2259747
Description
Flashcards by ashleypwainwright, updated more than 1 year ago
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Created by ashleypwainwright
almost 10 years ago
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| Question | Answer |
| Molecular Formula | Actual number of atoms of each element in a molecule. |
| Empirical Formula | Simplest whole number ratio of the atoms of each element in a molecule. |
| Homologous Series | Series of organic compounds having the same functional group with successive members differing by CH2. |
| Functional Group | Group of atoms responsible for the characteristic reactions of a compound. |
| Structural Isomers | Same molecular formula, different structures. |
| Hydrocarbon | A compound that contains hydrogen and carbon only. |
| Saturated | Contains only single C-C bonds. |
| Radical | Contains an unpaired electron. |
| Fractional Distillation | Separates due to differences in boiling point. |
| Fraction | Mixture of compounds of similar boiling point. |
| Cracking | Breaking a long chain alkane into a shorter chain alkane and alkene. |
| Biofuel | A fuel produced from plant or animal waste. |
| Stereoisomers. | Same structural formula but different arrangement in space. |
| E/Z Isomers | Isomers resulting from restricted rotation about a double bond, where two different groups are attached to each carbon of the C=C. |
| Cis/trans Isomers | A special case of E/Z isomerism in which two of the substituent groups are the same. |
| Unsaturated | Contains one or more double C=C bonds. |
| Electrophile | Electron pair acceptor. |
| Nucleophile | Lone pair donor. |
| Reflux | Continuously boil and condense. |
| Standard Conditions | Temperature 298k, Pressure 100kPa |
| Enthalpy Change of Reaction | Enthalpy change when the reaction occurs in the molar quantities shown in the chemical equation. |
| Enthalpy Change of Formation | Enthalpy change when one mole of a compound is formed from its elements. |
| Enthalpy Change of Combustion | Enthalpy change when one mole of a substance is completely burnt. |
| Hess's Law | Total enthalpy change is independent of route. |
| Average Bond Enthalpy | Energy needed to break one mole of gaseous bonds. |
| Activation Energy | Minimum energy needed for a reaction to occur. |
| Catalyst | Speeds up a reaction without being used up. |
| Le Chatelier's Principle | The position of equilibrium will shift so as to minimise the effect of any change in conditions. |
| Dynamic Equilibrium | Rates of forward and backward reactions are equal. Concentrations are constant. |
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