A series of organic compounds having the same functional group but with each succesive member differing by CH2.
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Functional Group
An atom or group of atoms responsible for the characteristic reactions of a compound.
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Saturated
Containing only C-C single bonds.
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Unsaturated
Containing at least one C to C multiple bond.
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Empirical Formula
The simplest whole number ratio of atoms of each element present in a compound.
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Molecular Formula
The actual number of atoms of each element present in a molecule.
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Structural Isomers
Compounds with the same molecular formula but with different structural formulae.
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Stereoisomers
Compounds with the same structural formula but with a different arrangement of atoms in space.
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E/Z Isomerism
Example of Stereoisomerism. Arises because a C=C bond cannot rotate. There must be two different groups attached to each C of the C=C double bond.
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Cis-Trans Isomerism
A special case of E/Z isomerism in which two groups, one on each C of the C=C double bond, are the same.
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Fractional Distillation
Separation of a liquid mixture into fractions with different boiling points.
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Catalytic Cracking
The breaking down of long chained alkanes to form more useful, shorter chained alkanes and alkenes.
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Biofuel
A fuel that is derived from recently living material such as plants or the waste of animals.
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'Curly Arrow'
The movement of a pair of electrons, showing either the breaking or forming of a covalent bond.
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Radical
A species with an unpaired electron.
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Homolytic Fission
The breaking of a covalent bond where the bond pair of electrons is split equally, forming two radicals.
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Heterolytic Fission
The breaking of a covalent bond where the shared pair of electrons are not split equally, forming a cation and an anion.
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Electrophile
An electron pair acceptor.
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Nucleophile
An electron pair donor.
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Exothermic
Heat is given out to the surroundings.
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Endothermic
Heat is taken in from surroundings.
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Activation Energy
The minimum energy required to start a reaction by the breaking of bonds.
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Standard Enthalpy Change of Reaction
The enthalpy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states.
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Standard Enthalpy Change of Formation
The enthalpy change when 1 mole of a compound is formed from its constituent elements in their standard states, under standard conditions.
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Standard Enthalpy Change of Combustion
The enthalpy change when 1 mole of a substance reacts completely with oxygen under standard conditions, all reactants and products being in their standard states.
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Average Bond Enthalpy
The average enthalpy change when 1 mole of gaseous bonds is broken by homolytic fission.
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Catalyst
Speeds up a reaction without being consumed by the overall reaction.
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Volatility
The ease with which a liquid turns into a gas.
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Le Chatelier's Principle
When a system in dynamic equilibrium is subjected to a change, the position of equlibrium will shift to minimise the effect of the change.
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Other cards in this set
Card 2
Front
A series of organic compounds having the same functional group but with each succesive member differing by CH2.
Back
Homologous Series
Card 3
Front
An atom or group of atoms responsible for the characteristic reactions of a compound.
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