Organic chemistry is the study of the properties of the compounds of carbon. Just about everything...
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Transcript of Organic chemistry is the study of the properties of the compounds of carbon. Just about everything...
Organic chemistry is the study of the properties of the compounds of carbon.
Just about everything in this world has carbon, C, in it!
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Learning Objectives
a. Organic molecules form the basis for life and include many natural products with medicinal properties.
b. After the structure of a biologically active compound is determined, organic chemists can often synthesize the compound, as well as new derivatives with more powerful activities.
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Learning Objectives (cont)
c. Most organic compounds contain a hydrocarbon framework containing chains of carbon atoms and bonded hydrogen atoms (“hydrocarbons”).
d. Hydrocarbons are classified according to types of carbon-carbon bonds. Alkanes contain only single bonds, alkenes contain at least one double bond, alkynes contain at least one triple bond, and aromatics are rings that contain alternating single and double bonds.
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Learning Objectives (cont)
e. Adding different atoms or groups of atoms (functional groups) to a hydrocarbon results in new classes of compounds with distinctive chemical properties.
f. The geometric arrangement of atoms within an organic compound determines its activity.
g. Two mirror-image molecules (enantiomers) with the same chemical formula and connections of the atoms can have different biological activities.
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• General Properties of Organic Compounds a. Review of Carbon
1. Carbon has four electrons in its outer shell and therefore can form four covalent bonds.
b. Polarity 1. Organic molecules contain many nonpolar C-H bonds
and are therefore generally hydrophobic.
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Three waysin which carbon can fulfill its octet
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Effect of differences in electronegativity on charge distribution
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• General Properties of Organic Compoundsc. Intermolecular Forces
1. Small hydrocarbons interact through relatively weak London forces and therefore tend to be gases at room temperature.
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Melting and BoilingPoints of Hydrocarbons
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• General Properties of Organic Compoundsc. Intermolecular Forces
3. Large hydrocarbons and those containing bonded polar atoms are often liquids or solids at room temperature.
4. Organic molecules containing bonded polar atoms are generally more water soluble than those containing only carbon and hydrogen. (Like dissolves like.)
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Water Solubility ofAlcohols vs. Alkanes
OH groups can make a molecule, with less than 8 carbons, water soluble
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• Natural Products a. Some compounds found in nature (natural
products) have interesting properties, such as medicinal activity.
b. Once the structure of a natural product is determined, chemists may seek to synthesize the compound in the laboratory.
c. Parent compounds, like salicin, serve as the structural basis for new synthetic molecules (derivatives or analogues).
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Synthesis of Derivatives
The willow tree, source of the active ingredient of aspirin
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The Pacificyew tree, source of taxol
A molecule with powerfulAnticancer activity!
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• Types of Hydrocarbons a. Alkanes: contain only single carbon-carbon
bonds
b. Alkenes: contain at least one double carbon-carbon bond
c. Alkynes: contain at least one triple carbon-carbon bond
d. Aromatics: ringed hydrocarbons with alternating single and double bonds between carbons.
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Examples of Straight-Chain Alkanes
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Reduction ofhydrocarbons vs. oxidation
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Reactivity of Alkanes
Hydrocarbon + O2 carbon dioxide + water + heat energy
Ex. CH4 + 2O2 CO2 + 2H2OHeat released is 802 kJ/molof methane
Effect of partially oxidizing a hydrocarbon, let’s look at the combustion reaction of CH3OH (methanol), in which 1 H has been replaced by an –OH group.
2CH3OH + 3O2 2CO2 + 4H2O Heat released is 640 kJ/molof methanol
(1.5 moles of O2 required to with 1 mole of CH3OH!)
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These reactions illustrates two important principles.
1st, the more reduced a molecule, the more energy is released during oxidation on a molar basis.
Methane is fully reduced and gives off more energy during combustion than methanol.
2nd, the number of oxygen molecules required to react with a fuel molecule gives an estimate of how much energy is available.
More highly reduced molecules require more oxygen during combustion and produce more energy.
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Examples of cycloalkanes
CyclopentaneC5H10
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The simplest alkene, ethylene
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Saturated fats contain threealkane chains, unsaturated fats three alkene chains
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Cis and trans refer todifferent geometries in two isomers
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Trans Fatty Acidsin Some Common Food Products
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The formation oftrans double bonds, hydrogenation
Polymerization: white plastic water bottles
Credit: Courtesy of Nalgene
monomers
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The simplest alkyne, acetylene
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Benzene Naphthalene, in mothballs
Anthracene, in insecticides and woodpreservatives
Aromatics Compounds, Polycyclic Aromatic Hydrocarbons (PAH’s)
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Bioaccumulation ofPolycyclic Aromatic Hydrocarbons
A process by which chemical contaminationincreases within organismshigher up the food chain.
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• Functional Groups are groups of atoms that
contribute to the properties of an organic compound a. Organic Halides ex. CH3-X (X = Cl, Br, I, or F)
b. Oxygen-Containing Functional Groups1. Ethers
2. Aldehydes
3. Ketones
4. Carboxylic Acids
5. Esters
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• Functional Groups
• Nitrogen-Containing Functional Groups1. Amines
2. Amides
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Alcohols and Ethers
An alcohol contains the hydroxyl (-OH) functional group.
In an ether, an oxygen atom is bonded to two carbon atoms.
–C–O–C– .
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Aldehydes and Ketones
An aldehyde contains a carbonyl group (C=O), which is a carbon atom with a double bond to an oxygen atom.
In a ketone, the carbon of the carbonyl group is attached to two other carbon atoms.
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Carboxylic Acids and Esters
Carboxylic acids contain the carboxyl group, which is a carbonyl group attached to a hydroxyl group.
O ║
— C—OH
An ester contains the carboxyl group between carbon atoms.
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Amines and Amides
In amines, the functional group is a nitrogen atom.
|
—N —
In amides, the hydroxyl group of a carboxylic acid is replaced by a nitrogen group.
Copyright © 2005 by Pearson Education, Inc.Publishing as Benjamin Cummings
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Functional Groups
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Functional Groups Cont.
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Learning Check
Classify each of the following as: alcohol, ether, aldehyde, ketone, carboxylic acid, ester, amine or amide.
1) CH3─CH2─CH2─OH
2) CH3─O─CH2─CH3
3) CH3─CH2─NH2
O O ║ ║
4) CH3─C─OH 5) CH3─C─O─CH3
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Solution
1) CH3─CH2─CH2─OH alcohol
2) CH3─O─CH2─CH3 ether
3) CH3─CH2─NH2 amine
O O ║ ║ 4) CH3─C─OH 5) CH3─C─O─CH3 carboxylic acid ester
Polymerization of Teflon
Teflon frying pan
Credit: Royalty Free/Alamy
ProblematicOrganic Halides Are No Longer Widely
Used
Examples of Polyhydroxy Alcohols
Examples of Phenols
Examples of Aldehydes
Acetone (A Ketone) is producedduring normal metabolism of fats
A common household Product: nail polish remover.
Acetone can be producedduringmetabolismof fats, particularly in casesof starvation or serious diabetes.
Examples of Carboxylic Acids
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• Isomers a. Isomers have the same chemical formula but
different arrangements of atoms.
b. One type of isomers is a pair of enantiomers, molecules that are “handed”.
c. Enantiomers often have different biological activities.
Ex. Ethanol (C2H5O) vs. dimethyl ether or Octane (C8H18) vs isooctane
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Enantiomers
Enantiomers are like a pairof gloves: similar shapes thathave “handedness” and areNonsuperimposable
R vs S enantiomers
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Key Words
• Organic chemistry• Hydrophobic• Parent compound• Derivative/analogue• Hydrocarbons• Alkanes• Alkenes• Alkynes
• Aromatic• Saturated• Cycloalkanes• Unsaturated• Cis isomer• Trans isomer• Polymer• Monomer