I. Carbon and Molecular Diversity

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

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

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

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

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

What type of isomer?

What type of isomer?

What type of isomer?

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

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

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

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

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

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

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

Functional Groups