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Atoms and Molecules

Atoms and Molecules
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Science Square

All matters in the world are made up of elements. And the basic building blocks of elements and compounds are made up of atoms and molecules. The invention of atoms and molecules exist in elements is the first advancement in the world of research regarding nanoparticles.

Science Class 9 Atoms and Molecules Featured

 

Laws of Chemical Combination

1. Law of conservation of mass

Law of conservation of mass states that “mass can neither be created nor destroyed in a chemical reaction".

2. Law of constant proportion 

According to the law of constant, “In a chemical substance, the elements are always present in definite proportions by mass".

 

Dalton’s Postulate Regarding Atoms

Science Class 9 Atoms and Molecules Dalton

  • All matter is made of very tiny particles called atoms.
  • Atoms are indivisible particles, which cannot be created or destroyed in a chemical reaction.
  • Atoms of a given element are identical in mass and chemical properties.
  • Atoms of different elements have different masses 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.

 

Atoms

 An atom is the smallest constituent unit of matter that has the properties of a chemical element. It has two parts. One of them is the nucleus which has the main mass of the atom and comprises of neutrons and protons. And around the nucleus, there are stationary orbits on which the electrons revolve. 

Science Class 9 Atoms and Molecules Atoms size

Symbols for Elements

 

Science Class 9 Atoms and Molecules symbols of elements

 

Dalton was the first scientist who was known to use the symbols for elements in a very specific sense. When he used a symbol for any element he would even define a definite quantity of that element which is one atom of that element.

 

Atomic Mass

Atomic mass is the characteristic mass of each atom in each element. One atomic mass unit is a mass unit equal to exactly one-twelfth (1/12th) the mass of one atom of carbon-12. The relative atomic masses of all elements have been found with respect to an atom of carbon-12. Carbon-12 isotope was chosen as the standard reference for measuring atomic masses.

Science Class 9 Atoms and Molecules atomic massMolecules

A molecule is, in general, a group of two or more atoms that are chemically bonded together that is, tightly held together by attractive forces. A molecule can be defined as the smallest particle of an element or a compound that is capable of an independent existence and shows all the properties of that Substance. Atoms of the same element or of different elements can join together to form molecules.

 Rules for Writing Formulas of Compounds

  • The valencies or charges on the ion must be balanced.
  • When a compound consists of a metal and a non-metal, the name or symbol of the metal is written.
  • In compounds formed with polyatomic ions, the ion is enclosed in a bracket before writing the number to indicate the ratio. In case, the number of a polyatomic ion is one, the bracket is not required.

 

Examples:

  1. Formula of hydrogen chloride

Formula: HCl

  1. Formula for aluminum oxide:

Formula: Al2O3

  1. Formula of sodium nitrate:

Formula: NaNO3

 

Molecular Mass 

The molecular mass of a substance is the sum of the atomic masses of all the atoms in a molecule of the substance. It is, therefore, the relative mass of a molecule expressed in atomic mass units (u).

 Recap

  • During a chemical reaction, the sum of the masses of the reactants and products remains unchanged. This is known as the Law of Conservation of Mass.
  • In a pure chemical compound, elements are always present in a definite proportion by mass. This is known as the Law of Definite Proportions.
  • An atom is the smallest particle of the element that cannot usually exist independently and retain all its chemical properties.
  • A molecule is the smallest particle of an element or a compound capable of independent existence under ordinary conditions. It shows all the properties of the substance.
  • A chemical formula of a compound shows its constituent elements and the number of atoms of each combining element.
  • Clusters of atoms that act as an ion are called polyatomic ions. They carry a fixed charge on them.
  • The chemical formula of a molecular compound is determined by the valency of each element.
  • In ionic compounds, the charge on each ion is used to determine the chemical formula of the compound.
  • Scientists use the relative atomic mass scale to compare the masses of different atoms of elements. Atoms of carbon-12 isotopes are assigned a relative atomic mass of 12 and the relative masses of all other atoms are obtained by comparison with the mass of a carbon-12 atom.
  • The Avogadro constant 6.022 × 1023 is defined as the number of atoms in exactly 12 g of carbon-12.
  • The mole is the amount of substance that contains the same number of particles (atoms/ ions/ molecules/ formula units etc.) as there are atoms in exactly 12 g of carbon-12.
  • Mass of 1 mole of a substance is called its molar mass.

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Quiz for Atoms and Molecules

Q.1

In coastal areas, during the day the air above the land gets heated faster and thus ____________.

a)

air from the land rushes towards the sea

b)

air from the land and sea rushes towards each other and collides

c)

air from the sea rushes towards the land

d)

air from the land rushes towards the sea creating a vacuum on land

Q.2

During lightening, high temperature and pressure converts nitrogen into _____________.

a)

carbonates of nitrogen

b)

oxides of nitrogen

c)

carbonic acid

d)

sulphates of nitrogen

Q.3

Heat trapped in the earth like glass house causes an increase in the temperature of the earth. This is called ___________.

a)

red house effect

b)

white house effect

c)

greenhouse effect

d)

sun heating effect

Q.4

_____ is the major process through which oxygen is returned to the atmosphere.

a) photosynthesis
b) respiration
c) combustion
d) all of these

Q.5

Fill in the blanks: All samples of carbon dioxide contain carbon and oxygen in the mass ratio of 3:8. This is in agreement with the Law of ___________.

a) Conservation of Mass
b) Constant Proportion
c) Multiple Proportion
d) Reciprocal Proportion

Q.6

Kalium is the latin name of which element?

a) Potassium
b) Krypton
c) Calcium
d) Phosphorus

Q.7

Ramesh poured a clear solution from test tube A and an equal quantity of solution from test tube B into a conical flask. He shook it well and kept undisturbed for some time. A white precipitate settled down below the clear solution in the flask after some time. Ramesh forgot to label the test tube A. What can it be?

a) Barium sulphate
b) Sodium chloride
c) Sodium sulphate
d) Barium chloride

Q.8

When we mix BaCl2(aq) with Na2SO4(aq), which of the following observations is correct?

a) no reaction takes place
b) colourless solution is obtained
c) green precipitate is formed
d) white precipitate is formed

Q.9

Fill in the blanks: Mixing of Pb(NO3)2 and KI solution should be done ___________.

a) slowly without stirring
b) slowly with constant stirring
c) fast without stirring
d) very fast with constant stirring

Q.10

An atom is 15 times heavier than 1/12th of the mass of carbon atom (C-12 isotopes). Find the mass in a.m.u?

a) 15
b) 14
c) 12
d) 1.25

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