Tricks to Learn CHEMISTRY easily

Study plan for ICSE CHEMISTRY......!?

Most of the students think Chemistry is a hard subject and it not easy to learn just like any other subject. But Chemistry is not so hard to study and score marks in it. Chemistry is a part of science just like Physics, biology etc. In fact Chemistry is one of those subjects where you score big and enhance your overall academic percentage in the school level.

Chemistry is the part of science which is based on the changes that matter undergoes, how a substance interacts with another, chemical reactions, the changes occur during the chemical reactions, Observations made etc.

Do you feel Chemistry hard ? What you need to do ?

What you need to do, to score maximum marks in chemistry, is work hard and smart. You must have a good knowledge in the terminology of Chemistry. Understand the basic concepts of Chemistry like what is an atom, element, molecule, compound, ion, chemical reaction etc. These are the minimum requirements to learn Chemistry and score in class 10 level.

What are the important topics in ICSE CHEMISTRY ?

All the chapters in ICSE Chemistry are given equal importance as per the board exam paper.

The chapters in ICSE CHEMISTRY are:

The Periodic Table
Chemical Bonding
Acids, Bases and Salts
Stoichiometry
Electrolysis
Metallurgy
Study of Compounds : Hydrogen chloride, Nitric acid, Sulphuric acid and Ammonia
Organic Chemistry
Practical Chemistry  

How to study ICSE CHEMISTRY

• Understand the Syllabus and the Topics.
• Study the Text book line to line and understand the concepts and prepare notes of important points.
• Practice and Test yourself using the previous papers.
• Note down the mistakes you made and analyze and spend more time on that particular topic to rectify and improve yourself.

Comparison between Ionic (Electrovalent) compound and Covalent compound for class 10 ICSE

 Comparison between Ionic (Electrovalent) compound and Covalent compound

Ionic compounds	Covalent compounds
1.      As the ions in ionic compounds are held by the strong electrostatic force of attraction they : ü  Exist in solid state ü  Are non volatile ü  Have high boiling and melting points	1.      In these compounds the molecules are have weak Vander waal’s forces so they: ü  Exist as soft solids, liquids and gases. ü  Are  non- volatile ü  Have low boiling and melting points.
2.      These compounds undergo dissociation and become free in their molten or aqueous solution form hence they conduct electricity. ü  They are non conductors in solid state because the ions are not free.	2.      Polar covalent compounds undergo ionization in their aqueous solutions and produce free ions so they conduct electricity in aqueous solutions. ü  Non-polar compounds do not undergo ionization so they are non-conductors. e.g. CCl4
3.      These can be electrolysed in their molten state or aqueous solutions.	3.      Polar covalent compounds can be electrolysed in their aqueous solutions.
4.      Soluble in water.	4.      Polar compounds are soluble in polar solvents like water. Non polar compounds are soluble in non polar solvents like Benzene
5.      Reactions between ionic compounds take place rapidly in their solutions since they produce free ions easily.	5.      Covalent compounds undergo slow reactions because they have to break the bonds and form new bonds.

Comparison between Polar and Non-polar compounds for class 10 ICSE

Comparison between Polar and Non-polar compounds

Polar covalent and non polar molecules

Polar molecules	Non-polar molecules
1.      Due to the electronegativity difference between the atoms the electrons are distributed unequally which leads to charge separation.	1.  There is no charge separation since the electron pair is equally distributed between the atoms.
2.      Example: HCl, H2O , NH3 etc.	2. Example: H2, Cl2, O2, N2, CCl4, CH4 etc

 

Ø  Charge separation in Hydrogen chloride molecule:

In HCl molecule Chlorine is more electronegative than Hydrogen so the electron pair is more strongly attracted by Chlorine atom due this a slight negative charge is developed on Chlorine and a slight positive charge on Hydrogen atom. Hence it becomes a polar compound

Class 10 Co-ordinate covalent bond - Dative bond - ICSE

 Co-ordinate covalent bond - Dative bond - ICSE

Co-ordinate covalent bond (or) Dative bond:

The bond formed by the sharing of electron pair between two atoms where one atom contributes both the electron.

 

Example 1  : Formation of Hydronium ion [H₃O⁺]:

 

    the co-ordinate covalent bond between Oxygen atom and Hydrogen where both the electrons coming from Oxygen atom but being shared by Oxygen and Hydrogen. This is due to the lone pair effect of Oxygen atom in water molecule.

Hydromium ion : 1-dative bond and 2 covalent bonds.

 

Example 2: Formation of Ammonium ion [NH₄⁺]:

Ammonium ion : 1- dative bond and 3- covalent bonds.

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Class 10 Practical Chemistry ICSE pdf

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Identification of Cations anions and Gases

 Class 10 Organic Chemistry notes ICSE pdf

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nomenclature-preparation of alkanes, alkenes, alkynes, test for unsaturation

Class 10 Nitric acid ICSE notes pdf free download

 Class 10 Nitric acid ICSE notes

class-10-nitric-acid-icse-notes-pdf-download-model papers-practice papers-worksheets

 Class 10 Ammonia ICSE notes pdf

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Ammonia notes class 10, ICSE class 10 Ammonia notes, Preparation of Ammonia gas, Haber's process, Properties of Ammonia gas, analytical use of Ammonium hydroxide....

Class 10 Hydrogen chloride- HCl ICSE notes pdf

Class 10 Metallurgy notes ICSE pdf

# Metallurgy notes, work sheets, model papers, practice papers 

ICSE class 10 CHEMISTRY notes pdf download

Acid base and salts class 10 notes

Class 10 Acids Bases and Salts ICSE notes

Acid base and salts class 10 notes

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Important questions from Acids Bases and salts in Chemistry ICSE CHEMISTRY

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CLASS 10 Chemical Bonding ICSE notes

 CLASS 10 Chemical Bonding ICSE notes

for complete chapter pdf file click here  class 10 Chemical Bonding pdf

Covalent bond:

The bond formed by the mutual sharing of electron pairs between the given pairs of atoms (of same or different kind) of non metals.

Covalent compound (molecule) : The compounds (molecules) formed as a result of mutual sharing of electrons between the atoms are called covalent compounds.

Covalency: The number of electron pairs that an atom shares with other atom/s to get stable electronic configuration.

Formation covalent molecules - Electron dot representation

·         The element which has 7 valence electrons (i.e. short of one electron for octet configuration) contributes one electron and shares one pair of electron with other atom.

     

            Cl - 2,8,7         Cl - 2,8,7                     Chlorine molecule     single covalent bond

·         The element having 6 valence electrons (short of 2 electrons) contributes 2 electrons hence shares two pairs of electrons.

Oxygen       Oxygen                       Oxygen molecule       Double bond

                 2,6               2,6

 

·         Similarly the element with 5 valence electrons contributes 3 electrons and shares three pairs of electrons.

Nitrogen        Nitrogen        Nitrogen molecule

2,5                  2,5                                                            Triple bond

 

·            Formation of Hydrogen molecule

 

 

·            Formation of Methane molecule (CH₄)

 

·         Formation of Carbon tetra chloride molecule (CCl₄)

Formation of Hydrogen chloride molecules (HCl)

 

·         Formation of Water molecule:

 

·         Formation of Ammonia molecule

Ø Lone pair: The pair of electrons which is not involved in any bond formation.

for complete chapter pdf file click here  class 10 Chemical Bonding pdf

Class 10 Chemical bonding ICSE notes

 Class 10 Chemical bonding icse notes 

[for complete chapter pdf file click here  class 10 Chemical Bonding pdf ]

Metallurgy Test

Electrolysis Test

Chemical Bonding - test

The Periodic Table

Practical Chemistry Test - anions

Practical Chemistry Test - Cations

Practical Chemistry Test - Observation Based

Sureshot questions in ICSE CHEMISTRY

Electrovalent bond (or) Ionic bond :

The electrostatic force of attraction which binds two or more oppositely charged ions formed by the transfer of electron/s from the metal atom to the non metal atom.

Electrovalent compound: The compounds formed as a result of the transfer electrons.

Electrovalency: The number of electrons lost or gained by an atom of an element to attain stability.

The electrovalent bond is possible between a metal and a non metal. The metal atom atom loses electron/s to nonmetal atom so that the metal and the nonmetal attain stable electronic configuration.

 

Formation of Electrovalent compounds - Electron dot representation

ü  As the metal loses electron/s it is oxidized and forms a cation (positive ion).

Oxidation:

Na – e^-  -->Na⁺

Mg – 2e^- --> Mg²⁺

ü  The non metal atom accepts electron/s and it is reduced to form an anion (negative ion).

Reduction:

Cl₂ + 2e^-   -->2Cl^-

O₂ + 4e^-  --> 2O^2-

Formation of Electrovalent (Ionic) Compounds:

 

Example 1 Sodium chloride ( NaCl):

Sodium is a metal with electronic configuration 2,8,1 – has one valence electron.

Chlorine is a non metal with electronic configuration 2,8,7 – has 7 valence electrons.

 

Sodium has to lose one electron from its valence shell to attain the electronic configuration of its nearest noble gas (Neon) i.e. 2, 8.

 

Chlorine has gain one electron for the electronic configuration of its nearest noble gas (Argon) i.e 2,8,8

Hence Sodium loses its one electron from the valence shell to the chlorine atom.

Representation of Sodium Chloride using electron dot structures

 

Example 2    Magnesium Oxide (MgO)

Mg – electronic configuration is 2, 8, 2- it loses 2 electrons

O – electronic configuration is 2,6 – it has to gain two electrons.

One Magnesium atom donates two electrons to the Oxygen atom.

Example 3 Magnesium Chloride (MgCl₂)

Mg – 2,8,2 – Mg atom has to lose 2 electrons and

Cl – 2,8,7 – each Chlorine atom requires one more electron to get the stable electronic configuration.

Hence Mg atom donates one electron to each chlorine atom.

for complete chapter pdf file click here  class 10 Chemical Bonding pdf

CHEMICAL BONDING ICSE class 10 NOTES

CHEMICAL BONDING Class 10 ICSE NOTES

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Click here for sample test (MCQs)

Metallurgy Test

Electrolysis Test

Chemical Bonding - test

The Periodic Table

Practical Chemistry Test - anions

Practical Chemistry Test - Cations

Practical Chemistry Test - Observation Based

Sureshot questions in ICSE CHEMISTRY

you can download chemical boning notes pdf file from here 

Acids bases and Salts notes ICSE class 10 chemistry notes - Preparation of acids

 Acids bases and Salts notes ICSE class 10 chemistry notes

Preparation of acids:

Preparations of acids:

1.      From non-metals :

H₂ + Cl₂  -->  2HCl

2.      By dissolving  Non-metallic oxides (acidic oxides) in water

CO₂ + H₂O -->   H₂CO₃

SO₂ + H₂O -->   H₂SO₃

 

3.      By heating salts with non-volatile acids:

NaCl  + Conc. H₂SO₄     --> HCl + NaHSO₄

            Non-volatile acid

 

4.      Oxidation of non-metals with strong oxidizing agents:

             S +    6HNO₃    -->  H₂SO₄ + 2H₂O + 6NO₂

                  Oxidizing        Sulphuric

                       agent              acid

Reactions of acids

1.      Neutralization : Acids react with bases to give salt and water.

HCl + NaOH -->NaCl + H₂O

H₂SO₄  + CuO  -->CuSO₄ + H₂O

 

2.      Dilute acids react with –

i) active metals to produce Hydrogen gas and corresponding salts.

           Zn + 2HCl -->ZnCl₂ + H₂

           H₂SO₄ + Fe -->FeSO₄ + H₂

ii) metal carbonates and bicarbonates to give Carbon dioxide

           2HCl + Na₂CO₃ --> 2NaCl + CO₂ + H₂O

iii) metal sulphites to give Sulphur dioxide gas

           2HCl + Na₂SO₃ --> 2NaCl + SO₂ + H₂O

 

iv) metal sulphides to give Hydrogen sulphide gas.

           2HCl + Na₂S -->2NaCl + H₂S

 

3.      Less volatile or non-volatile acids react with salts to give volatile acids.

NaCl  +    Conc. H₂SO₄     --> HCl + NaHSO₄

               Non-volatile acid

NaNO₃  +   Conc. H₂SO_{4     -->} HNO₃ + NaHSO₄

                 Non-volatile acid