CISCE Syllabus For Class 9 Chemistry: Knowing the Syllabus is very important for the students of Class 9. Shaalaa has also provided a list of topics that every student needs to understand.
The CISCE Class 9 Chemistry syllabus for the academic year 2023-2024 is based on the Board's guidelines. Students should read the Class 9 Chemistry Syllabus to learn about the subject's subjects and subtopics.
Students will discover the unit names, chapters under each unit, and subtopics under each chapter in the CISCE Class 9 Chemistry Syllabus pdf 2023-2024. They will also receive a complete practical syllabus for Class 9 Chemistry in addition to this.
Academic year:
CISCE Class 9 Chemistry Revised Syllabus
CISCE Class 9 Chemistry and their Unit wise marks distribution
CISCE Class 9 Chemistry Course Structure 2023-2024 With Marking Scheme
Syllabus
1 The Language of Chemistry
- Matter (Substance)
- Matter
- Creation of Matter
- Physical Nature of matter
- The matter is made up of particles
- How small is this particles of matter
- Colour, odour, melting point, boiling point, density
- Chemical properties: Composition, combustibility, activity with acids and bases
- Molecules
- Molecule
- Properties of molecule
- Pure Substances
- Pure substance
- Characteristics of Pure substance
- Examples of Pure Substance
- Elements
- Element
- Characteristics of Element
- Common Element
- In the universe
- In the Earth's crust
- Elements in the human Body
- Elements in air
- Birth of the Element
- Classification of Molecules
- Symbols Used to Represent Atoms of Different Elements
- Valency
- Variable Valency
- Ions (Radicals) and Its Types
- Radicals
- Types of Radicals
- Basic radical
- Acid radical
- Chemical Formula or Molecular Formula
- Chemical formulae of compounds : A recapitulation
- Naming Chemical Compounds
- To Calculate the Valency from the Formula
- Chemical Equation
- Chemical Equation
- Need for Chemical equation
- Limitation of Chemical equation
- Balancing Chemical Equation
- Steps in writing the skeleton equation
- Balancing chemical equation
- Information conveyed by a balanced chemical equation
- A chemical equation can be made more informative by writing the additional information.
- Atomic Mass
- Atomic mass
- Gram atomic mass
- Average atomic mass
- Molecular Mass
- Molecular mass
- Characteristics of molecular mass
- Gram molecular mass
- Percentage Composition, Empirical and Molecular Formula
- Percentage composition
- Chemical formula
1) Empirical formula
2) Molecular formula - Steps involved in determining the empirical formula
- Steps for determination of the molecular formula of a compound
- Empirical Formula of a Compound
- Hydrogen
- Hydrogen
- Discovery of Hydrogen
- Occurrence of Hydrogen
2 Chemical Changes and Reactions
- Classification of Change: Chemical Changes
- Chemical Change
- Properties of Chemical Change
- Importance of Chemical Change
- Chemical Reaction
- Chemical Reaction
- Reactants
- Products
- Word Equation
- Characteristics of Chemical Reactions
- Conditions Necessary for Chemical Reactions
- How will you know that a chemical change has taken place?
- Close contact
- Attraction in the physical state of the reactants (through the solution)
- Heat energy
- Light energy
- Electricity
- Pressure
- Catalysts: Positive catalyst and Negative catalyst
- Types of Chemical Change or Chemical Reaction
- Energy Change in Chemical Reactions
- Energy Change in Chemical Reactions:
- Exothermic Chemical Changes
- Endothermic Chemical Changes
- Photochemical Reaction
- Electrochemical Reaction
3 Water
- Water, Our Lifeline
- Introduction
- Water: A Compound
- Occurrence of water
- Physical Properties of Water
- Physical Properties of Water:
- Nature
- Boiling point
- The freezing point of water or melting point of ice
- Density
- Anomalous expansion of water
- Latent heat of fusion of ice
- Latent heat of vaporization of water
- Specific heat capacity
- Chemical Properties of Water
- Chemical properties
- Dissociation of water
- Amphoteric nature
- Oxidising and reducing nature
- Hydrolytic reactions
- Formation of hydrates with metal salts
- Water - a Universal Solvent
- Universal Solvent
- Experiment: To show that ordinary tap water contains dissolved solids.
- Importance of dissolved salts in water.
- Air dissolved in water.
- Experiment: To show that tap water contains dissolved gases (air).
- Importance of air dissolved in water.
- Solutions as 'Mixtures' of Solids in Water
- Homogeneous mixture
- Solution
- Solute
- Solvent
- Binary solution
- Ternary solutions
- Quaternary solutions
- Homogeneous solution
- Solid solution
- True solution
- Characteristics of a true solution
- Components of Solutions
- Different Types of Solutions
- Different Types of Solutions:
- Supersaturated solution
- Unsaturated solution
- Saturated solution
- Aqueous solution
- Non-aqueous solution
- Dilute solution
- Concentrated solution
- Saturated Solutions
- What is a Saturated Solution?
- How to Prepare a Saturated Solution?
- Factors affecting the Point of Saturation
- Effect of cooling and heating of Saturation
- Everyday Examples of Saturated Solution
- Concentration of a Solution
- Concentration of a Solution
- Mass percentage
- Volume percentage
- Solubility
- Solubility
- Factors affecting solubility
- Nature of the solute and solvent
- Effect of Temperature
- Effect of Pressure
- Solubility curves can be used
- Determination of the solubility of a solute at a particular temperature
- Effect of pressure and temperature on solubility of gases in water (liquids)
- Crystals and Crystallisation
- Crystals
- Crystallisation
- Experiment: To prepare large crystals of copper sulphate.
- Hydrated and Anhydrous Substances
- Efflorescence, Hygroscopic, and Deliquescence Substances
- Efflorescence
- Deliquescence
- Hygroscopy
- Drying and Dehydrous Substances
- Classification of water: Soft and Hard Water
- Soft and Hard water
- Types of Hard water
- Temporary Hardness
- Permanent Hardness
- Causes of Hardness
- Advantage and Disadvantage of Hard Water
- Removal of Hardness of Water
- Softening of water
- Removal of temporary hardness
a) By boiling
b) Clark's method - Removal of permanent hardness
a) By washing soda method
b) lon-exchange/Permutit method
c) Calgon method
d) Synthetic resins method
⇒ Ion exchange resins are of two types
i) Cation exchange resins
ii) Anion exchange resins
- Degree of hardness of water
- Salts
- Salts
- Family of Salts
- pH of Salts
- Prevention of Water Pollution
4 Atomic Structure and Chemical Bonding
- Chemical Bond
- Bond
- Chemical bond
- Kossel – Lewis approach to chemical bonds
- Lewis dot structure
- History of Atom
- Dalton’s atomic theory
- Elements
- Element
- Characteristics of Element
- Common Element
- In the universe
- In the Earth's crust
- Elements in the human Body
- Elements in air
- Birth of the Element
- Atoms: Building Blocks of Matter
- Atoms: Building Blocks of Matter
- How big are atoms?
- How do atoms exist?
- Discovery of Charged Particles in Matter
- Cathode Ray Tube (CRT) experiment
- Electrons (e)
- Electrons
- Discovery of Electrons
- Properties of Cathode rays
- Charge to Mass Ratio of Electron
- Charge on the Electron
- Protons (p)
- Protons
- Discovery of Protons
- Properties of Anode rays
- Nucleus
- Discovery of Nucleus
- Deflection of α-particle by a gold leaf
- Neutrons (n)
- Neutrons
- Discovery of Neutrons
- Properties of Neutrons
- J. J. Thomson’s Atomic Model
- Lord Rutherford’s Atomic model
- Biography of Ernest Rutherford
- Reason behind discovery of Rutherford’s atomic model
- Rutherford’s α-particle scattering experiment
- Observations of α-scattering experiment
- Conclusions of α-scattering experiment
- Rutherford's model of an atom
- Some terminologies related to the α- scattering experiment
1) Number of scattered particles
2) Distance of closest approach (Nuclear dimension)
3) Impact parameter (b)
- Neils Bohr’s Model of an Atom
- Bohr's model of an atom
- Postulates of Bohr's atomic model
- Merits of Bohr's model
- Drawbacks of Bohr's model
- Structure of an Atom
- Atomic Number (Z), Mass Number (A), and Number of Neutrons (n)
- Atomic number or Nuclear charge
- Nucleons
- Mass number
- Relationship between atomic number and mass number
- Representation of element
- Number of Neutrons (n)
- Atomic Mass
- Atomic mass
- Gram atomic mass
- Average atomic mass
- Electronic Configuration of Atom
- Valency Electrons
- Reason for Chemical Activity of an Atom
- Isotopes
- Isotopes
- Examples
- Properties of Isotopes
- Mass of Isotopes
- Isobars
- Isobars
- Example of Isobars
- Characteristics of Isobars
- Electrovalent (or Ionic) Bond
- Ionic Bond
- Electrovalent Bond
- Electronegativity and Ionic Bonding
- Ionic Bond Properties
- Characteristics of Ionic compounds
- Examples of Ionic Bonds
- Formation of an Electrovalent (or Ionic) Bond
- Conditions for the formation of an electrovalent (or ionic) bond
- Why Are Ionic Compounds Stable?
- Structures of some electrovalent compounds
- Sodium chloride (NaCl)
- Magnesium chloride (MgCl2)
- Calcium oxide (CaO)
- The Covalent Bond
- Covalent Bond
- Covalent Bonding can be Achieved in two Ways
- Covalent Bonding in Carbon Atom
- Properties of Covalent Bond
- Polar Covalent Bond
- Non-polar Covalent Bond
- Polarization of Covalent Bonds
- Types of Covalent Bond
- Types of Covalent Bond
- Single Covalent Bond
- Double Covalent Bond
- Triple Bond
- Formation of Covalent Bond
- Formation of Covalent Bond:
- Hydrogen molecule (Non-polar compound)
- Chlorine molecule (Non-polar compound)
- Oxygen molecule (non-polar compound)
- Nitrogen molecule (Non-polar compound)
- Hydrogen chloride (polar compound)
- Water molecule (polar compound)
- Ammonia molecule (polar compound)
- Carbon tetrachloride molecule (Non-polar compound)
- Methane molecule (Non-polar compound)
5 The Periodic Table
- History of Periodic Table: Early Attempts at the Classification of Elements
- Reasons for classification of elements
- Early Attempts at the Classification of Elements
- Dobereiner’s Triads
- Dobereiner’s Triads
- Limitations of Dobereiner’s Triads
- Newland's Law of Octaves
- Newlands’ Law of Octaves
- Limitations of Newlands’ Law of Octaves
- Mendeleev’s Periodic Table
- Mendeleev’s Periodic Table
- Features of Mendeleev’s Periodic Table
- Merits and Demerits of Mendeleev’s Periodic Table
- Modern Periodic Law
- Atomic number as the basis for modern periodic law
- The Modern Periodic Table
- Modern Periodic Table
- Salient features of the modern periodic table
- Features of Periods
- Features of Groups
- Position of hydrogen in the periodic table
- Position of Rare Gases
- Types of Element on the Basis of Periodic Table
- Representative elements
- Transition elements
- Inner transition elements
- Inert gases or noble gases
- s-Block Elements
- p-Block Elements
- d-Block Elements
- f – Block Elements
- Advantage and Disadvantage of Modern Periodic Table
- Periodic Properties
- Periodicity
- Periodicity of elements
- Cause of periodicity
- Study of Specific Groups in Periodic Table
- Uses of Periodic Table
- Types of Elements: Metals
- Metals
- Occurrence of metal
- Uses of Metals
6 Study of the First Element - Hydrogen
- Position of Hydrogen in Periodic Table
- Similarities Between Hydrogen and Alkali Metals
- Similarities Between Hydrogen and Halogens
- Hydrogen
- Hydrogen
- Discovery of Hydrogen
- Occurrence of Hydrogen
- Preparation of Hydrogen
- Application of Activity Series in the Preparation of Hydrogen
- Displacement of hydrogen from dilute acids
- Displacement of hydrogen from alkalis
- Laboratory Preparation of Hydrogen
- Manufacture of Hydrogen
- Manufacture of Hydrogen
- Bosch process
- By electrolysis of water
- Physical Properties of Hydrogen
- Chemical Properties of Hydrogen
- Uses of Hydrogen
- Oxidation, Reduction and Redox Reactions
- Oxidation
- Reduction
- Redox Reactions
- Oxidising agents and Reducing agents
- Oxidation reactions in daily life
- Oxidation number
7 Study of Gas Laws
- Gases and Its Characteristics
- Gases
- Behaviour and characteristic properties of gases
- Composition of gases
- Gases have neither a fixed volume nor a fixed shape
- Gases exert pressure in all directions
- Gases are highly compressible
- Gases are highly expansible
- Gases have low density
- Gases have a natural tendency to mix with one another (diffusion)
- Gases can be liquefied
- Molecular Motion : Relationship of Temperature, Pressure and Volume
- The Gas Laws
- The Gas Laws
- Standard variables for gas laws
- The volume (V)
- The pressure (P)
- The temperature (T)
- Fundamental Laws of Gases
- Pressure and Volume Relationship or Bolye's Law
- Boyle's law
- Mathematical expression of Boyle's law
- Graphical verification of Boyle's law
- Explanation of Boyle's law in terms of molecular motion (kinetic theory).
- Significance of Boyle's Law
- Experiment of Pressure and Volume relationship in gases
- Temperature - Volume Relationship or Charles's Law
- Charle's Law
- Mathematical expression of Charles's Law
- Graphical representation of Charle's law
- Significance of Charle's Law
- Pressure and Volume Relationship or Bolye's Law
- Absolute Zero
- Temperatures
- Temperature
- Unit of Temperature
- Scales of Thermometers
- Fahrenheit scale
- Celsius temperature scale
- Kelvin scale (Absolute scale)
- Relationship between the three scales of temperature
- Conversion of Temperature from celsius scale to kelvin scale and vice-versa
- Gas Equation
- Standard Temperature Pressure (S.T.P.)
- The Effect of Moisture and Pressure
8 Atmospheric Pollution
- Atmospheric Pollution
- Air Pollution and Its Causes
- Air Pollution
- Causes of Air pollution
- Sources of Air Pollution
- Effects of Air Pollution
- Prevention of Air Pollution
- Measures to control air pollution
- Devices to control air pollution
- Electrostatic precipitator (ESP)
- Scrubbers
- Catalytic converters
- Gaseous Pollutants and Their Effects
- Acid Rain
- Acid rain
- Effects of Acid rain
- Causes of Acid Rain
- Green House Effect
- Green House Effect
- Green House gases
- Advantage of Green House Effect
- Global Warming
- Global Warming
- Causes of Global warming
- Effect of Global Warming
- Preventive Measures of Global Warming
- Ozone
- Ozone
- Function of ozone in the atmosphere
- Harmful effects of ozone
- Ozone Layer Depletion
- Depletion of Ozone Layer
- Chemicals responsible for the destruction of the ozone layer
9 Elements, Compounds and Mixtures
- Differences Between Elements, Compounds, and Mixtures
- Types of Mixtures
- Mixture
- Separation of Mixtures
- Use of Solvent and Filtration
- Change of State of Matter
- Methods of Separation
- Chromatography Method
- Chromatography
- Types of chromatography
- Adsorption chromatography
i) Column chromatography
ii) Thin layer chromatography (TLC) - Partition chromatography: paper chromatography
- Chromatography Method
12 Matter and Its Composition: Law of Conservation of Mass
13 Practical Work
- Laboratory Preparation of Hydrogen
- Laboratory Preparation of Oxygen
- Laboratory Preparation of Carbon Dioxide
- Laboratory Preparation of Chlorine
- Laboratory Preparation of Hydrogen Chloride Gas
- Preparation of hydrogen chloride gas from common salt.
- Purification of HCI gas
- Laboratory Preparation of Sulphur Dioxide
- Laboratory Preparation of Hydrogen Sulphide
- Laboratory Preparation of Ammonia Gas
- Preparation of ammonia from ammonium chloride and calcium hydroxide.
- Preparation of ammonia from magnesium nitride.
- Laboratory Preparation of Water Vapour
- Laboratory Preparation of Nitrogen Dioxide
- Action of Heat on a Given Substance
- Action of heat on Copper carbonate (Green solid)
- Action of heat on Zinc carbonate (White solid)
- Action of heat on Washing soda (White crystals)
- Action of heat on Copper sulphate (Blue crystals)
- Action of heat on Zinc nitrate (White solid)
- Action of heat on Copper nitrate (Green solid)
- Action of heat on Lead nitrate (White solid)
- Action of heat on Ammonium chloride (White solid)
- Action of heat on Iodine Violet solid
- Action of heat on Ammonium dichromate (Orange solid)
- Action of Dilute Sulphuric Acid on a Given Substance
- The action of dilute sulphuric acid on magnesium.
- The action of dilute sulphuric acid on Zinc.
- The action of dilute sulphuric acid on Sodium carbonate
- The action of dilute sulphuric acid on Sodium bicarbonate.
- The action of dilute sulphuric acid on Iron(II) sulfide
- The action of dilute sulphuric acid on sodium sulfate
- The action of dilute sulphuric acid on Potassium sulfite
- Dry Test
- Recognition of Substances by Physical State
- Table of solubility of salts and bases in water
- Recognition of Substances by Action of Heat
- Identification of solids by the action of heat:
- Ammonium salt
- PbO2, Pb3O4, HgO, KNO3, NaNO3
- Carbonate and bicarbonate (except K2CO3 and Na2CO3)
- Hydrated salt
- Sulphite or sulphate
- Lead compounds decompose to give lead monoxide; PbO
- Zinc compounds decompose on heating to give zinc oxide
- Copper compound decomposes to give black copper oxide CuO.
- Some naturally occurring acids:
- Acetic acid
- Citric acid
- Butyric acid
- Hydrochloric acid
- Formic acid
- Lactic acid
- Malic acid
- Oleic acid
- Stearic acid
- Tartaric acid
- Uric acid
- Recognition of Substances by Physical State
- Classification of water: Soft and Hard Water
- Soft and Hard water
- Types of Hard water
- Temporary Hardness
- Permanent Hardness
- Simple Experiments Based on Hard Water and Soft Water
- Differentiating hard water from soft water.
- Differentiating between temporary and permanent hard water.
- Soap and detergents
- Comparing the effects of soaps and detergents on hard water.
- Water Pollution and Its Causes
- Water Pollution
- Causes of Water Pollution
- Sources of Water Pollution
- Water Quality
- Strength of Acidic or Basic Solutions
- pH Scale
- Importance of pH in Everyday Life
- Prevention of Water Pollution
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