## Carbon Compounds Science Notes

Importent points :

• Organic and inorganic compounds are the two important types of compounds
• The constituent elements common in these compounds are carbon (C), hydrogen (H) and oxygen (O).
• The element carbon belongs to group 14 and its electronic configuration is 24. The valency of carbon is 4.

Bonds in carbon compounds :

→ Properties of carbon compounds :

• Carbon compounds have low melting and boiling points.
• These compounds are bad conductors of heat and electricity.
• The chemical bonds in carbon compounds do not produce ions.
• The force of attraction which holds the atoms together in a molecule is called a chemical bond.
• The number of chemical bonds that an atom of an element forms is called catenation power
• Ionic bonds and covalent bonds are the two important types of chemical bonds.

→ Bonds in carbon compounds :

 Carbon atom Electronic configuration Number of electrons in the Valence shell Nearby noble gas and the electronic configuration He Ne 6C 2, 4 4 2 2, 8

→ Carbon has 4 valence electrons and to attain the configuration of neon by sharing four valence electrons of other atoms. The shared electrons are accommodated in the overlapping region of valence shells of both the atoms.

→ As a result, both the atoms attain a noble gas configuration without generating any net charge on them, which means that atoms remain electrically neutral. Atoms attain stability due to these factors. Therefore this route is adopted by carbon atom to attain a noble gas configuration.

→ The chemical bond formed by sharing of two valence electrons between the two atoms is called covalent bond.

→ A covalent bond is clearly represented by drawing an electron-dot structure. In this method a circle is drawn around the atomic symbol and each of the valence electrons is indicated by a dot or a cross. The covalent bond formed between the atoms is indicated by showing the circles around the atomic symbols crossing each other.

→ The shared electrons are shown in the overlapping regions of the two circles by dot or cross. The electron-dot structure is also drawn without showing the circle. One covalent bond constitutes one pair of shared electrons. A covalent bond is also represented by a small line joining the symbols of the two atoms. The line structure is also called structural formula.

Carbon : A versatile element :

→ Carbon: A versatile element : In short, the entire living kingdom is made from carbon. Carbon is the basic ingredient of our body. Millions of molecules ranging from the small and simple methane molecule to the extremely big D.N.A. molecule are made from carbon. The molecular masses of carbon compounds range up to 1012.

 Carbon Compound Molecular mass Methane CH4 (The smallest carbon compound) 16 Cooking gas (C3H8 + C4H10) 44/58 Benzene (C6H6) 78 Camphor (C10H16O) 152 Penicillin (C16H18N204S) 334 Sugar (C12H22On) 342 Sodium dodecyl benzene sulphate (a detergent) 347 Fat ~ 700 Starch ~103 Cellulose ~105 Protein ~105 Polyethylene ~ 106 D.N.A. ~ 1012

Carbon compounds and molecular masses

Characteristics of carbon :

→ Carbon has a unique ability to form strong covalent bonds with other carbon atoms; this results in formation of big molecules. This property of carbon is called catenation power.

→ One, two or three covalent bonds can bond together two carbon atoms. These bonds are called single covalent bond, double covalent bond and triple covalent bond respectively. Example : ethane (CH3 – CH3). ethene (CH2 = CH2) and ethyne (CH = CH) which contain two carbon atoms.

→ Carbon being tetravalent, one carbon atom can form bonds with four other atoms (carbon or any other). This results in formation of many compounds. These compound possess different properties as per the atoms to which carbon is bonded.

→ For example, five different compounds are formed using one carbon atom and two monovalent elements hydrogen and chlorine : CH4, CH3Cl, CH2Cl2, CHCl3, CCl4 Similarly carbon atoms form covalent bonds with atoms of elements like O, N, Shalogen and P to form different types of carbon compounds in large number

→ Isomerism is one more characteristic of carbon compound which is responsible for large number of carbon compounds.

Hydrocarbons, functional groups and homologous series :

→ Saturated hydrocarbon : In hydrocarbon, the four valencies of carbon atom are satisfied only by the single bonds, such compounds are called saturated hydrocarbons. e.g. Ethane (C2H6), Propane (C3H8).

→ Unsaturated hydrocarbon : The carbon compounds having a double bond or triple bond between two carbon atoms are called unsaturated hydrocarbons.

→ The unsaturated hydrocarbons containing a carbon-carbon double bond are called alkenes. e.g. Ethene (CH2 = CH2), Propene (CH3 – CH = CH2)
The unsaturated hydrocarbons containing a carbon-carbon triple bond are called alkynes. e.g. Ethyne (CH = CH)

→ In the course of millions of years the reserves of crude oil were formed from the dead organisms buried under the sea floor. This crude oil and natural gas are now recovered from the oil wells. The natural gas is mainly methane.

→ The crude oil is a complex mixture of thousands of different compounds. It mainly contains various hydrocarbons. Various useful components such as CNG, LPG, petrol (gasoline), rockel, diesel, engine oil, lubricant, etc. are obtained by separating crude oil using fractional distillation.

→ Structural Isomerism : Butane is represented by two different compounds, as their structural formulae are different. These two different structural formulae have the same molecular formula, i.e. C4 H10

→ The closed chain of carbon atoms are present in some carbon compounds, wherein, rings of carbon atoms form. For example, the molecular formula of cyclohexane is CH and its structural formula contains a ring of six carbon atoms.

→ Benzene is a cyclic unsaturated hydrocarbon. There are three alternate double bonds in the six membered ring structure of benzene. The compounds having this characteristic unit in their structure are called aromatic compounds.

→ Functional group : The compound acquire specific chemical properties due to these hetero atoms or the groups of atoms that contain hetero atoms, irrespective of the length and nature of the carbon chain in that compound. Therefore, these hetero atoms or the groups of atoms containing hetero atoms are called functional groups.

→ Homologous series : The length of the carbon chains in carbon compounds is different, their chemical properties are very much similar due to the presence of the same functional group in them. The series of compounds formed by joining the same functional group in place of a particular hydrogen atom on the chains having sequentially increasing length is called homologous series. Two adjacent members of the series differ by only one – CH2 – (methylene) unit and their mass differ by 14 units.

Characteristics of Homologous series :

→ In homologous series while going in an increasing order of the length of carbon chain

• one methylene unit ( – CH2 – ) gets added
• molecular mass increases by 14 u
• number of carbon atoms increases by one.

→ Chemical properties of members of a homologous series show similarity due to the presence of the same functional group in them.

→ Each member of the homologous series can be represented by the same general molecular formula

→ While going in an increasing order of the length there is gradation in the physical properties, i.e. the boiling and melting points.

Nomenclature of carbon compounds :

→ IUPAC nomeclature system : International Union for Pure and Applied Chemistry (IUPAC) put forth a nomenclature system based on the structure of the compounds, and it was accepted all over the world. There are three units in the IUPAC name of any carbon compound : parent, suffix and prefix.

→ IUPAC name :
CH3 – CH2 – OH
Parent name: Ethane
Suffix: -OH (ol)
(functional group)
Parent suffix: Ethanol
IUPAC name: Ethanol.

Parent name: Pentane
Suffix: – OH (ol)
(functional group)
Assign numbering : 2

Parent suffix: Pentan – 2 – ol
IUPAC name: Pentan – 2 – ol.

• Methane is the component of biogas that makes it useful as fuel.
• Carbon dioxide is formed by the combustion of elemental carbon.
• The biogas combustion is exothermic reaction.

Chemical properties of carbon compounds :

Properties of carbon compounds:

→ Combustion : Methane undergoes combustion in the presence of oxygen to emit heat and light to form carbon dioxide and water.

→ Oxidation : Ethanol gets oxidised in the presence of alkaline potassium permanganate to form ethanoic acid.

→ Addition reaction : Vegetable oil (unsaturated compound) undergoes addition reaction with hydrogen in the presence of nickel catalyst to form vanaspati ghee (saturated compound).

→ Substitution reaction : The reaction in which the place of one type of atom/group in a reactant is taken by another atom/group of atoms, is called substitution reaction. Chlorination of methane, is a substitution reaction which gives four products.

→ Ethanol : Ethanol is a colourless liquid at room temperature and its boiling point is 78 “C. Generally ethanol is called alcohol or spirit. Ethanol is soluble in water in all proportions. When aqueous solution of ethanol is tested with litmus paper it is found to be neutral.

→ Ethanol being good solvent, it is used in medicines such as tincture iodine (solution of iodine and ethanol), cough mixture and also in many tonics.

→ Methanol (CH,OH), the lower homologue of ethanol, is poisonous, and intake of its small quantity can affect vision and at times can be lethal. To prevent the misuse of the important commercial solvent ethanol, it is mixed with the poisonous methanol. Such ethanol is called denatured spirit. A blue dye is also added to it, so that it is easily recognised.

→ Chemical properties of ethanol : Reaction with sodium

→ All the alcohols react with sodium metal to liberate hydrogen gas and form sodium alkoxide salts. When ethanol reacts with sodium metal, hydrogen gas and sodium ethaoxide are formed.

→ Dehydration reaction: When ethanol is heated at the temperature 170 C with excess amount of concentrated sulphuric acid, to form ethene, with elimination of water molecule.

Here, concentrated sulphuric acid acts as a dehydrating agent.

→ Ethanoic acid : Ethanoic acid is a colourless liquid with boiling point 118 °C. Ethanoic acid is commonly known as acetic acid. Its aqueous solution is acidic and turns blue limus red. Vinegar, which is used as preservative in pickles, is a 5-8% aqueous solution of acetic acid. The melting point of pure ethanoic acid is 17 °C. Therefore during winter in cold countries ethanoic acid freezes at room temperature itself and looks like ice. Therefore it is named ‘glacial acetic acid’.

Chemical Properties of ethanoic Acid :

Reaction with base :

→ A reaction with strong base Ethanoic acid gives neutralization reaction with a strong base sodium hydroxide to form a. salt and water.

→ Ethanoic acid reacts with sodium carbonate to form sodium ethanoate, water and carbon dioxide.

→ Esterification reaction : Ethanoic acid reacts with ethanol in presence of an acid catalyst, ethyl ethanoate (ester) is formed. This reaction is known as esterification.

→ Esters have sweet odour. Esters are used for making fragrances and flavouring agents. Saponifaction: When an ester is reacted with the alkali sodium hydroxide, the corresponding alcohol and sodium salt of carboxyclic acid are obtained.

→ This reaction is called saponification reaction, as it is used for preparation of soap from fats. Ester + Sodium hydroxide → Sodium Carboxylate + Alcohol

→ When fat is heated with NaOH solution, soap and glycerin are obtained.

Macromolecules and polymers :

Macromolecules and polymers:

• Macromolecules : The giant carbon molecules formed from hundreds of thousands of atoms are called macromolecules.
• Natural macromolecules : Polysaccharides, proteins and nucleic acid and rubber, etc.
• Manmade macromolecules: Elastomers, plastic, nylon, etc.
• Polymers: A macromolecule formed by regular repetition of a small unit is called polymer. The small unit that repeats regularly to form a polymer is called monomer. The reaction by which monomer molecules are converted into a polymer is called polymerization.

→ Various polymers and their uses:

→ The polymer’s in the above examples are formed by repetition of single monomer. These are called homopolymers. The other type of polymers are formed from two or more monomers. They are called copolymers.

→ For example, PET is poly ethylene terephthalate. The structures of polymers are linear as in the above examples or they are branched and cross linked as well. Polymers aquire various properties as per the nature of the monomers and the type of structure.

→ Some natural polymers and their occurrence :

## Metallurgy Science Notes

Physical properties of metals :

Physical properties of nonmetals :

Properties of metals :

• Solid state (Exception : Mercury and gallium)
• Typical lustre
• Malleability and ductility
• Hardness (Exception : Lithium, sodium and potassium)
• Good conductors of heat and electricity
• High melting and boiling points (On the other hand, the melting and boiling points of the metals sodium, potassium, mercury and galium are very low.)
• Sonorous and produce sound on striking a hard surface.

Properties of nonmetals:

• Gaseous or solid state (Exception : Bromine in liquid state)
• Lack of any typical lustre (Exception : lodine and Diamond)
• Brittleness in the solid state (Exception : Diamond is the hardest natural substance)
• Bad conductors of heat and electricity (Exception: Graphite) (Diamond is good conductor of heat)
• Low melting and boiling points.

Chemical properties of metals :

→ Reaction of metals with oxygen : Metals combine with oxygen on heating in air and metal oxides are formed. Sodium and potassium are highly reactive metals. Sodium metal combines with oxygen in the air at room temperature to form sodium oxide.
4Na(s) + O2(g) → 2Na2O(s)

→ Sodium readily catches fire on keeping exposed to air producing a lot of heat. Therefore, to prevent accident in the laboratory or elsewhere it is kept in kerosene.

→ Sodium oxide reacts with water to form sodium hydroxide (alkali)
Na2 O(s) + H2O(l) → 2NaOH(aq)

→ Magnesium ribbon burns in air form magnesium oxide.

→ Reaction of metals with water : Sodium and potassium react vigorously with water to evolve hydrogen. Calcium reacts with water less vigorously to evolve hydrogen. Magnesium reacts with hot water to evolve hydrogen. Aluminium, iron and zinc do not react with cold or hot water but they react with steam to evolve their oxides and hydrogen.

→ Reaction of metals with acids : Metals react with dilute hydrochloric acid or dilute sulphuric acid to form metal chloride or metal sulphate and hydrogen gas. The rate of evolution of Hy is maximum in case of magnesium. The reactivity decreases in the order Mg > Al > Zn > Fe.

→ Reaction of metals with nitric acid : Metals react with nitric acid to form nitrate salts. Depending on the concentration of nitric acid, various oxides of nitrogen (NO, NO2,) are formed.

→ Aqua Regia: Aqua Regia is freshly prepared by mixing concentrated hydrochloric acid and concentrated nitric acid in the ratio 3 : 1. Aqua Regia is a highly corrosive and fuming liquid. It is one of the few reagents which can dissolve the noble metals like gold and platinum.

→ Reactions of metals with salts of other metals : The reactivity of all metals is not the same. All metals do not react with oxygen, water and acids. As a result, the relative reactivity of metals cannot be determined using these reagents. If a metal A displaces another metal B from the solution of its salt, it means that the metal A is more reactive than the metal B. Metal A+ Salt solution of metal B → Salt solution of metal A + Metal B.

Reactivity series of metals :

→ Reactivity series of metals : The arrangement of metals in the increasing or decreasing order of reactivity is called the reactivity series of metals. Metals are divided into the following groups according to their reactivity.

• Highly reactive metal.
• Moderately reactive metals.
• Less reactive metals.

Chemical properties of nonmetals :

→ Reaction of metals with nonmetals : The ionic compound is formed when metal reacts with nonmetal.

→ Ionic compound is formed as sodium loses one electron while chlorine accepts one electron. Reaction of nonmetals with oxygen: Nonmetals combine with oxygen to form acidic oxides. In some cases, neutral oxides are formed.

→ Reaction of nonmetals with water : Non metals do not react with water, (Exception-Halogen). Chlorine dissolves in water giving the following reaction.

→ Reaction of dilute acid with nonmetals: Nonmetals do not react with dilute acids, (Exception-Halogen). Chlorine reacts with dilute hydrobromic acid to form bromine and HCI.

Cl2(g) + 2HBr(aq) → 2HCl(aq) + Br2(aq)

→ Reaction of nonmetals with hydrogen : Nonmetals react with hydrogen under certain conditions such as proper temperature, pressure and use of catalyst.

S + H2 → H2S(g)
N2 + 3H2 → 2NH3(g)

Ionic compounds :

→ Ionic compounds : The compounds formed from two units, i.e. cation and anion are called ionic compounds. An electrostatic force of attraction between oppositely charged ions (cations and anions) is called an ionic bond.

General properties of ionic compounds:

• Ionic compounds are crystalline solids have a definite shape and hard due to strong electrostatic force of attraction between oppositely charged ions.
• They are generally brittle. When pressure is applied they break into pieces.
• They have high melting and boiling points.
• They are soluble in water and insoluble in solvents such as kerosene and petrol.
• They conduct electricity in the molten state and also in an aqueous solution.

Metallurgy : Various concepts :

→ Minerals and ores : The compounds of metals that occur in nature along with the impurities are called minerals. The minerals from which metals are extracted economically are called ores.

→ Metallurgy: The process of extraction of metal in pure form from the ores. The metals are further purified by different methods of purification. All this process is called metallurgy.

→ Concentration of ores : The process of separating gangue from the ores is called concentration of ores. Some general methods of concentration of ores as follows:

→ Separation based on gravitation : The gravitational method is used to separate the heavy particles of ores from the light particles of gangue. The processes to do this separation are as follows:

• Wilfey table method (Separation based on gravitation)
• Hydraulic separation method.
• Magnetic separation method
• Froth floatation method
• Leaching

→ When a metal loses electrons the process is called an oxidation while when a nonmetal gains electrons, it is called a reduction,
Na → Na+ + e (oxidation)
Cl + e → Cl (reduction)

→ Extraction of reactive metals : The extraction of highly reactive metals has to be done by electrolytic reduction.

→ Extraction of aluminium : Atomic number: 13, Electronic configuration : 2, 8, 3, Valency: 3. Aluminium is extracted from its main ore bauxite (Al2O3nH2O).
Extraction of aluminium involves the following steps:

• Concentration of bauxite ore (Hayer’s process)
• Electrolytic reduction of pure alumina
• Refining.

→ Concentration of bauxite ore : Powdered bauxite is heated with NaOH under high pressure and at 140 °C to 150 °C for 2 to 8 hours in a digester Al2O3 being amphoteric in nature forms sodium aluminate (NaAlO2) which is water soluble. The iron oxide impurities does not dissolve in aqueous NaOH and are separated by filtration.

→ However, silica reacts with sodium hydroxide to form soluble sodium silicate. NaAlO2 is hydrolysed to form insoluble Al(OH) by diluting it with water and cooling to 50 °C. Aluminium hydroxide precipitate is then filtered, dried and calcinated by heating at 1000 °C to obtain pure alumina.

→ Electrolytic reduction of alumina : Cell – A steel tank with graphite lining: Electrolyte – Alumina dissolved in fused cryolite; Cathode – The graphite (carbon) in the form of lining of the steel tank; Anode – Graphite (carbon) rods dipped in the electrolyte; cryolite (Na3AlF6) and fluorspar (CaF2) are added in the mixture to lower its melting point up to 1000°C.

→ Electrolysis products: Cathode – Aluminium metal, Anode – Oxygen gas.

At the anode : 2O2- → O2 + 4e
At the cathode : Al3+ + 3e → Al

→ Extraction of moderately reactive metals : In metals, in the middles of the reactivity series such as iron, zinc, lead, copper are moderately reactive. These metals occur in the form of their sulphide salts or carbonate salts.

→ The sulphides ores are strongly heated in air to convert them into oxides. This process is called roasting. Carbonate ores are strongly heated in a limited supply of air to convert them into oxides. This process is called calcination.

→ The following reaction occur during roasting and cacination of zinc ore.
Roasting : 2ZnS +3O2 → 2ZnO + 2SO2
Calcination: ZnSCO3 → ZnO + CO2
The zinc oxide is reduced to zinc by using suitable reductant such as carbon.
ZnO + C → Zn + CO↑

→ Extraction of less reactive metals : The less reactive metals are at the bottom of reactivity series of metal. These metals are found in free state in nature. For example, gold, silver, platinum. The reserves of copper in free state are exhausted long ago. Copper is found mainly in the form of Cu,s. Copper is obtained from Cu S ore just by heating in air.
2Cu2S +3O2 → 2Cu2O + 2SO2
2Cu2O + Cu2S → 6Cu + SO2

→ Refining of metals : Metals obtained by various reduction processes contain impurities Electrolysis method is used to remove impurities to obtain pure metals.

→ Corrosion is degradation of a material due to reaction with its environment.
When old iron bars in the buildings are exposed to moist air for a long time, they acquire a coating of brown flaky substance called rust. (Fe2O3.H2O)

→ If copper vessels are not cleaned for a long time, they react with moist carbon dioxide in the air, lose their shine and gain a green coat of copper carbonate. (CuCO3)

→ When silver ornaments or idols are kept exposed to air for a long time, silver reacts with sulphur in the air to form a coating of black silver sulphide. (Ag2S)

→ The metallic parts of the body of old cars are corroded, eaten up and sometimes become perforated. The old cars also lose the original colour due to formation of flakes of rust.

Prevention of corrosion :

→ By coating with some substance on the metal surface so that the contact of the metal with moisture and oxygen in the air is prevented and no reaction would occur between them.

→ By applying a layer of paint, oil, grease or varnish on the surface of a metal to prevent corrosion. For example, corrosion of iron can be prevented by this method.

→ Corrosion is prevented by coating a corrosive metals with a noncorrosive metal. This can be done in many ways:

• Galvanizing
• Tinning
• Anodization
• Electroplating
• Alloying.

## Lenses Science Notes

Important Points :

→ Indicate the following terms related to spherical mirrors in figure 7.1 : pole, centre of curvature, radius of curvature, principal focus.

→ The given part of a hollow spherical glass can be converted into a concave mirror by

• polishing (silvering) its inner side (inner surface or concave surface) to make it reflecting or
• coating its outer side with a thin layer of silver and painting it with red colour to protect the silver coating.

[Note: Case (i) corresponds to the front surface silvered concave mirror.

→ The given part of a hollow spherical glass can be converted into a convex mirror by

• polishing (silvering) its outer side (outer surface or convex surface) to make it reflecting or
• coating its inner side with a thin layer of silver and painting it with red colour to protect the silver coating.

Note : Case (1) corresponds to the front surface silvered convex mirror

Lenses :

Lens : A lens is a transparent material bound by two surfaces, out of which at least one surface is spherical

→ Convex lens: A lens having both spherical surfaces puffed up outwards is called a convex lens or double convex lens or biconvex lens. A lens having one surface plane and the other (spherical surface) bulging outward is called a planoconvex lens.

→ A convex lens is thicker in the middle than at the edges. It is a converging lens. The concavo-convex lens has one spherical surface concave and the other convex such that it behaves as a convex lens.

→ Concave lens: A lens having both spherical surfaces curved inwards is called a concave lens or double concave lens or biconcave lens. A lens having one surface plane and the other (spherical surface) curved inwards is called a plano-concave lens.

→ A concave lens is thicker at the edges than in the middle. It is a diverging lens. The convexo-concave lens has one spherical surface convex and the other concave such that it behaves as a concave lens.

→ Centre of curvature (C) of a lens : The centres of the spheres whose parts form the surfaces of a lens are called the centres of curvature of the lens. A lens has two centres of curvature C, and C for its two spherical surfaces.

→ Radii of curvature (R, R) of a lens : The radii of the spheres whose parts form surfaces of a lens are called the radii of curvature of the
lens.

→ Principal axis of a lens : The imaginary straight line passing through the two centres of curvature of a lens is called the principal axis of the lens.

→ Optical centre (O) of a lens : The point inside a lens on the principal axis, through which light rays pass without changing their path is called the optical centre (O) of the lens.

→ Principal focus (F) of a lens : When light rays parallel to the principal axis are incident on a convex lens, they converge at a point on the principal axis. This point is called the principal focus (F) of the convex lens.

→ Light rays travelling parallel to the principal axis of a concave lens diverge after refraction in such a way that they appear to be coming out of a point on the principal axis. This point is called the principal focus of the concave lens. A lens has two principal foci F, and F.

→ Focal length of a lens : The distance between the optical centre and the principal focus of a lens is called the focal length of the lens.

Ray diagram for refracted light :

→ Rules for obtaining an image formed by a convex lens:

• When the incident ray is parallel to the principal axis, the refracted ray passes through the principal focus.
• When the incident ray passes through the principal focus, the refracted ray is parallel to the principal axis.
• When the incident ray passes through the optical centre of the lens, it passes without changing its direction.

[Note: Here, a ray means a ray of light.]

→ Image formation by a convex lens:

 Position of the object Position of the image Size of the image (relative to the size of the object) Nature of the image At infinity At focus F2 Point image Real and inverted Beyond 2FX Between F2 and 2F2 Smaller Real and inverted At 2FX                   ‘ At 2F2 Same size Real and inverted Between Fx and 2FX Beyond 2F2 Larger    _ Real and inverted At focus Fx At infinity Very large Real and inverted Between Fx and O On the same side of the lens as the object Very large Virtual and erect

[Note: In this chapter, no distinction is made between the terms focus and principal focus. Focus is also called focal point.]

→ An image formed by convergence of reflected or refracted rays of light at a point is called a real image.
An image formed at a point from which the reflected or refracted rays of light appear to diverge is called a virtual image.

→ A real image can be obtained on a screen. A virtual image cannot be obtained on a screen. Thus, if an image can be obtained on a screen, it must be real; if it cannot be obtained on a screen, it must be virtual. This is how we can find out whether an image is real or virtual.

→ Rules for obtaining an image formed by a concave lens:

• When the incident ray is parallel to the principal axis, the refracted ray, when extended backwards, passes through the principal focus.
• When the incident ray is directed towards the principal focus Fy, the refracted ray is parallel to the principal axis.
• When the incident ray passes through the optical centre of the lens, it passes without changing its direction.

→ The image formed by a concave lens is always virtual, erect and smaller than the object. It is on the same
side of the lens as the object. Generally, it is formed between the optical centre of the lens and the principal focus F1. If the object is at infinity, the image is a point image formed at F1.

 Position of the object Position of the image Size of the image (relative to the size of the object) Nature of the image At infinity On the first focus Fx Point image Virtual and erect Anywhere between optical centre O and infinity Between optical centre and focus Fx Small Virtual and erect

→ According to the Cartesian sign convention, the pole (P) of a spherical mirror is taken as the origin and the principal axis is taken as X-axis of the coordinate system.

• The object is always placed on the left of the mirror.
• All distances parallel to the principal axis are measured from the pole of the mirror.
• All distances measured to the right of the origin (pole) are taken as positive while distances measured to the left of the origin (pole) are taken as negative.
• Distances measured perpendicular to and above the principal axis are taken as positive.
• Distances measured perpendicular to and below the principal axis are taken as negative.
• The focal length of a convex mirror is positive while that of a concave mirror is negative.

Sign convention :

→ Sign convention for a lens : In this case, the optical centre (O) of the lens is taken as the origin and the principal axis of the lens is taken as X-axis of the coordinate system. The sign conventions regarding the measurement of distances parallel to the principal axis and those perpendicular to the principal axis are the same as for a spherical mirror. Hence, the focal length of a convex lens is positive and that of a concave lens is negative.

→ Lens formula: The relationship between the object distance (u), image distance (v) and focal length of a lens is called the lens formula and is given as $$\frac{1}{v}-\frac{1}{u}=\frac{1}{f}$$

→ Magnification by a lens : The magnification (M) produced by a lens
= $$\frac{\text { height of the image }\left(h_{2}\right)}{\text { height of the object }\left(h_{1}\right)}=\frac{v}{u}$$

Magnification is positive for a virtual image and negative for a real image.

→ Power of a lens : The power (P) of a lens
= $$\frac{1}{\text { focal length }(f) \text { of the lens }}$$
Its SI unit is the dioptre (D).
If f = 1 metre, P = 1 dioptre.

→ Combination of lenses : If two lenses with focal lengths f1 and f2 fare kept in contact with each other, the effective focal length of the combination, f, is given by $$\frac{1}{f}=\frac{1}{f_{1}}+\frac{1}{f_{2}}$$

→ The effective power of the combination of the lenses, P, is given by P = P1 + P2, where
p = $$\frac{1}{f}$$, P1 = $$\frac{1}{f_{1}}$$ and P2 = $$\frac{1}{f_{2}}$$

Working of the human eye and lens :

→ Power of accommodation of the eye : The ability of the eye lens to adjust its focal length is called the power of accommodation of the eye.

→ The minimum distance of distinct vision and the near point: The minimum distance from the normal eye at which an object is clearly visible without stress on the eye is called the minimum distance of distinct vision. It is 25 cm for the normal human eye.

→ The position of the object at the minimum distance of distinct vision is called the near point of the eye. For a normal human eye, the near point is at 25 cm from the eye.

→ The minimum distance of an object from a normal eye, at which it is clearly visible without stress on the eye, is called as minimum distance of distinct vision. The position of the object at this distance is called the near point of the eye, for a normal human eye, the near point is at 25 cm.

→ The farthest distance of an object from a human eye, at which it is clearly visible without stress on the eye is called farthest distance of distinct vision. The position of the object at this distance is called the far point of the eye For a normal human eye, the far point is at infinity.

→ The eye ball is approximately spherical and has a diameter of about 2.4 cm. The working of the lens in human eye is extremely important. The lens can change its focal length to adjust and see objects at different distances. In a relaxed state, the focal length of healthy eyes is 2 cm. The other focus of the eye is on the retina

Defects of vision and their correction :

→ Myopia or Nearsightedness : Myopia or near sightedness is the defect of vision in which a human eye can see nearby objects distinctly but is unable to see distant objects clearly. In this case, the image of a distant object is formed in front of the retina. This defect can be corrected using a concave lens of suitable focal length.

→ Hypermetropia or Farsightedness: Hypermetropia or farsightedness is the defect of vision in which a human eye can see distant objects distinctly but is unable to see nearby objects clearly. In this case, the image of a nearby object would fall behind the retina. This defect can be corrected using a convex lens of
suitable focal length.

→ Presbyopia (also called old age hyper metropia): Presbyopia is the defect of vision in which aged people find it difficult to see the nearby objects comfortably and clearly without spectacles. This defect can be corrected using a convex lens of suitable focal length.

Uses of lenses :

→ Uses of a convex lens : Simple microscope, compound microscope, telescope, camera, projector, spectrometer, spectacles, etc., make use of one or more convex lenses. A simple microscope is used by watch repairers, Jewellers, etc. A compound microscope is used to observe bacteria, cells, microorganisms, etc. A telescope is used to observe distant terrestrial objects or astronomical objects like planets, stars and comets.

→ Uses of a concave lens: A concave lens is used in spectacles to correct myopia. It is also used in optical instruments.

→ Persistence of vision: The image of an object remains imprinted on our retina for $$\frac{1}{16}$$th of a second after the object is removed from the sight. The sensation on the retina persists for a while. This is called persistence of vision. The retina in our eyes is made of many light sensitive cells. Due to these cells, we get information about the brightness or dimness of the object as well as the colour of the object

## Refraction of light Science Notes

Reflection of light :

When light is incident on the surface of an object, in general, it is deflected in different directions. This process is called reflection of light.

Laws of reflection of light :

• The incident ray and the reflected ray of light are on the opposite sides of the normal to the reflecting surface at the point of incidence and all the three are in the same plane.
• The angle of incidence and the angle of reflection are equal in measure.

Refraction of light :

Refraction of light : The change in the direction of propagation of light as it passes obliquely from one transparent medium to another is called refraction of light. Refraction occurs as the velocity of light is different in different media.

Laws of refraction :

Laws of refraction of light:

→ The incident ray and the refracted ray are on the opposite sides of the normal to the surface at the point of incidence and all the three, i.e., the incident ray, the refracted ray and the normal are in the same plane.

→ For a given pair of media, the ratio of the sine of the angle of incidence to the sine of the angle of refraction is constant (Snell’s law). This constant is called the refractive index of the second medium with respect to the first medium.
[Note: Here, a ray means a ray of light)

Refractive index :

→ Refractive index : If i is the angle of incidence and r is the angle of refraction, then
$$\frac{\sin i}{\sin r}$$ = constant (Snell’s law).
This constant is called the refractive index of the second medium with respect to the first medium, and is denoted byn. Thus, 2n1 = $$\frac{\sin i}{\sin r}$$

→ Also, if y, is the magnitude of) the velocity of light in the first medium and u, is the magnitude of) the velocity of light in the second medium, then
2n1 = $$\frac{v_{1}}{v_{2}}$$

→ Similarly, the refractive index of the first medium with respect to the second medium is given by
1n2 = $$\frac{v_{2}}{v_{1}}$$

→ If the first medium is vacuum, 2n1 is considered with respect to vacuum. It is called the absolute refractive index of the medium 2 and is denoted by n.

→ The refractive index of a medium depends upon the magnitude of the velocity of light in the medium. [Note: The absolute refractive index of air is 1.003. This shows that for almost all practice purposes, the speed of light in air is very nearly the same as that in vaccum.]

→ Behaviour of a ray of light in refraction : When a ray of light passes obliquely from an optically rarer medium (medium of lower refractive index) to an optically denser medium (medium of higher refractive index), it bends towards the normal at the point of incidence. Here, i is greater than r, and 2n1 is greater than 1. The greater the value of 2n1, the greater is the bending towards the normal.

→ When a ray of light passes obliquely from an optically denser medium to an optically rarer medium, it bends away from the normal at the point of incidence. Here, r is greater than i, and 2n1 is less than 1. The greater the value of 2n1, the less is the bending away from the normal.

→ If a ray of light is incident normal to the interface between any two media (whether passing from an optically rarer medium to an optically denser medium or from an optically denser medium to an optically rarer medium), the angle of incidence is zero and so also the angle of refraction. Here, the light goes ahead in the same direction.
$$\frac{\sin i}{\sin r}$$ = constant = n

→ n is called the refractive index of the second medium with respect to the first medium. This second law is also called, Snell’s law. A ray incident along the normal (i = 0) goes forward in the same direction (r = 0).

→ Absolute refractive indices of some media

 Substance Refractive index Air 1.0003 Ice 1.31 Water 1.33 Alcohol 1.36 Kerosene 1.39 Fused quartz 1.46 Turpentine oil 1.47 Benzene 1.50 Crown glass 1.52 Rock salt 1.54 Carbon disulphide 1.63 Dense flint glass 1.66 ‘ Ruby 1.76 Sapphire 1.76 Diamond 2.42

→ Local atmospheric conditions affect refraction of light : e.g., mirage, objects beyond and above a holi fire appear to be shaking.

→ Twinkling of a star and atmospheric refraction : As a star is far away from the earth, it appears as a point source of light. When starlight enters the earth’s atmosphere, it undergoes refraction continuously in the medium with gradually varying refractive index.

→ The bending of starlight occurs towards the normal as it passes from the optically rarer, part of the medium to the optically denser part. Hence, when a star is observed near the horizon, its apparent position is slightly higher than the actual position.

→ Further, the apparent position varies with time as the medium is not stationary. Also, there is fluctuation in the brightness of a star when observed from the earth. This is called twinkling of a star.

→ The planets are relatively closer to the earth. Hence they appear as a collection of a large number of point sources of light. The net fluctuation in the brightness of a planet, therefore, turns out to be zero. Also, there is no change in the average position of a planet. Hence, planets do not twinkle.

The advanced sunrise and delayed sunset are also the result of atmospheric refraction.

Dispersion of light :

→ Dispersion of light: The process of separation of light into its component colours while passing through a medium is called dispersion of light. The band of coloured components of a light beam is called its spectrum.

→ The formation of a rainbow is due to refraction, dispersion, internal reflection and again refraction of sunlight by water droplets under appropriate conditions.

→ Our eyes are sensitive to electromagnetic radiation of wavelength in the range 400 nm to 700 nm. [1 nm – 10-m; nm nanometer] Wavelength of red light is close to 700 nm and that of violet light is close to 400 nm.

→ Partial and total internal reflection: When light travels from one medium to another, part of incident light comes back into the first medium. This is called partial reflection. Remaining part is refracted.

→ When light travels obliquely from a denser medium to a rarer medium, the angle of refraction r is greater than the angle of incidence i. Also, the ratio sini/sinr is constant For a particular value of 1, r becomes 90°. This particular angle of incidence is called critical angle.

→ For i > critical angle, as r cannot be greater than 90°, light is totally reflected in the denser medium. This is called total internal reflection. Here, 2n1 = $$\frac{\sin i}{\sin 90^{\circ}}$$ = sin i, where i is sin 90° the critical angle.

→ In vacuum, the speed of light does not depend on the frequency of light. But in a material medium, it is not so. Hence, the refractive index of glass (n) is different for different colours (different frequencies).

→ It is maximum for violet colour and minimum for red colour, n (violet) > n (indigo) > n (blue) > n (green) > n (yellow) > n (orange) > n (red).

## Heat Science Notes

Important Points :

• Heat is a form of energy. Particles of matter (atoms, molecules, etc.) possess potential energy and kinetic energy.
• Total energy (potential energy + kinetic energy) of all particles of matter in a given sample is called its thermal energy.
• When two bodies at different temperatures are in thermal contact with each other, there is transfer of thermal energy from a body at higher temperature to a body at lower temperature.
• This energy in transfer is called heat. It is expressed in joule, calorie and erg.
• Temperature is a quantitative measure of degree of hotness or coldness of a body.
• It is expressed in °C, °F or K (kelvin).
• Temperature determines the direction of energy transfer.
• Ways of heat transfer : conduction, convection and radiation.

[Note : heat = heat energy. In the textbook, both the terms are used.

Latent heat :

→ Latent heat : When there is a change of state of a substance, [solid ↔ liquid, liquid ↔ gas (vapour), solid ↔ gas (vapour)] heat energy is absorbed by the substance or heat energy is removed from the substance at constant temperature.

→ This heat energy is called latent heat of transition (or transformation or change of state). Latent heat per unit mass of the substance is called specific latent heat.

→ The amount of heat energy absorbed at constant temperature by unit mass of a solid to convert into liquid phase is called the specific latent heat of fusion, and that constant temperature is called the melting point of the substance.

→ The amount of heat energy absorbed at constant temperature by unit mass of a liquid to convert into gaseous phase is called the specific latent heat of vaporization and that constant temperature is called the boiling point of the substance.

→ Specific latent heat is expressed in J/kg, erg/g, cal/g, kJ/kg and kcal/kg.

Heat absorbed or given out in change of state = mL, where m is the mass of the substance.

Regelation:

Regelation: The phenomenon in which ice converts to liquid due to applied pressure and then re-converts to ice once the pressure is removed is called regelation.

Anomalous behaviour of water:

→ Anomalous behaviour of water : If water is heated from 0 °C to 4 °C, it contracts instead of expanding. At 4 °C its volume is minimum. If the water is heated further, it expands, i.e., its volume increases.

→ This abnormal behaviour of water in the temperature range 0 °C to 4 °C is called anomalous behaviour of water. The density of water is maximum at 4 °C. Hope’s apparatus is used to study anomalous behaviour of water.

Dew point and humidity :

→ Dew point temperature : If the temperature of unsaturated air is decreased, a temperature is reached at which the air becomes saturated with water vapour. This temperature is called the dew point temperature.

→ Absolute humidity : The mass of water vapour present in a unit volume of air is called absolute humidity. Generally it is expressed in kg/m.

→ Relative humidity : The ratio of the actual mass of water vapour content in the air for a given volume and temperature to that required to make the same volume of air saturated with water vapour at the same temperature is called the relative humidity. This ratio, multiplied by 100, gives the percentage relative humidity. At the dew point the relative humidity is 100%.

→ Take a bottle of cold water out of a refrigerator and keep it outside for a while. Observe the outer surface of the bottle.

→ Drops of water can be observed on the outer surface of bottle. In the same way, if we observe the leaves of plants/ grass or windowglass of a vehicle in the early morning we see water droplets collected on the surface.

→ Through these two observations, we sense the presence of water vapour in the atmosphere. When air cools, due to decrease in temperature it becomes saturated with water vapour. As a result, the excess water vapour gets converted into tiny droplets. The dew-point temperature is decided by the amount of vapour in the air.

→ Unit of heat : Heat can be expressed in various units, e.g. joule (J), erg, calorie (cal), kilocalorie (kcal). The amount of heat necessary to raise the temperature of 1 g of water by 1 °C from 14.5 °C to 15.5 °C is called one calorie.

→ The amount of heat necessary to raise the temperature of 1 kg of water by 1 °C from 14.5 °C to 15.5 °C is called one kilocalorie.
1 kcal = 103cal, 1 cal = 4.18 J,
1 kcal = 4.18 × 103 J.

Specific heat capacity :

→ Specific heat capacity (c): The amount of heat energy required to raise the temperature of a unit mass of an object by 1 °C is called the specific heat capacity or simply specific heat of the object. It is expressed in various units such as J/kg . °C, erg/g . °C, cal/g . °C, kcal/kg .°C.

 Substance Specific heat (c) (cal/g.°C) Water 1.0 Paraffin 0.54 Kerosene 0.52 Aluminium 0.215 Iron 0.110 Copper 0.095 Silver 0.056 Mercury 0.033
• Heat absorbed by an object = mcΔt, where m is the mass of the object and ΔT is the increase in the temperature of the object.
• Heat lost (given out) by an object = mcΔT
• Here ΔT is the decrease in the temperature of the object.

→ Principle of heat exchange : If a system of two objects is isolated from the environment by keeping it inside a heat resistant box, then no energy can leave the box or enter the box. In this situation, heat energy lost by the hot object = heat energy gained by the cold object. In due course, the two objects attain the same temperature.

→ Sublimation: The phenomenon in which a solid directly passes to the gaseous state without passing through the intermediate liquid state is known as sublimation. Iodine, ammonia and camphor possess the property of sublimation.

→ Effect of pressure on the melting point of a substance : At a given pressure, a given solidmelts at a fixed temperature. A change in pressure changes the melting point of the substance. In the case of the solids which expand on melting, an increase in the pressure raises the melting point of the solid, e.g., lead and wax.

→ In the case of the solids which contract on melting, an increase in pressure lowers the melting point of the solid, e.g., ice, antimony and bismuth.

→ Effect of pressure on the boiling point of a liquid : The boiling point of a liquid depends on the pressure on its surface. An increase in pressure raises the boiling point of a liquid while a decrease in pressure lowers its boiling point.

## Effects of Electric Current Science Notes

Important Points :

• A material which has very low electrical resistance is called a good conductor of electricity. Examples: silver, copper, aluminium.
• A material which has extremely high electrical resistance is called an insulator of electricity.
• Examples : rubber, wood, glass.
• When we pick up a piece of iron resting on the ground, we don’t get electric shock because that piece does not carry any electric current at that time.

Energy transfer in electric circuit :

→ Electric power : Electric power is the electric work done per unit time or electric energy used per unit time. Its SI unit is the watt (W).

→ Electric power (P)
=
P = VI = I2R = V2/R.

→ Mechanical power (P)

→ The watt: If one joule of electric work is done per second, the electric power is 1 watt.
1 watt (W) = $$\frac{1 \text { joule }(\mathrm{J})}{1 \text { second }(\mathrm{s})}$$

→  Commercial unit of electric energy : The commercial unit of electric energy is the kilowatt-hour (kWh).
1 kW.h -3.6 × 106 J
It is commonly known as the unit.

→  The unit of electric power 1 W is a very small unit, hence 1000 W or 1 kW is used as a unit to measure electric power, in practice. If 1 kW power is used for 1 hour, it will mean 1 kW × 1h of electric energy is used 1 kW.h -1 kilowatt-hour = 1000 W × 3600 S
= 3.6 × 106 W.s = 3.6 × 106 J

→  Electricity bill : Electricity bill shows the consumption of units (i.e., kW.h) and the cost of using electric energy Check monthly electricity bill received from the Electricity Distribution Co. Ltd. Observe various details and get information about them. The electricity bill specifies the usage in ‘Units’. What is this unit? When 1 kW.h electric energy is used, it is termed as 1 unit of energy.

Heating effect of electric current :

→  Joule’s law about heating effect of electric current: The quantity of heat produced (H) in a conductor of resistance R, when a current I flows through it for a time t is directly proportional to

• the square of the current
• the resistance of the conductor
• the time for which the current flows.

→  H = I2 Rt = VIt = $$\frac{V^{2}}{R}$$t, where V is the potential difference (RI) across the conductor. Here, H is expressed in joule, V in volt, I in ampere, R in ohm and t in second. 1 calorie (cal) = 4.18 joules (J). With V in volt, I in ampere, R in ohm and t in second, we have:

→  The working of an electric bulb, electric iron, fuse wire, etc., is based on the heating effect of electric current

Magnetic effect of electric current :

→  When an electric current is passed through an electric resistor (electric conductor), heat is produced in it. Passage of electric current through a conductor also produces a magnetic field around it. This effect, called magnetic effect of electric current, was discovered by Hans Christian Oersted. The unit of intensity of magnetic field, the oersted, is named after him.

→  Oersted’s discovery : Hans Christian Oersted (1777 – 1851), Danish physicist, discovered the magnetic effect of electric current in 1820. He observed the deflection of a compass needle when placed near a wire carrying an electric current. The experiment described on page 51 of the textbook refers to his discovery.

→  Right hand thumb rule : Imagine that you have held a current-carrying straight conductor in your right hand in such a way that your thumb points in the direction of the current. Then turn your fingers around the conductor. The direction of the fingers is the direction of the magnetic lines of force produced by the current.

Magnetic field due to a current-carrying conductor :

• The intensity of the magnetic field produced at a given point is directly proportional to the current passing through the conductor.
• The intensity of the magnetic field produced by a given current in the conductor decreases as the distance from the conductor increases.

→ A magnetic field is produced around a straight current-carrying conductor. If the current is unchanged, this magnetic field reduces as the distance from the wire increases. Therefore, the concentric circles representing the magnetic lines of force are shown bigger and rarefied as conditioners, use of electricity in shops, etc.

→ As a result, excessive current is drawn from the transformer supplying the electricity, and if the capacity of the transformer is insufficient, its fuse wire melts and the supply gets shut down. Such events occur due to overloading.

→ These days miniature circuit breaker (MCB) switches are used in homes. When the current in the circuit suddenly increases this switch opens and current stops. Different types of MCBs are in use. For the entire house, however the usual fuse wire is used.

• Lamps, TV, computer, electric fan, electric bell.
• Heating effect, magnetic effect, production of light, conversion of electric energy into mechanical energy and the conversion of that mechanical energy into sound.

## Chemical reactions and equations Science Notes

Importent points :

• Elements are divided into three classes i.e. metals, nonmetals and metalloids. When two or more elements combine chemically in a fixed proportion by weight, a compound is formed.
• The properties of a compound are altogether different from those of the constitutional elements.
• The number of electrons that an atom of an element gives away or takes up while forming an ionic bond, is called the valency of that element.
• While writing the molecular formulae of different compounds, the symbol of the radicals and their valence should be known.
• The number of the ions is written as subscript on the right of the symbol of the ion. By cross multiplication of valencies chemical formula is obtained

Chemical reactions :

→ During chemical reactions composition of the matter changes and that change remains permanent and during physical change only the state of matter changes and this change is often temporary in nature. Identify physical and chemical changes from the phenomena given in the following table.

 Phenomenon Physical change Chemical change 1. Transformation of ice into water ✓ 2. Cooking of food ✓ 3. Ripening of fruit ✓ 4. Milk turned into curd ✓ 5. Evaporation of water ✓ 6. Digestion of food in the stomach 7. Size reduction of naphtha balls exposed to air ✓ 8. Staining of Shahbadi or Kadappa tile by lemon juice ✓ 9. Breaking of a glass object on falling from a height ✓

Chemical reaction : A process in which some substances undergo bond breaking and are transformed into new substances by formation of new bonds is called a chemical reaction.

Rules writing chemical reaction :

→ Chemical equation : The representation of a chemical reaction in a condensed form using chemical formulae is called as the chemical equation.

Rules used in writing a chemical equation :

• The reactants are written on the left hand side (LHS), while the products are written on the right hand side (RHS).
• Whenever there are two or more reactants, a plus sign (+) is written between each two of them. Similarly, if there are two or more products, a plus sign is written between each two of them.
• Reactant side and product side are connected with an arrow (→) pointing from reactants to products. The arrow represents the direction of the reaction. Heat is to be given from outside to the reaction, it is indicated by the sign ∆ written above the arrow.
• The conditions like temperature, pressure, catalyst, etc., are mentioned above the arrow (→) pointing towards the product side.
• The physical states of the reactants and products are also mentioned in a chemical equation. The notations g. 1, s, and aq are written in brackets as a subscript along with the symbols /formulae of reactants and products.
• The symbols g. 1, s, and aq stand for gaseous, liquid, solid and aqueous respectively. If the product is gaseous, instead of (g) it can be indicated by an arrow↑pointing upwards.
• If the product formed is insoluble solid, then instead of (s) it can be indicated by an arrow↓pointing downwards.
• Special information or names of reactants/ products are written below their formulae.

Balancing a chemical equation :

→ In a chemical reaction, the number of atoms of the elements in the reactants is same as the number of atoms of those elements in the product, such an equation is called a balanced equation.

→ Example: AgNO3 + Nacl → AgCl + NaNO3
In the above reaction, the number of atoms of the elements in the reactants is same as the number of atoms of elements in the products.

Types of chemical reactions :

Types of chemical reactions :

• Combination reaction
• Decomposition reaction
• Displacement reaction
• Double displacement reaction.

→ Combination reaction : When two or more reactants combine in a reaction to form a single product, it is called a combination reaction.

→ An example of combination reaction : The ammonia gas reacts with hydrogen chloride gas to form the salt in gaseous state, immediately it condenses at room temperature and gets transformed into the solid state.

→ Decomposition reaction: The chemical reaction in which two or more products are formed from a single reactant is called decomposition reaction.

→ Examples of decomposition : Thermal decomposition: The reaction in which a compound is decomposed by heating it to a high temperature is called thermal decomposition At high temperature, calcium carbonate decomposes into calcium oxide and carbon dioxide.

→ Electrolytic decomposition : The reaction in which a compound is decomposed by passing an electric current through its solution or molten mass is called an electrolytic decomposition.
When an electric current is passed through acidulated water, it is electrolysed giving hydrogen and oxygen.

→ It is possible to produce hydrogen by decomposition of water by means of heat, electricity or light.

→ Displacement reaction : The reaction in which the place of the ion of a less reactive element in a compound is taken by another more reactive element by formation of its own ions, is called displacement reaction.

→ An example of displacement reaction : When zinc granules are added to the blue coloured copper sulphate solution, the zinc ions formed from zinc atoms take the place of Cu2+ ions in CuSO4, and copper atoms, formed from Cu2+ ions comes out i.e. the more reactive zinc displaces the less reactive Cu from copper sulphate.

→ Double displacement reaction: The reaction in which the ions in the reactants are exchanged to form a precipitate are called double displacement reaction.

→ An example of double displacement reaction : Solutions of sodium chloride and silver nitrate react with each other forming a precipitate of silver chloride and a solution of sodium nitrate.

→ White precipitate of AgCl is formed by exchange of ions Ag+ and Cl between the reactants.

→ Exothermic process. The process in which heat is given out is called an exothermic process. When NaOH dissolves in water, there is evolution of heat leading to a rise in temperature.
NaOH(s) + H2Ol → NaOH(aq) + Heat

→ Endothermic process. The reaction in which heat is absorbed is called an endothermic process. When KNO3(s) dissolves in water, there is absorption of heat during the reaction and the temperature of the solution falls.
KNO3(s) + H2O(l) + Heat → KNO3(aq).

→ Rate of chemical reaction : Some reactions are completed in short time, i.e., occur rapidly, while some other require long time for completion, i.e, occur slowly. It means that the rate of different reaction is different.

• One or more chemical reactions take place during every chemical change.
• Strong acid and strong base react instantaneously.
• In our body, enzymes increase the rate of physiological reactions.
• If the rate of the chemical reaction is fast, it is profitable for the chemical factories.
• The rate of chemical reaction is important with respect to environment.
• The ozone layer in the earth’s atmosphere protects the life on earth from the ultraviolet radiation of the sun. The process of depletion or maintenance of this layer depends upon the rate of production or destruction of ozone molecules.

Factors affecting the rate of a chemical reaction :

• Nature of reactants
• Size of the particles of reactants
• Concentration of the reactants
• Temperature of the reaction
• Catalyst.

→ Oxidation : The chemical reaction in which a reactant combines with oxygen or loses hydrogen to form the product is called oxidation reaction. The chemical substances which bring about an oxidation reaction by making oxygen available are called oxidants or oxidizing agents. In the combustion of carbon, oxygen is an oxidant.
Examples :

→ A variety of oxidants : K2 Cr2O7 / H2SO4, KMnO4 / H2SO4 are the commonly used chemical oxidants. Hydrogen peroxide (H2O2) is used as a mild oxidant. Ozone (O3) is also a chemical oxidant. Nascent oxygen is generated by chemical oxidants and it is used for the oxidation reaction.

O3 → O2 + [O]
H2O2 → H2O + [O]
K2 Cr2 O7 + 4H2SO4 → K2 SO4 + Cr2(SO4)3 + 4H2O + 3[O]
2KMnO4 + 3H2SO4 → K2SO4 + 2MnSO4 + 3H2O + 5[O]

→ Nascent oxygen is a state prior to the formation of the O2 molecule. It is the reactive form of oxygen and is represented by writing the symbol as [O].

→ Reduction : The chemical reaction in which a reactant gains hydrogen or loses oxygen to form the product is called reduction. The chemical substance that brings about reduction is called a reductant, or a reducing agent.

→ When hydrogen gas is passed over black copper oxide a reddish coloured layer of copper is formed.
CuO + H2 → Cu + H2O

→ Redox reaction : The reaction which involves simultaneous oxidation and reduction is called an oxidation-reduction or redox reaction.

• In a redox reaction, one reactant gets oxidised while the other gets reduced during a reaction.
• Redox reaction = Reduction + Oxidation
• In redox reaction, the reductant is oxidized by the oxidant and the oxidant is reduced by the reductant.

Examples :

MnO2 + 4HCl → MnCl2 + 2H2O + Cl2

→ Corrosion : Due to various components of atmosphere, oxidation of metals takes place, consequently resulting in their damage. This is called ‘corrosion’. Iron rusts and a reddish coloured layer is collected on it. This is corrosion of iron. This is also termed as rusting of iron. Its formula is Fe2 O3.H2O.

→ Prevention of corrosion : Corrosion damages buildings, bridges, automobiles, ships, iron railings and other articles made of iron. It can be prevented by using an anti-rust solution, coating surface by the paint by processes like galvanising and electroplating with other metals.

→ Rancidity : Fats and oils in food, is kept for a long time, gets oxidised, it is found to have foul odour called rancidity.

## Periodic Classification of Element Science Notes

Elements and their classification :

• The types of matter are solid, liquid, gas and plasma.
• The types of elements are metals, nonmetals and metalloids.
• The smallest particles are called atoms.
• Elements contain only one kind of atoms in the free state or combined state.
• An element cannot be decomposed into simple substances by any chemical reaction or simple physical process, e.g. copper, iron, oxygen.
• A compound is produced by a chemical reaction of two or more elements.
• The constituents of a compound can be separated by a chemical process, e.g. salt, water and sugar.

• Dobereiner’s Triads : In the year 1817 Dobereiner (a German scientist) proved that the properties of
elements are related to their atomic masses.
• He made groups of three elements each, showing similar chemical properties and called them triads.
• He arranged the three elements in a triad in an increasing order of atomic mass and showed that the atomic mass of the middle element was approximately equal to the mean of the atomic masses of the other two elements.

Newlands Law of Octaves :

→ Newlands’ Law of Octaves : In the year 1866, Newlands arranged the elements known at that time in an increasing order of their atomic masses, he found that every eighth element had properties similar to those of the first. For example, sodium is the eighth element from lithium and both have similar properties.

→ Limitations of Newlands’ Octaves :

• Newlands could arrange 56 elements only up to calcium in an increasing order of their atomic masses.
• This arrangement started with the lightest element hydrogen and ended up with thorium.
• Newlands placed the metals Co and Ni under the note Do along with halogens, while Fe having similarity with Co and Ni, away from them along with the nonmetals O and Sunder the note Ti.
• The properties of the new elements discovered later did not fit in the Newlands’ law of octaves.

Mendeleev’s Periodic Table :

→ Mendeleev’s Periodic table :

• The most important step in the classification of elements in Mendeleev’s periodic table is the fundamental property of elements, namely, the atomic mass, as standard.
• He arranged 63 elements known at that time in an increasing order of their atomic masses.
• Then he transformed this into the periodic table of elements according to their physical and chemical properties.
• Mendeleev found that the elements with similar physical and chemical properties repeat after a definite
• interval Mendeleev’s periodic law : The elements with physical and chemical properties are a periodic function of their atomic masses.

→ Introduction to scientist :

• Dmitri Mendeleev (1834-1907) was a professor in the St. Petersburg University.
• He made a separate card for every known element showing its atomic mass.
• He arranged the cards in accordance with the atomic masses and properties of the elements which resulted in the invention of the periodic table of elements.
• The vertical columns in the periodic table are called groups while the horizontal rows are
called periods.

→ Merits of Mendeleev’s periodic table :

• To give the proper place in the periodic table, atomic masses of some elements were revised in accordance with their properties.
• For example, the previously determined atomic mass of beryllium, 14.09, was changed to the correct value 9.4, and beryllium was placed before boron.
• Mendeleev had kept some vacant places in the periodic table for elements that were yet to be discovered.
• Three of these unknown elements were given the names eka-boron, eka-aluminium and eka-silicon from the known neighbours and their atomic masses were indicated as 44, 68 and 72, respectively.
• Their properties were also predicted. Later on these elements were discovered subsequently and were named as scandium (Sc), gallium (a) and germanium (Ge) respectively.
• The properties of these elements matched well with those predicted by Mendeleev. Due to this success all were convinced about the importance of Mendeleev’s periodic table.
• When noble gases such as helium, neon and argon were discovered, Mendeleev created the ‘zero group’ without disturbing the original periodic table in which the noble gases were placed very well.

→ Demerits of Mendeleev’s periodic table :

• The elements cobalt (Co) and nickel (Ni) have the same whole number atomic mass. As a result there was an ambiguity regarding their sequence in Mendeleev’s periodic table.
• Isotopes were discovered long time after Mendeleev put forth the periodic table.
• A challenge was posed in placing isotopes in Mendeleev’s periodic table as isotopes have the same chemical properties but different atomic masses.
• The rise in atomic mass does not appear to be uniform when elements are arranged in an increasing order of atomic masses.
• It was not possible, therefore, to predict the number of elements that could be discovered between two heavy elements.
• Position of hydrogen : Hydrogen shows similarity with halogens (group VII). It is difficult to decide the correct position of hydrogen whether it is in the group of alkali metals (group I) or in the group of halogens (group VII).

Modern Periodic Table :

→ Modern Periodic Law : Henry Moseley showed that the atomic number of an element is the most fundamental property and not its atomic mass. Accordingly Mendeleev’s Periodic law was modified into Modern Periodic law and it can be stated as : The chemical and physical properties of elements are a periodic function of their atomic numbers.

→ In the modern periodic table, the elements are arranged in the order of their increasing atomic numbers. There are seven horizontal rows called periods 1 to 7. There are eighteen vertical columns called groups 1 to 18. The arrangement of the periods and groups results into formation of boxes.

→ Each box corresponds to the place for one element. There are two series of elements placed separately at the bottom of the periodic table. These are called lanthanide series and actinide series. There are 118 boxes in the periodic table including the two series.

→ The elements in the modern periodic table are divided into four blocks : the s-block, the p-block, the d-block and the f-block. The groups, 1 and 2 together with hydrogen form the s-block elements. The groups 13 to 18 form the p-block elements. The groups 3 to 12 together form the d-block elements. The two series (the lanthanides and actinides) at the bottom of the periodic table together form the f-block elements.

→ The d-block elements are called transition elements. A zig-zag line is seen in the p-block of the periodic table. The metalloid elements lie along the border of this zig-zag line. All the metals lie on the left side of zig-zag line while all the nonmetals lie on the right side.

→ Modern Periodic Table and electronic configuration of the elements : The characteristics of the groups and periods in the modern priodic table are because of electronic configuration of the elements.

→ It is the electronic configuration of an element which decides the group and the period in which it is to be placed. The neighbouring elements within a period differ slightly in their properties while distant elements differ widely in their properties. Elements in the same group show similarity and gradation in their properties.

→ Groups and electronic configuration : Characteristics of the Groups and Periods. Various properties of all the elements in a group show similarity and gradation. However, the properties of elements change slowly while going from one end to the other (for example, from left to right) in a particular period.

→ The number of valence electrons in all these elements from the group 1, i.e. the family of alkali. metals, is the same. Similarly, the element from any other group, the number of their valence electrons to be the same.

→ For example, the elements beryllium (Be), magnesium (Mg) and calcium (Ca) belong to the group 2, i.e. the family of alkaline earth metals. There are two electrons in their outermost shell the number of valence electrons are 2.

→ Similarly, there are seven electrons in the outermost shell of the elements such as fluorine (F) and chlorine (Cl) from the group 17, i.e., the family of halogens. While going from top to bottom within any group, one electronic shell is added at a time. From this, the electronic configuration of the outermost shell is characteristics of a particular group.

→ In the modern periodic table :

• Elements are arranged in an increasing order of their atomic numbers.
• Vertical columns are called groups. There are 18 groups. The chemical properties of the elements in the same group show similarity and gradation.
• Uranium has atomic number 92. All the elements beyond uranium (with atomic numbers 93 to 118) are manmade. All these elements are radioactive and unstable, and have a very short life.

→ Periods and electronic configuration :

• In modern periodic table, there are seven horizontal rows called periods.
• In a period, the change in valency of an element varies with electronic configuration.
• In a period, while going from left to right, the atomic number increases by one at a time and number of valence electrons also increases by one at a time. In a period, there is gradation in properties of elements.
• The elements with the same number of shells occupied by electrons belong to the same period. The elements in the second period, have electrons in the two shells, K and L.
• The elements in the third period have electrons in the three shells; K, L and M.
• The chemical reactivity of an element is determined by the number of valence electrons in it and the shell number of the valence shell.
• Periodic trends in the modern periodic table : When the properties of elements in a period or a group of the modern periodic table are compared, certain regularity is observed in their variations.
• It is called the periodic trends in the modern periodic table.
• Valency, atomic size and metallic-nonmetallic character are some properties which show periodic trends in the modern periodic table.

→ Valency: The valency of an element is determined by the number of electrons present in the outermost shell of its atoms, that is, the valence electrons.

 Shell n 2n2 Electron capacity K 1 2 × 12 2 L 2 2 × 22 8 M 3 2 × 32 18 N 4 2 × 42 32
• For the shell K, the value of n is l. For the shell L, the value of n is 2. For the shell M, the value of n is 3.
• The maximum number of electrons that can be accommodated in a shell is 32 electrons. The formula is 2n2
• For the shell K, the maximum electron capacity is 2 electrons.
• For the shell L, the maximum electron capacity is 8 electrons.
• For the shell M, the maximum electron capacity is 18 electrons.

→ Atomic size : The size of an atom is indicated by its radius. Atomic radius is the distance between the nucleus of the atom and its outermost shell. Atomic radius is expressed in the unit picometre (pm) which is smaller than nanometre (1 pm = 10 -12 m).

→ Atomic size depends on number of shells of an atom. More the number of shells larger is the atomic size. While going down a group the atomic size goes on increasing. This is because while going down a group a new shell is added. Therefore the distance between the outermost electrons and the nucleus goes on increasing. As a result of this the atomic size increases.

→ While going from left to right within a period atomie radius goes on decreasing and the atomic number increases one by one, that means positive charge on the nucleus increases by one unit at a time. However, the additional electron gets added to the same outermost shell. Due to the increased nuclear charge the electrons are pulled towards the nucleus to a greater extent and thereby the size of the atom decreases.

→ Metallic-Nonmetallic character : It is observed that the metallic elements like sodium, magnesium are towards the left. The nonmetallic elements such as sulphur, chlorine are towards the right. The metalloid element silicon lies in between these two types.

• While going downwards in any group the electropositivity of elements goes on increasing while their electronegativity goes on decreasing
• While going from left to right in any period the electronegativity of elements goes on increasing while their electropositivity goes on decreasing.
• Larger the electropositivity or electronegativity of the element higher the reactivity.
• The periodic trend in the metallic character of elements is clearly understood from their position is the modern periodic table.
• In a group while going down a group a new shell is added, resulting in an increase in the distance between the nucleus and the valence electrons.
• This results in lowering the effective nuclear charge and thereby lowering the attractive force on the valence electrons.
• As a result of this the tendency of the atom to lose electrons increases. Also the penultimate shell becomes the outermost shell on losing valence electrons.
• The penultimate shell is a complete octet. Therefore, the resulting cation attains special stability.
• The metallic character of an atom is its tendency to lose electrons.
• Therefore, the following trend is observed : The metallic character of elements increases while going down the group. While going from left to right within a period the outermost shell remains the same.

→ However, the positive charge on the nucleus goes on increasing while the atomic radius goes on decreasing and thus the effective nuclear charge goes on increasing. Therefore valence electrons are held with greater attractive force. This is called electronegativity.

→ As a result of this the tendency of atom to lose valence electrons decreases within a period from left to right, i.e. electronegativity increases. Thus, non metallic character of elements increases within a period from left to right.

→ Gradation in Halogen Family : The group 17 contains the members of the halogen family. All of them have the general formula X2. A gradation is observed in their physical state down the group. Thus, fluorine (F2) and chlorine (Cl2) are gases, bromine (Br2) is a liquid while iodine (I2) is a solid.

→ Reaction of alkaline earth metal with water : A general chemical equation indicating the reaction of alkaline earth metals is M + 2H2O + M(OH)2 + H2. While going down the second group as Be → Mg → Ca → Sr → Ba, the gradation in this chemical property of the alkaline earth metals is observed.

→ While going down the second group the reactivity of the alkaline earth metals goes on increasing and thereby the ease with which this reaction takes place also goes on increasing. Thus beryllium (Be) does not react with water. Magnesium (Mg) reacts with steam, while calcium (Ca), strontium (Sr) and barium (Ba) react with water at room temperature with increasing rates.

## Gravitation Science Notes

Gravitation :

• A force can set a body in motion. For example, if a ball at rest on the floor is pushed, it rolls on the floor.
• A force can stop a moving body.
• For example, a moving bicycle can be brought to rest by application of brakes.
• A force acting on a body can change the speed of the body.
• For example, when brakes are applied to a moving bicycle, its speed decreases due to the friction between the brake shoes and the rim of the tyre.
• A force can change the direction of motion of the body.
• For example, in uniform circular motion of a body, the direction of motion of the body keeps on changing due to the applied force.
• A force can change the speed as well as the direction of motion of the body.
• For example, when a ball bowled by a bowler is hit by a batsman, there occurs a change in the speed as well as the direction of motion of the ball.
• A force can change the shape and size of the body force can cha on which it acts. For example, when a rubber ball is pressed, it gets deformed and hence no longer remains spherical.
• Also, there can be a decrease in its volume.
• The gravitational force between the earth and the moon, the electromagnetic force between two charged particles in motion, the nuclear force between a proton and a neutron in the nucleus of an atom.
• The gravitational force is a universal force, i.e., it acts between any two objects in the universe.
• Newton’s first law of motion : An object continues to remain at rest or in a state of uniform motion along a straight line unless an external unbalanced force acts on it.
• Newton’s second law of motion : The rate of change of momentum is proportional to the applied force and the change of momentum occurs in the direction of the force.
• Newton’s third law of motion : Every action force has an equal and opposite reaction force which acts simultaneously.

[Note: Equal in magnitude and opposite in direction)

Circular motion and centripetal force :

→ As long as we are holding the string. Fig. 1.1 : A stone tied to a string, moving we are pulling the stone alons a circular path towards us, i.e., towards and its velocity in the centre of the circle tangential direction and are applying a force towards it.

→ The force stops acting if we release the string. In this case, the stone will fly off along a straight line which is the tangent to the circle at the position of the stone when the string is released, because that is the direction of its velocity at that instant of time (Figure 1.1 (b)].

→ Thus, a force acts on any object moving along a circle and it is directed towards the centre of the circle. This is called the centripetal force. ‘Centripetal’ means centre seeking, i.e., the object tries to go towards the centre of the circle because of this force.

Kepler’s laws:

• “An ellipse is the curve obtained when a cone is cut by an inclined plane.
• It has two focal points. The sum of the distances to the two focal points from every point on the curve is constant.
• F, and F, are two focal points of the ellipse shown in figure 1.2. If A, B and C are three points on the ellipse then, AF1 + AF2 = BF1 + BF2 = CF1 + CF2 Kepler’s laws of planetary motion :
• The orbit of a planet is an ellipse with the Sun at one of the foci.
• The line joining the planet and the Sun sweeps equal areas in equal intervals of time.
• The square of the period of revolution of a planet around the Sun is directly proportional to the cube of the mean distance of the planet from the Sun.

[Note : Strictly speaking. (period of revolution)2 ∝  $$\left(\frac{a b}{2}\right)^{3}$$ (Fig. 12)]

Newton’s universal law of gravitation :

• Every object in the Universe attracts every other object with a definite force.
• This force is directly proportional to the product of the masses of the two objects and inversely proportional to the square of the distance between them.

The earth’s gravitational force :

• The gravitational force on any object due to the earth is always directed towards the centre of the earth.
• If the object is on the earth’s surface, in the usual notation,
$$F=\frac{\mathrm{G} m_{1} m_{2}}{r^{2}}$$
• The value of G was first experimentally measured by Henry Cavendish. In SI units its value is 6.673 × 10-11 Nm2 kg-2

Acceleration due to the gravitational force of the earth :

→ The acceleration produced in a body due to the earth’s gravitational force is called the acceleration due to gravity or the earth’s gravitational acceleration and its magnitude is denoted by g. It is directed towards the earth’s centre.

→ $$g=\frac{G M}{r^{2}}$$ for r = ≥ R (radius of the earth).
It depends on the location of the body.

→ Change in the value of g with height above the earth’s surface

 Place Height (km) g (m /s2) Surface of the earth (average) 0 9.81 Mount Everest 8.8 9.8 Maximum height reached by a man-made balloon 36.6 9.77 Height of a typical weather satellite 400 8.7 Height of a communication satellite 35700 0.225
• Mass : The mass of an object is the amount of matter present in it. Its SI unit is kg.
• Weight : The weight of an object is defined as the force with which the earth attracts the object. Its magnitude is mg and SI unit is the newton (N).

→ Colloquially we use weight for both mass and weight and measure the weight in kilogram which is the unit of mass. But in scientific language when we say that Rajeev’s weight is 75 kg, we are talking about Rajeev’s mass.

→ What we mean is that Rajeev’s weight is equal to the gravitational force on 75 kg mass. As Rajeev’s mass is 75 kg, his weight on the earth is F-mgee 75 × 9.8 = 735 N.

→ The weight of 1 kg mass is 1 × 9.8 = 9.8 N. Our weighing machines tell us the mass. The two-pan scale balance in a shop compares two weights, i.e., two masses.

• The force exerted by the person holding the stone, the force exerted by air and the earth’s gravitational force.
• The stone falls to the ground.
• The forces exerted by air and the earth’s gravitational force.

→ Yes. Two objects kept on a table do not move towards each other because there is a force of friction between each object and the table. Similarly, because there is a force of friction between our body and the floor, we (myself and my friend) do not move towards each other.

• High and low tides occur regularly in the sea.
• The level of sea water at any given location along sea shore increases and decreases twice a day at regular intervals.
• High and low tides occur at different times at different places. The level of water in the sea changes because of the gravitational force exerted by the moon.
• Water directly under the moon gets pulled towards the moon and the level of water there goes up causing high tide at that place.
• At two places on the earth at 90° from the place of high tide, the level of water is minimum and low tides occur there as shown in figure 1.3.

Free fall :

• Whenever an object moves under the influence of gravity alone, it is said to be falling freely.
• For a freely falling object, with v = 0 and a = 8, we have v = $$\frac{1}{2}$$gt, s = gt2 and v2 = 2gs (in the usual notation)
• For an object thrown upward, as the object moves upward, the direction of acceleration is opposite to that of the velocity. Hence, the acceleration is negative, with a = -g.
• The value of g is the same for all objects at a given place on the earth.
• Thus, any two objects, irrespective of their masses or any other properties, when dropped from the same height and falling freely will reach the earth at the same time.
• Galileo is said to have performed an experiment around 1590 in the Italian city of Pisa.
• He dropped two spheres of different masses from the leaning tower of Pisa to demonstrate that both spheres reached the ground at the same time.
• When we drop a feather and a heavy stone at the same time from a height, they do not reach the earth at the same time.
• The feather experiences a buoyant force and a frictional force due to air and therefore floats and reaches the ground slowly, later than the heavy stone.
• The buoyant and frictional forces on the stone are much less than the weight of the stone and do not affect the speed of the stone much.
• Recently, scientists performed this experiment in vacuum and showed that the feather and stone indeed reach the earth at the same time.

• Escape velocity : vese –$$\sqrt{\frac{2 G M}{R}}=\sqrt{2 g R}$$
• For u = vese (from the earth’s surface), the body overcomes the earth’s gravitational attraction.
• It will then move to infinity and come to rest there. The gravitational potential energy of an object at a heighth from the earth’s surface = $$=-\frac{G M m}{R+h}=-\frac{m g R^{2}}{R+h}$$
• The total energy of a body revolving around the earth – kinetic energy + potential energy
= $$\frac{1}{2} m v^{2}+\left(-\frac{G M m}{R+h}\right)$$

→ Uniform circular motion of a planet around the Sun :

• The formula for escape velocity given in the textbook, does not take into account the effect of atmosphere. In practice, the body becomes very hot due to friction with air and may even burn.
• Even when a body is projected obliquely from the earth’s surface, with u – vese, it will overcome the earth’s gravitational influence and move to infinity.

Weightlessness in space :

→ Space travellers as well as objects in the spacecraft appear to be floating. Though the spacecraft is at a height from the surface of the earth, the value of g there is not zero.

→ In the space station the value of g is only 11% less than its value on the surface of the earth. Thus, the height of a spacecraft is not the reason for their weightlessness.

→ Their weightlessness is caused by their being in the state of free fall. Though the spacecraft is not falling on the earth because of its velocity along the orbit, the only force acting on it is the gravitational force of the earth and therefore it is in a free fall.

→ As the velocity of free fall does not depend on the properties of an object, the velocity of free fall is the same for the spacecraft, the travellers and the objects in the craft. Thus, if a traveller releases an object from her hand, it will remain stationary with respect to her and will appear to be floating.

Gravitational waves :

• Waves are created on the surface of water when we drop a stone into it.
• Similarly you must have seen the waves generated on a string when its both ends are held in hand and it is shaken.
• Light is also a wave called the electromagnetic wave.
• Gamma rays, X-rays, ultraviolet rays, infrared rays, microwave and radio waves are all electromagnetic waves with different frequencies.
• Astronomical objects emit these waves and we receive them using our instruments.
• All our knowledge about the universe has been obtained through these waves.
• Gravitational waves are a very different type of waves.
• They have been called the waves on the fabric of space-time.
• Einstein predicted their existence in 1916.
• These waves are very weak and it is very difficult to detect them.
• Scientists have constructed extremely sensitive instruments to detect the gravitational waves emitted by astronomical sources.
• Among these, LIGO (Laser Interferometric Gravitational wave Observatory) is the prominent one.
Exactly after hundred years of their prediction, scientists detected these waves coming from an astronomical source.
• Indian scientists have contributed significantly in this discovery.
• This discovery has opened a new path to obtain information about the Universe.