Describe two reasons for abundance of carbon compounds
Distinguish between inorganic and organic carbon and other compounds
Distinguish between isomers and non-isomers
Describe differences between optical and geometric isomerism
Distinguish between aromatic and nonaromatic
Identify common functional groups
One element – one branch of chemistry
Organic compounds based on carbon: 13 million and rising (fast)
100,000 new compounds synthesized annually
All 91 other elements combined: only 300,000 compounds
Fairly abundant in earth’s crust – but not enough to explain domination
Key element in the human organism – and all others
“God’s goof”:
The absence of stable mass 5
C and O are abundant because the atom with mass 5 is unstable
Otherwise atom building after the Big Bang would have resulted in much heavier elements
The thoughts of a cosmological atheist Fred
Hoyle:
“Some supercalculating intellect must have designed the properties of the carbon atom, otherwise the chance of my finding such an atom through the blind forces of nature would be utterly minuscule….The numbers one calculates from the facts seem to me so overwhelming as to put this conclusion almost beyond question”
Inorganic carbon: ionic compounds where carbon is incorporated as carbonate – CO
3
2-
Organic carbon: compounds of carbon with itself, hydrogen and other elements – by far the most important
Organic carbon forms a thin canopy
Unique (?) conditions on earth that support life
Earth’s surface organic
Earth’s crust inorganic
Inorganic compounds were salts of the earth
Stable and easily synthesized
Organic compounds were of living organisms
Fragile and not easily synthesized
Belief in Vitalism posited that only living organisms possessed a vital force necessary to create organic compounds
In 1828 urea was synthesized and vitalism was on the way out
Seven ages of man - many ages of a carbon atom
Combustion: C + O
2
CO
2
Neutralization by seawater: CO
Reaction with acid rain: CaCO
Photosynthesis: CO
2
3
2
+ Ca(OH)
+ H
2
SO
4
2
CaCO
3
CO
2
Organic compounds (OC)
Vegetation decomposes: OC
fossil fuels (FF)
+ H
Vegetation consumed by animal: OC
new compounds
2
O
(proteins, DNA etc.)
Respiration: sugars
CO
2
+ energy
Industrialization: FF
C, CO
2
+ energy
Manufacturing: FF
Plastics, polymers, drugs etc.
Waste disposal
Fossil fuels, CO
2
Two reasons why carbon is unique
Carbon can form four bonds – four valence electrons
Carbon forms very strong bonds with itself – chains, rings etc.
Hydrocarbons are the simplest organic compounds
Contain only C and H
Simplest is CH
4
(natural gas)
Intermediate C
8
H
18
(petroleum)
Synthetic polymers contain thousands of atoms
All bonds are single
Saturated
No new bonds can be added
General formula C n
H
2n+1
Molecular formula
Shows atoms in the molecule
Structural formula
Shows how they are all connected
Condensed structural formula
Simplified representation of connections
Meth - ane
Number of carbon atoms
Type of compound
Numbers game: count the carbon atoms in the chain
Saturation bonding:
Multiple bonds and unsaturation
Saturated: no more bonds can be added
Unsaturated: more bonds can be formed
More reactive compounds
Going bananas:
Ethylene and fruit ripening
Same number and type of atoms
Different arrangements
Hydrocarbons can have straight and branched chains
Alkane isomers
General formula C n
H
2n+1
Three isomers of pentane
C
5
H
12
Five isomers of hexane
C
6
H
14
CH
4
C
C
3
2
H
6
– 1 possibility
– 1
C
4
H
8
C
5
H
10
– 1
– 2
C
8
C
10
H
12
H
18
C
20
H
22
H
42
– 3
– 18
– 75
– 366,319
Optical isomerism is a special variation
Molecules exhibit handedness – mirror images which are not superimposable
Must have tetrahedral carbon with four different groups attached
This carbon is chiral
Each chiral carbon produces two isomers
If there are n chiral carbon atoms there are 2 n isomers
Optical isomers are important in nature
Amino acids are building blocks of proteins
Amino acids are chiral
Proteins contain hundreds – thousands of amino acids
Getting the correct isomer is a big deal
Geometric isomers:
Isomerism and a healthy diet
What’s with all this trans fats anyway?
Ask a Chicago Alderman
Different geometry - same attachments
Cis isomers:
Don’t pack together
Cis isomers have low viscosity - good
Trans isomers:
Pack together tightly
Trans isomers are solids - bad
Benzene ring contains 6 C atoms
Bonding is resonant – more stable than expected
All aromatic compounds contain at least one benzene ring
Benzene, C
6
H
6
, is one of the most important industrial chemicals
Benzene is regarded as a highly carcinogenic substance
Use and disposal of benzene are regulated
Compounds containing benzene rings are not necessarily toxic
Chemistry of organic compounds is determined by functional groups
Functional group is an atom or group of atoms that are different from C
Heteroatoms confer very different properties on the substance
Heteroatoms affect physical and chemical properties
C
2
H
6
C
2
H
6
(ethane) is a gas at RT is insoluble in water
C
2
H
6
O (ethanol) is a liquid at RT
C
2
H
6
O is soluble in water
Differences in cohesive forces: O-H bonds are polar, C-H bonds are not
Chlorocarbons and the environment
Important uses – important problems
Solvents CH
2
Cl
2
Insecticides DDT
Refrigerants CFCs
Functional group –OH
Polar molecules dissolve in H
2
O
Ethanol: good for your health/bad for your health?
Smoke gets in my eyes: olefactory pleasures of aldehydes
C=O is carbonyl group
Aldehyde contains RCHO
Formaldehyde is a preservative and a product of burning wood
Acrolein is a product of barbequing
Common smells and flavours
Ketone is R
1
R
2
CO
Acetone is a common solvent
Smell found in cinnamon
Raspberries
Commonly found in citrus fruits and any sour foods
Formic acid present in ant and bee stings
Esters: sweet aromas and flavours
Ester group is R
1
COOR
2
Sweet aroma in pineapples, jasmine
Synthetic versions are very common
Ethers contain R
1
-O-R
2
No -OH bonds
Not soluble in water
Anesthetics
Amines contain NR
1
R
2
R
3
Rotting fish
Decaying flesh
Illicit drugs