Organic Chemistry Dr. Walker

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

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

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

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

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

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

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

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 .

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

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

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

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

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

Natural Polymers Proteins RNA

Natural Polymers Polysaccharides DNA

Pharmaceuticals Most pharmaceuticals are complex, organic molecules Can be natural or synthetic (manmade) Aspirin (willow bark) Penicillin (mold) Acetaminophen (aka Tylenol) (synthetic)

Pharmaceuticals Most pharmaceuticals are complex, organic molecules Can be natural or synthetic (manmade) Vitamin D3 (made in the body) Insulin (made in the pancreas) Vitamin C (citrus fruits)

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

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