Presentation is loading. Please wait.

Presentation is loading. Please wait.

Organic “Carbon” Chemistry Chapter 13-14 Science 10 CT03D01 Resource: Brown, Ford, Ryan, IB Chem.

Similar presentations

Presentation on theme: "Organic “Carbon” Chemistry Chapter 13-14 Science 10 CT03D01 Resource: Brown, Ford, Ryan, IB Chem."— Presentation transcript:

1 Organic “Carbon” Chemistry Chapter Science 10 CT03D01 Resource: Brown, Ford, Ryan, IB Chem

2 Organic “Carbon” Chemistry Chemistry for you, Lawrie Ryan Chapter 13 Pages Hydrocarbons, Fossil Fuels, Distillation of Crude Oil, Cracking, Plastics, Polymers Chapter 14 Pages Alcohols, Isomers, Ethanol, Alcohol Reactions, Carboxylic Acids

3 Hydrocarbons A hydrocarbon is a compound containing only hydrogen and carbon Crude Oil, which is very important to the survival Venezuela is a mixture of many hydrocarbons Not only vital for fuels but also the starting materials for plastics and other polymers

4 Alkanes The most common hydrocarbon found in crude oil is an alkane An alkane contains a ‘backbone’ of single-bonded carbon atoms and is saturated with hydrogen atoms Natural gas, methane, CH 4, is the shortest alkane Alkane Methane, CH 4 Ethane, C 2 H 6 Propane, C 3 H 8 Butane, C 4 H 10 Pentane, C 5 H 12 Hexane, C 6 H 14 Heptane, ______ Octane, _______

5 13.2 – Fossil Fuels Most common fuels are fossil fuels Coal, crude oil, natural gas, etc Coal, although it’s not a hydrocarbon, does contain carbon and hydrogen, as well as oxygen in some of it’s molecules From organic material (like trees) that died and were buried below swamps Crude oil, hydrocarbons Formed from tiny animals and plants which lived in the sea Takes millions of years to form fossil fuels  In reality the energy comes from the sun to produce fossil fuels, but it simply takes so long to produce

6 13.2 – Finding Oil Crude oil today was made from mainly plankton that died about 150 million years ago. Their bodies did not decay normally due to lack of oxygen and with high pressures and temperatures, formed oil and natural gas. We can find oil by surveying the land and it’s topography Look for dome shaped layers (cap rock or anti-cline) Seismic survey

7 13.3 – Distilling Crude Oil When crude oil reaches the refinery it’s a thick, black, and smelly liquid This liquid contains long hydrocarbon chains At the refinery the long chains can be sorted out into groups of useful substances called fractions We can separate these substances by fractional distillation which separates substances based on their boiling point FractionLengthColorThicknessReactivity Low BP (up to 80C) ShortClearRunnyEasily lit (flammable, clean flame) Medium BP ( C) MediumYellowThickerHarder to light, some smoke High BP (above 150C) LongDark orangeThickDifficult to light, smoky flame

8 13.4 – Fractional Distillation in Industry FractionLength of Carbon Chain Petroleum gasC 1 -C 4 PetrolC 4 -C 12 KerosineC 11 -C 15 DieselC 15 -C 19 Lubricating OilC 20 -C 30 Fuel OilC 30 -C 40 BitumenC 50 +

9 Cracking After distillation of crude oil companies are still left with long hydrocarbons and the need is for shorter chains like petrol The solution is cracking meaning big molecules are broken down by heating them over a catalyst This is competed inside a cracker

10 Plastics When oil companies crack large molecules into smaller ones, ethene is made Ethene is just like ethane, but with a double bond making it unsaturated This ethene molecule is the starting material for plastics. When the double bond is broken, new bonds can form between several molecules forming polymers  Lots of small, reactive molecules called monomers join together to make a polymer vs ethene

11 13.7 – Ethene and the Alkenes Alkenes, which are also hydrocarbons, are very similar to alkanes, but are not saturated. They have at least one double bond and less hydrogen atoms which makes them unsaturated. Their names end in –ene instead of –ane Contain double bonds Very reactive Building block for polymers Also react with  Br, Cl, I, F water  Strong acids  Water and sulfuric adid AlkaneAlkene Methane, CH 4 Ethane, C 2 H 6 Ethene, C 2 H 4 Propane, C 3 H 8 Propene, C 3 H 6 Butane, C 4 H 10 Butene, C 4 H 8 Pentane, C 5 H 12 Pentene, C 5 H 10 Hexane, C 6 H 14 Hexene, C 6 H 12 Heptane, ______Heptene, ______ Octane, _______Octene, _______

12 Polymerization There are two types of reactions that make polymers Addition – where at least two things simply join together Condensation – where water is given off in the process of joining molecules. Also known as dehydration synthesis

13 13.8 – Addition Polymerization Addition Reactions Monomers have at least one double bond The polymer is the only material formed in the reaction Easiest example is ethene used to make poly(ethene)  n C 2 H 4  -[-C 2 H 4 -]- n  Where n = large number The double bonds open up to form single bonds to the adjacent monomer R can be just about anything

14 13.9 – Condensation Polymerization Nylon is an example of a polymer formed through condensation Fumes are given off as the different monomers react together. These small molecules given off could be H 2 O, HCl, etc. It depends on the ends of the monomers. The monomers have reactive parts at both ends and join end-to-end to make long chain polymers + H 2 O

15 13.10 – Properties of Plastics Many materials are made out of plastics PVC piping, bags, surfaces, protective films, bottles, etc Plastics often have advantages over the use of metal compounds and cost much less When we run out of oil we will also run out of access to cheap plastics This is why recycling our plastics is so important!!

16 Chapter 14 – Organic Molecules Nomenclature! How do we name organic compounds?  Alkane vs alkene  Saturated vs unsaturated  Functional groups  Length of chain

17 Types of Organic Molecules SaturatedUnsaturated Compounds which contain only single bonds For example: alkanes Compounds which contain double or triple bonds For example: alkenes, arenes AliphaticsArenes Compounds which do not contain a benzene ring; may be saturated or unsaturated For example: alkanes, alkenes Compounds which contain a benzene ring; they are all unsaturated compounds For example: benzene, phenol 14.1 – Types of Organics

18 Differ by a CH 2 Can be represented by the same general formula Show gradation in physical properties Have similar chemical properties Members of Homologous Series

19 Members of Homologous Series… … differ by a –CH 2 group

20 Members of Homologous Series… … can be represented by the same general formula FormulaName CH 4 OHMethan-1-ol C 2 H 5 OHEthan-1-ol C 3 H 7 OHPropan-1-ol C 4 H 9 OHButan-1-ol C 5 H 11 OHPentan-1-ol C 6 H 13 OHHexan-1-ol C 7 H 15 OHHeptan-1-ol C 8 H 17 OHOctan-1-ol

21 Members of Homologous Series… … show gradation in physical properties AlkaneBoiling Point Methane, CH Ethane, C 2 H Propane, C 3 H Butane, C 4 H Pentane, C 5 H Hexane, C 6 H Heptane, C 7 H Octane, C 8 H Since the series differ by one –CH 2 they have successively longer carbon chains Results in gradual trend of phy. Props Not always a linear growth Density and viscosity are other examples

22 Members of Homologous Series… … show similar chemical properties As the have the same functional group Ex.1 – the alcohols have a functional –OH group, which can be oxidized to form organic acids Ex. 2 – the –COOH functional group, present in the homologous series of the carboxylic acids, is responsible for the acidic properties of these compounds

23 14.3 – Organic Formulas Emperical formula Simplest whole number ratio Ethane CH 3 Molecular formula Actual number of atoms Ethane C 2 H 6 Structural Formula Full, condensed, steriochemical

24 Emperical Formula The simplest whole number ratio of the atoms it contains. For example, the emperical formula of ethane, C 2 H 6, is CH 3. This formula can be derived from percentage composition data obtained from combustion analysis. It is, however, of rather limited use on it’s own, as it does not tell us the actual number of atoms in the molecule.

25 Molecular Formula Actual number of atoms of each element present. For example, the molecular formula of ethane is C 2 H 6. It is therefore a multiple of the emperical formula, and so can be deduced if we know both the emperical formula and the relative molecular mass M r.

26 Full Structural Formula Graphic formula or displayed formula – shows every bonded atom. Usually 90 o and 180 o angles are used to show the bonds because this is the clearest 2-D representation, although it is not the true geometry of the molecule

27 Condensed Structural Formula Often omits bonds where they can be assumed, and groups atoms together. It contains the minimum information needed to describe the molecule non- ambiguously – in other words there is only one possible structure that could be described by its formula.

28 14.4 – IUPAC Nomenclature Nomenclature for Organic Compounds: the IUPAC system International Union of Pure and Applied Chemistry Rule 1: Identify the longest straight chain of carbons Rule 2: Identify the functional group Rule 3: Identify the side chains or substituent groups

29 IUPAC Rule 1: Longest Chain Note: ‘straight chain’ does not mean just 180 o angles or unbranched chains of carbon atoms. Be careful, do not be confused by the way the molecule may appear on paper because of free rotation around the carbon-carbon single bonds. Example, all three below are the same….

30 IUPAC Rule 2: Functional Group The functional group is described by a specific ending (or suffix) to the name, that replaces the –ane ending of the name of the parent alkane. The suffixes used for some common functional groups are in the slides to follow. Those marked * will have slides with further information.

31 Functional Groups

32 IUPAC Rule 3: Side Chains

33 Structural Isomers Different arrangements of the same atoms make different molecules Molecular formula shows the atoms that are present in a molecule, but gives no information on how they are arranged. Consider, for example, C 4 H 10 Each isomer is a distinct compound, having unique physical and chemical properties.

34 Structural Isomers of Alkenes

35 Alkanes as Fuels Release significant amounts of energy when they burn, highly exothermic, because large amount of energy released when forming.. Double bonds of CO 2 Bonds in H 2 O C 3 H 8 + 5O 2  3CO 2 + 4H 2 O ΔH = kJ/mol However, when O 2 is limited….. 2C 3 H 8 + 7O 2  6CO + 8H 2 O when O 2 is extremely limited….. C 3 H 8 + 2O 2  3C + 4H 2 O These are examples of the incomplete combustion of fossil fuels which makes them an environmental concern

Download ppt "Organic “Carbon” Chemistry Chapter 13-14 Science 10 CT03D01 Resource: Brown, Ford, Ryan, IB Chem."

Similar presentations

Ads by Google