Organic Chemistry. What is it? Study of compounds involving carbon –Carbon has the ability to make...
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Transcript of Organic Chemistry. What is it? Study of compounds involving carbon –Carbon has the ability to make...
What is it?
• Study of compounds involving carbon
– Carbon has the ability to make chains and rings with itself
– Thousands of compounds contain only Carbon and Hydrogen
– Millions with other elements added
• Usually, Nitrogen, Oxygen, Sulfur, Halogens
Patterns
• Within the millions of compounds there are patterns that emerge
– Carbon forms 4 Bonds
– Hydrogen forms 1 Bond
– Oxygen forms 2 Bonds
– Halogens form 1 Bond
Identifying Compounds
• Name – Based on naming conventions (Usually IUPAC)
• Molecular Formula – Shows actual number of atoms present C4H8O2
• Empirical Formula – Shows the simplest whole number ratio of atoms C2H4O
• Structural Formula – Shows how the atoms are arranged CH3COCH2CH2OH
Cont.
• Graphical Formula – Shows how the atoms are arranged in space and bonded
• Similar to Lewis Structures but w/o the dots– CH3COCH2CH2OH
Cont.
• Skeletal Formula – Abbreviated form of graphical formula often omitting carbons and hydrogens CH3COCH2CH2OH
Alkanes• Straight chain organic compounds
containing only C, H, and sometimes halogens
• All carbons are sp3 hybridized• General formula CnH2n+2
• 1 C =
CH4
• 6 C’s =
C6H14
Properties
• Nonpolar – Dissolve other nonpolar compounds– Hydrophobic – Water hating
• Good Lubricants and metal preservers
• C1 to C4 = (Gas) Fuels - Methane
• C5 to C8 = (Liq.) Fuels - Gasoline
• C9 to C16 = (Viscous Liq.) – Diesel Fuel
• C17 and Up = (Very Viscous) - Greases
Hydrocarbons and Saturation
• Hydrocarbons are compounds that only contain Carbon and Hydrogen
• Alkanes are saturated hydrocarbons
– Carbons are saturated with hydrogen
• Compounds with double or triple bonds are unsaturated (more later)
Alkane Nomenclature
• Alkanes are named according to the longest carbon chain. (per IUPAC rules)
• System of prefixes to determine the number of carbons that are present.
1 = meth, 2 = eth, 3 = prop, 4 = but, 5 = pent
6 = hex, 7 = hept, 8 = oct, 9 = non, 10 = dec
• All alkanes end in -ane
Alkane Nomenclature
• Alkanes end in –ane
• Alkanes without branches are named according to the number of carbons
• Alkanes with branches are named according to longest chain of carbons
• The longest chain is numbered so that substituents receive the lowest number
Cont.
• When more than one of the same substituents is present use the prefixes di- tri-, tetra-
• If two or more substituents are present they are listed alphabetically (except prefix)
• Numbers are separated by commas, numbers and letters by hyphens
Substituent Groups
• Alkyl Groups – A hydrocarbon missing a hydrogen
CH3 – Methyl
CH3CH2 – Ethyl
CH3CH2CH2 – Propyl
CH3CH2CH2CH2 – Butyl • HalogensCl – Chloro Br – BromoF – Fluoro I – Iodo
Isomers
• Same formula different compound
• Structural Isomers
– Completely different bonding pattern
• Stereoisomers
– Same bond pattern
Dash Line Wedge Drawings
• A way of representing arragement in space
• Lines represent bonds in the plane
• Wedges come out of the plane and
• Dashed lines go into the plane
• Draw for Methane
Newman Projections
• Another way of showing arrangement in space.
• Look at the molecule for the end view
• Draw Newman Projection for Ethane
Alkane Confromations
• Alkanes are free to rotate because of single bond.
• Overlap of one orbital (sigma bond)
• Different arrangements are called rotamers.– A Stereoisomer
• Rotate to give minimum repulsion
Cycloalkanes
• Alkanes that from ring structures
• Not necessarily a circle
• All carbons are still sp3 hybridized
• Saturated compounds
• General Formula CnH2n
Cycloalkane Nomenclature
• Named by placing cyclo- in front of the alkane name of the longest carbon ring
• If there is only one substituent there is no need to number it
• If there are multiple substituents the must be numbered.– Number by alphabetical order
Conformations of Cycloalkanes
• Cycloalkanes take on interesting shapes
• Consider cyclopropane
• What must the bond angles be?
• 60 degrees!– Because 3 points determine a plane
Cont.
• Consider cyclobutane
• What are the bond angles?
• 88 degrees
• There is a slight “puckering” of the bonds
Cont.
• Consider cyclohexane
• What must the bond angles be?
• 109.5!
• Six membered rings are very common
• Takes on two puckered conformations
• Chair and boat conformations
Configurational Isomers
• Same bond pattern different arrangement in space
• Called cis- and trans- isomers
• Cis- same side Trans- opposite
• Cis and trans molecules are different molecules
• Different boiling points
• Fig. 2.7 in book. (Page 60)
Reactions of Alkanes
• Alkanes are fairly boring from a chemistry point of view.
• Meaning they are fairly unreactive
• Make very good solvents
• Two types of reactions
– Burning
– Reacting with halogens
Combustion
• When alkanes react with oxygen they can burn
• Complete combustion of alkanes yields carbon dioxide and water
CH4 + 2O2 CO2 + 2H2O + heat
• Incomplete combustion yeilds carbon monoxide and water
Halogenation
• Process of adding a halogen to an alkane
• Process must take place in the light
• General form
R – H + X – X R –X + H – X
• Where R is an alkane and X is a halogen
• Called a substitution reaction
• A hydrogen is substituted for a halogen
• When chlorine is added it is called chlorination and so on
Cont.
• Excess halogen allows the reaction to continue
CH4 + 4 X2 CX4 + 4 HX
• Reactions of straight chain alkanes gives a mixture of products
C3H8 + Cl2 ?
Cycloalkanes
• Unsubstituted cycloalkanes give only one product when reacted with a halogen
• Write the balanced reaction when cyclobutane is reacted with bromine
Mechanism of Substitution
• The Mechanism is a process by which the reaction takes place
• Halogenation is a Free Radical Chain Reaction
• Made up of three steps– Initiation– Propagation– Termination
Initiation
• Beginning step
• Energy from light is required to break the halogen bond (Weaker than C-C or C-H)
• Creates a radical (Free atom)
Propagation
• Continuing the reaction
• Radicals react with the alkane and more halogens to create more radicals