Atom of an element seldom exist alone, and usually join with the atom of another element to form the molecule of a compound. Eg: 2 atoms of Iron (Fe) may combine with 3 atoms of Oxygen to form one Molecule of Ferric Oxide, a compound. Thus the equation will read as Fe2O3.

About 40,40,000 such compounds have been described, of which about 63000 are in common use.

Any change in the original composition of an element/metal due to the combination of other atmospheric or induced elements over it. For example, when coal burns, Carbon and Hydrogen compounds within it combine with the oxygen in the air, Carbon-di-oxide and water vapours forms. This is a kind of induced chemical reaction or change because the coal has to be burnt. On the natural side, the Iron when exposed to atmosphere, the combination of Oxygen with Iron, makes the iron to rust forming Ferric Oxide. Such chemical changes have their own characteristics. For this purpose, the original constituent chemicals are called the "Reactants" and the converted products are called "Products".

1. The end product of a chemical change assumes new properties.
2. Mass value of reactant and product remains the same and equal.
3. When substances are formed in different ways i.e. by different chemical reactions, it always has the same composition. For instance, in carbon-di- oxide, carbon and oxygen are always in the ratio of 3:8 by mass, irrespective of it's nature of formation.
4. In a chemical reaction, energy is either let out or absorbed. For instance, i)when coal is burnt in air, energy in the form of heat and light is let out; ii) when carbon and sulphur are combined, heat is absorbed in the process.

It is a form of expressing the chemical changes by alphabets and numbers in which the alphabets representing the chemical while the numbers represent the number of atoms. For instance, C + O2 g CO2 in which C stands for carbon, O stands for Oxygen and the 2 stands for the number of atoms. Similarly, when Hydrogen and Chlorine combine and react to form Hydrogen chloride, the equation will be H2 + Cl2 g 2HCl, in this it expresses that one molecule containing two hydrogen atoms combined with one molecule with two Hydrogen atoms make up 2 molecule of Hydrogen Chloride.

A process in which two compounds react together to form two new compounds, one of the common chemical reaction of double decomposition. Eg: MgSO4 + 2NaOH g Na2SO4 + Mg(OH)2 , in this, Magnesium Sulphate MgSO4 with Caustic Soda solution (.......NaOH ) to form Sodium Sulphate Na2SO4 and antacid Magnesium Hydroxide ((Mg(OH)2).

A common chemical reaction. Most occurrences are due to the combination of oxygen. However, now the term refers to all analogous reactions in which Substances combine with other elements and lose electrons in the process. However, oxidation is always accompanied simultaneously with reduction in Which electrons are gained.

CuO + H2 g Cu + H2O where H2 Hydrogen reacts on copper oxide (CuO) and it is reduced to copper - gaining electrons in the reduction.

It may occur slowly in the case of formation of rust and quickly in the case of an explosion. The rate of chemical reaction can be increased by the presence of a catalyst.

A substance which influences the chemical reaction, but not change with it. There are various types of catalysts used for various purposes.

Oxygen, Hydrogen, Nitrogen, Carbon-di-oxide.

A gas having the following characteristics:
1. Colour, Odour and tasteless.
2. Sparingly soluble in water.
3. Slightly heavier than air.
4. Does not burn by itself but helps other substances to burn.
5. Available in abundance in the earth in free state and in combined state with other elements.
6. Essential for respiration for plants and animals and for any combustion.

By heating Potassium Chlorate and Manganese Di-oxide together. Can also be obtained in small quantities by heating oxides or salts which are rich in oxygen. Can also be separated from air by passing an electric current through water.

Atomic No. 8; Relative Atomic Mass 15.999; Melting Point - -218.4 degreeC Boiling Point - -183.0 degree ; Density at 0 degreeC - 1.329 Kg/ m3Valency - 2; Chemical Code - O.

Joseph Priestley of UK.

Colourless gas and the most abundant in the universe, with the following Characteristics: Highly flammable gaseous element. Lightest of all substances known. In free state, occurs in volcanic gases. Slightly soluble in water. Burns with pale blue flame but does not help combustion.

Can be obtained from water, acids and alkalies. In laboratory it is prepared by the combination and chemical action of dilute sulphuric acid on commercial zinc.

Vanaspati Ghee, Alcohol and Ammonia.

Atomic No. 1; Relative Atomic Mass - 1.008; Melting Point - -259.14 degreeC; Boiling Point - -252.5 degreeC; Density - 0.08988 Kg/ m3 Valency - 1.

A gas constituting nearly 4/5th of the air by volume. Its characteristics are:
1. Colour, odour and tasteless.
2. Neither combustible nor helps combustion.
3. Slightly soluble in water.
4. An almost inert diatomic gas.

In laboratory it can be prepared by heating Ammonium Nitrate. In large scale it can be obtained from air by liqueification process.

Nitric Acid, Ammonia and other Nitrogen based fertilizers.

Atomic Number - 7; Relative Atomic Mass - 14.007; Melting Point - -209.86 degreeC - Boiling Point - -195 degreeC; Valencies - 3 and 5.

A gas formed during respiration, combustion and organic decomposition.

It is prepared by the action of dilute acids on carbonates or by fermentation of sugar. In a laboratory it can be prepared by treating marble pieces with dilute Hydrochloric acid.

1. Colour and odourless. 2. Incombustible 3. Acidic.

Food Refrigeration, Carbonated beverages, Fire extinguishers etc.,

1. Acetylene, Ethylene: Produce hot flame for welding and cutting,
2. Ammonia: Fertilizer, Synthetic Fibre, Refrigeration,
3. Butane: Cigarette lighters, Domestic fuel,
4. CS Gas: Tear Gas used for controlling riots,
5. Cyanogen: Welding, Chemical weapons, rocket propellant
6. Ether: Anaesthetic, Industrial process,
7. Ethylene: Plastics,
8. Helium:  Fluorescent Tubes, Laser, Balloon,
9. Krypton: Fluorescent Tubes, High Speed photography,
10. Nitrous Oxide:  Mild anaesthetics,
11. Methane:  To make chloroform,
12. Neon:  Illuminated Signs,
13. Propane:  Fuel and Refrigerant,
14. Radon:  Radio Therapy, Atomic Research,
15. Xenon: Flash Lamps, Lasers etc.

A sour tasting chemical substance which in it's aqueous nature is capable of effecting physical changes, corroding, dissolving metals/elements viz: turning blue litmus into red, dissolves certain metals into salts and reacts with bases or alkalies to form salt and gives Hydrogen ((H+) ) ions. An acid consists of two parts of Hydrogen (CH2) and an acid radical. Eg: HNO3 - Nitric Acid - in this NO3 is acid radical with (H2) Hydrogen. Acids come under two categories:- Organic or Natural Acids. Inorganic or Mineral Acids.

1. Sulphuric Acid - H2SO4, 2. Hydrochloric Acid - HCl, 3. Nitric Acid - HNO3, 4. Phosphoric Acid - H3PO4

1. Acetic Acid - Vinegar, 2. Amino Acid - Proteins, 3. Ascorbic Acid -Vitamin C, 4. Citric Acid - Lemon/Citrus Fruits, 5. Hydrochloric Acid - Digestive Juices, 6. Lactic Acid - Milk, 7. Malic Acid - Unripe Apples/Fruits, 8. Tannic Acid - Tea, 9. Uric Acid - Urine.

Both are same. It was earlier called as Organic Chemistry and now Carbon Compound. It was earlier (before 1828) believed that organic compounds occur only in living organisms and thus it was called Organic Chemistry. In 1828, a German chemist Friedreich Wohler prepared an organic compound Urea by evaporating the inorganic compound ammonium cyanide solution CO(NH2)2 Urea an organic compound is formed. NH4CNO (Ammonium Cynaide) the inorganic compound when heated and evaporated CO(NH2)2 Urea an organic compound is formed. This effort of Wohler disproved the "vitalist theory" that is - to produce Organic compounds vital energy is required. This effort of Wohler disproved the "vitalist theory" that is - to produce Organic compounds vital energy is required.

Organic Compounds - 1. Most of them can be burnt, 2. Most of them are gases, 3. volatile liquids and solids, 4. Low melting points, 4. Most are insoluble in water. Inorganic Compounds - 1. Most of them cannot be burnt, 2.Most of them are solids, 3. High Melting Points, 4. Majority of them are soluble.

1. Aerosol: A colloidal system in which pesticides are dispersed in a gas as in High Melting Points. Smoke or mist. Majority of them are soluble.
2.Alcohol: A colourless, volatile and flammable liquid, synthesized or fermented through sugars and starches containing the hydroxyl (-OH) group. The simplest alcohol is methyl alchohol or methanol CH3OH. typical of the group is ethyl alcohol in wine, or ethanol, C2H5OH the alcohol in wine and spirit.
3.Aldehyde: One of a family of organic chemicals containing the characteristic group >C=O. Best known is the gas formaldehyde, HCHO, which when dissolved in water becomes the preservative fermaline.
4.Alkali: Is a metal hydroxide that is soluble in water and is a strong base. For example : The Hydroxides of sodium and Potassium (Caustic Soda, Caustic Potash). The aqueous solution of an alkali does not change colour of Bluelitmus but instead turns red litmus blue. Alkalis have a soapy touch and bitter taste.
5. Alakali Metal: A group of elements that react with water to form alkalies. Eg: Sodium, Potassium, Rubidium, Caseium.
6. Alkane: Simple Hydrocarbons that are commonly called "Paraffins". The series of alkane begins with Methane CH4.
7. Allotropy: The existence of elements in more than one form in the same Physical state i.e. the existence of two or more crystalline or molecular structural forms of an element e.g. Carbon (Diamond and Graphite).
8.Amino Acids: An organic compound containing both an amino group ((NH2)) and a carboxyl group (CooH) which are essential components of proteins. There are about 100 amino acids, of which the simplest is Glycine (CH2(NH2),) found in gelatine and silk.
9. Anhydride: A chemical compound formed from another by the removal of water; otherwise, a compound that forms an acid or base when water is added.
10.Aqua Regia: A mixture of concentrated Nitric and Hydrochloric acid in the ratio of 1:3.
11. Aromatic Compound: An organic compound derived from benzene - has a powerful and pleasant aroma.
12.Atomic Number: Number of protons in the atomic nucleus of an element.
13. Azetropic Mixture: A mixture of two or more liquids that cannot be Separated by distillation. When most liquid mixtures boil, the vapour has a different composition from the liquid, which enables separation of the constituents, to be achieved. Alcohol and water in the ratio of 96:4 form an azetrope which boils at 78.15 degreeC.
14.Base: A chemical substance which reacts with and neutralizes an acid to give a salt and water; solution of which turns red litmus blue. Eg: Calcium Hydroxide, Magnesium Hydroxide, Sodium Hydroxide.
15. Boiling Point: The temperature at which a liquid is converted into vapour. The boiling point of water is 100 degreeC.
16. Carbonate: A compound made from Carbonic Acid. (H2CO3).. In Nature they occur as Chalk or Lime Stone etc.,
17. Carbohydrates: One of a large group of organic compounds found in most Foods. Eg: Starch, Cereals, Sugar etc., They contain Carbon, Hydrogen and Oxygen. 18.Chemical Bond: The force that holds atoms and ions together.
19. Colloid: A mixture or suspension of very fine particles within a fluid as in fog or paint.
20. Catalyst: A substance that affects the rate of chemical reaction without Itself being consumed in the process. It accelerates the chemical action. 21.Condensation: A process of reduction to a denser form such as vapour to liquid.
22.Corrosion: Destruction of a metallic body by chemical action or electro Chemical action or electro chemical attack. It can be prevented by giving the Metal a protective coating of paint, bitumen or plastic.
23.Crystal: A solid pattern of substance composed of a group of atoms or molecules which is repeated in space to form a very regular structure. Eg: Common Salt, Sugar, Diamond etc.,
24. Carbide: A combination of carbon with a metal or sometimes with a non metal.
25. Catalysis: A process in wh;ich chemical reaction is speeded up by the presence of an extra substance - catalyst - which remains unchanged at the end of the reaction.
26. Decantation: The process of separating a solid held in suspension in a liquid by allowing the former to settle down after which the liquid is poured out.
27. Deliquescence: A property possessed by some substances of absorbing moisture from the air on exposure. Anhydrous calcium chloride, which possesses this property is widely used as a drying agent.
28. Dessication: A process of drying or removal of moisture from a substance.
29. Diffusion: The natural process by which one gas is disseminated through another, or, a process by which one material moves through another, from a state of high concentration to one of low concentration. Odours, for example, diffuse through air.
30. Dopant: An impurity added to a pure substance such as a semi conductor, to alter its properties.
31. Distillation: The process of converting a liquid into vapour and then condensing this vapour into the liquid form again. Eg: Distilled Water.
32. Double Salt: A compound of two salts formed by the crystallization of a liquid solution containing both of them.
33. Electrolysis: The process of chemical decomposition of an electrolyte by Means of an electric current.
34. Electrolyte: A compound which in molten state or when dissolved in solution dissociates into oppositely charged ions.
35.Electrons: A negatively charged particle orbiting the atomic nucleus.
36.Emulsion: A colloidal dispersion one liquid into another.
37.Ester: An organic compound obtained by reaction of an acid with alcohol and has a fruity smell. In nature esters gives flower their smell and flavours to fruits.
38. Ether: A class or organic compound made from alcohol. It is volatile, heavier than air, inflammable and is only slightly soluble in water.
39.Fatty Acids: The organic carboxylic occurring in fats and oils. They do not occur as acid itself but as a glycerol, an ester derived from alcohol. Most common fatty acids are palmitic, stearic, oleic and tinoleic.
40. Fermentation: The chemical changes brought about by living organisms, (yeast, bacteria etc.,) in which bigger organic molecules are converted into Smaller molecules. Eg: Conversion of glucose and cane sugar into alcohol and Carbon dioxide.
41. Freezing Mixture: Salt of Metals ((NaCl, MgSO4)) which, when mixed with crushed ice, lower its temperature below 0 degreeC.
42. Glycerine: A colourless, thick liquid prepared by the hydrolysis of fats and oils. Also called Glycerol.
43. Grignard Reagent: An organic compound alkylhalide and Magnesium used to synthesize organic chemicals.
44. Halide: The halogen element compounds like Fluorides, Chlorides, Bromides, and Iodides.
45. Halogen Group: Non metallic elements like Fluorine (F), Chlorine (C), Bromine (Br), Iodine (I) and Astatine (At).
46. Hard Water: Water that contains salts of calcium and magnesium and does not lather with soap easily.
47. Heavy Water: A liquid like water containing "Deuterium" (an isotope of Hydrogen) in place of Hydrogen.
48. Helium: The lightest of the noble gases.
49. Homologous Series: A group of chemical compounds whose structures Differ by a simple unit. Most popular homologues series include the alkanes in which structures differ by Methylene (CH2) units. The series begins with Methane, Ethane, Propane and the more complex Butane.
50. Hydrocarbon: An organic compound of carbon and Hydrogen. Eg: Methane.
51. Hydrolysis: A process of decomposing a compound by the reaction of water. For example, in digestion, starches and sugars are broken down by hydrolysis into more digestible sugars such as Glucose.
52. Inert Gases: Also called "Noble Gases".
53. Ideal Gases: Also called "Perfect Gas". The gas conforming accurately to the gas laws. Eg. Nitrogen and Hydrogen which conform fairly well to the laws.
54. Ion: An atom or group of atoms which has either gained or lost electrons from its normal complement.
55. Isomer: Refers to different organic compounds having the same number of atoms of the same element arranged in a different manner. The have the same basic chemical formula.
56. Isotope: An atom of an element having the same number of neutrons. Eg: Protium, Deutrium, and Tritium are isotopes of Hydrogen.
57. Litmus Paper: A dyed paper that turns red when treated by acids but remains, or reverts to blue when treated by alkalies.
58. Mass Number: Total Number of Protons and neutrons in the nucleus of an atom.
59. Metalloid: Element having both metallic and non-metallic properties. Eg: Boron, Silicon, Arsenic, Antimony etc.,
60. Molecular Weight: Ratio of the weight of one molecule of a compound with that of one atom of carbon 12 taken as 12.
61. Molecule: The smallest particle of a compound that is capable of independent existence. The properties of a compound are the properties of its molecule.
62. Neutralization: A process in which acid and alkali react together and the resultant solution is neutral to litmus.
63. Neutron: Electrically neutral particles in the nucleus of an atom.
64. Noble Gas: These are inert gases. Eg. Helium, Neon, Argon, Krypton, Xenon, Radon.
65. Nucleus: The positively charged central core of an atom containing Protons and Neutrons.
66. Octane: A hydrocarbon of paraffin series occurring in fuel gases.
67. Osmosis: The diffusion of substances from one solution to another through A semi permeable membrane due to a difference in concentration of the solutions. This is the principle of the process of dialysis where solution of less concentration passes to the more concentrated solution.
68. Oxidation: Adding of Oxygen to compound or removal of hydrogen from it. A reaction in which atoms, molecules or the like, gain electrons.
69. Oxide: A compound in which oxygen is combined with another element.
70. Ozone: An allotropic form of oxygen, found between 15-30 Kms above the Earth's surface in the atmosphere. Responsible for absorbing a large Proportion of sun's radiation.
71. Pasteurization: The process of killing bacteria or retarding their growth in milk. Milk is pasteurized by heating it to a temperature of about 67 degreeC maintaining it at the temperature for about half an hour and then chilling it.
72. pH Value: A measure of acidity or alkalinity of a solution expressed in Numbers and measure of Hydrogen ions by the equation of pH= -log(l/H+)
73: Polymerization: The formation of an insoluble chemical compound or residue in a solution as a result of a chemical reaction. The residue thus formed is called "precipitate".
74: Proton: The positively charged heavy particle of the nucleus of an atom, having equal and opposite charge that of an electron.
75. Radical: A group of atoms that stay together when a compound dissociates, but yet not a stable group to qualify as a molecule.
76. Rare Gases: Chemically inactive or inert gases. Eg: Argon, Krypton etc.,
77. Rare Earth: Any group of metallic element with atomic number 57 to 71. Also called "Lanthanides".
78. Reagent: A chemical commonly used in chemical laboratories for experiments and analyses such as dilute hydrochloric acid, ammonium hydroxide, dilute nitric acid etc.,
79. Real Gases: The gases which do not follow ideal gas laws.
80. Salt: A product formed as a result of acid base reaction. It is formed when the Hydrogen in an acid is replaced by a metal. Eg: Potassium Nitrate and Calcium Sulphate. Sodium Chloride (NaCl) is a salt in the chemical sense but Is also called a Common Salt.
81. Saponification: The reaction in which esters are hydrolyzed with the help Of alkalies into acids and alcohol.
82. Slag: A non metallic material obtained during smelting of ores.
83. Solution: A mixture of two or more substances not chemically mixed.
84. Solvent: A substance which can dissolve other substances in it forming a solution.
85. Sublimation: Conversion of a solid directly into vapour, or, the process of change from the solid to the gaseous state or from the gaseous state to the solid state without becoming a liquid.
86. Sulphonation: The process in which one of the hydrogen atoms of the same Organic compound is replaced by a sulphnic group (-SO2OH.).
87. Suspension: A mixture consisting of very small undissolved or partially Dissolved particles of a solid, distributed in a liquid dispersion medium.
88. Synthesis: Formation of a compound directly from its elements or a Simple compound.
89. State of Matter: The material substance of any kind exists in three states viz: solid, liquid and gas, each of which can change into one or the other according to change in temperature and pressure. The so called fourth state of matter is called "plasma" where negatively charged ions are in flux.
90. Transuranium: These are man made elements that have a higher atomic numbers ( number of protons in the nucleus) than Uranium - 92. Eg: Plutonium - 94. 91. Valency: The combining capacity of an element measured by the number of hydrogen atoms which combine with, or, are displaced by an atom of other elements.

1. Brown Ring Test: Used for chemical analysis of nitrates in which the solution to be tested is mixed with iron sulphate solution in a test tube and concentrate Sulphuric Acid (H2SO4) is carefully poured along the side of the test tube. In nitrate containing substances a brown ring is formed where the layer acid touches the solution. (FENO) SO4.
2.Flame Test: Used to identify certain elements in which a clear Platinum wire is dipped into the mixture to be tested and the wire is heated using a busen flame. The presence of certain elements can be detected by the change in the colour of flame. For example: brilliant orange yellow will indicate sodium; Crimson will indicate Strontium and apple green will indicate Barium.
3. Beilstein's Test: Used for the detection of halogen in an organic compound in which a clean copper wire is heated in an oxidizing flame till the flame is no longer green. The wire is then dipped in a solution of the substance to be analyzed and heated again. If Chlorine (Cl), Bromine (Br) or Iodine (I) are present, the flame turns a bright green.
4. Fehling's Test: Used to detect sugars and aldehydes in a solution. Equal amounts of solution of Copper Sulphate (Fehling A) and Sodium Tartate (Fehling B) are mixed in a test tube. On boiling this with a given solution, a red precipitate forms if sugar or aldehyde is present.
5. Kjedhal Method: Is used to measure nitrogen in an organic compound. The compound is boiled with concentrated sulphuric acid and copper sulphate (catalyst) to convert nitrogen to ammonium sulphate. An alkali is added to the mixture and boiled to distill ammonia which is passed into a standard acid solution and estimated by titrating the solution.
6.Molish's Test: Used to detect carbohydrates in a solution. The solution to be tested is mixed with a small quantity of alcoholic alphanaphthol and concentrated sulphuric acid slowly poured down the side of the test tube. When the two liquids meet the formation of a deep violet rings indicates The presence of carbohydrates. 7.Rast's Method: Used to determine molecular weight by measuring the depression of freezing point of a camphor by a known weight of the solute.
8.Schiff's Test: Used to distinguish aldehydes and ketones. An aqueous Solution of rosaniline and sulphorous acid (Schiff's reagent) is used to test for the presence of aldehydes, which oxidize the reduced form of the dye rosaniline back to its original magenta colour. The aldehydes restore the colour immediately, whereas, ketones restore the colour slowly.

1. Beer's Law: States that in photo chemistry, the proportion of light absorbed by a solution depends on the thickness of the absorbing layer and on the concentration of the absorbing substance in the solution.
2. Boyle's Law: States that the volume (v) of a given mass of gas at a constant Temperature is inversely proportional to its pressure(p), that is, pv=constant. This means that if a gas is compressed threefold its volume is reduced by two thirds. Boyle was the first to define that an element as a substance cannot be Broken down into something simpler by a chemical process.
3.Charle's Law: States that under constant pressure the volume of a fixed mass of gas varies directly with its absolute temperature. The absolute temperature is that measured from absolute zero, about -273 degreeC. In other words, the pressure of a gas increases by 1/273 of its volume at 0 degreeC for every 1 degreeC rise in temperature. In other words, if the pressure of a gas remains constant, the volume of a Gas increases by 1/273 of its volume at 0 degreeC for every 1 degreeC rise in temperature. Alternatively, at constant pressure the volume of a given mass of gas is Directly proportional to the absolute temperature. The principle was formulated by the French Scientist Jacques Alexandre Charles.
4. Faraday's Law of Electrolysis: States that i) the amount of decomposition during electrolysis is proportional to the quantity of current passed; and ii) for the same quantity of electricity passed through different solutions, the extent of decomposition is proportional to the chemical equivalent of the element or group liberated. The law was formulated by the English chemist Michael Faraday.
5. Gay Lussac's Law: 1. Law of Gaseous Volume: States that when gases combine chemically the volumes of the reactive gases or gaseous products are in simple proportion at the same temperature and pressure. In other words, when gases combine they do so in volumes which are in a simple ration to each other and to that of the product, if it is also gaseous. Eg: One volume of Nitrogen combines with three volumes of hydrogen to form two volumes of Ammonia. 2. Law of Thermal Expansion: It states that at constant pressure all gases Expanded by the same amount for the same increase in temperature. These laws were formulated by the French Chemist Joseph Lois Gay Lussac.
6. Hess' Law: States that heat exchange in a chemical reaction is the same, no matter whether the reaction takes place in one stage or more. The principle was formulated by the German chemist Henri Hess.
7. Graham's Law of Diffusion: States that the rate at which two gases diffuse Is inversely proportional to their densities. It means that the lighter the gas, the faster it will diffuse through any medium. The law was defined by a Scottish Chemist Thomas Graham.
8. Henry's Law: States that the mass of a gas which is dissolved in a given volume of liquid at constant temperature is directly proportional to the pressure of the gas. It applies to gases that do not react with the liquid (solvent). The principle was formulated in 1803 by the British Chemist William Henry.
9. Lambert's Law: States that layers of equal thickness of homogenous material absorb equal proportion of light. Eg: coloured filter.
10. Raoult's Law: States that the lowering of the vapour pressure of a solvent By a solute (dissolved substance) is proportional to the Mole fraction of the solute - the proportion of solute molecules to the total number of molecules, solute and solvent present. Since the lowering of vapour pressure causes an elevation of the boiling point and a depression of the freezing point, it is used to determine the molecular mass of a solute. The law is named after the French chemist Francois Marie Raoult.
11. Law of Conservation of Mass and Matter: Matter can neither be created nor destroyed. The sum total of mass or matter for a system always remains constant without any increase or decrease in quantity.

1. Bessemer Process: A method of converting pig iron to steel by blowing air through the molten metals to oxidize impurities such as Carbon, Silicon, Phosphorous and Manganese normally present in pig iron. 2. Clemmensen Reduction: A process used to convert aldehydes and ketones To the corresponding hydrocarbons. 3. Gattermann Reaction: A process used to convert an aromatic amine into The corresponding halogen derivative through diazonium salt formation using copper as a catalyst. 4. Haber's Process: An industrial process of producing ammonia by the Reaction of nitrogen with hydrogen in the presence of a catalyst. 5. Kolbe Reaction: Used for the preparation of saturated or unsaturated hydrocarbons by the electrolysis of solutions of the alkali salts of aliphatic carboxylic acids. 6. Solvay Process: A process of snaking sodium carbonate from Calcium Carbonate and sodium chloride in large scale. The process involves heating calcium carbonate to give calcium oxide and carbon di oxide which is bubbled into a solution of sodium chloride in ammonia. Sodium hydrogen carbonate is precipitated which on heating gives Sodium carbonate. 7. Bayer Process: A process used to extract Aluminium oxide (Al2O3) or aluminia by treating powdered bauxite with hot caustic soda solution under pressure. The process was developed by German Chemist Karl Joseph Bayer in 1888. 8. Berguis Process: A process for making lubricants and synthetic fuel. Eg: Petrol from coal by heating a mixture of powdered coal and heavy oil Or tar with hydrogen under pressure in the presence of a catalyst - Iron, Tin or Lead. This process was developed by German Chemist Friedreich Beruguis - 1930. 9. Bosch Process: A process used to make industrial hydrogen by passing Steam over white hot coke to produce water gas ( a mixture of carbon monoxide and hydrogen) which is the presence of a catalyst ( a metal oxide ) reacts with more steam to liberate hydrogen and carbon dioxide. The process is named after German Chemist Carl Bosch. 10. Down Process: A process of making sodium metal by electrolysis of molten Sodium chloride. The molten sodium and calcium formed at the cathode are separated. 11. Frasch Process: Used to extract sulphur from subterranean deposits in which superheated water is forced down the deposits which melts the sulphur under the ground. Molten sulphur is collected by forcing compressed air from another side. The process was developed by German Chemist Herman Frasch in 1891. 12. Harl Heroult Process: A process used to prepare aluminium by electrolysis in which aluminia (aluminium oxide) is developed in cryolite (sodium aluminium fluoride) and electrolysed. This process was developed by Charles Harl in 1885 in USA and by P J Heroult of France. 13. Parkes Process: A process used for extraction of silver traces from lead ore galena. Molten zinc is added to molten galena and lead is separated leaving Zinc silver, which on heating distills off zinc freeing the silver.