Organic Chemistry Basics
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Transcript Organic Chemistry Basics
Organic
Chemistry
Basics
Chapter 3
Organic compounds
Carbon
covalently bonded to each other
and other atoms
Originally thought only found in living
things
Wide diversity in compounds: more than 5
million have been identified
Macromolecules: cells make large
molecules from smaller ones
Properties of Carbon
4
valence electrons = 4 covalent bonds
Can form bonds with itself
Carbon to carbon bonds are strong but
not unbreakable, making them good for
structural components
Carbon can also form double and triple
bonds with itself
Carbon can form straight or branched
chains as well as rings
Isomers
Compounds
with the same molecular
formula but different structures
Do not have identical physical or
chemical properties
Three types:
Structural – different covalent arrangement
Geometric – different spatial arrangement
Enantiomers – mirror images of each other
Structural isomers
Geometric isomers
Enantiomers
Hydrocarbons
Carbon
+ hydrogen
Nonpolar
Tend to be hydrophobic
Hydrogen atoms can be replaced with a
functional group
Polar and ionic functional groups are
hydrophilic
Functional groups
Hydroxyl
Alcohols
Carbonyl
bond
group: R-OH
ethanol
group: carbon to oxygen double
Aldehyde:
R-CHO (at end of C skeleton)
Ketone:
R-CO-R (internal carbonyl group)
Functional groups…
Carboxyl
group: R-COOH
Amino group: R-NH2
Both essential in amino acids
Phosphate
Part of DNA backbone
Sulfhydryl
group: R-PO4H2
group: R-SH
Thiols – important in proteins
Polymers
Formed by linking small organic molecules
together
Hydrolysis reactions (‘break with water’)
Breaks apart a polymer
Condensation reactions (‘remove water’)
Example: 20 different amino acids form
thousands of different proteins
Joins monomers into a polymer
In biological systems these are regulated by
different enzymes.