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Description
Flashcards by Becky Emmerson, updated more than 1 year ago
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Created by Becky Emmerson
almost 9 years ago
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| Question | Answer |
| Molecular Formula | The actual number of atoms of each element in a molecule, with any functional groups indicated. |
| Empirical Formula | Simplest whole number ratio of atoms of each element in a compound. |
| Homologous Series | Compounds that have the same functional group and general formula |
| Functional Group | A group of atoms responsible for the particular characteristics of the reaction of a compound. |
| Chain Isomers | A regular isomer - similar chemical properties, different physical properties |
| Positional Isomers | Functional group attached to a different carbon atom - different physical properties, possible different chemical properties. |
| Functional Group Isomers | Arranged into different functional groups - Very different physical and chemical properties |
| Stereoisomers | Same structural formula, different arrangement in space |
| E/Z Isomerism | When a double bonded carbon has two different atoms or groups bonded to it, e.g. H and CH3 |
| Cis/Trans Isomerism | Same as E/Z, but cannot be used if there are more than two different groups bonded to the carbon atoms (other than hydrogen) |
| Atom Economy | Molecular mass of desired product/sum of molecular masses of all products x100 |
| Percentage Yield | Actual Yield/Theoretical Yield x100 |
| Saturated | No double bonds |
| Hydrocarbons | Molecule made up of hydrogen and carbon ONLY |
| Unsaturated | Contains double bonds |
| Complete Combustion | Forms carbon dioxide and water |
| Incomplete Combustion | Forms carbon monoxide and water |
| Fractional Distillation | Cracking of large hydrocarbons into smaller fractions that are more useful. |
| Efficient Combustion | Use shorter branched chains to avoid knocking in engines and make combustion more efficient. |
| Isomerisation | Heating straight chain alkanes witha catalyst whilst they are stuck on AlO - Alkanes will join back together as shorter chained, branched isomers |
| Reforming | Converting alkanes into cyclic hydrocarbons using a catalyst made of platinum. |
| Fossil Fuels | Finite resources including coal, oil and natural gas that produce greenhouse gases that are usually harmful. |
| Bioethanol | Made from the fermentation of sugar from crops such as maize. It is said to be carbon neutral, but the actual production process and making of the equipment will change that. |
| Biodiesel | Made from renewable fats and oils, can be carbon neutral but is also cancelled out by the production of the machinery. |
| Heterolytic Fission | Two different substances are formed - a positive cation and a negative anion |
| Homolytic Fission | When two radicals are formed from two non radicals. |
| Radical | A particle with an unpaired electron. Very reactive. |
| Initiation | Free radicals are produced |
| Propagation | Free radicals are used up and created in a chain reaction. |
| Termination | Free radicals are joined together which cancels them out as they form full molecules |
| Free Radical Substitution | Hydrogen atom is substituted by a radical Cl or Br. |
| Alkene | Unsaturated hydrocarbon |
| Addition Reaction | Where two molecules combine to form one bigger molecule |
| Substitution Reaction | When one functional group of a compound is replaced by another. |
| Sigma Bond | When two s orbitals overlap, giving the highest possible electron density between the two nuclei. Single covalent bond. |
| Pi Bond | When two p orbitals overlap, forming one bond above and one below. |
| Double Bond | Cannot rotate, which causes E/Z isomerism. |
| Addition Polymers | When alkenes have joined together at the double bonds to make long chain polymers. |
| Advantages of Polymers | Very unreactive. Some can be biodegradable. Can be used as a heat source for electricity. Can be recycled. |
| Disadvantages of Polymers | Too unreactive - most aren't biodegradable. Often buried in landfill. Burning often produces toxic gases that have to be neutralized before being released. |
| Electrophilic Addition Reaction | Double bonds are opened up and atoms are added to the carbons. |
| Electrophile | Electron pair acceptor - attracted to areas where there are lots of electrons |
| Nucleophilic | Attracted to places with low electron density. |
| Hydrogen + Alkene (Hydrogenation) | Makes an alkane. Needs a nickel catalyst and 150 degrees. |
| Alkene + Bromine (Bromination/electrophilic addition) | Shake with bromine, orange to colourless colour change. Also done with chlorine and iodine. |
| Alkenes + HBr (Electrophilic Addition) | If the alkene is unsymmetrical two isomers are formed. Heterolytic fission |
| Ethanol Manufacture | Steam hydration - ethane is hydrated by steam at 300 degrees with a solid acid catalyst. Fermentation - Yeast in anaerobic conditions with glucose. Needs purification. |
| Primary Alcohol | OH is attached onto a carbon with 1 carbon attached to that. |
| Secondary Alcohol | OH is attached to a carbon with two carbons attached. |
| Tertiary Alcohol | OH is attached to carbon with 3 carbons attached. |
| Alcohol and Water | Alcohol is soluble in water as the OH allows it to form hydrogen bonds between itself and the water. As an alcohol increases in size, the ability to mix with water decreases. Hydrogen bonding gives high boiling points as they are strong and hard to break. |
| Alcohol Uses | Ethanol - Alcoholic drinks. Methylated spirits - Industrial solvent. Ethanol - Fuel. Unleaded petrol - Contains methanol. Methanol is used as a feedstock for organic chemical synthesis. |
| Dehydration Reactions | Eliminate water to form alkenes. Acid catalyst and 170 degrees. |
| Esterification | Alcohol added to a carboxylic acid makes an ester. Strong acid catalyst required. |
| Simple Alcohol Oxidation | Burn them in a combustion reaction. Forms CO2 and H20. |
| Primary Alcohol Oxidation | Alcohol - Aldehyde - Carboxylic Acid. Use Potassium Dichromate. Orange to green colour change. |
| Secondary Alcohol Oxidation | Alcohol - Ketone. Use Potassium Dichromate. Orange to green colour change. Reflux. |
| Tertiary Alcohol Oxidation | Do not react with potassium dichromate. No colour change. Can only oxidise via combustion. |
| CFC's | Stable, volatile, non-flammable and non toxic. |
| Hydrolysis (Halogenoalkanes) | Use warm NaOH or KOH and reflux it. C-Br bond breaks heterolytically. |
| Hydrolysis Speed of Halogenoalkanes | Hydrolysis speed is based on carbon-halogen bond strength. The further down the group you go, the faster they hydrolyse. |
| Silver Nitrate Halide Test | Add sliver nitrate to the mixture, and the silver ions will react with the halide ions. Use a black cross drawn under a flask containing the mixture to measure rate of reaction. |
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