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73 Cards in this Set
- Front
- Back
ethene -> ethane
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reacted with hydrogen gas, nickel catalyst,150degees, high pressure,
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Bromine + alkene
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electrophilic addition
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electrophile
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electron pair acceptor, partially positively charged
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Alkenes +hydrogen halids
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alkenes undergo addition with hydrogen halides. rtp
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alkene -> alcohol
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react alkene with water, H2SO4 catalyst, H2SO4 + alkene in electrophilic addition, water added, hydrolysis and catalyst regenerated,
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ethene -> ethanol
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ethene hydrated by steam 300degrees, 60atm pressure, solid phosphoric(v) acid catalyst
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alcohol -> alkene
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reflux, alcohols dehydrated, elimination of water, hot aluminum oxide catalyst, of reflux with excess h2so4 170degrees ethene collected over water
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alcohol oxidised by
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burning, oxidising agent
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primary alcohol oxidises to
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aldehydes then carboxylic acid
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secondary alcohol oxidises to
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ketones
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Aldehyde or carboxylic acid from primary oxidisation
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distillation equipment used so aldehyde distilled off so it doesn't oxidise again to carboxylic acid
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copolymer
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made from more than one type of monomer in random order
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Thermoplastic polymer
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no cross linking, weak intermolecular bonds, can melt and remold
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Thermosetting polymers
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covalent cross linking, giant 3d structure, strong, insoluble, char when heated doest soften
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stereoisomers
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same structural formula, different arrangement in space
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E/Z
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E when one above one bellow double bond, Z when both above / both bellow
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Fingerprint region
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between 1000cm-1 - 1550cm1, unique to each compound. less than 1500cm-1
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polymer with lots of OH groups
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strong hydrogen bonds between molecules so insoluble as too much energy to break
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polymers with few OH groups
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not many H bonds with water so insoluble
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CO2, SiO2
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CO2 simple molecule, SiO2 giant molecular structure
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Homogeneous catalyst
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Forms intermediates, activation enthalpy of intermediates lower
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anthropogenic
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effect due to humans
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infra red
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bonds vibrate more
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UV/Visible
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gives electrons more energy
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Heterolytic fission
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two different substances formed, different charges
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Homolytic fission
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two radicals formed, same charge, no charge
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Halogen+alkane
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halogenoalkanes, photochemical reaction, free-radical substitution reaction, 3 stages
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Photochemical reaction
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started by UV light/radiation
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Initiation
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free radicals produced
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propagation
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free radicals used up but remade
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Termination
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free radicals form stable molecules
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Carbon-Halogen bonds
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UV can break up Carbon-Halogen bonds, homolytic fission
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ozone layer situated
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edge of stratosphere
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ozone at ground level
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causes photochemical smog by mixing with solid particles, eg carbon, ozone toxic to humans
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elsastomers
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polymers that are soft and springy and return to their original shape
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fibre
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polymers that do not deform easily so can be made into strong threads, nylon
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two double bonds present
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-diene
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electrophile from non polar molecule
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instantaneous dipole makes electrophile
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carbocation
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a carbon in a molecule with a positive charge
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polymer stereo-regularity
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more regular arrangement, can fit together closer stronger imf
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polymer chain flexibility
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rigid chain stronger, benzene rings make stronger
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F,O,N,Cl
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permanent dipoles think foncle
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oxidation of alcohols conditions
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reflux, excess acidified potassium dichromate
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reflux
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to continually evaporate and condense
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photon
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tiny packets of energy, E=hv
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quanta
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exact amount of energy required to bring about a change in an atom or molecule
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excitation: energy levels etc
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UV/Visible-energy levels, infra red-vibrational energy, Microwave-Rotational energy, Translational energy- continuous/when other energies relax to nomal
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ozone cycle
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5 different stages
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biradical
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when there is 2 unpaired electrons, oxygen, group6/4, molecules can be biradicals
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free radical mechanism
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LEARN ME
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enthalpy profile not best representation of reaction
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enthalpy profile doesn't take into account reactions that happen in more than on step
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CFC
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they are un-reactive so pass unchanged to the stratosphere where heterolytic fission occurs
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methane helps ozone as
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methanoic bacteria make methane, CH4+Cl->HCl+CH3’
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dynamic equilibrium
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overall the system is unchanging but individuals within the system can change
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indicators
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methyl orange-yellow to red adding acid. phenolphalein- red to colorless adding acid
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chromium and copper
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one 4s electron goes towards 3d
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redox reaction
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electrons are transferred, oilrig
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oxidation states
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o always -2 h+1 in metal hydrides -1, metals normally positive, non-metals negative
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sulfate(VI)
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means sulfur +6 oxygen -2
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metals reduce dilute acid
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hydrogen gas created metal is oxidised
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electronegativity
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The ability to attract the bonding electrons in covalent bond
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first ionising enthalpy
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energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mol of gaseous 1+ ions
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3 factors of ionisation enthalpies
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atomic radius, nuclear charge, electron shielding.
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group 7 trends
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B.P decreases down group, less reactive down group, electronegativity decreases down group
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Cl,Br,I color in water
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Cl=colorless, Br=yellow/orange, I=Brown
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Cl,Br,I color in hexane
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Cl=Colorless, Br=orange/red, I=pink/violet
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silver nitrate test colors
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F=no precipitate, Cl=white prec, Br=Cream prec, I=Yellow prec
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Halogenoalkanes
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alkanes with at least 1 halogen atom in place of a hydrogen atom.
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halogenoalkanes BP
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B.P increases down group
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halogenoalkanes + hydroxxide ions
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nucleophilic substitution, also with water
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Halogenoalkanes + ammonia
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forms amines, nucleophilic substitution.
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Reactivity of halogenoalkanes
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iodoalkanes most reactive.
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card front
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