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52 Cards in this Set
- Front
- Back
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Structural isomer
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same molecular formula, different structure
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Hydrocarbon
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a compound that contains hydrogen and carbon only
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Saturated
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contains only single C-C bonds
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Radical
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species with an unpaired electron
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Fractional distillation
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separates due to differences in boiling point
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Fraction
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mixture of compounds of similar boiling point
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Cracking
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breaking a long chain alkane into a shorter chain alkane and an alkene
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Fuel
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a substance that is burned to produce heat
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Biofuel
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a fuel produced from plant or animal waste
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Stereoisomer
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same structural formula but different arrangement in space
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E/Z isomers
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isomers resulting from restricted rotation about a double bond, where two different groups are attached to each carbon of the C=C
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Unsaturated
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contains one or more C=C bond
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Electrophile
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electron pair acceptor
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Nucleophile
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lone pair donor
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Reflux
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continuously boil and condense
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Standard conditions
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Temperature 298K, pressure 101 kPa, 1moldm3
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Enthalpy change of reaction
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Enthalpy change when the reaction occurs in the molar quantities shown in the chemical equation
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Enthalpy change of formation
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Enthalpy change when one mole of a compound is formed from its elements
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Enthalpy change of combustion
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Enthalpy change when one mole of a substance undergoes complete combustion
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Hess’s Law
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Total enthalpy change is independent of route
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Average bond enthalpy
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Energy needed to break one mole of gaseous bonds
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Activation energy
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Minimum energy needed for a reaction to occur
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Catalyst
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increases rate of reaction without being consumed by overall reaction
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Le Chatelier’s Principle
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When the conditions on a system in equilibrium are changed, the position of equilibrium shifts to minimise the change
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Dynamic equilibrium
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Rates of forward and backward reactions are equal
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why straight chain isomers higher bp than branched?
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branched chains have less surface contact therefore weaker Van der Waals forces
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how is ozone concentration maintained?
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O2 + O ↔ O3
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why is ozone important to life on earth
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absorbs harmful UV
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why increasing concentration increases rate of reaction
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more crowded particles means more collisions per second
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how catalysts increase rate of reaction
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activation energy is lowered more molecules have enough energy to react
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how high temp increase rate of reaction
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activation energy does not change more molecules have enough energy to react
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atom economy equation
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(mass of desired product/mass of all products) x 100
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how to reduce environmental damage from disposal of polymers
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Develop photodegradable or biodegradable polymers. Develop ways to sort and recycle polymers
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why alcohols soluble in water
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has hydroxyl group so forms hydrogen bond with water
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bond ____ releases energy
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forming
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bond ____ absorbs energy
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breaking
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exothermic enthalpy change
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more energy released than absorbed (negative value)
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endothermic enthalpy change
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more energy absorbed than released (positive value)
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enthalpy change units
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kJmol⁻¹
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homologous series
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Series having same functional group and a general formula
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percentage yield equation
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(actual mol product/theorectical mol product) x 100
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effect of absorption of infrared radiation on bonds between molecules
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vibrate more
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environmental problem of NO
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causes photochemical smog. depletes ozone
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environmental problem of CO
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toxic (reduces capacity of blood to carry oxygen)
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primary alcohol + acidified dichromate ions (heat and distil)
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aldehyde
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primary alcohol + acidified dichromate ions (reflux)
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carboxylic acid
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alcohol + carboxylic acid (acid and heat)
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ester
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secondary alcohol + acidified dichromate ions (heat reflux)
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ketone
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tertiary alcohol + acidified dichromate ions
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no reaction
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If alcohol is oxidised, acidified K₂Cr₂O₇ changes from
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orange to green
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alkene + steam (heat and acid)
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alcohol (hydration)
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alcohol + conc. acid (heat)
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alkene + water (elimination)
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