1. I. Carbon and Molecular Diversity

2. A. Foundations of Organic Chemistry
Organic chemistry- specialized in the study of carbon compounds
Organic chemistry had its origins in vitalism, a theory that only living things could produce organic compounds because their synthesis require “Life force” outside physical and chemical law
Scientists were later able to synthesize organic compounds and belief shifted to mechanism, a theory that hold that all natural phenomena are governed by physical and chemical law

3. B. The Versatility of Carbon in Molecular Architecture
Carbon is tetravalent. That is, carbon can make up to 4 covalent bonds which allows carbon to make large complex molecules
Examples:
Carbon dioxide
Urea

4. C. Variations in the Carbon Skeleton
Chains may vary in length
Chains may be branched or unbranched
Carbon chains may contain double bonds
Carbon chains may form rings
Fossil fuels are mainly hydrocarbons which are chains of hydrogen and carbon

6. Double and triple bonds can occur in carbon chains. Rings can also form.

7. 6. Isomers- compounds with the same molecular formula, but different structural formulas
Structural Isomers- differ in the covalent arrangement of their atoms. Butane and isobutane.
Geometric Isomers- have same covalent partnerships but different spatial arrangements
Stereoisomers- contain variations around an asymmetrical carbon- a carbon that is attached to 4 different atoms. This results in molecules that are mirror images

8. What type of isomer?

9. What type of isomer?

10. What type of isomer?

11. Found in alcohols. Polar covalent bond. Dissolves in water
D. Functional Groups- specific groups of atoms that covalently bond to carbon skeletons and give the overall molecule distinctive properties
1. Hydroxyl -OH
Found in alcohols. Polar covalent bond. Dissolves in water

12. 2. Carbonyl –C=O
a) If found at the end of a carbon skeleton it is called an aldehyde
b) If it is found in the middle of the carbon skeleton it is called a ketone
Polar, soluble in water

13. 3. Carboxyl -COOH Found in carboxylic and organic acids.
Hydrogen dissociates to form a weak acid
Polar (negatively charged) and soluble in water

14. 4. Amino –NH2 Found in amino acids- the building blocks of protein.
Can accept H+ ions, thereby acting as a weak base
Polar (positively charged) and soluble in water

15. 5. Sulfhydryl -SH Aids in the stabilization of proteins
Polar and water soluble

16. 6. Phosphate –PO4 Bonds to carbon group by oxygen bridge
Found in nucleic acids, dinucleotides and energy transfer molecules like ATP
Releases hydrogen ions in solution. Acidic
Polar (negatively charged) and soluble in water

17. Methyl -CH3
Least reactive. Non-polar, insoluble in water

18. Functional Groups