Short Notes - Atoms and Molecules Class 9 Notes | EduRev

➢ Laws of Chemical Combination 

Given by Lavoisier and Joseph L. Proust as follows:

(i) Law of conservation of mass: Mass can neither be created nor destroyed in a chemical reaction.
Example:
A + B → C + D
Reactants → Products
Mass of reactants = Mass of products

(ii) Law of constant proportion: In a chemical substance the elements are always present in definite proportions by mass.

Example: In water, the ratio of the mass of hydrogen to the mass of oxygen is always 1:8 respectively.

These laws lacked explanation. Hence, John Dalton gave his theory about the nature of matter. He said that the smallest particles of matter is called ‘atom’.

➢ Dalton's Atomic Theory 

• Every matter is made up of very small or tiny particles called atoms.
• Atoms are not divisible and cannot be created or destroyed in a chemical reaction.
• All atoms of a given element are same in size, mass and chemical properties.
• Atoms of different elements are different in size, mass and chemical properties.
• Atoms combine in the ratio of small whole numbers to form compounds.
• The relative number and kinds of atoms are constant in a given compound.
• Atom Atoms are the smallest particles of an element which can take part in a chemical reaction.

➢ Size of an atom: Atomic radius is measured in nanometres.

Atomic radii of hydrogen atom = 1 × 10^–10 m.

➢ Symbols of atoms:
(a) Symbols for some elements as proposed by Dalton:

(b) Symbols of some common elements:

➢ Molecule

• It is the smallest particle of an element or a compound which can exist independently.
• Molecules of an element constitutes same type of atoms.
• Molecules may be monoatomic, di-atomic or polyatomic.
• In molecules of compounds atoms of different elements join together in definite proportions and constitutes different type of atoms.

➢ Atomicity

• The number of atoms constituting a molecule is known as its atomicity.

➢ Ions

• The charged particles (atoms) are called ions, they are formed by attaining positive charge or negative charge on it.
• Negatively charged ion is called anion (Cl^–).
• Positively charge ion is called cation (Na⁺).

➢ Valency 

• The combining capacity of an element is known as its valency. Valency is used to find out how atom of an element will combine with the atom of another element to form a chemical compound. (Every atom wants to become stable, to do so it may loose, gain or share electrons.)
  (i) If an atom consists of 1, 2 or 3 electrons in its valence shell then its valency is 1, 2 or 3 respectively,
  (ii) If an atom consists of 5, 6 or 7 electrons in the outermost shell, then it will gain 3, 2 or 1 electron respectively and its valency will be 3, 2 or 1 respectively.
  (iii) If an atom has 4 electrons in the outermost shell than it will share these electrons and hence its valency will be 4.
  (iv) If an atom has 8 electrons in the outermost shell then its valency is 0.

• Some elements show more than one valency hence, termed as variable valency.

➢ Chemical Formulae 

• The chemical formula of a compound is a symbolic representation of its composition.

Rules 

• The valencies or charges on the ion must balance.
• A metal and non-metal compound should show the name or symbol of the metal first.
  Example: 
• If a compound consist of polyatomic ions. The number of ions present in the compound is indicated by enclosing the formula of ion in a bracket and writing the number of ions outside the bracket.
  Example:

Chemical Formula of Some Simple Compounds

➢ Molecular Mass

• It is the sum of the atomic masses of all the atoms in a molecule of the substance. It is expressed in atomic mass unit (u).

➢ Formula
Unit Mass It is the sum of the atomic masses of all atoms in a formula unit of a compound. The constituent particles are ions.

➢ Mole Concept
Definition of Mole: It is defined as one mole of any species (atoms, molecules, ions or particles) is that quantity in number having a mass equal to its atomic or molecular mass in grams. 1 mole = 6.022 × 10²³ in number

Molar mass = mass of 1 mole → is always expressed in grams, and is also known as gram atomic mass.
1u of hydrogen has → 1 atom of hydrogen
1g of hydrogen has → 1 mole of hydrogen
= 6.022 × 10²³ atoms of hydrogen