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Download Packet 14: Organic Chemistry
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Organic Chemistry TOPIC 11 REVIEW BOOK TA B L E S P, Q A N D R What is Organic Chemistry? study of carbon and the compounds that it forms carbon has 4 valence electrons so it will form 4 covalent bonds- lends itself to a great variety of compounds May also contain but are not limited to the following elements: a) Oxygen e) Phosphorus b) Nitrogen f) Sulfur c) Fluorine g) hydrogen d) Bromine Properties of Organic Compounds Covalent bonds generally nonpolar- what does that mean? insoluble in water low mp’s and bp’s: boiling point is directly related to the length of carbon chain nonelectrolytes slow to react because of the covalent bonds – many reactions require a catalyst Hundreds of thousands of organic compounds because C can form so many bonds Quick Review How many valence electrons does an atom of carbon have? How many bonds can an atom of carbon make? Draw a Lewis structure for CH4 Draw C2H6 Draw C6H14 Hydrocarbons (Tables P and Q) molecules that contain only carbon and hydrogen May have single, double or triple bonds May form straight chains, branched chains or rings homologous series different groups of hydrocarbons each group contains molecules that have similar structures and properties as the molecular mass increases, the boiling point increases (why?) 1. Alkanes Only single bonds Saturated the general formula is CnH2n+2 End in –ane Prefix tells you the number of carbon atoms Example: Methane, Ethane, Propane, etc May be straight or branched chains 2. Alkenes One double bond (C = C) rest are single Unsaturated The general formula is CnH2n First member is ethene Examples: Propene, Butene, Pentene May be straight or branched chains 3. Alkynes one triple bond, the rest are single unsaturated the general formula is CnH2n-2 First member is ethyne Example: Propyne, Butyne, Pentyne May be straight or branched Aromatic Hydrocarbons Made up of a chain of hydrocarbons that form a ring Most common one is benzene C6H6 in a ring of alternating double And single bonds Isomers molecules that have the same number and types of elements but are arranged differently They will have different properties Naming and Drawing Straight Chain Alkanes Without Branches identify the number of carbons use table P to get the prefix for that number add the suffix “ane” Ex: CH4= “meth” + “ane” = methane ethane propane Butane Pentane Hexane octane Naming and Drawing Straight Chain Alkenes Alkenes without branches Name alkenes the same way you would alkanes, EXCEPT you must specify the location of the double bond by using the lower number of the two that it is in between Examples: Ethene Propene Butene (1 Butene, 2 Butene) Pentene (1 Pentene, 2 Pentene, 3 Pentene) Naming and Drawing Alkynes The rules for naming alkynes are the same for alkenes, except there is a triple bond instead of a double bond 2-butyne 2-hexyne 3 hexyne 1 pentyne 3 octyne Naming and Drawing Branched Alkanes You need to be able to identify three things: Parent chain, branch name, location 1. Identify the longest continuous chain (parent chain)- use table P for the prefix and add -ane 2. Find the branches 3. Number the carbons in the parent chain, starting at the side closest to the branch 4. Count the number of carbon atoms in the branch and get the prefix from Table P and add the suffix –yl 5. Use the number of the parent carbon atom, the name of the side chains and the name of the parent chain Example 4 ethyl octane Naming Branched Alkanes If the same group occurs more than once as a side chain, you indicate this using prefixes (ex: di, tri). Indicate the positions of each group with a number If the side chains are different, name the one with the smallest carbon number first 2,3 dimethyl pentane Naming and Drawing Branched Alkenes and Alkynes Branched Alkenes and Alkynes follow the same rules for naming branched alkanes, EXCEPT when numbering the carbons, start with the side closest to the double bond or triple bond rather than the nearest side chain Functional Groups – Replacement of One or More H Other types of organic compounds can form when different atoms replace one or more of the hydrogens happens to alkanes These atoms or groups of atoms are called functional groups They give the compound specific physical and chemical properties 1. Halides When one of the halogens (F, Cl, Br, I) replaces a hydrogen atom called a halide or a halocarbon The functional group is the halogen Naming: Specify the location of the halogen and use the following prefixes: chloro, fluoro, bromo, iodo Uses: Teflon, Freon, CFC’s, dry cleaning solvents, pesticides 2. Alcohols a hydrogen on an alkane is replaced with an -OH group (hydroxyl group- NOT hydroxide ion!) the functional group is –OH Classified according to the number of carbons bonded to the carbon where the –OH is Primary, secondary, tertiary Naming: Drop the “e” and add “ol”; specify the location of the –OH Uses: fuel, solvents, industrial feedstock (used to make other products, such as formaldehyde, etc) 3. Ethers The functional group is -O Naming: you name the left group and the right group and you follow it by the word ether if both group are the same, use "di“ Used to be used as anesthetics, used for 4. Aldehydes contain a carbonyl (C=O) group on an end carbon No numbering Naming: Drop the “e” and add “al” 5. Ketones Carbonyl group on any carbon atom except the end ones Formed by the oxidation of a secondary alcohol Naming: drop the “e” and add “one”, specify the location 6. Organic Acids The functional group is -COOH which is called a carboxyl group Usually formed by oxidizing alcohols Carboxyl groups are only attached to end carbons, so no numbering is needed Naming: drop the “e” and add “oic acid” 7. Esters They are formed from a reaction between a carboxylic acid and an alcohol Naming: The name of the alcohol is given first, with the suffix changed to “yl” Then the name of the acid is given with the suffix changed to “oate” 8. Amines The functional group is -NH2 called an amino group Naming: drop the “e” and adding “amine”, specify location 9. Amides They contain an amino group attached to the carbon atom of a carbonyl group Naming: drop the “e” and add “amide” Organic Reactions Hydrocarbons are not reactive at room temperature because of strong C-C and C-H bonds at very high temps, hydrocarbons can undergo many different reactions 1. Substitution replacement of one or more hydrogen atoms in an alkane with another atom or group ex. halogen atoms replace a hydrogen atom on an alkane to make a halide and an acid ex. C2H6 + Cl2 C2H5Cl + HCl 2. Addition involves adding one or more atoms at the site of a double or triple bond occurs in alkenes or alkynes Ex. C2H4 + Cl2 C2H4Cl2 3. Hydrogenation type of addition it is the addition of hydrogen to an unsaturated compound to make it saturated it requires a catalyst and a raised temp Ex. C2H4 + H2 C2H6 4. Esterification the reaction of an organic acid with an alcohol to produce an ester plus water slow reaction that is reversible usually have pleasant odors 5. Saponification when an ester (fat) reacts with an inorganic base (NaOH) to produce an alcohol and a soap 6. Polymerization the formation of large molecules called polymers by combining smaller units called monomers used to make plastics and rubber, proteins, starches and cellulose Condensation polymerization: the bonding of monomers by a dehydration reaction ex. glucose + glucose sucrose + water Addition polymerization: the joining of monomers by eliminating double or triple bonds Ex. ethene + ethene = butane 7. Fermentation when yeast breaks down 6-carbon sugars to produce carbon dioxide and an alcohol ex. C6H12O6 2C2H5OH + CO2 8. Combustion (and so...we end as we began) When a saturated hydrocarbon reacts with oxygen to produce water and carbon dioxide A lot of energy (heat) is given off C3H6 +5O2 3CO2 + 4H2O Lastly… Practice your regents exams Use the Barron’s book Bring a NON-GRAPHING calculator, a black pen and pencil (for drawing) to the Regents Exam Have a great summer and come back to visit next year!
