Past Many Years Question Papers Solutions for Class 10 Chemistry are provided here with simple step-by-step explanations. These solutions for are extremely popular among class 10 students for Chemistry . Solutions come handy for quickly completing your homework and preparing for exams. All questions and answers from the Past Many Years Question Papers Book of class 10 Chemistry are provided here for . I will help you online for any doubt / clarification.

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Class 10 Chemistry (India)

Welcome to class 10 chemistry (cbse syllabus), unit 1: chemical reactions and equations, unit 2: acids, bases, and salts, unit 3: metals and non metals, unit 4: carbon and its compounds, unit 5: periodic classification of elements.

CBSE NCERT Solutions

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Assignments For Class 10 Chemistry

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NCERT Solutions for Class 10 Science Chapter 1 - Chemical Reactions and Equations

• NCERT Solutions
• Chapter 1 Chemical Reactions And Equations

NCERT Class 10 Science Chapter 1 - Chemical Reactions and Equations FREE PDF Download

Vedantu’s NCERT Solutions for Class 10 Chemistry Chapter 1 - Chemical Reactions and Equations solves all the questions in the chapter. This chapter delves into the fascinating world of chemical reactions, helping students understand and master the principles of balancing chemical equations and different types of reactions. Students gain comprehensive insights into these fundamental concepts by accessing the Science Class 10 Chapter 1 PDF. Vedantu provides straightforward and detailed answers, making it easier for students to grasp complex concepts and processes in chemical reactions.

Download our NCERT Solutions for Class 10 Science Chapter 1 - Chemical Reactions And Equations, which is revised based on the Class 10 Science syllabus . Get started with Vedantu’s NCERT Solutions for Chapter 1 to embark on a journey of academic excellence. 

Quick Insights of Chemical Reactions And Equations NCERT Solutions for Class 10 Science

Gain a comprehensive overview of chemical reactions and their significance in everyday life.

Learn the crucial skill of balancing chemical equations, which is fundamental for understanding chemical processes.

Chapter 1 Science Class 10 explores various chemical reactions, including combination, decomposition, displacement, and double displacement reactions.

NCERT Solutions for Class 10 Science Chapter 1 comprehensively covers all questions from the chapter and ensures thorough exam preparation .

Class 10 Science Chapter 1 Question Answer will help to develop proficiency in solving numerical problems related to chemical equations and reactions, enhancing problem-solving skills.

To reinforce learning, Vedantu provides additional resources such as class notes, important concepts, formulas, and exemplar solutions.

Access NCERT Solutions for Class 10 Science Chapter 1: Chemical Reactions and Equations

Intext Exercise 1

1. Why should a magnesium ribbon be cleaned before burning in air?

Ans: Magnesium is a reactive metal. It will react with oxygen and form a white layer of magnesium oxide (MgO) on its surface. Magnesium oxide is a stable compound and will prevent the further reaction of the metal. So, a magnesium ribbon is cleaned before burning in air to remove the layer of magnesium oxide from its surface.

2. Write the balanced equation for the following chemical reactions.

i) Hydrogen + Chlorine $\to $ Hydrogen chloride

Ans: A balanced equation consists of the same number of moles on the reactants and the products side. The balanced equation for the given reaction is:${{H}_{2(g)}}+C{{l}_{2(g)}}\to 2HC{{l}_{(g)}}$

ii) Barium chloride + Aluminium sulphate $\to $ Barium sulphate + Aluminium chloride

Ans: A balanced equation consists of the same number of moles on the reactants and the products side. The balanced equation for the given reaction is:$3BaC{{l}_{2(s)}}+A{{l}_{2}}{{(S{{O}_{4}})}_{3(s)}}\to 3BaS{{O}_{4(s)}}+2AlC{{l}_{3(s)}}$

iii) Sodium + Water $\to $ Sodium hydroxide + Hydrogen 

A balanced equation consists of the same number of moles on the reactants and the products side. The balanced equations for the given reaction is $2N{{a}_{(s)}}+2{{H}_{2}}{{O}_{(l)}}\to 2NaO{{H}_{(aq)}}+{{H}_{2}}_{(g)}$ 

3. Write a balanced chemical equation with state symbols for the following reactions.

i) Solutions of barium chloride and sodium sulphate in water react to give insoluble barium sulphate and the solution of sodium chloride.

Ans: A balanced chemical equation has the same number of moles of reactants and products. The balanced chemical equation is:$BaC{{l}_{2(aq)}}+N{{a}_{2}}S{{O}_{4(aq)}}\to BaS{{O}_{4(s)}}+2NaC{{l}_{(aq)}}$ 

ii) Sodium hydroxide solution (in water) reacts with hydrochloric acid solution (in water) to produce sodium chloride solution and water.

Ans: A balanced chemical equation has the same number of moles of reactants and products. The balanced chemical equation is:$NaO{{H}_{(aq)}}+HC{{l}_{(aq)}}\to NaC{{l}_{(aq)}}+{{H}_{2}}{{O}_{(l)}}$ 

Intext Exercise 2

1. A solution of a substance 'X ' is used for white washing.

i) Name the substance 'X' and write its formula.

Ans: Substance ‘X’ is calcium oxide also known as quicklime that is used in white washing. Its chemical formula is CaO.

ii) Write the reaction of the substance 'X' named in (i) above with water. 

Ans: Calcium oxide reacts with water in a combination reaction to from calcium hydroxide also called slaked lime, the reaction is:

$Ca{{O}_{(s)}}+{{H}_{2}}{{O}_{(l)}}\to Ca{{(OH)}_{2(aq)}}$ 

2. Why is the amount of gas collected in one of the test tubes in Activity 1.7 double of the amount collected in the other? Name this gas. 

Water consists of hydrogen and oxygen atoms. It is a combination of two hydrogen and one oxygen atom. In electrolysis, hydrogen moves towards the cathode and oxygen towards the anode. So, the ratio of hydrogen and oxygen is 2:1. And hydrogen is double the amount of oxygen. 

$2{{H}_{2}}O\to 2{{H}_{2}}+{{O}_{2}}$ 

Intext Exercise 3

1. Why does the color of copper sulphate solution change when an iron nail is dipped in it?

When an iron nail is dipped in a solution of copper sulphate, then the more reactive metal displaces the less reactive metal. As a result the blue solution of copper sulphate gets faded and forms a green compound known as ferrous sulphate.

\[\underset{\text{Iron}}{\mathop{F{{e}_{(s)}}}}\,+\underset{\begin{smallmatrix}\text{ Copper sulphate } \\ (\text{Blue}) \end{smallmatrix}}{\mathop{CuS{{O}_{4(aq)}}}}\,\to \underset{\text{Ferrous sulphate}}{\mathop{FeS{{O}_{4(aq)}}}}\,+\underset{\begin{smallmatrix} \text {Copper} \\ (\text{Green}) \end{smallmatrix}}{\mathop{C{{u}_{(s)}}}}\,\]  

2. Give an example of a double displacement reaction other than the one given in Activity 1.10. 

A double displacement reaction consists of two ions replacing each other’s position from the reactants to form new compounds in the products. A double displacement reaction occurs when Potassium iodide reacts with lead nitrate to form lead iodide (yellow precipitate) and potassium nitrate. 

\[2KI+Pb{{(N{{O}_{3}})}_{2}}\to Pb{{I}_{2}}\downarrow +2KN{{O}_{3}}\] 

3. Identify the substances that are oxidised and the substances that are reduced in the following reactions

i) $\text{4N}{{\text{a}}_{\text{(s)}}}\text{+}{{\text{O}}_{\text{2(g)}}}\to \text{2N}{{\text{a}}_{\text{2}}}{{\text{O}}_{\text{(s)}}}$ 

Ans: Any species is said to be oxidised when it loses electrons and increases the oxidation state, while any species is said to be reduced when it gains electrons and decreases the oxidation state. Sodium (Na) is oxidised and oxygen gets reduced.

\[4\text{Na}+{{\text{O}}_{2}}\to 2\text{N}{{\text{a}}_{2}}\text{O}\] 

ii) $\text{Cu}{{\text{O}}_{\text{(s)}}}\text{+}{{\text{H}}_{\text{2(g)}}}\to \text{Cu(s)+}{{\text{H}}_{\text{2}}}{{\text{O}}_{\text{(l)}}}$ 

Ans: Any species is said to be oxidised when it loses electrons and increases the oxidation state, while any species is said to be reduced when it gains electrons and decreases the oxidation state. Copper oxide (CuO) is reduced to copper (Cu) as it loses oxygen and hydrogen $\left( {{H}_{2}} \right)$is oxidized to water $({{H}_{2}}O)$ 

    \[CuO+{{H}_{2}}\xrightarrow{\Delta }Cu+{{H}_{2}}O\]  

NCERT exercises

1. Which of the statements about the reaction below are incorrect?

$\text{2Pb}{{\text{O}}_{\text{(s)}}}\text{+}{{\text{C}}_{\text{(s)}}}\to \text{2P}{{\text{b}}_{\text{(s)}}}\text{+C}{{\text{O}}_{\text{2(g)}}}$ 

a. Lead is getting reduced.

b. Carbon dioxide is getting oxidised.

c. Carbon is getting oxidised.

d. Lead oxide is getting reduced. 

i) (a) and (b)

ii) (a) and (c) 

iii) (a),(b) and (c)

Incorrect option is (i) (a) and (b)

Explanation :

(a) Oxygen is being removed

(b) The Oxygen removed from lead is transferred to the elemental Carbon.

2. $\text{F}{{\text{e}}_{\text{2}}}{{\text{O}}_{\text{3}}}\text{+2Al}\to \text{A}{{\text{l}}_{\text{2}}}{{\text{O}}_{\text{3}}}\text{+2Fe}$ 

The above reaction is an example of a _______________

 Options:

a) Combination reaction.

b) Double displacement reaction.

c) Decomposition reaction.

d) Displacement reaction.

  Ans:

(d) The given reaction is an example of a single displacement reaction.

Explanation : The oxygen from ferrous oxide is transferred to aluminum metal, forming aluminum oxide. In this reaction, aluminum, being more reactive than iron, displaces iron from its oxide. This process is known as a displacement reaction, where a more reactive element replaces a less reactive one.

3. What happens when dilute hydrochloric acid is added to iron filings? Tick the correct answer.

a. Hydrogen gas and iron chloride are produced.

b. Chlorine gas and iron hydroxide are produced.

c. No reaction takes place,

d. Iron salt and water are produced. 

(a) Hydrogen gas and iron chloride are produced. The reaction is as follows:

\[F{{e}_{(s)}}+2HC{{l}_{(aq)}}\to FeC{{l}_{2(aq)}}+{{H}_{2}}\uparrow \] 

4. What is a balanced chemical equation? Why should chemical equations be balanced? 

A balanced chemical equation consists of the equal number of moles of the elements in the reactants and that in the products.

Chemical equations should be balanced, as according to the law of conservation of mass, mass can neither be created nor can be destroyed. Therefore, in a chemical reaction, the total mass of reactant should be equal to the total mass of products. Hence, a balanced chemical equation has total mass of reactants equal to total mass of products.

5. Translate the following statements into chemical equations and then balance them.

a) Hydrogen gas combines with nitrogen to form ammonia.

Ans: $3{{H}_{2(g)}}+{{N}_{2(g)}}\to 2N{{H}_{3(g)}}$

b) Hydrogen sulphide gas burns in air to give water and sulphur dioxide.

Ans: $2{{H}_{2}}{{S}_{(g)}}+3{{O}_{2(g)}}\to 2{{H}_{2}}{{O}_{(l)}}+2S{{O}_{2(g)}}$

c) Barium chloride reacts with aluminium sulphate to give aluminium chloride and a precipitate of barium sulphate.

Ans: $3BaC{{l}_{2(aq)}}+A{{l}_{2}}{{(S{{O}_{4}})}_{3(aq)}}\to 2AlC{{l}_{3(aq)}}+3BaS{{O}_{4(s)}}$

d) Potassium metal reacts with water to give potassium hydroxide and hydrogen gas 

Ans: $2{{K}_{(s)}}+2{{H}_{2}}{{O}_{(l)}}\to 2KO{{H}_{(aq)}}+{{H}_{2(g)}}$

6. Balance the following chemical equations

a)$\text{HN}{{\text{O}}_{3}}+\text{Ca}{{(\text{OH})}_{2}}\to \text{Ca}{{\left( \text{N}{{\text{O}}_{3}} \right)}_{2}}+{{\text{H}}_{2}}\text{O}$ 

Ans: $2HN{{O}_{3}}+Ca{{(OH)}_{2}}\to Ca{{\left( N{{O}_{3}} \right)}_{2}}+2{{H}_{2}}O$

b)$\text{NaOH}+{{\text{H}}_{2}}\text{S}{{\text{O}}_{4}}\to \text{N}{{\text{a}}_{2}}\text{S}{{\text{O}}_{4}}+{{\text{H}}_{2}}\text{O}$ 

Ans: $2NaOH+{{H}_{2}}S{{O}_{4}}\to N{{a}_{2}}S{{O}_{4}}+2{{H}_{2}}O$

c)$\text{NaCl}+\text{AgN}{{\text{O}}_{3}}\to \text{AgCl}+\text{NaN}{{\text{O}}_{3}}$ 

Ans: \[NaCl+AgN{{O}_{3}}\to AgCl+NaN{{O}_{3}}\]

d)$\text{BaC}{{\text{l}}_{\text{2}}}\text{+}{{\text{H}}_{\text{2}}}\text{S}{{\text{O}}_{\text{4}}}\to \text{BaS}{{\text{O}}_{\text{4}}}\text{+HCl}$ 

Ans: $BaC{{l}_{2}}+{{H}_{2}}S{{O}_{4}}\to BaS{{O}_{4}}+2HCl$

7. Write the balanced chemical equations for the following reactions.

a) Calcium hydroxide + Carbon dioxide $\to $ Calcium carbonate + Water

Ans: $Ca{{(OH)}_{2}}+C{{O}_{2}}\to CaC{{O}_{3}}+{{H}_{2}}O $

b) Zinc + Silver nitrate $\to $Zinc nitrate +Silver

Ans: $Zn+2AgN{{O}_{3}}\to Zn{{\left( N{{O}_{3}} \right)}_{2}}+2Ag$

c) Aluminium + Copper chloride $\to $Aluminium chloride + Copper

Ans: $2Al+3CuC{{l}_{2}}\to 2AlC{{l}_{3}}+3Cu$

d) Barium chloride + Potassium sulphate$\to $Barium sulphate + Potassium chloride

Ans: $BaC{{l}_{2}}+{{K}_{2}}S{{O}_{4}}\to BaS{{O}_{4}}+2KCl$ 

8. Write the balanced chemical equation for the following and identify the type of reaction in each case.

a) Potassium bromide (aq) + Barium iodide (aq) $\to $Potassium iodide (aq) + Barium bromide(s)

Ans: $2KB{{r}_{(aq)}}+Ba{{I}_{2(aq)}}\to 2K{{I}_{(aq)}}+BaB{{r}_{2(aq)}}$ ; Double displacement reaction

b) Zinc carbonate (s) $\to $Zinc oxide (s) + Carbon dioxide (g)

Ans: $ZnC{{O}_{3(s)}}\to Zn{{O}_{(s)}}+C{{O}_{2(g)}}$ ; Decomposition reaction

c) Hydrogen (g)+ Chlorine (g)$\to $Hydrogen chloride (g)

Ans: ${{H}_{2(g)}}+C{{l}_{2(g)}}\to 2HC{{l}_{(g)}}$ ; Combination reaction

d) Magnesium (s) + Hydrochloric acid (aq) $\to $Magnesium chloride (aq) + Hydrogen (g) 

Ans: $M{{g}_{(s)}}+2HC{{l}_{(aq)}}\to MgC{{l}_{2}}_{(aq)}+{{H}_{2}}_{(g)}$ ; Single displacement reaction

9. What does one mean by exothermic and endothermic reactions? Give examples.  

Exothermic Reaction: The reactions in which heat is evolved along with the formation of new products are called exothermic reactions. In these reactions the energy of the reactants is more than that of the products, so energy is released to complete the reaction.

Energy of reactants > Energy of products

Example : Complete combustion of methane gas produces carbon dioxide and water along with heat and light.

\[C{{H}_{4}}(~g)+2{{O}_{2}}(~g)\to C{{O}_{2}}+2{{H}_{2}}O+heat+light\]

Another example of exothermic reactions is respiration and decomposition of vegetable matter.

Endothermic Reaction: The reactions in which energy is absorbed by the reactants to carry on the reaction are called endothermic reactions. In this type of reaction, the energy of the reactants is less than that of the products, so energy is needed and absorbed.

Energy of reactants <Energy of products

Example : Process of Photosynthesis, where plants absorb sunlight in the presence of carbon dioxide and water and make their food in the form of glucose and release oxygen.

\[6C{{O}_{2(g)}}+6{{H}_{2}}{{O}_{(l)}}\xrightarrow{sunlight}{{C}_{6}}{{H}_{12}}{{O}_{4(aq)\text{ }}}+6{{O}_{2(g)}}\] 

10. Why is respiration considered an exothermic reaction? Explain. 

Exothermic reactions are the reactions in which heat is going to be released. These reactions result in the formation of energy as the energy of reactants is greater than that of products. Respiration is the process in which the glucose from our body combines with oxygen in the cells to provide us with energy. The glucose is broken down through the process of digestion that along with oxygen provides us with energy and hence respiration is an exothermic reaction. The reaction that happens is as follows:

\[{{C}_{6}}{{H}_{12}}{{O}_{6(aq)}}+6{{O}_{2(g)}}\to 6C{{O}_{2(g)}}+6{{H}_{2}}{{O}_{(l)}}+energy\] 

11. Why are decomposition reactions called the opposite of combination reactions? Write equations for these reactions. 

A decomposition reaction consists of a single reactant that breaks down into two or more simpler products.

Example : Decomposition of calcium carbonate to give calcium oxide and carbon dioxide as,

\[CaC{{O}_{3}}+\text{ }Energy\text{ }\to CaO+C{{O}_{2}}\]

A combination reaction consists of two reactants that combine or mix together to form a single product.

Example : Combination of Calcium oxide and carbon dioxide to form one single product calcium carbonate

\[CaO+C{{O}_{2}}\to CaC{{O}_{3}}+\text{ }energy\text{ }\]

Hence, decomposition reactions are the opposite of combination reactions.

12. Write one equation each for decomposition reactions where energy is supplied in the form of heat, light or electricity.

Decomposition reactions are the reactions where a reactant breaks down into two or more products.

a) Decomposition by heat:

Ferrous sulphate decomposes to give ferrous oxide, sulphur dioxide and sulphur trioxide as,

\[2FeS{{O}_{4(s)}}\xrightarrow{\Delta }F{{e}_{2}}{{O}_{3(s)}}+S{{O}_{2(g)}}+S{{O}_{3(g)}}\]

b) Decomposition by light:

Silver chloride decomposes in light to form silver and chlorine as,

\[2AgC{{l}_{(s)}}\xrightarrow{Light}2A{{g}_{(s)}}+C{{l}_{2(g)}}\]

c) Decomposition by electricity:

Water decomposes in presence of electricity to form hydrogen and oxygen gases as,

\[2{{H}_{2}}O\xrightarrow{Electricity}2{{H}_{2}}+{{O}_{2}}\]

13. What is the difference between displacement and double displacement reactions? Write equations for these reactions.

A displacement reaction is a reaction in which a more reactive element displaces a less reactive element from its compound. The elements at the top in the activity series can replace the elements at the bottom. 

Example : Zinc is more reactive than copper and replaces copper from copper sulphate as:

\[CuS{{O}_{4(aq)}}+Z{{n}_{(s)}}\to ZnS{{O}_{4(aq)}}+C{{u}_{(s)}}\]

Double displacement reaction is the type of reaction where two compounds react in the way that there is exchange of positive and negative ions and new compounds are formed as products.

Example : On mixing sodium sulphate solution with barium chloride solution, a white precipitate of barium sulphate is formed as:

\[N{{a}_{2}}S{{O}_{4(aq)}}+BaC{{l}_{2(aq)}}\to BaS{{O}_{4(s)}}+2NaC{{l}_{(aq)}}\] 

14. In the refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal. Write down the reaction involved. 

The equation of recovery of silver from silver nitrate solution in silver refining is as follows:

\[2AgN{{O}_{3(aq)}}+C{{u}_{(s)}}\to Cu{{(N{{O}_{3}})}_{2(aq)}}+2A{{g}_{(s)}}\]

Here displacement of silver by copper happens as copper is more reactive than silver.

15. What do you mean by a precipitation reaction? Explain by giving examples. 

The type of reaction where an insoluble substance called a precipitate is formed when there is exchange of ions between the reactants is called a precipitation reaction.

Example 1 : On mixing sodium carbonate solution with calcium chloride solution, a white precipitate of calcium carbonate is formed.

\[N{{a}_{2}}C{{O}_{3(aq)}}+CaC{{l}_{2(aq)}}\to CaC{{O}_{3(s)}}\downarrow +2NaC{{l}_{(aq)}}\]

Example 2 : On mixing sodium sulphate solution with barium chloride solution, a white precipitate of barium sulphate is formed.

\[N{{a}_{2}}S{{O}_{4(aq)}}+BaC{{l}_{2(aq)}}\to BaS{{O}_{4(s)}}\downarrow +2NaC{{l}_{(aq)}}\]

16. Explain the following in terms of gain or loss of oxygen with two examples each.

a) Oxidation

Ans: Oxidation:  A type of reaction in which oxygen or an electronegative species is added to a substance or there is removal of hydrogen or a positive species from a substance is called oxidation.

For Example :

$C{{O}_{2}}+{{H}_{2}}\to CO+{{H}_{2}}O$ (Addition of oxygen to${{H}_{2}}$)

$2Cu+{{O}_{2}}\to 2CuO$ (Addition of oxygen to Cu)

b) Reduction 

Ans: Reduction: A type of reaction in which hydrogen or an electropositive species is added to a substance or oxygen or an electronegative species is removed, is called reduction.

$C{{O}_{2}}+{{H}_{2}}\to CO+{{H}_{2}}O$ (Oxygen is removed from$C{{O}_{2}}$)

$CuO+{{H}_{2}}\xrightarrow{\Delta }Cu+{{H}_{2}}O$ (Oxygen is removed from CuO)

17. A shiny brown-coloured element ‘X’ on heating in air becomes black in colour. Name the element ‘X’ and the black-coloured compound formed.

Copper (Cu) is ‘X’ and the black colour compound is copper (II) oxide (CuO). Copper reacts with oxygen to form a black colour compound called copper (II) oxide as: 

\[2Cu+{{O}_{2}}\to 2CuO\] 

18. Why do we apply paint on iron articles?

Iron is a reactive metal and can react with moisture and air. Iron articles, if exposed for a long time in moisture or air, can get corroded and form rust. So, paint is applied on iron articles to prevent rusting and form a protective layer for exposure to air and moisture.

19. Oil and fat containing food items are flushed with nitrogen. Why?

Oils and fat containing items are perishable and can be spoiled when exposed to oxygen. This is because oil and fats are reactive and can react with oxygen easily and get oxidised. To prevent oxidation, these items are flushed with nitrogen gas. Nitrogen is an inert gas and cannot react with oils or fats easily. So, food items with oils and fats are kept in packets having nitrogen gas that increases the shelf life and makes these items last for a long time.

20. Explain the following terms with one example each.

a) Corrosion

Ans: Corrosion: Corrosion is defined as a process where a substance, generally metal deteriorates and forms a layer of oxide on its surface. Metals get converted into their hydrated oxides or sulphides. Ex; Iron, Cu, Ag

\[4Fe+3{{O}_{2}}+n{{H}_{2}}O\to \underset{Hydrated\,iron\,oxide}{\mathop{2F{{e}_{2}}{{O}_{3}}.n{{H}_{2}}O}}\,$\]

\[2Ag+{{H}_{2}}~S\to A{{g}_{2}}~S+{{H}_{2}}\] 

b) Rancidity

Ans: Rancidity: It is a process in which food items like fats and oils are oxidised. This results in the change in taste and smell of the food item and is called rancidity. For example, when any fried food is exposed to air for a long time then it has a change in smell and taste and it becomes rancid.

Rancidity can be avoided by:

Adding antioxidants like BHA (Butylated tri hydroxy anisole)

Refrigerate the food items

keep food items in airtight containers

Adding nitrogen to food packets to prevent oxidation.

Science Chapter 1 Class 10 - Quick Overview on Chemical Reaction and Equations

Important Concepts Covered in Class 10 Science Chapter 1

Ch 1 Science Class 10 covers the following concepts which are very important from an exam point of view:

Types of Chemical Reactions:

Combination Reactions : Reactions where two or more substances combine to form a single product.

Decomposition Reactions : Reactions where a single compound breaks down into two or more simpler substances.

Displacement Reactions : Reactions where an element displaces another element from its compound. This includes:

Single Displacement Reactions : A more reactive element displaces a less reactive element from its compound.

Double Displacement Reactions : The ions of two compounds exchange places in an aqueous solution to form two new compounds.

Oxidation and Reduction Reactions : Understanding redox reactions, where oxidation involves electrons' loss and reduction involves electrons' gain.

Corrosion and Rancidity : Learning about the chemical processes involved in the corrosion of metals and rancidity of food, and methods to prevent them.

Benefits Referring NCERT Solutions for Class 10 Science Chapter 1 Chemical Reactions and Equations

Below are some of the benefits of Chapter 1 of Class 10 Science NCERT Solutions.

Students will get a clear idea of balancing various types of equations.

Chapter 1 Science Class 10   solutions make it easier for the students to formulate chemical equations.

To get more insights on Ch 1 Chemistry Class 10, Vedantu provides many practice questions of varying difficulty levels so that board examinations may be taken without worry.

Every question from ch 1 chemistry class 10 is explained in a step-by-step manner and these solutions are provided keeping in mind CBSE patterns.

Related Study Materials for Chemical Reaction and Equation Class 10

Students can also download additional study materials provided by Vedantu for Chemistry Class 10, Chapter 1 –

Class 10 Science Ch 1 , "Chemical Reactions and Equations," solutions are presented straightforwardly, containing all essential details to help students understand chemical reactions and equations. With completely revised solutions and critical points aligned with exam specifications, students can rely on these solutions for effective exam preparation. NCERT Class 10 Science Chapter 1 introduces numerous new concepts, making comprehending challenging. NCERT Solutions for Class 10 Science Chapter 1 are prepared by Vedantu's experts to provide students with an ideal resource for practice, enhancing the learning process and ultimately helping students achieve better exam marks.

Chapter-wise NCERT Solutions Class 10 Science

Related Links for Class 10 Science

FAQs on NCERT Solutions for Class 10 Science Chapter 1 - Chemical Reactions and Equations

1. Before burning a magnesium ribbon in the air, why should it be cleaned

Magnesium ribbon must be cleaned before burning in the air, so as to remove the layer of MgO formed due to the reaction between magnesium and air. 

2. Why not immediately a wall acquires a white colour when a coating of slaked lime is applied to it?

When a solution of slaked lime is applied on the wall, CO 2 gas present in the air slowly reacts with a thin layer of calcium hydroxide to form a thin layer of calcium carbonate, that is quite white. Therefore, the newly formed calcium carbonate impart a white look to the walls. 

Ca(OH) 2 (aq) + CO 2 (g) →  CaCO 3 (s) + H 2 O (l)

3. Consider the following reaction:

2FeSO 4 (s) → Fe 2 O 3 (s) + SO 2 (g) + SO 3 (g)

Is it a redox reaction or not? If yes, why?

It is a redox reaction because ferrous (Fe 3+ ) whereas SO 2- 4 is getting reduced to SO 2 .

4. Identify the oxidizing agent in the following equation.

MnO 2 (s) + 4HCL à MnCl 2 (aq) + Cl 2 (g) + 2H 2 O

MnO 2 is the oxidizing agent in the equation.

5. Why should students refer to NCERT Solutions provided by Vedantu?

NCERT Solutions provided by Vedantu is very comprehensive and developed in a step-by-step method that makes it self-explanatory. After extensive research and as per the latest syllabus and guidelines of NCERT, our subject-matter experts have designed the notes and the solutions for you to give a better understanding of the concept and they are easily accessible on the Vedantu’s official website. Our experienced teachers are available to clear all your doubts and strengthen your conceptual understanding. Students have shown drastic improvement in their overall performance by the solutions and the reference notes provided by Vedantu.

6. What is the chemical reaction and equations?

A chemical reaction is a process in which one or more substances react with one another and form a different substance known as a product. The product will usually have different physical and chemical properties compared to the reactants. An equation is a symbolic representation of this reaction using formulae, where reactants are on the left hand side and products on the right hand side.

7. What is a balanced chemical equation? Why should chemical equations be balanced?

A chemical equation is a symbolic representation of the entire chemical reaction. It consists of a left-hand side with all the reactants and a right hand side with the products. According to the law of conservation of mass, atoms can neither be created nor destroyed. To follow this universal law, the equation should be balanced so that the total atoms on the left side are equal to the atoms on the right side.

8. What is Chapter 1 of Class 10 Science?

Chapter 1 of NCERT Class 10 Science is Chemical Reactions and Equations. This is one of the basic chapters which is of great importance for building the foundation of Chemistry. It discusses important concepts like chemical formulae, equations reactions, writing a chemical equation, and balancing of chemical equations. These are very important topics that are covered in this chapter and are explained in depth in NCERT Solutions for Chapter 1 of Class 10  by  Vedantu .

9. List out the topics and subtopics covered in the NCERT Solutions for Chapter 1 of Class 10 Science.

Chapter 1 of Class 10 Science Chemical Reactions and equations is a very important chapter from an exam point of view and also for building up the basics of the subject. Some of the topics covered are:

Chemical reactions and equations

Chemical equations

Writing a chemical equation

Balanced chemical equation

Types of chemical reactions

Combination reaction

Decomposition reaction

Displacement reaction

Double displacement reaction

Oxidation and reduction

Have you observed the effects of oxidation reactions in everyday life?

10. How do solutions provided by Vedantu help in studying Chapter 1 of Class 10 Science?

Class 10 Science forms the building blocks of the basics of Science in Biology, Chemistry and Physics. Many important concepts and theories are covered in it. Therefore it is very important for students to understand these concepts and study the topics with a strong base. Vedantu has solutions for all the  important questions of Chapter 1 of Class 10 Science  explained in a very detailed yet simple manner so that the students can remember them for long. There are plenty of diagrams, graphs, flow charts and bullet point answers making the student’s work very easy. These solutions can be downloaded from the Vedantu app and from the Vedantu website at free of cost.

11. What are the important topics in class 10 ch 1 science?

The important topics in class 10 science ch 1 are as follows:

Chemical Equations

Types of Chemical Reactions

You can clear your concepts on the following topics with Vedantu’s NCERT Class 10 Science Chapter 1 and excel in your exams. Happy Learning with Vedantu!

12. What are some good questions for chemical reactions?

Some of the questions that can be asked from Chemistry Class 10 Chapter 1 are:

NCERT Solutions for Class 10 Science Chapter 1 provides all important questions for the examination.

13. What is important in a chemical reaction and equation?

Effects of Oxidation Reactions on Everyday Life

14. What are four types of chemical reactions according to NCERT Solutions Class 10 Science?

The four types of Chemical Reactions are:

NCERT Solutions for Class 10 Science

Ncert solutions for class 10.

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NCERT Books

NCERT Books for Class 10 Science PDF Download [2021 -22 Edition Revised Syllabus]

NCERT Books Class 10 Science : The National Council of Educational Research and Training (NCERT) publishes Science textbooks for Class 10. The NCERT Class 10th Science textbooks are well known for it’s updated and thoroughly revised syllabus. The NCERT Science Books are based on the latest exam pattern and CBSE syllabus.

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NCERT Class 10 Science Books in English PDF Download

NCERT Class 10 Science Books are provided in PDF form so that students can access it at any time anywhere. Class 10 NCERT Science Books are created by the best professors who are experts in Science and have good knowledge in the subject.

NCERT Books for Class 10 Science – English Medium

NCERT books Class 10 Science PDF (chapter-wise) in English, Hindi (Vigyan), and Urdu are provided as under:

• Class 10 Science NCERT Book PDF Download
• Class 10 Science NCERT Book Introduction
• Chapter 1: Chemical Reactions and Equations

NCERT Solutions for class 10 Science

• Chapter 2: Acids, Bases and Salts
• Chapter 3: Metals and Non-Metals
• Chapter 4: Carbon and its Compounds
• Chapter 5: Periodic Classification of Elements
• Chapter 6: Life Processes
• Chapter 7: Control and Coordination
• Chapter 8: How do Organisms Reproduce?
• Chapter 9: Heredity and Evolution
• Chapter 10: Light – Reflection and Refraction
• Chapter 11: Human Eye and Colourful World
• Chapter 12: Electricity
• Chapter 13: Magnetic Effects of Electric Current
• Chapter 14: Sources of Energy
• Chapter 15: Our Environment
• Chapter 16: Management of Natural Resources
• Class 10 NCERT Science Book Answers

NCERT Books for Class 10 Science – Hindi Medium

• Class 10 Science NCERT Book in Hindi PDF Download
• Class 10 Science NCERT Book in Hindi Introduction
• पाठ 1: रासायनिक अभिक्रियाएं एवं समीकरण
• पाठ 2: अम्ल, क्षारक एवं लवण
• पाठ 3: धातु एवं अधातु
• पाठ 4: कार्बन एवं उसके यौगिक
• पाठ 5: तत्वों का आवर्त वर्गीकरण
• पाठ 6: जैव प्रक्रम
• पाठ 7: नियंत्रण एवं समन्वय
• पाठ 8: जीव जनन कैसे करते हैं?
• पाठ 9: आनुवंशिकता एवं जैव विकास
• पाठ 10: प्रकाश – परावर्तन तथा अपवर्तन
• पाठ 11: मानव नेत्र तथा रंगबिरंगा संसार
• पाठ 12: विधुत
• पाठ 13: विधुत धरा के चुंबकीय प्रभाव
• पाठ 14: ऊर्जा के स्रोत
• पाठ 15: हमारा पर्यावरण
• पाठ 16: प्राकृतिक संसाधनों का प्रबंधन
• Class 10 Science NCERT Book in Hindi Answers

The NCERT syllabus mainly focuses on this book to make it student-friendly to make it useful for both the students and the competitive exam aspirants. The book covers a detailed Science based on the syllabuses of various boards. NCERT Science Books for Class 10 is perfectly compatible with almost every Indian education state and central boards.

We hope that this detailed article on NCERT Books Class 10 Science helps you in your preparation and you crack the Class 10 exams or competitive exams with excellent scores.

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NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12

NCERT Solutions for Class 10 Science Chapter 5 Periodic Classification of Elements

April 19, 2023 by Veerendra

NCERT Solutions For Class 10 Science Chapter 5 Periodic Classification Of Elements : Students who are in search for periodic classification of elements class 10 question and answers can refer to this article. Working on NCERT Solutions for  class 10 science chapter 5 notes will help candidates to build a strong foundation over the subject Science. NCERT Solutions For Class 10 Science Chapter 5 Periodic Classification Of Elements will further help in clearing the UG competitive exams.

Going through this  periodic classification of elements class 10 NCERT activity solutions will help candidates to understand the theory behind every concept which in turn helps candidates to solve the questions at the end of every topics and subtopic. Read on to find everything about the periodic classification of elements class 10 question and answers.

Before getting into the details of  NCERT Solutions For Class 10 Science Chapter 5 Periodic Classification Of Elements, let’s have an overview of topics & subtopics under NCERT Solutions for class 10 science chapter 5 notes:

• Periodic Classification Of Elements
• Making Order Out Of Chaos – Early Attempts At The Classification Of Elements
• Making Order Out Of Chaos – Mendeléev’S Periodic Table
• Making Order Out Of Chaos – The Modern Periodic Table

Free download NCERT Solutions for Class 10 Science Chapter 5 Periodic Classification Of Elements PDF in Hindi Medium as well as in English Medium for CBSE, Uttarakhand, Bihar, MP Board, Gujarat Board, and UP Board students, who are using NCERT Books based on updated CBSE Syllabus for the session 2019-20.

• तत्वों के आवर्त वर्गीकरण कक्षा 10 विज्ञान हिंदी में
• Class 10 Periodic Classification of Elements Important Questions
• Periodic Classification of Elements Class 10 Notes
• Periodic Classification of Elements NCERT Exemplar Solutions
• Periodic Classification of Elements Class 10 Extra Questions
• Class 10 Periodic Classification of Elements Mind Map

NCERT Solutions for Class 10 Science Chapter 5 Intext Questions

Page Number: 81

Question 1 Did Dobereiner’s triads also exist in the columns of Newlands’ Octaves ? Compare and find out. Answer: Yes, Dobereiner’s triads also existed in the columns of Newland’s Octaves. For example, Li, Na, K. If we consider lithium (Li) as the first element, then sodium (Na) is eighth element. If we consider sodium as the first element, then potassium is the eighth element.

Question 2 What were the limitations of Dobereiner’s classification ? Answer: It failed to arrange all the then known elements in the form of triads of elements having similar chemical properties. Dobereiner could identify only three triads from the elements known that time.

Question 3 What were the limitations of Newlands’ law of octaves ? Answer: (i) Newlands law of octaves was applicable to the classification of elements upto calcium only. After calcium every eighth element did not possess the properties similar to that of the first element. (ii) Newlands assumed that only 56 elements existed in nature and no more elements would be discovered in the future. But later on, several new elements were discovered whose properties did not fit into Newlands’ law of Octaves. (iii) In order to fit elements into his table, Newlands put even two elements together in one slot and that too in the column of unlike elements having very different properties. For example, the two elements cobalt (Co) and nickel (Ni) were put together in just one slot and that too in the column of elements like fluorine, chlorine and bromine which have very different properties from these elements. (iv) Iron (Fe) element which resemble elements like cobalt and nickel in properties, was placed far away from these elements.

Page Number: 85

Question 1 Use Mendeleev’s Periodic Table to predict the formulae for the oxides of the following elements : K, C, Al, Si, Ba Answer: K 2 O, CO 2 , Al 2 O 3 , SiO 2 , BaO.

Question 2 Besides gallium, which other elements have since been discovered that were left by Mendeleev in his periodic table ? (any two) Answer: Scandium and Germanium.

Question 3 What were the criteria used by Mendeleev in creating his Periodic Table ? Answer: Mendeleev used the relationship between the atomic masses of the elements and their physical and chemical properties. He used similarity in physical properties, similarity in the formation of hydrides and oxides of element.

Question 4 Why do you think the noble gases are placed in a separate group ? Answer: Noble gases are chemically inert and are present in atmosphere in extremely low concentrations. Therefore, owing to their similar inert behaviour and similar electronic configuration, they are justified to be placed in a separate group.

Page Number: 90

Question 1 How could the modern periodic table remove various anomalies of Mendeleev’s periodic Table ? Answer: (i) The modern periodic table is based on atomic number, while Mendeleev’s periodic table was based on atomic mass. (ii) The isotopes of an element have same number of protons (or atomic number). So they are alloted the same position in modern periodic table. (iii) Cobalt and nickel are placed at 9th and 10th position respectively. (iv) Hydrogen has been alloted special position, i.e., it is placed at the top of alkali metals in the first group.

Question 2 Name two elements you would expect to show chemical reactions similar to magnesium. What is the basis for your choice ? Answer: Beryllium (Be) and Calcium (Ca). Both Be (atomic number 4) and Ca (atomic number 20) have similar electronic configuration, i.e. two electrons in outermost shells. Be               2,2 Ca             2, 8, 8, 2 Both Be and Ca react with oxygen to give basic oxides, BeO and MgO.

Question 3 Name : (a) three elements that have a single electron in their outermost shells. (b) two elements that have two electrons in their outermost shells. (c) three elements with filled outer most shells. Answer: (a) Lithium : Atomic number – 3(2, 1); Sodium : Atomic number – 11(2, 8, 1); Potassium : Atomic number – 19(2, 8, 8, 1). (b) Beryllium : Atomic number – 4(2, 2); Calcium : Atomic number – 20(2, 8, 8, 2) (c) Helium : Atomic number – 2(2); Neon : Atomic number – 10(2, 8); Argon : Atomic number – 18(2, 8, 8).

Question 4 (a) Lithium, sodium, potassium are all metals that react with water to liberate hydrogen gas. Is there any similarity in the atoms of these elements ? (b) Helium is an unreactive gas and neon is a gas of extremely low reactivity. What, if anything, do their atoms have in common ? Answer: (a) Lithium, sodium and potassium all belong to the same group. The atoms of lithium, sodium and potassium all have only one electron in their outermost shells and all of these are metals. All of these react with water to form alkalies. (b) The atoms of helium and neon have their outermost shells completely filled. Helium has its first shell completely filled, while neon has its first and second shells (K and L) completely filled.

Question 5 In the modern periodic table, which are the metals among the first ten elements ? Answer: The first ten elements in modern periodic table are hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine and neon. Out of these, lithium, beryllium and boron are metals, because they have 1, 2 and 3 electrons respectively in their outermost shells.

Question 6 By considering their position in the Periodic Table, which one of the following elements would you expect to have maximum metallic characteristics ? Ga, Ge, As, Se, Be Answer: Beryllium (Be). In the periodic table, the elements placed on the left show maximum metallic characteristics. Since beryllium occupies the most left position in comparison to other elements, hence it shows maximum metallic characteristics.

NCERT Solutions for Class 10 Science Chapter 5 Textbook Chapter End Questions

Question 1 Which of the following statements is not a correct statement about the trends wlien going from left to right across the periods of Periodic Table. (a) The elements become less metallic in nature. (b) The number of valence electrons increases. (c) The atoms lose their electrons more easily. (d) The oxides become more acidic. Answer: (c) The atoms lose their .electrons more easily.

Question 2 Element X forms a chloride with the formula XCl 2 , which is solid with a high melting point. X would most likely to be in the same group of the periodic table as (a) Na (b) Mg (c) Al (d) Si Answer: (b) Mg

Question 3 Which element has (a) two shells, both of which are completely filled with electrons ? (b) the electronic configuration 2, 8, 2 ? (c) a total of three shells, with four electrons in its valence shell ? (d) a total of two shells with three electrons in its valence shell. v (e) twice as many electrons in its second shell as in its first shell ? Answer: (a) Neon (2, 8) (b) Magnesium (c) Silicon (2, 8, 4) (d) Boron (2, 3) (e) Carbon (2, 4)

Question 4 (a) What property do all elements in the same column of the Periodic Table as boron have in common ? (b) What property do all elements in the same column of the Periodic Table . as fluorine have in common ? Answer: (a) Elements in the same column or group as boron have valency of three and have three valence electrons. (b) Elements in the same column or group as fluorine form acidic oxides and have seven electrons in their outermost shells and have valency of one.

Question 5 An atom has electronic configuration 2, 8, 7. (a) What is the atomic number of this element ? (b) To which of the following elements would it be chemically similar ? (Atomic numbers are given in parentheses.) N (7), F (9), P (15), Ar (18) Answer: (a) The atomic number of the given element is 2 + 8 + 7(= 17). (b) It would be chemically similar to fluorine [F(9)] because its electronic configuration is 2, 7.

Question 6 The positions of three elements A, B and C in the periodic table are shown below : (a) State whether A is a metal or non-metal.

(b) State whether C is more reactive or less reactive than A. (c) Will C be larger or smaller in size than B ? (d) Which type of ion, cation or anion, will be formed by element A ? Answer: (a) Since the valency of group 17 elements is 1 and all these elements accept electrons, thus A is a non-metal. (b) C is less reactive than A because as we move down in a group, the reactivity of non-metals increases. (c) C is smaller in size than B because B and C both are related to the same period and the size decreases as one moves from left to right in a period. (d) A will form anion because it is a non-metal.

Question 7 Nitrogen (atomic number 7) and phosphorus (atomic number 15) belong to group 15 of the periodic table. Write the electronic configuration of these two elements. Which of these will be more electronegative ? Why ? Answer: Electronic configuration of nitrogen -2,5 Electronic configuration of phosphorus = 2, 8, 5 Nitrogen will be more electronegative because outermost shell is nearer to nucleus and therefore nucleus will attract electrons more strongly. In a group of the periodic table, electron attracting tendency decreases as we move from top to bottom.

Question 8 How does the electronic configuration of an atom relate to its position in the Modern Periodic Table ? Answer: Modern periodic table is based on the atomic number and atomic number is directly related to the electronic configuration. One can find the group number and period number of an element on the basis of electronic configuration. For example, if an element has 1 or 2 electrons in its outermost shell, then it would belong to group 1 or group 2. And if it has 3 or more electrons in its outermost shell, then it would belong to group 10 4- the number of electrons in the outermost shell.

All the alkali metals have one electron in their outermost shell, so they are placed in group 1. Thus, all the group 2 elements have 2 electrons in their outermost shell. In group 15 elements, there are 5 electrons in their outermost shell. Similarly, the number of shells in an element indicates its period number. For example, the atomic number of magnesium is 12 and its electronic configuration is 2, 8, 2. Thus it is an element of 3rd period.

Question 9 In the Modern Periodic Table, calcium (atomic number 20) is surrounded by elements with atomic number 12, 19, 21 and 38. Which of these have physical and chemical properties resembling calcium ? Answer: The electronic configuration of elements with : Atomic number 12 = 2, 8, 2 Atomic number 19 = 2, 8, 8, 1 Atomic number 20 = 2, 8, 8, 2 Atomic number 21 = 2, 8, 9, 2 Atomic number 38 = 2, 8, 18, 8, 2 Elements with atomic number 12 i.e., magnesium (Mg) and 38 i.e., strontium (Sr) will have similar physical and chemical properties as element with atomic numbers 20 i.e., calcium (Ca).

Question 10 Compare and contrast the arrangement of elements in Mendeleev’s Periodic Table and the Modern Periodic Table. Answer:

Periodic classification of elements: Needs for classification, Modern Periodic table, gradation in properties, valency, atomic number, metallic and non-metallic properties.

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Question 1 Did Dobereiner’s triads also exist in the columns of Newlands Octaves? Compare and find out. Solution: Yes, Dobereiner’s triads also exist in the columns of Newlands Octaves. For example, the second column of Newlands classification has the elements lithium (Li), sodium (Na) and Potassium (K), which constitute a Dobereiner’s triad.

Question 2 What were the limitations of Dobereiner’s classification? Solution: All the known elements could not be arranged in the form of triads. For very low mass or for very high mass elements, the Dobereiner’s triads are not applicable. Take the example of F, Cl and Br. Atomic mass of Cl is not an arithmetic mean of atomic masses of F and Br. As the techniques for measuring atomic masses accurately, improved, the Dobereiner’s triad was unable to remain strictly valid.

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Question 3 What were the limitations of Newland’s Law of Octaves? Solution: It was not valid for elements that had atomic masses higher than Ca.When more elements were discovered, such as elements from the noble gases such as He, Ne, Ar, they could not be accommodated in his table.

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Question 4 Use Mendeleev’s periodic table to predict the formulae for the oxides of the following elements: K, C, Al, Si, Ba. Solution: K 2 O – Potassium Oxide CaO – Calcium Oxide Al 2 O 3 – Aluminium Oxide SiO 2 – Silicon dioxide BaO – Barium Oxide.

Question 5 Besides gallium, which other elements have been left by Mendeleev in his periodic table, since the time they were discovered? (Any two) Solution: Scandium and Germanium.

Question 6 What were the criteria used by Mendeleev in creating his periodic table? Solution: He observed the relationship between the atomic masses of the elements and their physical properties. Among chemical properties, he concentrated on the compounds formed by elements with oxygen and hydrogen.

Question 7 Why do you think, the noble gases are placed in a separate group? Solution: Due to its inert and low concentration in our atmosphere, they could be placed in a new group without disturbing the existing order.

Question 8 How could the Modern periodic table remove various anomalies of Mendeleev’s periodic table? Solution: When the elements are arranged according to their atomic numbers on the basis of modern periodic law, all the anomalies (defects) of Mendeleev’s classification disappear. For example, Position of isotopes: All the isotopes of an element have the same number of protons, so their atomic number is also the same. Since all the isotopes of an element have the same atomic number, they can be put at one place in the same group of the periodic table.

Question 9 Name two elements, which you would expect to show chemical reactions similar to magnesium. What is the basis for your choice? Solution: Calcium and Beryllium are the elements that will show chemical reactions similar to magnesium. This is because beryllium and calcium belong to the same group of periodic table as magnesium. All of them have similar electronic configurations with 2 valence electrons each.

Question 10 Name: a. Three elements that have a single electron in their outermost shell.< b. Two elements that have two electrons in their outermost shell.< c. Three elements with filled outermost shell. Solution: a. Three elements that have a single electron in their outermost shell are: 1. Lithium 2. Sodium 3. Potassium b. Two elements that have two electrons in their outermost shell are: 1. Magnesium 2. Calcium c. Three elements with filled outermost shell are: 1. Argon 2. Helium 3. Neon.

Question 11 a. Lithium, sodium, potassium are metals that react with water to liberate hydrogen. Is there any similarity in the atoms of these elements? b. Helium is an unreactive gas and neon is a gas of extremely low reactivity. What, if anything, do their atoms have in common Solution: a. These elements are alkali metals and they have 1 valence electron in their outermost shell and are therefore very unstable and reactive. b. These elements each have full outermost subshell, which results in high stability. They only react with other elements in extreme circumstances, the trait for which they are named.

Question 12 In the Modern periodic table, which are the metals among the first ten elements? Solution: The metals are Lithium and Beryllium.

Question 13 By considering their position in the periodic table, which one of the following elements would you expect to have maximum metallic characteristic? Ga, Ge, As, Se, Be Solution: Beryllium

Question 14 Which of the following statements is not a correct statement about the trends when going from left to right across the periods of the periodic table?< (i)The elements become less metallic in nature (ii) The number of valence electrons increases (iii) The atoms lose their electrons more easily (iv) The oxides become more acidic Solution: (iii) The atoms lose their electrons more easily – Incorrect statement.

Question 15 Element X forms a chloride with the formula XCl 2 , which is a solid with a high melting point. X would most likely be in the same group of the periodic table as a. Na b. Mg c. Al d. Si Solution: b. Mg

Question 16 Which element has? a.Two shells, both of which are completely filled with electrons?< b. The electronic configuration of 2,8,2?< c. A total of three shells, with four electrons in its valence shell?< d. A total of two shells, with three electrons in its valence shell?< e. Twice as many electrons in its second shell, as in its first shell? Solution: a. Neon (2,8) b. Magnesium (2,8,2) c. Silicon (2,8,4) d. Boron (2,3) e. Carbon (2,4)

Question 17 What property do all elements in the same column of the periodic table as fluorine have in common? Solution: These elements all have 7 electrons in their outermost shells and these often exist as salts, combined with elements from the Alkali metal group.

Question 18 An atom has electronic configuration 2,8,7. i. What is the atomic number of this element? ii. To which of the following elements would it be chemically similar< N (7) F (9) P (15) Ar (18) Solution: (i) Chlorine – 17 (ii) F (9)

Question 19 Which type of ion, cation or anion, will be formed by element A? Solution: C is less reactive than A “C” will be smaller in size than “B” as the atomic size decreases as we go across a period. Anion will be formed by element A

Question 20 Nitrogen (atomic number 7) and phosphorus (atomic number 15) belong to group 15 of the periodic Table. Write the electronic configuration of these two elements. Which of these will be more electronegative? Why? Solution: Electronic configuration – Nitrogen – 2s 2 2p 3 and Phosphorus – 1s 2 2s 2 2p 6 3s 2 3p 3 . Nitrogen will be more electronegative; this is because its atom has small size due to which the attraction of its nucleus for the incoming electron is more.

Question 21 How does the electronic configuration of an atom relate to its position in the Modern periodic table? Solution: The electronic configuration of an atom increases in the outermost valence shell which relates to its position in the Modern periodic table.

Question 22 In the Modern periodic table, calcium (atomic number 20) is surrounded by elements with atomic numbers 12, 19, 21 and 38. Which of these have physical and chemical properties resembling calcium? Solution: The atomic number of calcium is 20, so its electronic configuration is 2, 8, 8, 2. Thus, calcium has 2 valence electrons (in its outermost shell). Now, the element which has 2 valence electrons, will have physical and chemical properties resembling to that of calcium. The electronic configuration of element having atomic number 12 is 2, 8, 2. It has 2 valence electrons just like calcium. So, the element having atomic number 12 will have physical and chemical properties resembling that of calcium.

Question 23 Where do you think should hydrogen be placed in the Modern periodic table? Solution: Hydrogen element has been placed at the top of group 1, above the alkali metals because the electronic configuration of hydrogen is similar to those of alkali metals.

Multiple Choice Questions (MCQs) [1 Mark each]

Question 1. Which of the following is the outermost shell for elements of 2nd period? [NCERT Exemplar] (a) K-shell (b) L-shell (c) M-shell (d) N-shell Answer: (b) The elements of 2nd period involve the filling of 2nd shell, i.e. Z-shell. Because in period 2, there are two shell, K and L

Question 2. An element which is an essential constituent of all organic compounds belongs to [NCERT Exemplar] (a) group 1 (b) group 14 (c) group 15 (d) group 16 Answer: (b) Constituent of all organic compounds is carbon. It belongs to group 14.

Question 3. Which one of the following elements exhibit maximum number of valence electrons? [NCERT Exemplar] (a) Na (b) Al (c) Si (d) P Answer: (d) Na (group 1) has one, A1 (group 13) has three (13 -10), Si (group 14) has four (14-10) and P (group 15) has five (15 – 10) valence electrons. Therefore, P has maximum number of valence electrons, i.e.3 (maximum among the given elements).

Question 4. Which of the given elements A, B, C, D and E with atomic number 2, 3, 7, 10 and 30 respectively belong to the same period? [NCERT Exemplar] (a) A, B, C (b) B, C, D (c) A, D, E (d) B, D, E Answer: (b) 2nd period contains elements with atomic number 3(Li), 7(N), 10(Ne). Since, 2nd period has elements having atomic number 3 to 10.

Question 5. The elements A, B, C, D and E have atomic number 9, 11, 17, 12 and 13 respectively. Which pair of elements belong to the same group? [NCERT Exemplar] (a) A and B (b) B and D (c) A and C (d) D and E Answer: (c)Electronic configuration of A (atomic number = 9) is 2, 7. Electronic configuration of B (atomic number = 11) is 2, 8,1. Electronic configuration of C (atomic number = 17) is 2, 8, 7. Electronic configuration of D (atomic number =12) is 2, 8, 2. Electronic configuration of E (atomic number =13) is 2, 8, 3. Elements which differ in atomic number by 8, i.e. 9 (A, fluorine) and 17 (C, chlorine) lie in the same group, i.e. group 17 (halogen).

Question 6. In Mendeleev’s periodic table, gaps were left for the elements to be discovered later. Which one of the following elements found a place in the periodic table later? [NCERT Exemplar] (a) Germanium (b) Chlorine (c) Oxygen (d) Silicon Answer: (a) Mendeleev’s left some gaps in the periodic table for those elements which were not known at that time. Germanium element found a place in the periodic table later and Mendeleev’s predictions were found to be remarkably correct

Question 7. Which of the following are the characteristics of isotopes of an element? [NCERT Exemplar] (i) Isotopes of an element have same atomic masses. (ii) Isotopes of an element have same atomic number. (iii) Isotopes of an element show same physical properties. (iv) Isotopes of an element show same chemical properties. (a) (i), (iii) and (iv) (b) (ii), (iii) and (iv) (c) (ii) and (iii) (d) (ii) and (iv) Answer: (d) Isotopes of an element have same atomic number and show same chemical properties.

Question 8. Which of the following elements would lose an electron easily? [NCERT Exemplar] (a) Mg (b) Na (c) K (d) Ca Answer: (c) Electronic configuration of Mg (atomic number = 12) 2, 8, 2 Electronic configuration of Na (atomic number = 11)2, 8, 1 Electronic configuration of K (atomic number=19) 2, 8, 8, 1 Electronic configuration of Ca (atomic number =20) 2, 8, 8, 2 From the above electronic configurations, it is clear that K and Na will lose electron easily to achieve stable configuration. But out of K and Na, K will lose electron more easily because the force of, attraction on valence electron of K is least among the given elements.

Question 9. Which among the following elements has the largest atomic radii? [NCERT Exemplar] (a) Na (b) Mg (c) K (d) Ca Answer: (c) Atomic radius increases on moving down in a group. Na and K are in the same group and K is below Na, so K will have higher atomic radius, i.e. K > Na. In a period on moving left to right, atomic radius decreases. Since, K and Ca are in the same period and K is in 1st group and Ca is in 2nd group, so atomic radius of K will be more than Ca, i.e. K > Ca. Also Na and Mg are in the same period, but Na belongs to 1st group and Mg belongs to 2nd group, so atomic radius of Na is more than Mg, i.e. Na > Mg. Thus, if we take all these together we get K > Na >Mg and K > Ca > Mg. Hence, we can say that the atomic radius of K is largest.

Question 10. Which of the following statements is not a correct statement about the trends when going from left to right across the periods of periodic table? [NCERT] (a) The elements become less metallic in nature (b) The number of valence electrons increases (c) The atoms lose their electrons more easily (d) The oxides become more acidic Answer: (c) On moving from left to right, the atomic number increases and hence, the nude charge increases. With the increase of nudear charge, the force binding the electron increases so the atom lose the electrons with more difficulty, not easily.

Question 12. Which of the following statement(s) about the modern periodic table are incorrect? (i) The elements in the modern periodic table are arranged on the basis of their decreasing atomic numbers. (ii) The elements in the modern periodic table are arranged on the basis of their increasing atomic masses. (iii) Isotopes are placed in adjoining group(s) in the periodic table. (iv) The elements in the modern periodic table are arranged on the basis of their increasing atomic number. [NCERT Exemplar] (a) Only (i) (b) (i), (ii) and (iii) (c) (i), (ii) and (iv) (d) Only (iv) Answer: (b) Only statement (iv) is correct. All the elements in the modern periodic table are arranged on the basis of their increasing atomic number. All the isotopes can be placed at one place in the same group of the periodic table.

Question 13. The element with atomic number 14 is hard and forms acidic oxide and a covalent halide. To which of the following categories does the element belong? [NCERT Exemplar] (a) Metal (b) Metalloid (c) Non-metal (d) Left-hand side element Answer: (c) Its outermost shell has 4 electrons. So, it is a non-metal. Non-metal forms acidic oxide and by sharing of electrons with halogen, it forms covalent halide.

Question 14. Arrange the following elements in the order of their decreasing metallic character Na, Si, Cl, Mg, Al. [NCERT Exemplar] (a) Cl > Si > Al > Mg > Na (b) Na > Mg > Al > Si > Cl (c) Na > Al > Mg > Cl > Si (d) Al > Na > Si > Ca > Mg Answer: (b) Metals lie on the extreme left side of the periodic table. Metallic character decreases from left to right in a period. Na, Si, Cl, Mg, Al belong to same period in the order Na, Mg, Al, Si, Cl. On moving in a i period from left to right, the metallic character decreases. Thus, the order of decreasing metallic character is: Na > Mg > Al > Si > Cl

Question 15. Which of the following set of elements is written in order of their increasing metallic character? [NCERT Exemplar] (a) Be, Mg, Ca (b) Na, Li, K (c) Mg, Al, Si (d) C, O, N Answer: (a) Metallic character increases as we go down in a group.

Question 16. Which one of the following does not increase while moving down the group of the periodic table? [NCERT Exemplar] (a) Atomic radius (b) Metallic character (c) Valence electrons (d) Number of shells in an element Answer: (c) Elements in each group has some number of valence electrons hence have same valency and thus exhibit similar chemical properties.

Question 17.

The elements X, Y and Z are shown in a portion of periodic table. What would be the representations of ionic forms of X and Z respectively? (a) X – and Z + (b) X + and Z – (c) X 2- and Z 2+ (d) X 2+ and Z 2- Answer: (a) X having 1 electron less than that of Y, which is a noble gas (having complete octet), will tend to gain 1 electron while Z will tend to lose 1 electron to achieve complete octet configuration. Hence, they will have ionic formula as X – and Z + .

Ionic Formula Calculator gives the formula of an ionic compound and net ionic charge details quickly. All you need to do is provide the ionic compound name and hit the calculate button to check the ionic radii, net ionic charge and its formula.

Question 18. which of the following elements will form an acidic oxide? [NCERT Exemplar] (a) An element with atomic number = 7 (b) An element with atomic number = 3 (c) An element with atomic number = 12 (d) An element with atomic number = 19 Answer: (a) Non-metals form acidic oxides in general. Non-metals have 4 to 8 electrons in the outermost shell. The electronic configuration of given elements are (a) i.e. 7 = 2, 5 (b) i.e. 3 =2, 1 (c) i.e. 12 =2, 8, 2 (d)i.e. 19=2, 8, 8,1. So, element with atomic number = 7 (electronic configuration = 2, 5) with is non-metal (N) and it will form an acidic oxide. Rest three elements with atomic- numbers, 3 (Li), 12 (Mg) and 19 (K) are metals and hence, form basic oxides.

Question 19. what type of oxide would Eka-aluminium form? [NCERT Exemplar] (a) EO 3 (b) E 3 O 2 (C) E 2 O 3 (d) EO Answer: (c) Gallium has a valency of 3. Hence, it forms an oxide having molecular formula E 2 O 3 . In other options, valency of E is not 3.

Question 20. The diagram given below shows the position of elements in a portion of the periodic table. Ionic compound is formed between ………. and ………

(a) A and B (b) B and E (c) C and D (d) D and E Answer: (D) being in group IIA is most electropositive among given elements while E being in group VIIA is most electronegative among the given elements. Hence, both of these will form ionic compound, more readily than the other given elements.

Question 21. Element X forms a chloride with formula, XCl 2 , which is a solid with a high melting point. X would most likely to be in the same group of the periodic table as [NCERT] (a) Na (b) Mg (c) Al (d) Si Answer: (b) The formula of chloride is XCl 2 , that means the valency of the element X is 2. The element having valency 2 will be present in group 2. Out of the given choices magnesium (Mg) belongs to group 2.

NCERT Solutions for Class 10 Science Chapter 5 Periodic Classification of Elements (Hindi Medium)

Class 10 Science Periodic Classification of Elements Mind Map

Dobereiners’s Triads

• Dobereiner found that when elements are arranged into groups of three in the order of their increasing atomic mass, the atomic mass of the element; which comes in the middle, is the arithmetic mean of rest of the two.
• He arranged three elements in one group which is known as Dobereiner’s Triads. For e.g.: (Li) 7.0 (Na) 23.0 (K) 39.0 (Ca) 40.0 (Sr) 87.5 (Ba) 137.0
• Here atomic mass of sodium is equal to arithmetic mean of atomic masses of lihtium and potassium. Similarly, atomic mass of strontium is equal to arithmetic mean of atomic masses of calcium and barium

Limitations of Doberiner’s Triads

• He could identify only a few such triads and so the law could not gain importance.
• In the triad of Fe, Co, Ni, all the three elements have a nearly equal atomic mass and thus it does not follow the above law.

Mendeleev’s Periodic Classification

• Mendeleev periodic law, states that ‘the properties of elements are the periodic function of their atomic masses’.
• Mendeleev’s periodic table contains vertical columns called ‘groups’ and horizontal rows called ‘periods’.

Characteristics of the Mendeleev’s Periodic Table

• The elements are arranged in vertical rows called groups and horizontal rows called periods.
• There are eight groups indicated by Roman Numerals I, II, III, IV, V, VI, VII, VIII. The elements belonging to first seven groups have been divided into sub-groups designated as A and B on the basis of similarities. Group VIII consists of nine elements arranged in three triads.
• There are six periods (numbered 1,2,3,4,5 and 6).

Limitation of Mendeleev’s Periodic Table

• Some elements in Mendeleev’s Table have not been arranged in the increasing order of their atomic masses. For example, Co and Ni.
• Hydrogen forms similar compounds as Group 1 elements. However, it also forms similar diatomic molecules as Group 7 elements (H2, F2, C12, Br2, 12). Hence, it could not be assigned a fixed position in the table.
• Isotopes posed a challenge to Mendeleev’s table. For example, Cl has two major isotopes – Cl-35 and Cl-37.

Merits of Mendeleev’s Periodic Tabl e

• Mendeleev left some blank spaces in his periodic table in order to place the elements having similar properties in the same group.
• Mendeleev predicted the discovery of some elements and named them as eka-boron, eka- aluminium and eka-silicon.
• One of the strengths of Mendeleev, s periodic table was that, when inert gases were discovered they could be placed in a new group without disturbing the existing order.

Newlands’ Law of Octaves

• According to this law “if elements are arranged by the increasing order of their atomic masses, property of every eighth element repeats.”
• The arrangement of elements in Newlands’ Octave resembles the musical notes.

Limitation of Newlands’ Octaves

• Law of Octaves could be valid up to calcium only; as after calcium, elements do not obey the rules of Octaves.
• It was assumed by Newlands that only 56 elements existed in nature and no more elements would be discovered in the future
• More than one element had to be placed in some of the groups; in order to place the elements having similar properties in one group. But in order to do so, he also put some dissimilar elements in same group.
• Iron; which has similar property as cobalt and nickel, was placed far from them.
• Cobalt and nickel were placed in the group with chlorine and fluorine in spite of having different properties.

Modern Periodic Table In 1913, Henry Moseley showed that atomic number of an element is a more fundamental property than its atomic mass. According to this law “’properties of elements are a periodic function of their atomic number”.

Trends in Modern Periodic Table

Position of Elements in the Modern Periodic Table Position of Elements

Elements are placed in groups according to the number of valence electrons and placed in periods according to the number of shells present in them.

Helium has valence electrons equal to 2, but it is placed in group number 18 because it is a noble gas and has completely filled outermost shell.

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NCERT Solutions for Class 10 Science All Chapters

• Chapter 1 Chemical Reactions and Equations
• Chapter 2 Acids, Bases and Salts
• Chapter 3 Metals and Non-metals
• Chapter 4 Carbon and Its Compounds
• Chapter 5 Periodic Classification of Elements
• Chapter 6 Life Processes
• Chapter 7 Control and Coordination
• Chapter 8 How do Organisms Reproduce?
• Chapter 9 Heredity and Evolution
• Chapter 10 Light Reflection and Refraction
• Chapter 11 Human Eye and Colourful World
• Chapter 12 Electricity
• Chapter 13 Magnetic Effects of Electric Current
• Chapter 14 Sources of Energy
• Chapter 15 Our Environment
• Chapter 16 Management of Natural Resources

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Class 10 Chemistry Index

This Class 10 Chemistry Index page contains all the topics that fall under each chapter of the class 10 chemistry syllabus as per the NCERT textbook. Students may follow the links on the subtopics to access free study material on the associated concepts (prepared by chemistry subject experts for CBSE students). Furthermore, an overview of all the chapters and topics in the CBSE class 10 chemistry textbooks can also prove useful while crafting a preparation strategy for the CBSE board examination and other competitive examinations.

Class 10 Chemistry Chapters

Chapter 1 – chemical reactions and equations  .

• Chemical reactions
• Balanced chemical equation
• Types of chemical reactions
• Oxidation and reduction

Chapter 2 – Acids, Bases and Salts                         

• Acids, bases and salts
• Concept of pH scale
• Preparation of Sodium Hydroxide
• Uses of Sodium Hydroxide
• Bleaching powder  
• Baking soda
• Washing soda  
• Plaster of Paris

Chapter 3 – Metals and Non-metals                      

• Metals and nonmetals
• Properties of metals and non-metals
• Reactivity series
• Formation and properties of ionic compounds
• Basic metallurgical processes
• Corrosion and its prevention

Chapter 4 – Carbon and its Compounds

• Carbon compounds
• Covalent bonding in carbon compounds
• Versatile nature of carbon
• Homologous series
• Nomenclature of carbon compounds containing functional groups ( halogens , alcohol , ketones, aldehydes , alkanes and alkynes ) 
• Difference between saturated hydrocarbons and unsaturated hydrocarbons
• Chemical properties of carbon compounds ( combustion , oxidation, addition and substitution reaction )
• Ethanol and Ethanoic acid (only properties and uses)
• Soaps and detergents

Chapter 5 – Periodic Classification of Elements

• Periodic classification of elements : Need for classification
• Early attempts at classification of elements
• Dobereiner’s Triads & Newland’s Law of Octaves
• Mendeleev’s Periodic Table
• Modern periodic table, gradation in properties
• Atomic number
• Metallic and non-metallic properties

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The full list of chapters and subtopics of the Class 10 NCERT textbook has been provided above. This page can help provide context and structure for learning the fundamental principles covered under the Class 10 CBSE chemistry syllabus, thereby empowering the students to develop from simple to relatively complex concepts in a systematic manner.  The list of chapters and subtopics given above has been prepared in accordance with the current CBSE syllabus for class 10 chemistry. The content provided in the respective sub-topics has been designed by our expert chemistry professors for the benefit of all students. Click the links listed under each chapter to read more about all Class 10 topics in depth.

Chemistry is the science that tries to understand the properties of substances and the changes that substances undergo. Class 10 Chemistry concepts deal with the understanding of basic constituents of matter, atoms and molecules. Students must study these principles in detail in order to improve their expertise in the subject and to establish a strong foundation.

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