1. Organic Chemistry …oh what fun…

2. Organic Chemistry  What does it mean to be organic?  To be an organic compound means that you contain carbon … that’s it… if you contain carbon, you are organic  There are a few exceptions, but you don’t have to worry about those Carbon atoms comprise about 20% (by mass) of all animals Fossil Fuels Common products like plastic, adhesives, soaps, etc

3. Organic Compounds  Why so many carbon compounds? Carbon is tetravalent  Four bonding electrons – this means carbon can form long chains and rings with other carbon atoms Carbon atoms form single, double, and triple covalent bonds The same atom can join together to produce isomers (molecules with the same formula, but different structures)

4. Homologous Series  Homologous Series: General formula can be written to represent all member of a series Each successive member of the series differs by a common structural unit The chemistry of any one member is similar to that of the other members  Similar preparation and similar chemical properties

5. Formulae  Molecular Formula Tells the number of atoms in a molecule, but not the arrange of the molecules (H 2 O)  Structural Formula Shows the arrangement of atoms in a molecule Can show all atoms and bonds  Condensed Structural Formula Shows all bonds expect bonds to hydrogen, or only shows the bonds to the substituents  CH 3 -CH 2 -CH 2 -OH

6. Simplest Organic Compounds  Simplest organic compounds are hydrocarbons Meaning that they only contain carbon and hydrogen

7. Hydrocarbons  Alkanes – only single bonds b/w carbons General Formula: C n H 2n+2  Alkenes – at least 1 double bond b/w carbons General Formula: C n H 2n  Alkynes – at least 1 triple bond b/w carbons General Formula: C n H 2n-2

8. Functional Groups  An atom or group of atoms that always react a certain way  Adding a functional group to a hydrocarbon will always change the physical and chemical properties of that hydrocarbon And a functional group will always change these properties the same way

9. Functional Groups  Halide (Haloalkane)  Alcohol  Ether  Aldehyde  Ketone  Organic acid  Ester  Amine  Amide Carbonyl Group: carbon with a double-bonded oxygen

10. Halide (Haloalkane)  Compound containing a halogen (or group 17 of the periodic table) bonded to the compound  General Formula: R- X  R= compound, X = halogen  Example: CH 3 CHClCH 3 2-chloropropane

11. Amine  Contain nitrogen atoms bonded to carbon atoms  General Formula: R’’ | R- N- R’  Example: CH 3 CH 2 CH 2 NH 2 1-propanamine

12. Alcohol  Compound where a hydroxyl group (-OH) replaces one of the hydrogens on a carbon  General Formula: R- OH  Example: CH 3 CH 2 CH 2 OH 1-propanol

13. Organic (Carboxylic) Acid  Compound with a carboxyl group (a carbonyl group bonded with an alcohol)  General Formula:  Example: propanoic acid

14. Physical Properties of Organic Compounds  Colour: colourless  State @ Room Temp: Hydrocarbons: gases then liquids, then solids as molar mass increases Haloalkanes, alcohols, carboxylic acids and amines: liquids then solids as molar mass increases

15. Physical Properties of Organic Compounds  Solubility in Water: Hydrocarbons and Haloalkanes insoluble (non- polar) Alcohols, carboxylic acids and amines:  Lower molar mass members are soluble in water (polar)  Higher molar masses insoluble  The more carbons, the less polar it becomes

16. Naming Hydrocarbons  There is very simple nomenclature for hydrocarbons First of all, we’ll start with naming straight chains 1. Each chain that contains only single bonds ends with –ane 2. Count the carbons and add the correct the prefix for that number of carbons.  What are the prefixes?

17. Naming Hydrocarbons Number of CarbonsPrefix 1Meth- 2Eth- 3Prop- 4But- 5Pent- 6Hex- 7Hept- 8Oct- 9Non- 10Dec-

18. Practice Naming: Butane

19. Practice Naming: Heptane

20. Practice Naming: Heptane

21. Different Diagrams  There are different ways to represent carbon chains. 1) there is the standard way where you draw in every hydrogen atom 2) You can simply draw in dashes and not label the ‘H’ s because we know what they are

22. Different Diagrams 3) The stick-figure drawing  Here we know that each carbon has 4 bonds and we can leave out the bonds for hydrogen completely  Here we count each point on this line as a carbon  So what is it?  PENTANE

23. Naming Branched Alkanes:  What do you do if it’s not a straight chain?

24. Naming Branched Hydrocarbons

25. How to Name Branched Chains 1. Find and name the longest “straight” chain (This doesn't mean that the carbons all have to be in one straight line... you just have to be able to connect them with one pen-stroke) What is the longest chain in this molecule? Hexane

26. How to Name Branched Chains 2. Locate your branches. Name these like you name regular hydrocarbons, except these will end with -yl (instead of -ane) What is the name of the branch on this molecule? Methyl … so now we have methyl-hexane

27. How to Name Branched Chains 3. Tell me where the branch is located. (a) Start counting so you have the lowest number combination possible... (b) So let's name this one again... (c) 2-methyl-hexane

28. How to Name Branched Chains 4. If there are multiple chains, the naming order is: where the chains are, how many, what they are

29. How to Name Branched Chains 5. If the branches have different names (methyl vs. ethyl for example)... arrange them alphabetically in the name