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ICSE Class 9 Chemistry Chapter 3 Elements, Compounds and Mixtures Digital Edition
For Class 9 Chemistry, this chapter in ICSE Class 9 Chemistry Chapter 03 Elements, Compounds and Mixtures provides a detailed overview of important concepts. We highly recommend using this text alongside the ICSE Solutions for Class 9 Chemistry to learn the exercise questions provided at the end of the chapter.
Chapter 3 Elements, Compounds and Mixtures ICSE Book Class Class 9 PDF (2026-27)
Chapter 3
Elements, Compounds and Mixtures
Latest Syllabus - Scope of Syllabus
Elements, Compounds and Mixtures
General characteristics and differences between elements, compounds and mixtures. Reasons for considering a substance as an element, compound or mixture must be given to make the concepts clear.
Types of mixtures: of two solids, a solid and a liquid, two liquids, liquid and gas, two gases. Definition of mixture: each type of mixture should be shown to the students including both homogeneous and heterogeneous types - true solutions, suspension and colloidal solution to make the concepts clear.
Separation of mixtures involving use of a solvent, filtration, evaporation and distillation, fractional distillation, simple paper chromatography. Centrifugation - immiscible liquid.
The following examples should be used to illustrate the principles of separation of mixtures by using methods: (a) use of solvent and filtration [e.g. sodium chloride + sand, water as solvent], carbon and sulphur [Carbon tetra chloride as solvent]. (b) evaporation e.g. sodium chloride from its aqueous solution. (c) distillation e.g. purification chloride as solvent]. (b) evaporation e.g. sodium chloride from its aqueous solution. (c) distillation e.g. purification of water containing dissolved solids. (d) fractional distillation involves the difference of boiling points of liquids of water containing dissolved solids. (e) simple paper chromatography [limited to separation of colouring matter in ink]. e.g. benzene + toluene. (f) centrifugation [involving separation of cream from milk]. (g) immiscible liquids [separating funnel e.g. water + carbon tetra chloride].
A. Introduction
Matter - Can Be Broadly Classified Into - Pure and Impure Substances
A substance is any type of matter of recognizable, definite composition and character.
Matter occupies space and has mass.
Pure Substances
Homogeneous material, has particles of one kind, has definite set of properties.
Impure Substances - Mixtures
Two or more substances, mixed in any proportion, substances retain their properties.
Elements
Pure substance, cannot be broken down into two or more simpler substances.
Compounds
Pure substance composed of two or more elements, can be broken down into its elements by chemical means.
Matter is built up of elementary particles i.e. atoms, molecules or ions.
| Atoms | Molecules | Ions |
|---|---|---|
| An atom is the smallest particle of an element which can take part in a chemical reaction and is considered the basic unit of matter. eg. O, H, Cl are - atoms. Mass of an atom cannot be determined practically. Ratio of atomic mass of an element to that of an atom of carbon is known as relative atomic mass of that element. | A molecule is the smallest particle of a substance that can normally exist separately and retain the characteristics of the substance. e.g.O2, H2, Cl2 are - molecules. The sum of masses of individual atoms constitute the mass of a molecule. Ratio of molecular mass of a substance to that of an atom of carbon is known as relative molecular mass of the substance. | An ion is any atom or a group of atoms which has a resultant charge due to loss or gain of electrons. eg. O2-, H+1, Cl- are - ions. The positively and negatively charged ions are called - cations and anions. A substance composed of ions is electrically neutral since the total amount of charge carried by the - cation and anion is equal. |
Teacher's Note
When salt dissolves in water, it breaks into ions - this is why salt water conducts electricity, unlike pure water.
B. Elements
Elements - The Term
An elements - is a pure substance which cannot be converted or broken down into two or more simpler substances by any physical or chemical process.
An element is made up of - only one kind of atoms having the same atomic number.
Atom - The smallest particle of an element which may or may not have independent existence but takes part in a chemical reaction is called an atom.
Metallic elements - generally occur as - solids [e.g. mercury is a liquid at room temp.]
Non-metallic elements - occur as - solids [e.g.carbon] liquids [bromine at room temp.] or - gases [e.g. hydrogen]
Metalloids - are generally solids [e.g. arsenic, antimony] and
Noble gases - are gaseous [e.g. neon, argon]
Examples of Gaseous Elements
Monoatomic gaseous elements - Helium [He], Neon [Ne], Argon [Ar]
Diatomic gaseous elements - Hydrogen [H2], Oxygen [O2], Chlorine [Cl2]
Polyatomic gaseous elements - Ozone [O3]
Number of Elements
There are almost 118 elements discovered so far both - normal elements and radioactive elements. The most abundant element in the earth's crust is oxygen [49.9%]. The human body consists of elements - oxygen [65%], carbon [18%] and hydrogen [10%].
Elements are categorized into - metals, non-metals, metalloids and noble gases.
| Metals | Non-Metals | Metalloids | Noble Gases |
|---|---|---|---|
| Elements which - generally have: | Elements which - generally: | Elements which - generally have: | Elements which: |
| Characteristic lustre. Are good conductors of heat and electricity. Are malleable [beaten in sheets] and ductile [drawn into wires]. Contain one kind of atoms - mono-atomic. | Do not have lustre. Are bad conductors of heat and electricity. Are not malleable or ductile. Contain one kind of atoms - mono-atomic or di-atomic. | Properties midway between metals and non-metals are referred to as metalloids. Contain one kind of atoms - mono-atomic. | Occur in the free gaseous state in traces in the atmosphere. Are chemically inactive or inert. Contain one type of atoms and are mono-atomic. |
| Examples: K, Na, Ca, Mg, Al, Zn, Fe, Pb, Cu, Hg, Ag, Pt, Au. Exceptions to properties: Mercury [Hg] - Liquid at room temperature. Zinc [Zn] - Non-malleable, non-ductile. Tungsten [W] - Poor conductor of electricity. | Examples: Gaseous: H, N, O, F, Cl. Liquid: Bromine [Br]. Solid: C, S, P, Si. Exceptions to properties: Iodine, graphite - Lustrous. Graphite - A good conductor of electricity. | Examples: At.No. Germanium Ge 32. Arsenic As 33. Antimony Sb 51. Bismuth Bi 83. | Examples: At.No. Helium He [2]. Neon Ne [10]. Argon Ar [18]. Krypton Kr [36]. Xenon Xe [54]. Radon Rn [86]. Radon - ejected from radioactive matter. |
Teacher's Note
Copper is a great conductor of electricity, which is why it is used in electrical wiring throughout our homes and buildings.
C. Compounds
Compounds - The Term
A compound is -
A pure substance, composed of - two or more elements.
Combined chemically - in a fixed proportion.
Particles in a Compound
Particles in a compound - are of one kind only.
Properties of Compounds
Compounds have - a definite set of properties.
Components in a compound - do not retain their original properties and - can be separated by chemical means only.
Example of a Compound
Water - H2O
Composed of two elements - hydrogen and oxygen.
Elements combined in a - fixed proportion by weight.
Properties of water are - different from those of its constituent elements
Other Examples of Compounds
| Compound | Elements in the Compound | Formula |
|---|---|---|
| Common salt | Sodium, chlorine | NaCl |
| Methanol | Carbon, hydrogen, oxygen | CH3OH |
| Benzene | Carbon, hydrogen | C6H6 |
| Washing soda | Sodium, carbon, oxygen, hydrogen | Na2CO3-10H2O |
| Caustic soda | Sodium, oxygen, hydrogen | NaOH |
| Epsom salt | Magnesium, sulphur, oxygen, hydrogen | MgSO4-7H2O |
Differences Between Elements and Compounds
| Elements | Compounds |
|---|---|
| Contains - only one type of atoms. | Contains - different types of atoms. |
| Can not be broken down - into simpler substances by physical or chemical means. | Can be broken down - into simpler substances by chemical means. |
| Has characteristic - physical and chemical properties. | Has characteristic - physical and chemical properties but they are - different from those of its constituent elements. |
Teacher's Note
Table salt appears white and tastes salty, but its components - sodium is a reactive metal and chlorine is a toxic gas - have completely different properties.
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ICSE Book Class 9 Chemistry Chapter 3 Elements, Compounds and Mixtures
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