User:NILESH RANJAN/sandbox

CARBON COMPOUND CARBON                  Atomic no. - 6                  Atomic mass- 12         Symbol- C             Valency- 4

ORGANIC CHEMISTRY 	They are colourful and have their distinct odour. 	They are generally volatile. 	They have low Boiling & Melting point. 	They don’t dissolve in water. 	They only dissolve in organic solvent. 	They catch fire easily. 	They form covalent compound. 	These compounds are non-electrolyte.

FORMATION OF CARBON COMPOUND •	Carbon atoms have unique ability to combine with one another to form chain. a)	Straight chain                                b)	Branched chain c)	Cyclic chain                                                                                                                                                       Carbon has capacity to form new compounds with non-metal like - O2, H2 ,CI2, N2. •	Carbon also combines with some metal like Calcium. •	Carbon is neither electropositive like alkali metal nor electronegative like halogens. SOURCES OF ORGANIC COMPOUND 1.	ORGANISM- sugar, starch, vegetable oil, tea, coffee, paper, wood, rubber. 2.	COAL- Benzene, phenol, Naphthalene. The compound formed by the combination of carbon & hydrogen atoms are called hydrocarbon.                    They are of two types 1)	 SATURATED  HYDROCARBON 2)	UNSATURATED HYDROCARBON
 * HYDROCARBON|

SATURATED HYDROCARBON The hydrocarbons in which carbon atoms are connecting only by single bond are called saturated hydrocarbons. EX- C2H6, C3H8, C5H10. (ALKANES) IT HAS OF ONLY ONE TYPE 1)	ALKANES (Single Bond)                   EX- Methane, ethane, propane. General formula---      CnH2n+2 Put n = 1 - CH4   methane            n = 2 - C2H5  ethane UNSATURATED HYDROCARBON

The hydrocarbons in which carbon atoms are connected by double or triple bond are called unsaturated hydrocarbons. They are of two types 1)	ALKENES (Double Bond)   Gen formula- CnH2n Put n = 2  C2H4        ETHENE         n = 3  C3H6       PROPENE

2)	ALKYNE (Triple Bond) Gen formula CnH2n-2 Put  n = 2 -- C2H2      acetylene Number of carbons	Prefix 1                                            	Meth                   2	Eth 3	Prop 4	But 5	Pent 6	Hex 7	Hept 8	Oct 9	Non 10	Dec 11	Undec 12	Dodec 14	Tetradec 16	Hexadec 17	Heptadec 18	Octadec 20	Eicos 22	Docos 24	Tetracos 26	Hexacos 28	Octacos 30	Triacont 40	Tetracont

Homologous SERIES

A series of compound which can be represented by a general formula and differ by a fixed group of atom is called homologous series.

The members of this series are called homologues. ALKANE CH4-C2H6--- C3H8    Difference--CH2 ALKENE C2H4---C3H6C4H8    Difference---CH2 ALKYNE C2H2--C3H6C4H8    Difference---CH2 CHARACTERISTICS OF HOMOLOGUS SERIES 	All members of series can be represented by same molecular formula. 	The difference between two members of series is CH2. 	Chemical properties are same of all members of series. 	M.P and B.P increases with increases in molecular formula. ISOMERS Organic compound with same molecular formula but different structures are called isomers. EX- [n-Butane and Isobutane,] [n-Propane, Isopropane, and Neopentane.] CHARACTERISTICS OF ISOMERS 	All isomers of a compound have same molecular formula. 	But they have different structure. 	The physical and chemical properties of isomers of a compound are differing from another.

ALKANES General formula-- CnH2n+2 They are also called paraffins means little affinity or short relationship. The main sources of alkane are petroleum, natural gas and crude oil.

PHYSICAL PROPERTIES 	The first four members are Gas, next thirteen are liquid, and rests are solid. 	M.p and B.P increases with increase in molecular mass. 	They are nonpolar molecules. 	Alkanes are lighter than water. 	They are insoluble in water and alcohol but soluble in nonpolar solvents.

CHEMICAL PROPERTIES 1)	Combustion—when alkanes are burnt in air or oxygen, they completely oxidized to carbon dioxide and water and releases large amount of heat.    CnH2n+2  +  (3n+1/2)O2 ---   nCO2   +   ( n + 1 )H2O   + HEAT EX-         CH4    + 2O2       --     CO2   +   2H2O   +    heat   ( n=1)         2C4H10  +   13O2     8CO2    +   10H2O  +   heat   (n=4) 2)	Substitution—one or more hydrogen atoms of an Alkane are replaced by a more reactive atoms or group of atoms. a.	Nitration Alkane undergoes nitration when treated with fuming Nitric acid at 4750C. ex-    CH4 + HNO3   --  CH3NO2  +  H2 b.	Halogenation Alkane reacts with in the presence of sunlight. Ex-  CH4     +   Cl2 --  CH3Cl   +  HCl c.	Cracking- When heated to high temperature in the absence of oxygen Alkanes decomposed? Ex C2H6      -- C2H4   +   H2 USES OF ALKANE 	Alkanes are excellent fuel. 	Methane & Butane (LPG) are used as domestic fuel. 	Petrol & Diesel are used in vehicles. METHANE It is the simplest hydrocarbon in nature. It occurs along with petroleum in the earth’s crust called natural gas. It is also known as marsh gas occurs in mud and coal mines. It is major constituent of Gobar- gas & biogas. PREPARATION The mixture of four parts by weight of soda lime and one part of anhydrous sodium acetate is taken in a hard gas test tube and heated strongly then methane gas is obtained. PHYSICAL PROPERTIES 	It is a colourless, odourless & tasteless gas. 	It is sparingly soluble in water, so it is collected over water. 	It is lighter than water. CHEMICAL PROPERTIES 1)	Combustion—Methane does not support combustion, but burns with non luminous flame and explode violently when mixed with air or oxygen and fired. On burning with oxygen, it gives carbon dioxide and water. Ex- CH4 + 2O2 -  CO2 + H2O. 2)	Action of chlorine--- When it is mixed with chlorine in sunlight, it explodes to fume of hydrogen chloride, and black particles of carbon separate out. CH4        +        2Cl2                 4HCl   +     C Such reactions, in which one or more atoms in a molecule are replaced by equivalent atoms, are called substitution reaction. STRUCTURES Methane has four hydrogen atoms attached to a central carbon atom. So its molecular formula is CH4. In methane carbon forms four covalent bonds. The methane molecule has tetrahedral shape. USES OF METHANE 	It is used as gaseous fuel for domestic cooking. 	Black carbon, obtained from methane is used as filler in the rubber industry. 	It is basic materials to form organic compounds. 	It is major constituent of biogas.

NATURAL GAS Natural gas is a mixture of gaseous hydro carbons. It is found in earth’s crust with petroleum. Natural gas consists of Methane (85%), Ethane (10%), Propane (3%), butane (1%) and some CO2, H2, H2S, and He. USES OF NATURAL GAS 	It burns to produce heat so used as domestic fuel. 	Compressed natural gas (CNG) has been found to be an alternative to petrol as automobile fuels. 	In the manufacture of fertilizers. 	It is used to produce black carbon used in tyres. LIQUEFIED PETROLEUM GAS It is a mixture of gaseous hydrocarbon, mainly ethane, propane, and butane. It is obtained during the refining of petroleum at below 400 K temperatures. It is also obtained by natural gas. It is used as a domestic fuel stored in cylinders. •	LPG doesn’t have their self smell so a gas called Ethyl mercaptan (C2H5SH) is mixed into it to detect leakage of LPG. ADVANTAGES 	It is used as domestic fuel. 	It burns without producing smoke. 	It is a clean fuel can be easily handled. PETROL & GASOLINE •	It is a complex mixture of Hexane, Heptanes, & Octane. It is obtained by fractional distillation of petroleum. •	It is used as fuel in motors, cars, scooters etc •	It is also used as a solvent for cleaning clothes.

COMPOUND CONTAINING C, H, & O Functional group— an atom or a group of atoms in an organic molecule that is responsible for the compound’s characteristic reaction and determines their property is called functional group. i.	It is the most reactive part of organic molecule. ii. Chemical properties of an organic compound are determined by its functional group. •	Hydroxyl group (-OH) - All organic compound containing -OH as functional group are known as alcohol. Ex- methanol (CH3OH), ethanol (C2H5OH). •	Aldehyde group (-CHO) Organic compound containing –CHO as the functional group are known as Aldehyde. Ex- methanol (HCHO), ethanol (CH3CHO). •	Carbonyl or Ketone group (>CO) Organic compound containing >CO as the functional group are called ketones. Ex- Propanone (CH3COCH3). •	Carboxyl group (-COOH) All organic acids contain carboxyl group as functional group. Ex- methanoic acid (HCOOH), Propanoic acid (CH3CH2COOH).

Alcohols are a class of compounds which contain carbon, hydrogen and oxygen. It is obtained by replacement of one hydrogen atoms in an alkane by a hydroxyl group.
 * ALCOHOLS |

CH4          ---        CH3OH Alcohols are organic compounds which contain hydroxyl group bonded to a carbon atom. The general formula for alcohols is R-OH where R is an alkyl group and –OH is the functional group. NAMING OF ALCOHOLS 	There are two methods for naming alcohols. 1.	The common method  In this method, the nature of the parent alkyl group is combined with, the word alcohol. Ex methyl alcohol, ethyl alcohol. 2.	The IUPAC system in this method, the last ‘e’ in the nature of parent hydrocarbon of alcohol is replaced by Ol. Ex- methane--methanol Ethaneethanol CLASSIFICATION OF ALCOHOL 1.	A primary alcohol has general formula R-CH2OH. 2.	A secondary alcohol has general formula R-CH2OH-R’. 3.	A tertiary alcohol has the general formula RR’R”C-HOH. They are also classified as monohydric, dihydric, trihydric etc. It is based on the number of OH group they have— Monohydricmethanol, ethanol Dihydric-ethylene glycol Trihydric--glycosol PHYSICAL PROPERTIES 	The first two members of the alcohol series methanal and ethanol are volatile liquid. 	The alcohols containing 1 to 10 carbon atoms are oily liquids, while those containing more than 10 carbon atoms are solids. 	All alcohols are neutral to indicators. 	The boiling point of alcohol increases as their molecular mass increases. 	Straight chain alcohols boil at higher temperature than branched chain isomers. BOILING POINT INCREASES IN ORDER Primary > Secondary > Tertiary 	Alcohols are bad conductor of electricity. CHEMICAL PROPERTIES 1)	With acids  they react with acids to form a class of compound called esters.                                    R-OH + HONO2 (Nitric acid) -   R-ONO2  +  H2O                        R-OH + CH3COOH (ethanoic acid) ---   CH3COOR (alkyl ethanoate) +  H2O 2)	With sodium   It reacts with metallic sodium to liberate hydrogen. 2R-OH + 2Na -- 2RO-Na+ + H2 3)	Oxidation i.	Oxidation of primary alcohol gives Aldehydes. ii.	Oxidation of secondary alcohol gives Ketones. iii.	Under special conditions tertiary alcohols give a mixture of Ketone and acid. 4)	Combustion   Alcohols burns readily in air, forming carbon dioxide and water vapour. 2CH3OH (methanol) + 3O2  -  2CO2  +  4H2O. Tests for alcohols 1.	Sodium test  when some amount of organic compound is mixed with sodium they reacts to form a alcoholic group with evolution of hydrogen. 2R-CH2OH +  2Na  ---  2R-CONa+  +  3H2 2.	Ester formation test  The organic compound is heated is with glacial ethanoic acid and with some sulphuric acid, ester is formed. R-CH2OH +  CH3COOH  ---  R-CH2-COO-CH3   +  H2O

METHANOL (or Methanoic acid) It is the simplest alcohol. It is the first member of homologous series of alcohols. It is initially                                                        obtained   by destructive distillation of wood. PROPERTIES 	It is a colourless liquid with a boiling point of 337k. 	It is miscible with water in all properties. 	It is lighter than water. 	It is neutral to litmus 	It is highly toxic, it can cause blindness even death. USES OF METHANOL 	It is used as a denaturant 	It is used for making of perfumes and synthetic. 	It is used in synthesis of methanol used in plastic industry 	Along with petrol, methanol is used as a motor fuel.

ETHANOL (or ETHYL ALCOHOL) It is the second member of homologous alcoholic series. It is also known as methyl carbinol. PHYSICAL PROPERTIES 	Ethanol is colourless liquid have a pleasant smell. 	It boils at 351k 	It is miscible with water in all proportions. 	It is a nonconductor of electricity because it does not contain ions. 	It is neutral to litmus CHEMICAL PROPERTIES 1.	Combustion- Ethanol burns in air with a blue flame to form carbon dioxide and water. C2H5OH +  3O2 -  2CO2  +  3H2O 2.	Oxidation a)	Ethanol is oxidised to ethanoic acid by the oxygen of the air in presence of copper.                               CH3CH2OH  +  O2    Cu---  CH3COOH  +  H2O b)	It is oxidised to ethanoic acid by an acidic solution of potassium dichromate. CH3CH2OH +  2[O]  k2cr2o7 + H2so4  CH3COOH  +  H2O c)	Ethanol on treatment with a 5% solution of chromium anhydride in a glacial ethanoic acid is oxidized to ethanol.     CH3CH2OH  --Cro3 + ethanoic acid CH3CHO 3.	Reaction with carboxylic acid -- When it is warmed with ethanoic acid in the presence of a few drop of H2SO4, ETHYL ETHONATE IS PRODUCED, this process is called esterification.              2C2H5OH  +  2Na  ---  2C2H5ONa  +  H2O. 4.	Reaction with sodium- Ethanol reacts with sodium to produce hydrogen gas & sodium ethoxide.                               2C2H5OH  +  2Na  +  --- 2C2H5ONa  + H2 5.	Dehydration--  When it is heated with concentrated sulphuric acid at 1700C, it is dehydrated to form ethane or ethyle.                           CH3CH2OH       -H2SO4---  H2C  =  CH2  +  H2O USES OF ETHANOL 	It is a constituent of beverages like beer, wine, whisky etc. 	It is used to sterilize wounds& syringes. 	It is used as transport fuel. 	It is used in manufacture of perfumes, paints, medicines, rubber etc.