1. Organic Chemistry and Biochemistry
The study of carbon-containing compounds and their properties.
The vast majority of organic compounds contain chains of rings of carbon atoms.
The study of the chemistry of living things.
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Hydrocarbons
. . . compounds composed of carbon and hydrogen.
Saturated: carbon-carbon bonds are all single - alkanes [CnH2n+2]
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3. Hydrocarbons (continued)
Unsaturated: contains carbon-carbon multiple bonds.
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4. Rules for Naming Alkanes
1. For alkanes beyond butane, add -ane to the Greek root for the number of carbons.
C-C-C-C-C-C = hexane
2. Alkyl substituents: drop the -ane and add -yl.
-C2H5 is ethyl
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5. Rules for Naming Alkanes
3. Positions of substituent groups are specified by numbering the longest chain sequentially. C 
C-C-C-C-C-C
3-methylhexane
4. Location and name are followed by root alkane name. Substituents in alphabetical order and use di-, tri-, etc.
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6. Substitution Reactions
Primarily where halogen atoms replace hydrogen atoms.
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Cyclic Alkanes
Carbon atoms can form rings containing only carbon-carbon single bonds.
C3H6, C4H8, C6H12
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Alkenes and Alkynes
Alkenes: hydrocarbons that contain a carbon-carbon double bond. [CnH2n]
CC=C propene
Alkynes: hydrocarbons containing a carbon- carbon triple bond.
CCCCC pentyne
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9. Nomenclature for Alkenes
1. Root hydrocarbon name ends in -ene
C2H4 is ethene
2. With more than 3 carbons, double bond is indicated by the lowest numbered carbon atom in the bond.
C=CCC is 1-butene
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Addition Reactions
. . . in which (weaker)  bonds are broken and new (stronger)  bonds are formed to atoms being added.
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11. Aromatic Hydrocarbons
A special class of cyclic unsaturated hydrocarbons.
+ Cl2
+ HCl
benzene
Chlorobenzene
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12. The Common Functional Groups
Class General Formula
Halohydrocarbons RX
Alcohols ROH
Ethers ROR
Aldehydes
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13. The Common Functional Groups
Class General Formula
Ketones
Carboxylic Acids
Esters
Amines RNH2
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Polymers
. . . are large, usually chainlike molecules that are built from small molecules called monomers.
Monomer Polymer
Ethylene Polyethylene
Vinyl chloride Polyvinyl chloride
Tetrafluoroethylene Teflon
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15. Types of Polymerization
Addition Polymerization: monomers “add together” to form the polymer, with no other products. (Teflon)
Condensation Polymerization: A small molecule, such as water, is formed for each extension of the polymer chain. (Nylon)
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Proteins
Natural polymers made up of -amino acids (molecular weight from  6000 to >1,000,000 g/mol).
Fibrous Proteins: provide structural integrity and strength to muscle, hair and cartilage.
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Proteins (continued)
Globular Proteins:
roughly spherical shape
transport and store oxygen and nutrients
act as catalysts
fight invasion by foreign objects
participate in the body’s regulatory system
transport electrons in metabolism
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-Amino Acids
NH2 always attached to the -carbon (the carbon attached to COOH)
C = -carbon
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19. Bonding in -Amino Acids
+ H2O

A peptide linkage
There are 20 amino acids commonly found in proteins.
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Levels of Structure
Primary: Sequence of amino acids in the protein chain.
Secondary: The arrangement of the protein chain in the long molecule (hydrogen bonding determines this).
Tertiary: The overall shape of the protein (determined by hydrogen-bonding, dipole-dipole interactions, ionic bonds, covalent bonds and London forces).
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Carbohydrates
Food source for most organisms and structural material for plants.
Empirical formula = CH2O
Monosaccharides (simple sugars)
pentoses - ribose, arabinose
hexoses - fructose, glucose
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22. Carbohydrates (continued)
Disaccharides (formed from 2 monosaccharides joined by a glycoside linkage)
sucrose (glucose + fructose)
Polysaccharides (many monosaccharide units)
starch, cellulose
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Nucleic Acids
DNA (deoxyribonucleic acids): stores and transmits genetic information, responsible (with RNA) for protein synthesis. (Molar mass = several billion)
RNA (ribonucleic acid): helps in protein synthesis. (Molecular weight = 20,000 to 40,000)
messenger RNA
transfer RNA
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