Term
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Definition
R-OH
remove the -e at the end and put -ol in its place |
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Term
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Definition
| R-X (X=Halogen (Cl, Br, etc) add halogen to beginning, Fluoro-, Chloro- Bromo- Iodo- |
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Term
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Definition
R-CHO
remove -e and put -al |
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Term
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Definition
R-COR' (R' is another functional group)
Remove -e and put -one |
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Term
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Definition
| R-COOHremove -e and put -oic acid |
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Term
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Definition
R-COOR' (R' is another functional group)
Remove -e and put -oate |
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Term
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Definition
R-NH2
Change Methane to Methyl and add -amine to the end (methane is an example) |
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Term
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Definition
| R-, represents an ARYL GROUP, contains a benzene ring (the circular loopy carbon chain thing) |
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Term
| Physical Properties of Alkanes |
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Definition
| not soluable, low melt and boiling point |
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Term
| Physical Properties of Polar Function Group |
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Definition
| more polar they are the greater the melting and boiling point, more soluable in water they are |
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Term
| Intermolecular Forces Of Attraction (alkanes) |
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Definition
| Alkanes: van der waals', very low bp, non soluable |
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Term
| Intermolecular Forces of Attraction (halogenoalkanes) |
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Definition
| Weak Dipole-dipole, low bp, non soluable in water |
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Term
| Intermolecular Forces of Attraction (aldehydes) |
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Definition
| dipole-dipole, moderate bp, soluable in water |
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Term
| Intermolecular Forces of Attraction (alcohols) |
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Definition
| Hydrogen bonding, high bp, soluable in water |
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Term
| Intermolecular Forces of Attraction (carboxylic acids) |
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Definition
| Hydrogen bonding, high bp, soluable in water |
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Term
| Intermolecular Forces of Attraction (ketones) |
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Definition
| Dipole-dipole, moderate bp, soluable in water |
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Term
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Definition
| liquid with a high vapour pressure and readily evaporates at low temperature *GENERALLY REFERS TO LIQUIDS THAT EVAPORATE BELOW 100 DEGREES C* (below bp of water) |
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Term
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Definition
Non soluable in water, low bp for atomic mass, a chain of carbons for "spine" with Hydrogens surrounding it. Ending is -ane.
Also, they burn well. |
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Term
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Definition
| Ability to form chains and rings |
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Term
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Definition
| series in which all members have the same formula |
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Term
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Definition
| two or more compounds have same molecular but different STRUCTURAL formula |
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Term
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Definition
| -CH3 group, formed by removing 1 hydrogen from methane. This is true of all Alkanes, remove 1 hydrogen from Butane and you get Butyl |
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Term
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Definition
| solid Alkanes at room temp, not very reactive |
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Term
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Definition
| low for their molar mass, b/c electronegativit values for carbon and hydrogen are similar, and so they are either non-polar or very low polarity. BP and MP raise as carbons are added because Van der Waals' force rises with molar mass |
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Term
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Definition
| old name for alkanes, means Little Activity (from the Latin Parum Affinis) |
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Term
| Complete Combustion (Octane) |
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Definition
products: Carbon Dioxide and water
formula: 2C8H18(l) + 25O2(g) --> 16CO2 + 18H2O(l) |
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Term
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Definition
Products: Carbon Monoxide, Carbon, water, carbon dioxide
example reaction: C8H18(l) + 9O2 --> C(s) + 5CO(g) + 2CO2 (g) + 9H2O(l) |
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Term
| Methane + Halogen Reaction |
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Definition
| CH4(g) + Cl2(g) + UV Rays --> CH3Cl(g) +HCl(g) |
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Term
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Definition
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Term
| Free Radical Substitution |
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Definition
| Reaction involving the removal of a hydrogen atom from a carbon chain and its replacement by a free radical |
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Term
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Definition
| First step in a Free Radical Substitution, involves the formation of free radicals |
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Term
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Definition
| bonds break to create free radicals |
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Term
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Definition
| bonds break to form a positive and a negatively charged atom |
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Term
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Definition
| unpaired electron in one of the orbitals, highly energetic and reactive |
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Term
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Definition
| radicals react and generate new radicals |
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Term
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Definition
| a step that ends the free radical propagation steps and instead removes the free radicals from the equation and ends the reaction |
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Term
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Definition
| things that go after the R- to complete the compound |
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Term
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Definition
change the end to -yl
formed when a hydrogen is removed from an alkane |
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Term
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Definition
alkanes with a carbon to carbon double bond, general formula is C(n)H(2n).
Named by taking the longest carbon chain then specifying where the double bond begins |
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Term
| Alkenes (Physical Properties) |
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Definition
| Similar to Alkanes, either non polar or low polarity, low bp, insoluable in polar solvents |
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Term
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Definition
alkenes burn in excess oxygen to give carbon dioxide and water for complete combustion
limited oxygen, burn yelow and sooty |
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Term
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Definition
unsaturated, because the double bond can be broken
can be changed to Alkanes in the presence of hydrogen and a nickel catalyst at a temperature of 180 degree C |
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Term
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Definition
| React with halogens to produce the di-substituted product. Ethene + Bromine makes 1,2-dibromoethane (rips off two hydrogens and replaces them) |
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Term
| Alkenes (hydrogen halides) |
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Definition
hydrogen halides react with alkenes to form the addition product. Ethane + hydrogen Chloride forms chloroethane.
(basically breaks the double bond and adds on, (hydrogen chloride is HCl) the H goes on one part of the broken double bond and the Cl on the other.) |
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Term
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Definition
| Usually doesnt mix, but if concentrated sulfuric acid is used, then hydrogen sulfate addition product is formed (basically breaks the double bond and the H bonds to one part and the OSO3H bonds to the other part of the now broken double bond, then that compound mixes with water to form ethanol and H2SO4 (example on page 201) |
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