1. Organic Chemistry
Dr. Walker

2. What is Organic Chemistry?
Organic chemistry is the study of carbon compounds.
Organic compounds have carbon AND hydrogen
Carbon Dioxide is NOT organic
The versatility and stability of carbon’s molecular structures provides the enormous range of properties of its compounds.
Carbon can bond to other carbons
Reason for the degree of structural complexity

3. Ridiculous Complexity
Palytoxin – made by species
of some species of seaweed
and coral
Synthesized by Kishi, et. al.
at Harvard in 1994

4. Organic Chemistry Carbon Has 4 valence electrons
Makes 4 covalent bonds to fill its octet
Can include double and triple bonds
Hydrocarbon
Compound with only carbon and hydrogen

5. Organic Chemistry in Everyday Life
Smells & tastes: fruits, fish, mint
Medications: aspirin, Tylenol, decongestants, sedatives, insulin
Addictive substances: caffeine, nicotine, alcohol, narcotics
Hormones/Neurotransmitters: adrenaline, dopamine, serotonin
Food: carbohydrates, protein, fat, vitamins
Genetics: DNA, RNA
Consumer products: plastics, nylon, rayon, polyester

6. Organic Materials Addition to previous notes
Before, it was stated that covalent compounds were mostly liquid/gas at room temp
This is primarily for binary compounds (2 elements)
More complicated structures can be solid at room temp

7. General Formulas Alkanes Alkenes Alkynes
Contains only single bonds
Cx H2x+2
Alkenes
Contains at least one double bond
Alkynes
Contains at least one triple bond
Alkenes and Alkynes are more reactive than alkanes

8. Saturation
Saturated: a carbon chain contains as many hydrogens as possible.
Saturated compounds contain only single C-H bonds. Alkanes are saturated.
Unsaturated means that a carbon chain contains at least one multiple (double or triple) bond.
Alkene = double bond
Alkyne = triple bond

9. Hydrocarbons IUPAC name Molecular Formula Structural Formula
Boiling Point (°C)
Methane
CH4
-161.5
Ethane
C2H6
CH3CH3
-88.6
Propane
C3H8
CH3CH2CH3
-42.1
Butane
C4H10
CH3(CH2)2CH3
-0.5
Pentane
C5H12
CH3(CH2)3CH3
36.1
Hexane
C6H14
CH3(CH2)4CH3
68.7
Heptane
C7H16
CH3(CH2)5CH3
98.4
Octane
C8H18
CH3(CH2)6CH3
125.7
Nonane
C9H20
CH3(CH2)7CH3
150.8
Decane
C10H22
CH3(CH2)8CH3
174.1 .

10. Structure and Physical Properties
Methane
16 g/mol
-161.5oC
Ethane
30 g/mol
-88.6oC
Propane
44 g/mol
-42.1oC
Butane
58 g/mol
-0.5oC
Larger molar mass = higher boiling point
Bigger compound – higher boiling point

11. Petrochemicals Simple, small hydrocarbons are petrochemicals
Chemicals isolated from crude oil (petroleum)
Octane – used in gasoline
Propane – used in grills, heaters, etc.
Butane – lighter fluid

12. Functional Groups
Functional Group – group of atoms which control how the molecule reacts

13. Polymers
Polymers
Large molecules with many, many repeating units, made from smaller molecules
Polyethylene

14. Polymers Nylon, Kevlar, and PVC are other examples of manmade polymers
PVC (polyvinyl chloride)

15. Natural Polymers
Proteins
RNA

16. Natural Polymers
Polysaccharides
DNA

17. Pharmaceuticals Most pharmaceuticals are complex, organic molecules
Can be natural or manmade
Acetaminophen
(aka Tylenol)
aspirin
penicillin

18. Terms To Know Hydrocarbon Alkane Alkene Alkyne Saturated Unsaturated
Petrochemicals
Functional Group
Polymers

19. Skills To Master Differentiating alkanes, alkenes, and alkynes
Differentiating saturated and unsaturated compounds
Differentiating natural polymers and manmade polymers
Recognizing common pharmaceuticals