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L-4 Carbon and Its Compounds Formation of Hydrogen Molecule

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L-4 Carbon and Its Compounds Formation of Hydrogen Molecule L-4 Carbon and its compounds Covalent Bond: The chemical bond formed by the sharing of electrons between two atoms is known as covalent bond The sharing of electrons takes place in such a way that each atom in the resulting molecule gets the stable electron configuration of inert gases. Whenever a non metal combines with another non metal sharing of electrons takes place between their atoms. The bond formed between the atoms of the same element is a covalent bond. The shared electrons are counted with both the atoms due to which each atom in the resulting molecules gets an inert gas electron arrangement of either 8 electrons or 2 electrons in the outermost shell. Types of covalent bond : i. Single covalent bond ii. Double covalent bond iii. Triple covalent bond i. Single covalent bond Single covalent bond or single bond is formed by the sharing of one pair of electrons between two atoms. A single covalent bond is denoted by putting a short line (-) between two atoms. Formation of Hydrogen Molecule Hydrogen atom has only one electron in its outermost shell, and requires one more to acquire the nearest noble gas configuration of helium (He: 1s2). To do so, two hydrogen atoms contribute one electron each to share one pair of electrons between them. This leads to the formation of a single covalent bond between the two hydrogen atoms. Formation of Chlorine Molecule Chlorine atom has seven valence electrons. Thus, each Cl atom requires one more electron to acquire the nearest noble gas configuration (Ar:2, 8, 8). They do this by mutual sharing of one pair of electrons as shown below. Formation of Methane (CH4) Carbon atom has four electrons in its outermost shell. Thus, it requires four more electrons to acquire a stable noble gas configuration. Each hydrogen atom has only one electron in its outermost shell and requires one more electron to complete its outermost shell (to acquire He configuration). This is done as follows: Formation of ethane – C2H6 2. Double covalent bond Double covalent bond is formed by the sharing of two pairs of electrons between two atoms. A double covalent bond is denoted by putting 2 short line (=) between two atoms. Formation of CO2 : Formation of O2 Formation of C2H4 Electronic configuration of C = K L 2 4 Electronic configuration of H = K 1 3. Triple covalent bond : Triple covalent bond is denoted by putting 3 short lines ( ) between the two atoms. Eg: a. Formation of N2 : Electronic configuration of N = K L 2 5 b. Formation of ethyne ( C2H2) ; Electronic configuration of C = K L 2 4 Electronic configuration of H = K 1 Properties of covalent compounds : 1. Covalent compounds are usually liquids and gases . only a few of them are solids. Solid covalent compounds i. Iodine ii. Glucose iii.Naphthalene iv.Camphor Liquid covalent compounds i. Methane ii. Propane 2. They usually have low melting and low boiling points. 3. They are insoluble in water but they are soluble in organic solvents. 4. They do not conduct electricity Carbon compounds : Carbon is an element (a non metal). It belongs to 2nd period, 14th group of the periodic table. Carbon derived its name from the Latin word carbo means coal. Atomic number of carbon is 6 Electronic configuration is K L 2 4 hence carbon is tetravalent. Availability of Carbon in earth’s crust is 0.02% in the form of minerals like CO3 an HCO3. Availability of carbon in the atmosphere is 0.03% in the form of CO2 More than 5 million carbon compounds are known to chemists Carbon has four electrons in its outermost shell and needs to gain or lose 4 electrons to attain noble gas configuration. If it were to gain or loose electrons i. It could gain 4 electrons to form C4- anion but it would be difficult for the nucleus with 6 protons to hold on to 10 electrons. ii. It could loose 4 electrons forming C4+ cation but it would requires a large amount of energy to remove 4 electrons leaving behind a carbon cation with 6 protons in its nucleus holding on to 2 electrons. Carbon overcomes this problem by sharing its electrons with other atoms of carbon or with atoms of other elements. Versatile nature or unique nature of carbon : Carbon shows unique properties like tetravalency, catenation, formation of multiple bonds and most of its compounds form isomers. Catenation : The property of self linking of carbon atom through covalent bonds in order to form straight or branched chains and rings of different sizes is known as catenation. Eg: Carbon atom poses the property of catenation to a greater extent than any other element. Tetravalency of Carbon : Carbon has four electrons, it can neither loose nor gain electrons to attain octet, it forms covalent bonds by sharing its 4 electrons with other carbon atoms or atoms of other elements. “The characteristic property of carbon atom by virtue of which it form four covalent bonds is called tetravalency of carbon atom.” Carbon form compounds with oxygen, hydrogen, nitrogen, sulphur, halogens and many other elements. Carbon forms very strong bonds with most other elements making these compounds exceptionally stable. The reason for the formation of strong bonds by carbon is its small size. This enables the nucleus of the carbon atom to hold on to the shared pair of electrons strongly. Tendency to form multiple bonds : Due to small size, carbon atom forms double or triple bonds. As a result It can form variety of compounds. Isomerism: The organic compounds having same molecular formula but different structural formulae are called isomers and the phenomenon is isomerism. Organic compounds with minimum 4 carbon atoms show the phenomena isomerism Hydrocarbons : A compound made up of hydrogen and carbon only is called hydrocarbon E.g. Methane CH4 Ethane C2H6 Ethene C2H4 Ethyne C2H2 The carbon atoms are arranged in hydrocarbons in straight chain, branched chain or ringed structures. Hydrocarbons Aliphatic Cyclic hydrocarbons hydrocarbons Saturated Unsaturated Alicyclic Aromatic Alkane Alkeness Alkynes Aliphatic hydrocarbons : The hydrocarbons in which carbon atoms are arranged in straight or branched chains are called aliphatic hydrocarbons Aliphatic hydrocarbons are of two types: a. saturated aliphatic hydrocarbons b. Unsaturated aliphatic hydrocarbons. Saturated hydrocarbons (Alkanes) A hydrocarbon in which the carbon atoms are connected by only single bonds is called saturated hydrocarbons. Saturated hydrocarbons are called alkanes and are also called paraffins Param - Little Affin - Affinity Eg : Methane ,CH4 , Ethane ; C2H6 Propane : C3H8 Condensed structure : CH3CH2CH3 Butane : C4H10 Condensed structure CH3CH2CH2CH3 The general formula of alkanes is CnH2n+2 The saturated hydrocarbons are chemically not reactive Unsaturated hydrocarbons Hydrocarbons in which the two carbon atoms are connected by a double bond or a triple bond then these hydrocarbons are called unsaturated hydrocarbons Alkenes: An unsaturated hydrocarbon in which the two carbon atoms are connected by a double bond is called alkene. Eg: Ethene C2H4 : Propene C3H6 Condensed formula : CH3CH=CH2 Butene C4H8 Structural formula : Condensed formula : CH3 CH2 CHCH2 Alkenes contain –C=C-- group The general form of alkene is CnH2n. Alkenes are also called olefins. Since an alkene has double bond between two carbon atoms, simplest alkene will have two carbon atom in its molecule. There can be no alkene having only one carbon atom. ii. Alkynes : An unsaturated hydrocarbon in which two carbon atoms are connected by a triple bond is called an alkyne. Eg: Ethyne C2H2 Propyne C3H4 Butyne C4H6 An alkyne contains –C C – graph. General form of alkyne CnH2n-2 Unsaturated hydrocarbons (Alkenes, Alkynes) are more reactive than saturated hydrocarbons (Alkanes) Alkyl group: The group formed by the removal of one hydrogen atom from an alkane molecule is called an alkyl group Eg: CH4 Methyl group C2H6 Ethyl group C3H8 Propyl group The alkyl groups are denoted by R. The general formula of alkyl group is CnH2n+1 One valancy of carbon atom is free in an alkyl group Write the structure, electron dot structure, formula of ethane, ehene, ethyne i. Ethane C2H6 ii. Ethene C2H4 iii. Ethyne C2H2 b.Cyclic hydrocarbons : The hydrocarbons in which the carbon atoms are arranged in form of closed chains or rings. The cyclic hydrocarbons may be saturated or unsaturated. They are classified as Alicyclic hydrocarbons Aromatic hydrocarbons Alicyclic hydrocarbons : These hydrocarbons contain a ring chain of three or more carbon atoms. This cyclic compounds are named by prefixing “cyclo” before the name of the corresponding straight chain hydrocarbon i. Saturated Cyclo propane Cyclo Butane CycloPentane Cyclohexane Unsaturated e.g.: Cyclopropene cyclobutene cyclopentene cylcohexene Cyclobutyne Aromatic Hydrocarbons: The hydrocarbons contain at least benzene ring in their molecules. The benzene ring is a specific type of ring structure of six carbon atoms having C-C single bond and C=C double bond in alternate positions. Toluene Phenol Naphthalene Hetero atoms: The atom replacing the hydrogen atom in an organic compound is called hetero in an organic compound is called hetero atoms. These hetero atoms give characteristic properties to compounds regardless the length and nature of carbon atom. Functional group : A functional group be defined as an atom or group of atoms which determine the properties of organic compounds. The functional group is the site of chemical reactivity in the organic molecule Homologous series : A series of organic compounds having similar structures and similar chemical properties in which the successive members differ in their molecular formula by CH2 group. The different members of the series are called homologous Eg: An alkane family represents a homologous series. All the alkanes have similar structure with the single covalent bond and show similar chemical properties. Each successive members differ by a CH2 group Methane –CH4 Ethane - C2H6 Propane –C3H8 Butane – C4H10 Similarly alkene and alkyne family also represent homologous series.
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