OZ - Reaction mechanisms *01 (and sustainability) Flashcards

1
Q

what is a substitution reaction?

A

when a functional group in a compound is replaced by another functional group

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2
Q

what is a nucleophile?

A

something that is attracted to the slightly +ve carbon atom

is usually -ve

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3
Q

What does the relative reactivities of haloalkanes depend on?

A

The carbon halogen bond strength determines reactivity
- decreases down group

C-F bond the strongest (despite being the most polar) as it has the highest bond enthaply

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4
Q

What can you test the relative reactivities of the haloalkanes?

A

react the haloalkanes with water in the presence of silver nitrate

  1. see which reacts the fastest.
    - put a chloroalkane, bromoalkane, and iodoalkane in three different test tubes
    - add silver nitrate solution and some ethanol

Ag+ + X- —> AgX (s)

  1. the silver halide forms a precipitate
  2. the precipitate forms fastest with iodoalkane - so must be the most reactive
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5
Q

what is bond fission?

A

breaking a covalent bond

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6
Q

bond fission - heterolytic

A

two different substances are formed

  • a positively charged cation
  • a negatively charged anion
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7
Q

bond fission - homolytic

A

two electrically uncharged radicals are formed

eg.

X-Y —> X* + Y*

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8
Q

what are chain reactions?

A

When a product causes more reactions to take place

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9
Q

chain reactions - initiation

A

free radicals are produced

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10
Q

chain reactions - propagation

A

free radicals react with molecules and produce new radicals

these go on to react with more molecules, producing even more radicals

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11
Q

chain reactions - termination

A

two radicals react together to form a stable molecule

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12
Q

Radical mechanism for reaction of alkanes with halogen - initiation

A
  1. sunlight provides enough energy to break the Cl-Cl bond - photodissociation
  2. the bind splits equally - homolytic fission
  3. the molecule form two highly reactive free radicals

Cl-Cl —UV—> Cl* + Cl*

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13
Q

Radical mechanism for reaction of alkanes with halogen - propagation

A
  1. Cl* attacks a methane molecule, forming a hydrogen halide and a methyl radical

Cl* + CH4 –> HCl + *CH3

  1. the new methly radical, *CH3, can attack another Cl2 molecule

CH3 + Cl-Cl —–> CH3Cl + Cl
the new Cl* can attack another CH4 and so on until all the Cl2 and CH4 molecules are wiped out

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14
Q

Radical mechanism for reaction of alkanes with halogen - termination

A
  1. if two free radicals join together they make a stable molecule
  2. there are lots of possible termination reactions
    eg.
    * CH3 + Cl* —–> CH3Cl

*CH3 + *CH3 —> C3H6

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15
Q

what is ozone?

A

in the stratosphere

contains ozone molecules, O3

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16
Q

How is Ozone formed?

A

when UV radiation from the sun hits oxygen molecules

O2 + hV —-> O + O

O + O2 —-> O3

17
Q

how is the ozone layer constantly being replaced?

A

O2 + O < —> O3

it is a reversible reaction
ozone is continuously being destroyed and replaced as UV hit the molecules

an equilibrium is set up so concentrations stay fairly constant

18
Q

Why is ozone important?

A

protects us from UV radiation
- UVB can damage DNA in cells and cause skin cancer (also sunburn)

however in small amounts UV needed
- vitamin D

19
Q

Ozone at ground level (troposphere) causes and effects

A

due to the effect of sunlight on mixtures of nitrogen dioxide and hydrocarbons
- from vehicle engine and power stations

in industrialised areas ozone mixes with solid particles of carbon to create PHOTOCHEMICAL SMOG

  • can cause respiratory problems
  • damages plants and materials
  • ozone itself is toxic to humans
20
Q

How is Ozone broken down in the stratosphere

A
by CFCs (chlorofluorocarbons) 
- haloalkanes that have all their hydrogens replaced by Cl and F atoms 

the C-Cl bond can be broken down by high energy UV in the stratosphere to form chlorine radicals
- these act as catalysts in the breakdown of ozone

21
Q

ease of photodissociation of haloalkanes

A

all haloalkanes have carbon and halogen atoms - UV can break these bonds
- the carbon-halogen bonds split homolytically to create two free radicals

the ease it is broken depends on the halogen

  • carbon-iodine most likely to break because it has the lowest bond enthalpy
  • carbon-fluorine lest likely to break because it has the highest bond enthalpy
22
Q

How is the ozone layer destroyed by homogeneous catalysis

A

Chlorine free radicals formed when CFCs are broken down by high energy UV in the stratoshpere
- these free radicals are catalysts
INITATION - CCl3F3 (g) + hv —> CCl2F3 (g) + Cl (g)

These radicals react with ozone to form an intermediate ClO* and an oxygen molecule
PROPAGATION :
Cl* + O3 —> O2 + ClO*
ClO* + O —-> O2 + Cl* (the Cl* radical is regenerates and goes onto destroy more ozone)

the reaction will only terminate if two radicals react together
TERMINATION: Cl* + Cl* —> Cl2

OVERALL REACTION: O3 + O —-> 2O2 ….. and Cl* is the catalyst

23
Q

what other free radical can destroy ozone?

A

NO from nitrogen oxides

eg. NO2 + hv —> NO* + O