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7409939
Organic Chemistry + Alkanes/Alkenes
Description
AS - Level Chemistry Mind Map on Organic Chemistry + Alkanes/Alkenes, created by Ella Cannings on 20/01/2017.
No tags specified
organic chemistry
isomerism
stereoisomers
radical substitution
alkanes
reactions of alkanes
reactions of alkenes
electrophillic addition
chemistry
as - level
Mind Map by
Ella Cannings
, updated more than 1 year ago
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Created by
Ella Cannings
over 7 years ago
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Resource summary
Organic Chemistry + Alkanes/Alkenes
Carbon based, except for CO2 (inorganic)
Carbon can produce such a diverse range due to 4 outer electrons so 4 covalent bonds
non- polar and stable
Classifications
Homologous series = related compounds with similar structure and generalised formula
so similar chemical properties
Hydrocarbons = molecules made up of only carbon and hydrogen
Alkynes = triple C-C bonds
Aliphatic = Carbon atoms joined in straight unbranched chains
Alicyclic = Carbon atoms joined in rings
prefix - cyclo
Aromatic = contains a benzene ring
unreactive as each carbon has only 1 electron not used for bonding
Functional group = group of atoms added onto a carbon chain responsible for reactivity
Naming
1) Identify longest continuous carbon chain
2) Identify any side chains ( meth, eth, prop show how long and 'thyl' shows its a side chain)
3) Use numbers to show where on the parent chain, the side chains are positioned
Number as low as possible
If 2 possible parent chains, choose the one with most branches
Halogenalkanes prefix-
Fluoro
Chloro
Bromo
Iodo
Alcohols suffix - ol
Aldehydes suffix -al
Ketones suffix -one
Carboxylic acids suffix - oic acid
Ester suffix - oate
Representing Formula
Molecular formula = shows number and type of atom, but not how they're joined
Empirical Formula = shows the simplest whole number ratio of atoms
General Formula = simplest formula for all members of a homologous series
Displayed Formula = shows all the bonds in a structure
Structural Formula = shows how atoms/ groups are arranged but NOT all the bonds e.g CH3(CH3)
Skeletal Formula = simplified carbon backbone
Isomerism
Structural Isomerism = same molecular formula but a different structural formula
Positional Isomers = same functional group can be at different positions along the carbon chain
Functional Isomers = different functional groups yet the same molecular formula
Reaction Mechanisms
Curly arrows represent the movement of electrons
single headed arrow represents the movement of a single electron
Homolytic bond fission
Bond breaks into 2 equal parts, each atom takes 1 electron from the shared bonds forming radicals
Radical = species with a single unpaired electron
Very reactive
Often photo-chemical / gaseous processes
this occurs with halogens with high UV energy
Heterolytic bond fission
Bond breaks unevenly, one atom takes both electrons forming ions
Often aqueous / polar bonds
show the steps of a reaction in electron and molecule transfer
Radical Substitiution
1) Initiation Step (forms radical)
2) Propogation (radical makes a new radical)
3) Chain reaction - unpredictable
Termination (radical meets another radical and s reaction stops)
Alkanes react with Halogens to produce Haloalkanes via Radical Substitution
end up with a mixture of products
Types of Reaction
Substitution (molecule is replaced for a more reactive one)
Elimination (small molecule removed from a larger one)
Addition (2 molecules reacting to form a 1 molecule)
Alkanes
CnH2n+2
Saturated
Hydrocarbons
Tetrahedral, 109.5
non-polar
Don't dissolve in water
bpt increases as chain increases
due to more points of contact so stronger IMF
C1-C4 are gaseous and fuels combust to produce lots of energy as exothermic
C5-C16 are colourless liquids
C17+ white waxy solids
sigma bonds = result from the direct overlap of 2 atomic
Alkenes
unsaturated
Hydrocarbons
CnH2n
Trigonal Planar 120
pi bonds = result from sideways overlap of p orbitals
pi bonds are weaker than sigma bonds
only occur in alkenes
alkenes are more reactive as pi bonds break and electrons can form new bonds
Stereoisomerism
same molecular and structural formula yet a different arrangement in space
Double bond means there is no free rotation
Cis / trans if one of the attached groups are Hydrogen
E/Z if the attached groups aren't hydrogen
Higher atomic number = higher priority
opposite sides = E
same side = Z
Reactions
Electrophile = Atom/ group of atoms attracted to an electron rich area accepting an electron pair to form a new bond
Electrophillic Addition
induced dipole causes heterolytic bond fission of Br2
causes a carbo - cation to be formed
needs UV light to occur to break halogen bond
Test for an alkene = turns bromine water colourless
Markownikoff's rule
2 step process with carbocation intermediate, the prefered route depends on stability
Most stable is a tertiary chain
Hydrogenation
When adding H2
Nickel Catalyst, 150 dC
causes an alkane to form, pack together better and more solid
With H20
produces a saturated alcohol
Phosphoric acid catalyst
high pressure
gaseous atoms, higher than 100 dC
Media attachments
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