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Lecture 8.1 – Organic Chemistry and Alkanes

Lecture 8.1 – Organic Chemistry and Alkanes. I. Organic Chemistry and Carbon. Organic Chemistry is the branch of chemistry that studies carbon. Carbon can form long chains and rings by bonding to itself. I. Hydrocarbons. A molecule of only hydrogen and carbon is called a hydrocarbon .

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Lecture 8.1 – Organic Chemistry and Alkanes

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  1. Lecture 8.1 – Organic Chemistry and Alkanes

  2. I. Organic Chemistry and Carbon • Organic Chemistryis the branch of chemistry that studies carbon. • Carbon can form long chains and rings by bonding to itself

  3. I. Hydrocarbons • A molecule of only hydrogen and carbon is called a hydrocarbon. • Hydrocarbons can be classified as alkanes, alkenes, or alkynes • Alkanesare completely saturated hydrocarbons

  4. II. Properties of Alkanes • Alkanes release a large amount of energy when burned • Alkanes are not soluble in water • The heavier an alkane is, the higher its boiling point (only intermolecular force = London Dispersion Forces)

  5. Lecture 8.2 – Alkenes and Alkynes

  6. I. Alkenes • Alkenes are unsaturated hydrocarbons that contain at least 1 double C – C bond.

  7. II. Alkynes • Alkenes are unsaturated hydrocarbons that contain at least 1 triple C – C bond.

  8. III. Naming Alkenes and Alkynes • When naming alkenes and alkynes, you need to state the location of the double/triple bond by stating the carbon it is located on • E.g. 1 – propene, 2-octyne, etc.

  9. Lecture 8.3 – Naming Hydrocarbons

  10. I. Naming Hydrocarbons • Circle the LONGEST carbon chain • Number all of the carbons in the longest chain • Circle all side chains • Name the side chains by writing the carbon number it is attached to and the name of the chain. NOTE – Add di, tri, etc. when you have the same side chain multiple times

  11. II. Isomers • Isomersare compounds that have the same molecular formula, but different structural formulas • This different structure leads to different physical and chemical properties.

  12. III. Practice • Draw 3 isomers of pentane.

  13. IV. Practice • Draw 4 isomers of octane.

  14. Lecture 8.4 –Functional Groups

  15. I. Functional Groups • Functional groups are specific groups of atoms or bonds that alter the physical and chemical properties of the hydrocarbon.

  16. II. Halides (Halocarbon) • Halocarbonsare when a simple halogen from group 17 replaces a hydrogen atom in an alkane. • Tend to be used as solvents and pesticides

  17. III. Halocarbon Properties • Nonflammable and low reactivity • Boiling points are higher than alkanes because of larger molecular weight and increased strength of London Dispersion Forces • Haloalkanes are better solvents due to increased polarity

  18. Lecture 8.6 – Types of Organic Reactions

  19. I. Combustion Reactions • When a hydrocarbon reacts with oxygen, carbon dioxide and water are produced. • Ex. CH4 + O2 CO2 + H2O

  20. II. Addition Reactions • Addition reactions involve adding one or more atoms to an unsaturated hydrocarbon. • A double covalent bond is converted into a single covalent bond and a triple covalent bond is converted into a double covalent bond.

  21. III. Substitution Reactions • In a substitution reaction, one type of atom is replaced with a different atom or group of atoms. • Substitution reactions only happen to saturated hydrocarbons.

  22. IV. Polymerization • A polymeris a large molecule composed of many repeating units called monomers.

  23. Lecture 8.7 – Types of Organic Reactions

  24. I. Esterification • Anesterificationreaction is: ORGANIC ACID + ALCOHOL ESTER + WATER • This process produces many common smells in foods (especially fruits) and perfumes.

  25. II. Saponification • The general formula for asaponification reaction is: • ESTER + INORGANIC BASE  ALCOHOL + SOAP • REMEMBER THIS REACTION MAKES SOAP!

  26. III. Fermentation • In a fermentationreaction, the general reaction occurs: Sugar  Alcohol + Carbon Dioxide • Sugars have the empirical formula of CH2O

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