alkenes Flashcards

1
Q

Describe alkenes

A
  • unsaturated which means there is at least 1 = covalent bond
  • can undergo addition reactions
  • = have a high e- density making them reactive
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2
Q

what are sigma bonds

A
  • are when 2s orbitals overlap
  • align horizontally to give a single covalent bond
  • strong electrostatic attraction between the nuclei of the shared pair of electrons (bc of high electron density between the nuclei)
  • high bond enthalpy
  • strongest type of covalent bond
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3
Q

what are pi bonds

A
  • sideways overlap of 2 p orbitals above and below the C=C.
  • PB are weaker than SB bc the e- density is spread out above and below the nuclei
  • electrostatic attraction is weaker so SB have a lower bond enthalpy
  • PB locks the 2 C-atoms in position and prevents them from rotating around the =, so rotation is restricted.
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4
Q

describe the reactivity of alkenes

A
  • alkenes have SB + PB
  • 3/4 used in SB.
  • this is a high electron density area that makes them reactive
  • PB stick out a little and the = has a high ED
  • open to attack from electrophiles
  • PB has a low bond enthalpy so alkenes are reactive bc not a lot of energy needed
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5
Q

shape of alkenes

A
  • trigonal planar
  • three regions of e- density around each carbon atom
  • three regions repel AFAP
  • bond angle is 120
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6
Q

stereoisomers

A
  • same structural formula
  • different arrangement of atoms in space
  • e/z isomerism occurs when there is restricted rotation around = and requires 2 diff FG attached to each c-atom
  • E + trans= opposite
  • Z + cis- same side
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7
Q

describe the Cahn Inlog Prelog rules

A
  • when there are 4 diff groups around a double bond
  • priority based on their atomic number
  • calculate the atomic number of the first element directly bonded to C=C.
  • if first element is the same number, move down the chain .
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8
Q

describe test for alkenes

A
  • decolourisation of Br water
  • adding Br water to alkenes causes a colour change from brown/orange to colourless
  • Br is the electrophile and adds to the alkene forming dibromo alkane
  • Br2 is polarised as the e- in the = repels the e- in Br2
  • Br(-)-(Br(+)
  • Br2 bond breaks by heterolytic fission
  • double bond breaks
  • one carbon bonds to a Br
  • carbocation intermediate is formed and a Br- with 2 electrons
  • addition product formed
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9
Q

what is an electrophile

A
  • electron pair acceptor
  • deficient in electrons so are attracted to a =
  • H+ , NO2+
  • E.g polar molecules (delta+) H-Br
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10
Q

Hydration of alkenes

A
  • alcohol is formed
  • sue steam and acid catalyst to create and alcohol
  • can make ethanol by reacting steam and ethene using a phosphoric acid catalyst + 300C + 60atm
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11
Q

addition of hydrogen halides to alkenes

A
  • electrophilic addition

- halogenoalkanes formed,

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12
Q

reaction of alkenes with unsymmetrical hydrogen halide

A
  • 2 different products are formed
  • the more stable carbocation forms the major product
  • the less stable carbocation forms the minor product
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13
Q

what determines the stability of a carbocation

A
  • the more alkyl groups bonded to carbocation the more stable
  • bc alkyl groups push e- towards the +ve carbocation stabilising it
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14
Q

describe addition polymers

A
  • alkenes are the monomers which join to form addition polymers
  • natural : proteins and natural rubber
  • synthetic : poly(ethene) and poly(propene)
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15
Q

how to make poly(propene)

A
  • need several monomers of propene
  • the double bond opens up to form the polymer
  • the monomer will have a bracket around it
  • each carbon will have no = and a single bond coming out of the bracket to form 4 bonds
  • poly(alkanes) are saturated, normally non-polar and unreactive.
  • they don’t degrade well in landfill.
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16
Q

positives of landfill in the disposal of plastic

A
  • most polymers aren’t biodegradable so need to be disposed of carefully
  • landfill is useful for disposing of plastics that are :
  • too difficult to recycle
  • too difficult to separate from other materials
  • ## not enough plastic to extract to make in economically viable
17
Q

negatives of landfill in the disposal of plastics

A
  • not sustainable as large amounts of land needed
  • increasingly expensive to use land for waste disposal (land tax)
  • there is a need to reduce our reliance on landfill.
18
Q

recycling plastics

A
  • most plastics made from crude oil (non renewable)
  • recycling means we reduce reliance on crude oil making plastics
  • some plastics (polypropene) can be remoulded into new objects
  • other plastics can be cracked into monomers to be used as organic feedback for plastics or other substances.
19
Q

incineration

A
  • burning waste plastics
  • if can’t be recycled
  • energy from burning can be used to generate electricity
  • can release toxic fumes
  • chlorine based plastic s(PVC) can produce harmful HCL gas when burnt
  • glue gas scrubbers neutralise acidic gases (HCL). fire a base at the acidic gas to form a neutral salt.
20
Q

biodegradable polymers

A
  • decompose under certain condition by organisms
  • made from oil fractions and renewable sources (starch)
  • more expensive
  • to degrade you need good supply of O2 and moisture
  • can use BP in frost protective sheets for plants. made form polyethene and starch grains. over time micro-organisms break down the polymer so you don’t need to dispose of the old sheeting.
  • photodegradable polymers degrade when exposed to sunlight.