Chapter 12: Properties of the alkanes Flashcards
What are alkanes?
- The main components of natural gas and crude oil
- Among the most stable organic compounds
- Their lack of reactivity has allowed crude oil deposits to remain in the earth for many millions of years
- They are mainly used in fuels
Bonding in alkanes
- Alkanes are saturated hydrocarbons, containing only carbon and hydrogen atoms joined together by single covalent bonds
- Each carbon atom in an alkane is joined to 4 other atoms by single covalent bonds
- These are a type of covalent bond called a sigma bond
What is a sigma bond?
- The result of the overlap of two orbitals, one from each bonding atom
- Each overlapping orbital contains one electron, so the sigma bond has two electrons that are shared between the bonding atoms
Each carbon atom in an alkane has how many sigma bonds
4 sigma bonds
- Either C-C or C-H
- Each sigma bond acts as axes around which the atoms can rotate freely, these shapes are not rigid
The shape of alkanes
- Each carbon atom is surrounded by four electron pairs in four sigma bonds
- Repulsion between these electron pairs results in 3D tetrahedral arrangement around each carbon atom
- Each bond is approximately 109.5 degrees
Briefly describe fractional distillation
- Oil refineries separate the crude oil into fractions by fractional distillation in a distillation towers
- Each fraction contains a range of alkanes
- Separate like this is possible because the boiling points of the alkanes are different, increasing as their chain length increases
Why does boiling point of alkanes increase?
- The answer lies with the weak intermolecular forces called London forces
- These forces hold molecules together in solids and liquids but, once broken, the molecules move apart from each other and the alkane becomes a gas
- The greater the intermolecular forces, the higher the boiling point
Effect of chain length on boiling point
- London forces act between molecules that are in close surface contact
- As the chain length increases, the molecules have a larger surface area, so more surface contact is possible between molecules
- The london forces between the molecules will be greater and so more energy is required to overcome the forces
The effect of branching on boiling point
- Isomers of alkanes have the same molecular mass
- If you compare the boiling points of branched isomers with straight-chain isomers, you find that the branched isomers have lower boiling points
Explain the effect on boiling point
- The reason for this difference lies again London forces
- There are fewer surface points of contact between molecules of the branched alkanes, giving fewer London forces
- Another factor lies with the shape of the molecules
- The branches get in the way and prevent the branched molecules getting as close together as straight-chained molecules, decreasing the intermolecular forces further
Reactivity of alkanes
- Alkanes do not react with most common reagents. The reasons for their lack of reactivity are:
- C-C and C-H sigma bonds are strong
- C-C bonds are non-polar
- The electronegativity of carbon and hydrogen is so similar that the C-H bond can be considered to be non-polar
Combustion of alkanes
- Despite their low reactivity, all alkanes react with a plentiful supply of oxygen to produce carbon dioxide and water
- This reaction is called combustion
- All combustion processes give out heat, and alkanes are used as fuels because they are readily available, easy to transport
In a plentiful supply of oxygen, alkanes burn completely. What does this produce
Carbon dioxide + water
Incomplete combustion of alkanes
- In a limited supply of oxygen, there is not enough oxygen for complete combustion
- Carbon monoxide is produced
Reactions of alkanes with halogens
- In the presence of sunlight, alkanes react with halogens
- The high-energy ultraviolet radiation present in sunlight provides the initial energy for a reaction to take place
- This is a substitution reaction
The mechanism for the bromination of methane is an example of what?
radical substitution
Mechanism for bromination of alkanes: Step 1 (Initiation)
- The covalent bond in the bromine molecule is broken by homolytic fission
- Each bromine atom takes one electron from the pair, forming two highly reactive bromine radicals
- The energy for this bond fission is provided by UV radiation
Mechanism for bromination of alkanes: Step 2 Propogation
- In the first propagation step, a bromine radical, reacts with a C-H bond in the methane, forming a methyl radical and a molecule of HBr
- In the second propogation each methyl radical reacts with another bromine molecule, forming the organic product bromoethane, CH3Br, together with a new bromine radical
When is propogation terminated?
When two radicals collide
Describe termination
- Two radicals collide, forming a molecule with all electrons
paired - When two radicals collide and react, both radicals are removed removed from the reaction mixture, stopping the reaction
Limitations of radical substitution in organic synthesis
- Although radical substation gives us a way of making haloalkanes this reaction has problems that limit it’s importance for synthesis of just one organic compound
Further substitution
- In the mechanism above, bromoethane, CH3Br, was formed in the second propogation step
- Another bromine radical can collide with a bromoethane molecule, substituting a further hydrogen atom to form dibromoethane, CH2Br
- Further substitution can continue until all hydrogen atoms have been substituted
- The result is a mixture of CH3Br, CH2Br, CHBr3 and CBbr4
Substitution at different points in the carbon chain
- For methane, all four hydrogen atoms are bonded to the same carbon atom, so only one monobromo compound, CH3Br is possible
- With ethane, similarly only one monosaturated C2H5Br is possible
- If the carbon chain is longer, we will get a mixture of monosubstituted isomers by substitution at different positions in the carbon chain