7.1 tetrahedral carbon alcohols 7.1
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This document summarizes key information about alcohols including their classification, physical properties, and uses. It lists common alcohols like methanol, ethanol, propan-1-ol, and butan-1-ol. It describes that primary alcohols have one carbon attached to the hydroxyl group, while secondary alcohols have two. The document also discusses how alcohols have higher boiling points than alkanes due to polarity. It provides examples of how solubility changes with alcohol size and explains their comparison to water. Finally, it gives details on methanol and ethanol, including their production and uses in drinks, fuels, and solvents.
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7.2 planar carbon alkenes 7.2
Alkenes are unsaturated hydrocarbons containing a carbon-carbon double bond. Common alkenes include ethene, propene, but-1-ene, and but-2-ene, which have the general formula CnH2n. Alkenes are planar molecules and exist as gases. They are insoluble in water but soluble in non-polar solvents such as cyclohexane. Major uses of alkenes include producing plastics like polythene from ethene and ethanol for industrial purposes.
7.2 planar carbon carboxylic acids 7.2
This document discusses four carboxylic acids: methanoic, ethanoic, propanoic, and butanoic acid. It notes that methanoic and ethanoic acids are liquids while propanoic and butanoic acids are solids. Carboxylic acids are soluble in water and non-polar solvents due to their polar COOH groups. Carboxylic acids have higher boiling points than alcohols because they form dimers held together by hydrogen bonds between their C=O and O-H groups.
7.2 planar carbon aldehydes 7.2
This document discusses four common aldehydes - methanal, ethanal, propanal, and butanal. It notes that while aldehydes are liquids, methanal is a gas at room temperature. Aldehydes have higher boiling points than alkanes but lower than alcohols due to their polar carbonyl group. Short chain aldehydes are soluble in water because of this polar group, but solubility in water decreases with longer carbon chains while solubility in cyclohexane increases. The document also mentions benzaldehyde, an aromatic aldehyde found in almond kernels.
7.2 planar carbon esters 7.2
Esters are formed from the reaction of carboxylic acids and alcohols, with the loss of a water molecule. Their names are derived from the parent alcohol and acid, with the endings changed to -yl and -oate respectively. Esters have physical properties between their precursor alcohols and acids, such as higher boiling points than alkanes but lower than alcohols. They are soluble in both water and non-polar solvents like cyclohexane. Esters occur naturally in fruits and flowers, responsible for flavors and scents, and as fats and oils. Ethyl ethanoate is used as a solvent for printing inks and paints.
7.2 planar carbon ketones 7.2
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7.1 tetrahedral carbon alkanes 7.1 (1)
The document discusses alkanes, a class of saturated hydrocarbons with the general formula CnH2n+2. It provides examples of common alkanes like methane, ethane, propane and butane. The document notes that alkanes have single bonds, tetrahedral molecular geometry, and physical properties like being gases at low molecular weights and liquids at higher weights, insoluble in water but soluble in non-polar solvents. It concludes that alkanes are used as fuels in mixtures like petrol, diesel, LPG and natural gas.
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7.1 tetrahedral carbon alkanes 7.1 (1)
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7.1 tetrahedral carbon alkanes 7.1 (1)
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6.2 factors affecting rates of reaction
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7.1 tetrahedral carbon alcohols 7.1
- 1. Alcohols
- 2. Alcohols Methanol CH3OH Ethanol C2H5OH Propan-1-ol C3H7OH Propan-2-ol C3H7OH Butan-1-ol C4H9OH Butan-2-ol C4H9OH
- 9. Classification of alcohols 1. Primary alcohol: contains one carbon atom directly attached to the carbon that contains the hydroxyl group, e.g. propan-1-ol
- 10. 2. Secondary alcohol: contains two carbon atoms directly attached to the carbon that contains the hydroxyl group, e.g. propan-2-ol
- 11. Physical properties Physical state: Liquid Boiling points much higher than the corresponding alkanes, due to polar OH group
- 12. Physical properties Solubility of methanol in (i) cyclohexane – not very soluble methanol is polar cyclohexane is not (ii) water - completely soluble because it is polar. As alcohol molecule gets bigger the polar part becomes less significant so the alcohol becomes less soluble in water and more soluble in cyclohexane
- 13. Butan-1-ol is – (i) soluble in cyclohexane – (ii) not very soluble in water The polar OH group is becoming less significant as the molecule gets bigger
- 14. Comparison with water Both have polar OH groups Alcohols have a non-polar part Both form hydrogen bonds between their molecules Water is more polar and has a greater capacity to form hydrogen bonds and so has a higher boiling point than methanol or ethanol
- 15. Methanol Methanol: is toxic (can cause blindness, insanity and death) It is added to industrial alcohol to prevent people drinking it. This mixture is called methylated spirits. The methanol acts as a denaturing agent – it renders a substance unfit for purpose without destroying the usefulness or applications of the substance. A purple dye is often added as a warning.
- 16. Ethanol Ethanol: is produced by fermentation. Fruits provide the sugar and yeast may need to be added. The enzyme zymase in yeast catalyses the reaction. C6H12O6 2C2H5OH + 2CO2
- 18. Ethanol To produce drinks of higher alcohol concentration the fermented liquids must be distilled. Spirits (whiskey, brandy, gin, vodka) contain 40% alcohol.
- 19. Gasohol Ethanol obtained from sugar cane is used for making gasohol in Brazil. This is then used as a fuel.
- 20. Uses of ethanol 1. Alcoholic drinks 2. Fuel 3. Solvent (can dissolve both polar and nonpolar solutes)