Notes of Ch 3 Atoms and Molecules| Class 9th Science

Study Material and Notes of Ch 3 Atoms and Molecules Class 9th Science

Topics in the Chapter

• Introduction
• Laws of Chemical Combination
→ Law of Conservation of Mass
→ Law of Constant Proportions
• Dalton's Atomic Theory
• Atoms
→ Modern day symbols of Elements
→ Atomic Mass
→ Atom existence
• Molecules
→ Molecules of Elements
→ Molecules of Compounds
→ What is an ion?
• Atomicity
• Writing a Chemical Formulae
→ Formulae of simple compounds
• Molecular Mass
→ Formula Unit Mass
• Mole Concept

Introduction

→ Around 500 B.C., Indian philosopher Maharishi Kanad, postulated the theory if we go on dividing matter (padarth), we will obtain smallest particle beyond which further division can't be possible which is known as 'parmanu'.

→ Ancient Greek philosophers – Democritus and Leucippus called these particles atoms.

→ Antoine L. Lavoisier laid the foundation of chemical sciences by establishing two important laws of chemical combination.

Laws of Chemical Combination

• This law established after the experiments by Lavoisier and Joseph L. Proust.

• The chemical reaction between two or more substances give rise to products which is governed by certain laws called Laws of Chemical Combination.
• Law of Conservation of Mass

→ During a chemical reaction, the total mass of reactants will be equal to the total mass of the products.

→ Mass can neither be created nor destroyed in a chemical reaction.

→ Example: A (reactant) + B (reactant) → AB (product)
mass of A + mass of B = mass of AB

• Law of Constant Proportions

→ In a chemical reaction, compounds always contain the same elements present in definite proportions by mass irrespective of their source.

→ It was given by Lavoisier.

→ For example: (i) 18 gm of H2O = 2 gm of hydrogen + 16 gm of oxygen
⇒ mass of hydrogen/mass of oxygen = 2/16 = 1/8
(ii) 36 gm of H2O = 4 gm of hydrogen + 32 gm of oxygen
⇒ mass of hydrogen/mass of oxygen = 4/32 = 1/8
(iii) 9 gm of H2O = 1 gm of hydrogen + 8 gm of oxygen
⇒ mass of hydrogen/mass of oxygen = 1/8
This verifies law of constant proportions as the ratio of mass of hydrogen to oxygen is always same.

Dalton's Atomic Theory

→ According to Dalton’s atomic theory, all matter, whether an element, a compound or a mixture is composed of small particles called atoms.

Six Postulates of Dalton's atomic theory:

(i) All matter is made of very tiny particles called atoms.
(ii) Atoms are indivisible particles, which cannot be created or destroyed in a chemical reaction.
(iii) Atoms of a given element are identical in mass and chemical properties. (Law of conservation of mass)
(iv) Atoms of different elements have different masses and chemical properties.
(v) Atoms combine in the ratio of small whole numbers to form compounds. (Law of constant proportion)
(vi) The relative number and kinds of atoms are constant in a given compound.

Atoms

• Atoms are building blocks of all matter.

• According to modern atomic theory, an atom is the smallest particle of an element which takes part in chemical reaction.

•  Atoms are very small and which can’t be seen even through very powerful microscope.

• Atomic radius is measured in nanometres. Nanometres = 10-9 m


• Modern day symbols of Elements

→ Dalton was the first scientist to use the symbols for elements.

→ Berzilius suggested that the symbols of elements should be made from one or two letters of the name of the element.


→ The name copper was taken from Cyprus, a place from where it was found for first time.

→ Now, IUPAC (International Union of Pure and Applied Chemistry) approves names of elements.

→ The first letter of a symbol is always written as a capital letter (uppercase) and the second letter as a small letter (lowercase). For example: hydrogen (H), aluminium (Al), cobalt (Co).

→ Some other symbols have been taken from the names of elements in Latin, German or Greek. For example: Fe from its Latin name ferrum, sodium is Na from natrium, potassium is K from kalium.


• Atomic Mass

→ Dalton’s atomic theory proposed the idea of atomic mass which explained the law of constant proportions so well.

→ The mass of an atom of an element is called its atomic mass.

→ In 1961, IUPAC have accepted ‘atomic mass unit’ (u) to express atomic and molecular mass of elements and compounds.

→ The atomic mass unit is defined as the quantity of mass equal to 1/12 of mass of an atom of carbon-12.

1 amu or u = 1/12 × Mass of an atom of C12
1 u = 1.66 × 10-27 kg


• Atom existence

→ Atoms of most of the elements are very reactive and does not exist in free state.

→ Only the atoms of noble gases (such as He, Ne, Ar, Kr, Xe and Rn) are chemically unreactive and can exist in the free state as single atom.

→ Atoms of all other elements combine together to form molecules or ions.

• Molecules

A molecule is in general a group of two or
more atoms that are chemically bonded
together
A molecule is a group of two or more atoms which are chemically bonded
with each other.
•  A molecule is the smallest particle of matter (except element) which is
capable of an independent existence and show all properties of that
substance.
→ Molecules of Elements
→ Molecules of Compounds
→ What is an ion?
• Atomicity
• Writing a Chemical Formulae
→ Formulae of simple compounds
• Molecular Mass
→ Formula Unit Mass
• Mole Concept



NCERT Solutions of Atoms and Molecules

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