Chains, Energy and Resources
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- Created by: Emma Taylor
- Created on: 31-03-13 10:44
Hydrocarbon
An organic compound that contains only carbon and hydrogen
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Saturated Hydrocarbon
A hydrocarbon with single bonds only
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Unsaturated Hydrocarbon
A hydrocarbon containing carbon-to-carbon multiple bonds
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Aliphatic Hydrocarbon
A hydrocarbon with carbon atoms joined together in straight or branched chains
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Alicyclic Hydrocarbon
A hydrocarbon with carbon atoms joined together in a ring structure
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Functional Group
The part of the organic molecule responsible for its chemical reactions
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Homologous Series
A series of organic compounds with the same functional group but with each successive member differing by CH2
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Alkanes
The homologous series with the general formula CnH2n+2
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Nomanclature
A system of naming compounds
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Alkyl Group
An alkane with a hydrogen atom removed
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General Formula
The simplest algebraic formula of a member of a homologous series
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Displayed Formula
Shows the relative positioning of all the atoms in a molecule and the bonds between them
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Structural Formula
Shows the minimal detail for the arrangement of atoms in a molecule
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Skeletal Formula
A simplified organic formula, with hydrogen atoms removed from alkyl chains, leaving just the carbon skeleton and associated functional groups
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Structural Isomers
Molecules with the same molecular formula but with different structural arrangements of atoms
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Stereoisomerism
Compounds with the same structural formula, but with a different arrangement of the atoms in the space
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E/Z Isomerism
A type of stereoisomerism in which different groups attatched to each carbon of a C=C double bond may be arranged differently in space because of the restricted rotation of the C=C double bond
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cis-trans Isomerism
A special type of E/Z isomerism in which there is a non-hydrogen group and hydrogen on each carbon atom of the C=C bond
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cis Isomer (Z Isomer)
Has the hydrogen atoms on each carbon on the same side
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trans Isomer (E Isomer)
Has the hydrogen atoms on each carbon on different sides
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Homolytic Fission
The breaking of a covalent bond, with one of the bonded electrons going to each atom, forming two radicals
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Radical
A species with an unpaired electron
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Heterolytic Fission
The breaking of a covalent bond when both of the bonded electrons going to one of the atoms, forming a cation (+ ion) and an anion (- ion)
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Nucleophile
An atom (or group of atoms) that is attracted to an electron-deficient area, where it donates a pair of electrons
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Electrophile
An atom (or group of atoms) that is attracted to an electron-rich area, where it accepts a pair of electrons
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Addition Reaction
A reaction in which a reactant is added to an unsaturated molecule to make a saturated molecule
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Substitution Reaction
A reaction in which an atom or group of atoms is replaced by a different atom or group of atoms
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Elimination Reaction
Refers to the removal of a molecule from a saturated molecule to make an unsaturated molecule
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Fractional Distillation
The separation of the components in a liquid mixture into fractions which differ in boiling point (and hence chemical composition) by means of distillation
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Cracking
Refers to the breaking down of long chained saturated hydrocarbons to form a mixture of shorter-chained alkanes and alkenes
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Catalyst
A substance that increases the rate of a chemical reaction without being used up in the process
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Radical Substitution
A type of substitution reaction in which a radical replaces a different atom or group of atoms
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Mechanism
A sequence of steps showing the path taken by electrons in a reaction
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Initiation
The first step in a radical substitution in which the free radicals are generated by ultraviolet radiation
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Propogation
The two repeated steps in radical substitution that build up the products in a chain reaction
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Termination
The step at the end of a radical substitution when two radicals combine to form a molecule
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pi-bond
The reactive part of a double bond formed above and below the plane of the bonded atoms by sideways overlap of p-orbitals
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Electrophilic Addition
A type of addition reaction in which an electrophile is attracted to an electron rich centre or atom, where it accepts a pair of electrons to form a new covalent bond
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Carbocation
An organic ion in which a carbon atom has a positive charge
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Curly Arrow
A symbol used in reaction mechanisms to show the movement of an electron pair in the breaking or formation of a covalent bond
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Polymer
A long molecular chain built up from monomer units
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Monomer
A small molecule that combines with many other monomers to form a polymer
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Addition Polymerisation
The process in which unsturated alkene molecules (monomers) add on to a growing polymer chain one at a time, to form a very long saturated molecular chain
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Addition Polymer
A very long molecular chain, formed by repeated addition reactions of many unsaturated alkene molecules
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Repeat Unit
A specific arrangement of atoms that occurs in the structure over and over again
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Biodegradeable Material
A material that is broken down naturally in the environment by living organisms
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Volatility
The ease that a liquid turns into a gas
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Reflux
The contiual boiling and condensing of a reaction mixture to ensure that the reaction takes place without the contents of the flask boiling dry
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Esterification
The reaction of an alcohol with a carboxylic acid to produce an ester and water
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Dehydration
An elimination reaction in which water is removed from a saturated molecule to make an unsaturated molecule
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Hydrolysis
A reaction with water or aqueous hydroxide ions that breaks a chemical compound into two compounds
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Nucleophilic Substitution
A type of substitution reaction in which a nucleophile is attracted to an electron-deficient centre or atom, where it donates a pair of electrons to form a new covalent bond
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Limiting Reagent
The substance in a chemical reaction that runs out first
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Molecular Ion
The positive ion formed in mass spectrometry when a molecule loses an electron
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Fragmentation
The process in mass spectrometry that causes a positive ion to split into pieces, one of which is a positive fragment ion
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Enthalpy
The heat content that is stored in a chemical system
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Exothermic
A reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants, resulting in heat loss to the surroundings
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Endothermic
A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants, resulting in heat being taken in from the surroundings
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Enthalpy Profile Diagram
A diagram for a reaction to compare the enthalpy of the reactants with the enthalpy of the products
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Activation Energy
The minimum energy required to start a reaction by the breaking of bonds
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Standard Conditions
A pressure of 100kPa (1 atm.) and 298K (25 degrees C)
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Standard State
The physical state of a substance under the standard conditions 100kPa and 298K
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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 Combustion
The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, all reactants and products being in their standard states
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Standard Enthalphy Change of Formation
The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states, under standard conditions
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Specific Heat Capacity
The energy required to raise the temperature of 1g of a substance by 1 degreeC
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Bond Enthalpy
The enthalphy change that takes place when breaking by homolytic fission one mole of a given bond in the molecule of a gaseous species
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Average Bond Enthalpy
The average enthalpy change that takes place when breaking by homolytic fission one mole of a given type of bond in the molecules of a gaseous species
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Hess' Law
States that, if a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same for each route
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Enthalpy Cycle
A diagram showing alternative routes between reactants and products which allows the indirect determination of an enthalpy change from other known enthalphy changes using Hess' law
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Rate of Reaction
The change in concentration of a reactant or a product in a given time
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Heterogeneous Catalysis
Catalysis of a reaction in which the catalyst has a different physical state from the reactants
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Homogeneous Catalysis
Catalysis of a reaction in which the catalyst and reactants are in the same physical state
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Boltzmann Distribution
The distribution of energies of molecules at a particular temperature, often shown as a graph
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Le Chatelier's Principle
States that when a system in dynamic equilibrium is subjected to a change, the position of the equilibrium will shift to minimise this change
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Dynamic Equilibrium
The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction
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Greenhouse Effect
The process in which the absorption and subsequent emission of infrared radiation by atmospheric gases warms the lower atmosphere and the planet's surface
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Troposphere
The lowest layer of the Earth's atmosphere, extending from the Earth's surface up to about 7km above the poles and 20km above the tropics
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Stratosphere
The second layer of the Earth's atmosphere, containing the ozone layer, about 10km to 50km above the Earth's surface
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Adsorption
The process that occurs when a gas, liquid or solute is held to the surface of a solid or, more rarely, a liquid
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Other cards in this set
Card 2
Front
A hydrocarbon with single bonds only
Back
Saturated Hydrocarbon
Card 3
Front
A hydrocarbon containing carbon-to-carbon multiple bonds
Back
Card 4
Front
A hydrocarbon with carbon atoms joined together in straight or branched chains
Back
Card 5
Front
A hydrocarbon with carbon atoms joined together in a ring structure
Back
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