1. Chapter 8 Compounds of Carbon

2. Why is Carbon important?  T hey make up over 90% of all chemical compounds, is the backbone of all living things.  Make element in “organic substances”.  Proteins, carbohydrates and fats all contain carbon.

3. Natural Gas-formed by the natural degradation of organic matter. Found with deposits of petroleum. Hydrocarbons Compounds of Carbon and Hydrogen.  Methane (CH 4 ) is the simplest hydrocarbon and belongs to the alkane group.  Alkanes end with suffix –ane.  Carbon-Carbon single bonds. Other alkanes  General formula: C n H 2n+2  n= number of carbon atoms  As the number of C atoms increases the structure has an additional –CH 2 group. This is known as homologous series.

5. Structural formulas and condensed formulas Condensed formula of alkanes E.g. Butane C 4 H 10 Structural formulas Shows how the elements are arranged relative to one another (straight chain representation). E.g. Butane

6. Branched chain- when alkyl groups branched off the main parent chain. Alkyl groups – C n H 2n+1 Alkyl groups end with suffix -yl NameFormula Methyl-CH 3 Ethyl-CH 2 CH 3 Propyl-CH 2 CH 2 CH 3 Butyl-CH 2 CH 2 CH 2 CH 3 Pentyl-CH 2 CH 2 CH 2 CH 2 CH 3

7. Isomers- have the same molecular formula but different structural formula The general formula of a 4 carbon alkane is C 4 H 10 C 4 H 10 has 2 isomers : Butane and 2-methyl propane Note: the importance of numbering carbons in branched chains.

8. Alkanes summary 1. End with suffix –ane. 2. Single bonds between C-C atoms, hence saturated hydrocarbons. 3. As the number of carbon atoms increase the hydrocarbons change from gases to liquids to solids.

9. Alkenes- have a double bond between C=C (note there’s one double bond only, the rest are single bonds)  End with suffix –ene.  General formula: C n H 2n Ethene to Decene FormulaName C2H4C2H4 Ethene C3H6C3H6 Propene C4H8C4H8 Butene C 5 H 10 Pentene

10. Alkenes are considered unsaturated hydrocarbons due to the presence of a double bond. Under the right conditions alkenes can react with hydrogen to form alkanes.

11. Alkynes- have a triple bond between carbon-carbon bonds (one triple bond only) so are unsaturated  Alkynes have a General formula: C n H 2n-2

12. Important- the double or triple bond should be on the 1 st carbon

13. Rules for naming branched hydrocarbons Identify the parent chain (the longest continuous carbon chain) Identify the branch or substituent (usually an alkyl group) Number the carbon atoms in such a way (from the end that gives the branched group the lowest number possible). Refer to pages 142-143 of your Chemistry textbook. I will do a few examples on the board before you start the worksheets!!!

14. Quick quiz!!!  Which hydrocarbon has a double bond?  What does saturation mean?  What is the general formula of an alkyne?  What are isomers?  What is a parent chain?  Are alkenes saturated or unsaturated?  What happens to the states of alkanes as the number of carbon atoms increase?  What number is assigned to the carbon that has a side or branched chain?

15. Answers Alkenes Single bond between carbon atoms C n H 2n-2 Same general formula but different structural formula Longest straight carbon chain Unsaturated due to double bond between Carbon to Carbon Changes from gases to liquids and then to solids Lowest number possible

16. Properties of alkanes and alkenes Physical properties (both similar for alkanes and alkenes)  Smaller molecules are more volatile than larger ones (less energy is needed to overcome forces between molecules).  Smaller molecules are less viscous (thickness of fluid) so flow more freely.  Petrol is less viscous than oil and more volatile so burns more readily.  Boiling temperature increases as the number of carbon atoms increase (However, alkenes are slightly lower than alkanes)

17. Forces between Hydrocarbon molecules Non-polar because of the similar electronegativities between C and H. Dispersion forces exist- this force increases as size of molecule increases. More energy is required to overcome the intermolecular dispersion forces of larger molecules hence higher boiling temperatures Also stronger intermolecular dispersion forces between larger molecules means it is harder for the liquid to evaporate (less volatile) Larger molecules are more viscous due to longer chain hydrocarbons becoming “tangled together”.

18. Chemical properties of alkanes 1. Combustion Alkanes burn in oxygen to form carbon dioxide and water. Methane + Oxygen → Carbon dioxide + Water Balanced chemical equation (You should be able to balance equations using coefficients) CH 4 + 2O 2 → CO 2 + 2H 2 O

19. Chemical Properties of alkenes Like alkanes, alkenes also burn in oxygen to produce carbon dioxide, water + heat. The presence of a double bond allows alkenes to react more readily with others. 1. Addition Reactions with Bromine The double bond breaks forming: Red brown colour of bromine d disappears as it reacts with ethene. This is the test for unsaturation.

20. Reactions with Bromine 2. Reactions with Hydrogen In the presence of a catalyst (Platinum-Pt) ethene reacts with hydrogen to form ethane. This is an addition reaction where the double bond breaks to allow hydrogen to bond with carbon.

21. 3. Reaction with steam Ethanol is now being made by adding steam (H 2 O) to ethene. Phosphoric acid is used as a catalyst. This is also an addition reaction with steam. Ethene + Steam → Ethanol

22. 4. Formation of polyethylene Another name used for ethene is ethylene. Polyethylene or polyethene means “many ethylene” or “many ethene”. Polyethylene is a polymer that is a large molecule made by many small units of ethene (monomer). This type of reaction is also called an addition polymerisation reaction. n in this reaction is very large (10,000 or more)