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Atoms and Molecules Class 9 Notes Science Chapter 3

Table of contents

Introduction

Laws of Chemical Combination

What is an Atom?

What is a Molecule?

Molecules of Compounds

Writing Chemical Formulae

Molecular Mass

Introduction
Atoms and molecules are the building blocks of matter, forming the
foundation for everything we see and touch in the world around us.
Understanding these fundamental particles helps us grasp how different
substances interact and combine to create the diverse materials and
phenomena we encounter daily

Maharishi Kanad and Pakudha Katyayama in India suggested that matter can
be divided into smaller particles called Parmanu.
Democritus and Leucippus in Greece proposed that matter can be divided until
it reaches indivisible particles called atoms.
These ideas were based on philosophical considerations and lacked
 experimental validation until the eighteenth century.
In the late 18th century, Antoine L. Lavoisier laid the foundation of chemical
sciences by establishing two important laws of chemical combination.
Lavoisier and Joseph L. Proust conducted numerous experiments to establish
the laws of chemical combinations.
These laws of chemical combination became crucial in understanding the
combination and behavior of elements and compounds.

Question for Chapter Notes: Atoms and Molecules

Try yourself: Who proposed the idea that matter can be divided into smaller
particles called Parmanu?

a. Maharishi Kanad

b. Democritus

c. Antoine L. Lavoisier

d. Joseph L. Proust

View Solution

Laws of Chemical Combination

Understanding the fundamental principles that govern chemical reactions is
crucial for grasping the nature of matter. Two key laws—the Law of
Conservation of Mass and the Law of Constant Proportion—established
through the pioneering work of Lavoisier and Proust, provide essential
insights into how substances interact and combine."
1. Law of Conservation of Mass
Law of conservation of mass states that mass can neither be created nor
destroyed in a chemical reaction.

Example of Law of conservation of Mass

The Law of Conservation of Mass, established by Lavoisier and Joseph L. Proust,

addresses the question of mass change during a chemical reaction. An experiment is
conducted using different pairs of chemicals (X and Y), observing the mass before
and after mixing the solutions. The law asserts that mass remains constant in a
chemical reaction—neither created nor destroyed.

Question for Chapter Notes: Atoms and Molecules

Try yourself: According to the Law of Conservation of Mass, what happens to

the mass during a chemical reaction?

a. The mass increases.

b. The mass decreases.

c. The mass remains constant.

d. The mass is converted into energy.

 View Solution

2. Law of Constant Proportion

The law states that in a chemical substance, the elements are always present in
de nite proportions by mass.

Example of Law of Constant Proportion

For example, water always contains hydrogen and oxygen in the same proportion 1 :
8 by mass, whatever the source of water, from the river, well or rainwater.

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John Dalton's Atomic Theory

John Dalton's Atomic Theory, emerging as a result of these laws, introduces
the concept of atoms as the fundamental particles of matter.

John Dalton

Postulates of Atomic Theory

1. All matter consists of atoms participating in chemical reactions.

2. Atoms are indivisible and remain unchanged in reactions.
3. Atoms of the same element are identical in mass and properties.
4. Atoms of different elements have distinct masses and properties.
5. Atoms combine in simple whole-number ratios to form compounds.
6. The composition of atoms in a compound is constant.

Background on John Dalton

 Born in 1766, Dalton's atomic theory revolutionized the understanding of
matter.
His theory explained the Law of Conservation of Mass and the Law of De nite
Proportions.

What is an Atom?
An atom is the de ning structure of an element, which cannot be broken by
any chemical means.

Atoms are remarkably small, surpassing easy visualization.

Stacking millions of atoms results in a layer as thin as a sheet of paper.

Atomic Radius: Measured in nanometers (1/109 meters = 1 nm).

Question for Chapter Notes: Atoms and Molecules

Try yourself: Which statement best describes the Law of Constant

Proportion?

a. It states that in a chemical substance, elements are always present

in de nite proportions by volume.

b. It states that in a chemical substance, elements are always present

in de nite proportions by mass.

c. It states that in a chemical substance, elements are always present

in inde nite proportions by mass.

d. It states that in a chemical substance, elements can be present in

any proportions by mass.
 View Solution

What Are The Modern Day Symbols Of Atoms Of Different

Elements?
Element symbols have evolved signi cantly over time, re ecting changes in
scienti c understanding and international standards. From Dalton's early use
of symbols to represent atoms to the modern IUPAC-approved symbols, these
notations now follow a standardized format that ensures clarity and
consistency in the representation of elements.

Historical Background: John Dalton was the rst scientist to use symbols for
elements, where each symbol represented a de nite quantity, speci cally one
atom of the element. Berzilius suggested that element symbols be derived from
one or two letters of the element's name.
Origin of Element Names: Element Names are often derived from the place of
discovery (e.g., copper from Cyprus). Some names re ected speci c colors (e.g.,
gold from the English word for yellow).
Modern Symbols: The International Union of Pure and Applied Chemistry
(IUPAC) now approves element names and symbols. Most symbols are derived
from the element's English name, using one or two letters. The rst letter is
always capitalized (uppercase), and the second letter, if present, is lowercase.
First Letter + Another Letter: Symbols are sometimes formed from the rst
letter and another letter from the name (e.g., Chlorine: Cl, Zinc: Zn).
Here are some examples of symbols approved by IUPAC
 Symbols for Some Elements

Latin, German, or Greek Roots: Some symbols come from the element's name
in other languages:
Iron: Fe (from Latin "ferrum")
Sodium: Na (from Latin "natrium")
Potassium: K (from Latin "kalium")

Question for Chapter Notes: Atoms and Molecules

Try yourself: Which scientist pioneered the use of symbols for elements?

a. Berzelius

b. Dalton

c. IUPAC

d. None of the above

View Solution
Atomic Mass
Atomic mass is the total of the masses of the electrons, neutrons, and protons
in an atom, or in a group of atoms, the average mass.

The mass of an atomic particle is called the atomic mass.

This is commonly expressed as per the international agreement in terms of a

uni ed atomic mass unit (AMU).

It can be best de ned as 1/12 of the mass of a carbon-12 atom in its ground
state.

Atomic mass of some

elements

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How Do Atoms Exist?

Atoms of most elements cannot exist independently.
Atoms form molecules and ions, and these aggregate to form visible matter.
What is a Molecule?
A molecule may be de ned as the smallest particle of an element or a
compound that is capable of independent existence and shows all the
properties of that substance.

Molecules of Elements
1. Monoatomic Molecules: Elements like Argon (Ar) and Helium (He) consist of
only one atom of that element in their molecules.
2. Diatomic Molecules: Nonmetals like Oxygen (O2), Hydrogen (H2), Nitrogen
(N2), and Chlorine (Cl2) form molecules with two atoms of the same element,
and this is known as diatomic molecules.
3. Polyatomic Molecules: Some elements, like Phosphorus (P4) and Sulphur (S8),
can form molecules consisting of more than two atoms. For example,
phosphorus forms tetra-atomic molecules (P4), and sulphur forms polyatomic
molecules.

Question for Chapter Notes: Atoms and Molecules

Try yourself: What is the atomic mass of an atom?

a. The total mass of the electrons, neutrons, and protons in an atom.

b. The mass of a carbon-12 atom in its ground state.

c. The average mass of a group of atoms.

d. The mass of an atomic particle.

View Solution
Atomicity
The number of atoms constituting a molecule is known as its atomicity.

Atomicity of some non-metals

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Chapter Notes: Atoms and Molecules

Molecules of Compounds
Atoms of different elements combine in de nite proportions to form
molecules of compounds.
What is an Ion?
Compounds composed of metals and non-metals contain charged species called
ions.
Ions can be single-charged atoms or groups of atoms with a net charge.
An ion can be positively charged (cation) or negatively charged (anion).
Polyatomic ions are groups of atoms with a net charge.

Writing Chemical Formulae

The chemical formula of a compound serves as a symbolic representation of its
composition.
To write chemical formulas, it is essential to understand the symbols and
combining capacities (valencies) of the elements involved.
The combining power or capacity of an element is termed its valency.
This property determines how atoms of an element will combine with atoms of
another element to form a chemical compound.
Valency can be likened to the arms or hands of an atom.
Rules for Formula Writing

The valencies or charges on ions must balance.

In compounds with both a metal and a non-metal, the metal's name or symbol is
written rst.
Examples: Calcium oxide (CaO), sodium chloride (NaCl), iron sul de (FeS), and
copper oxide (CuO).
For compounds formed with polyatomic ions, the number of ions present is
indicated by enclosing the ion's formula in brackets and writing the number of
ions outside the bracket.
Examples: Mg(OH)₂, NaOH.

Question for Chapter Notes: Atoms and Molecules

Try yourself: What is the atomicity of a molecule?

a. The number of atoms in a molecule

b. The number of ions in a molecule

c. The number of elements in a molecule

d. The number of protons in a molecule

View Solution

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Formulae of Simple Compound
To write the chemical formulae of binary compounds (made up of two different
elements), one can use the valencies of the ions involved. The process involves a
"crossover" of the valencies of the combining atoms. Example

The formula of Carbon Tetrachloride (CCl₄): Carbon is a non-metal with a

valency of 4, and chlorine is a non-metal with a valency of 1. The formula
involves crossover: CCl₄.

The formula of Magnesium Chloride (MgCl₂): Magnesium is a metal with a

valency of 2, and chlorine is a non-metal with a valency of 1. The formula
involves crossover: MgCl₂.

Molecular Mass
The molecular mass of a substance is the sum of the atomic masses of all the atoms in
a molecule of that substance. It is expressed in atomic mass units (u).

Example 1:
(a) Calculate the relative molecular mass of water (H₂O).

(b) Calculate the molecular mass of HNO₃.

Solution:
(a) Atomic mass of hydrogen = 1u, oxygen = 16u. So, the molecular mass of water (2H
+ 1O) = 2 × 1 + 1 × 16 = 18u.

(b) Molecular mass of HNO₃ (H + N + 3O) = 1 + 14 + 3 × 16 = 63u.

 Question for Chapter Notes: Atoms and Molecules

Try yourself: What is the chemical formula for magnesium chloride?

a. MgC2

b. ZnCl2

c. MgCl2

d. Mg

View Solution

Formula Unit Mass

Formula unit mass, calculated similarly to molecular mass, is applicable to
substances with ions as constituent particles. It represents the sum of the
atomic masses of all atoms in a formula unit of a compound.

Example 2: Calculate the formula unit mass of CaCl₂.

Solution: Atomic mass of Ca + (2 × atomic mass of Cl) = 40 + 2 × 35.5 = 40 + 71 =

111u.

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FAQs on Atoms and Molecules Class 9 Notes Science Chapter 3

1. What are the different laws of chemical combination?

Ans. The laws of chemical combination include the Law of Conservation of Mass, which
states that mass is neither created nor destroyed in a chemical reaction; the Law of
De nite Proportions, which states that a chemical compound always contains the same
proportion of elements by mass; and the Law of Multiple Proportions, which states that
when two elements combine to form more than one compound, the masses of one
element that combine with a xed mass of the other are in a ratio of small whole
numbers.

2. What is the difference between an atom and a molecule?

3. How do you write chemical formulae for compounds?

4. What is a molecular mass and how is it calculated?

5. What are molecules of compounds and how do they differ from

molecules of elements?
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Study Chapter Notes: Atoms and Molecules on the App

Students of Class 9 can study Chapter Notes: Atoms and Molecules alongwith tests &
analysis from the EduRev app, which will help them while preparing for their exam. Apart
from the Chapter Notes: Atoms and Molecules, students can also utilize the EduRev App for
other study materials such as previous year question papers, syllabus, important questions,
etc. The EduRev App will make your learning easier as you can access it from anywhere you
want. The content of Chapter Notes: Atoms and Molecules is prepared as per the latest Class
9 syllabus.

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