3.3 Haloalkanes Flashcards
Outline the following steps in the mechanism for the reaction of methane with fluorine to form fluoromethane
- Initiation step
F2->2F. - First propagation step
CH4 +F. -> C.H3 + HF - Second propagation step
C.H3 + F2 -> CH3F +F. - Termination step
C.H3 +F. -> CH3F
What does it mean when a haloalkane is described as primary, secondary and tertiary
Primary : carbon bonded to halogen is bonded to only one other carbon atom
Secondary : Carbon bonded to halogen is bonded to two other carbon atoms
Tertiary : Carbon bonded to halogen is bonded to three other carbon atoms
State the essential condition for free radical substitution and why it is necessary
UV light
- as it provides the energy to break the halogen-halogen bond to form free radicals and start the reaction
Define free radical
A species with an unpaired electron
What is homolytic fission
When the halogen - halogen bond is broken
Write overall reaction for reaction of chlorine with methane to form chloromethane (CH3CL)
Initiation step : Cl2 -> 2Cl.
Propagation step 1 : CH4 + Cl. -> C.H3 + HCl
Propagation step 2 : C.H3 + Cl2 -> CH3Cl + Cl.
Termination step : Cl. + C.H3 -> CH3Cl
Write overall equation for reaction of chlorine with methane to form trichloromethane
CH4 + 3CL2 -> CHCL3 + 3HCl
Methane reacts with IBr to form many products. Outline the mechanism that produces iodomethane and hydrogen bromide
- UV light needed
Initiation step : IBr -> Br. + I.
Propagation step 1: CH4 + Br. -> C.H3 + HBr
Propagation step 2 : C.H3 + IBr -> CH3I + Br.
Termination step : I. + C.H3 -> CH3I
Br. + C.H3-> CH3Br
C.H3 + C.H3 -> C2H6
(there are more termination steps but you only need to show 3)
Which species is produced in a propagation step during reaction of propane with an excess of chlorine in presence of UV light
1. H.
2.C3H5CL
3.C3H6CL2
4.C6H14
- C3H6CL2
How to reduce amount of further substitution
Use excess alkane
What are CFCS
Haloalkanes that contain both chlorine and fluorine
Chlorotrifluoromethane (CClF3) decomposes in presence of UV light forming a reactive intermediate that catalyses the decomposition of ozone. Write an equation to show how CClF3 decomposes to form the reactive intermediate.
Write two equations to show how this reactive intermediate is involved in catalysing the decomposition of ozone
CFCL3 -> C.FCL2 + Cl.
Cl. + O3 -> ClO. + O2
ClO. +O3 -> Cl. + 202
Identify condition that causes CCl4 to break in upper atmosphere
UV light
Small amount of freon CF3Cl has mass 1.78 x 10^-4 kg goes into a room with a volume of 100m^3. Calculate number of freon molecules in a volume of 500cm^3
Avogadro constant = 6.022 x 10^23 mol^-1
Mr of Freon : 104.5
moles in freon = (1.78 x 10^-4) divided by 104.5 = 1.7 x 10^-3
Number of molecules = (1.7 x10^-3) x (6.022 x 10^23) = 1.02 x 10^21
molecules in 500cm^3
(1.02 x 500 x 10^-6) divided by 100 = 5.1 x 10^15 (2.s.f)
State role of chlorine atoms in the ozone layer reactions
Acts as a catalyst
This is because it is regenerated and is unchanged at the end of
Boiling point of iodomethane is higher than that of fluoromethane even though electronegativity of iodine is less than that of fluorine
Why does iodomethane have a higher boiling point
Iodine is bigger than fluorine so van de waals forces between CH3I molecules are stronger than those between CH3F mlecules
The permanent dipole-dipole forces in CH3F are stronger than CH3I. However van de waals forces are stronger than the permanent dipole-dipole forces