Alkanes Flashcards
Alkanes
Main component of natural gas, crude oil
Most stable organic compound
Cn H2n+2
Uses
Domestic fuel, CH4
Petrol, C5H12
Kerosene, C10H22
Diesel, C12H26
Alkanes bonding
Saturated hydrocarbon Single covalent bond joined to 4 atoms, Sigma bond results in the overlap of 2 orbitals Each overlapping orbital has1 electron 4 sigma bonds per C
Alkanes shape
4 electron pairs, 4 sigma bonds, axis where atoms rotate freely into different shapes
Tetrahedral, 109.5
Boiling points of alkanes
Fractional distillation separates alkanes possible due to its boiling points
Chain length increases, boiling point increases
Chain length increases, surface area increases, more surface contact possible between molecules, more force needed to overcome London Forces
Branching on boiling point
Branched isomers have lower boiling point
Fewer surface points of contact between molecules, fewer London forces
Branches get in the way, prevent branched molecules getting close as straight chain molecules, decrease intermolecular forces
Reactivity of alkanes
Not reactive with most reagents
Strong sigma bonds
C-C, non polar bonds
Electronegativity of C, H are similar, not polar
Combustion of alkanes, complete
Alkanes + Oxygen => Carbon dioxide +Water
Incomplete combustion
Hydrogen in alkane oxidised to H2O
Result in CO and water/ Carbon and water
Effects of carbon monoxide
Combines irreversibly with haemoglobin to form carboxyhaemoglobin
Reactions of alkanes with halogens
UV radiation provides initial energy for reaction
Forms haloalkanes
Radical substitution
Bromination of alkanes, show movement of electrons during reaction
Initiation reaction
Covalent bond broken by homolytic fission
Very reactive radicals
Propagation reaction
Chain reactions
Start and end with a radical
Termination reactions
2 radicals collide, forms molecules, ends reactions