Alkenes And Addition Polymers Flashcards
What are alkenes?
•Unsaturated hydrocarbons- they have one or more carbon-carbon double bond.
Are alkenes more reactive than alkanes?
•Yes.
Why are alkenes more reactive than alkanes?
•The double bond makes them more reactive due to the high concentration of electrons (high electron density) between the two carbon atoms.
What is ethene a starting material for? (3)
- Polymers e.g. polyethene, PVC, polystyrene and terylene fabric.
- Antifreeze.
- Paints.
How are alkenes produced?
•In large quantities when crude oil is thermally cracked.
What is the general formula of alkenes?
•CnH2n.
How do you name alkenes? (2)
- The same way alkanes are names but use ‘ene’ ending.
* Use a number to show where the double bond is.
What kind of shape are alkenes?
•Planar (flat)- the double bond prevents the rotation.
Draw the shape of ethene. (2)
•Planar molecule.
•Each bond angle is roughly 120 degrees.
(See textbook page 216)
Why can’t double bonds rotate? (3)
•As well as a normal C-C single bond, there is a p-orbital (which contains a single electron) on each carbon.
•These two orbitals overlap to form an orbital with a cloud of electron density above and below the single bond (π-orbital, its presence means the bond cannot rotate).
•Also known as restricted rotation.
(See textbook page 217)
Alkenes with more than three carbons form… (3)
- Chain isomers.
- Position isomers.
- Geometrical isomers.
What are position isomers?
•Isomers with the double bond in different positions, between a pair of adjacent carbon atoms in different positions in the carbon chain.
Give an example of a position isomer for C4H8. (Draw diagram)
•But-2-ene and but-1-ene.
What is geometrical isomers? (3)
- A form of stereoisomerism.
- The two stereoisomers have the same structural formula but the bonds are arranged differently in space.
- It occurs only around the C=C double bonds.
Give an example of geometrical isomerism for C4H8. (Draw diagram)
•Z-but-2-ene and E-but-2-ene.
What are the physical properties of alkenes? (3)
- The double bond doesn’t greatly affect properties such as boiling and melting points.
- vdW forces are the only IMF between alkene molecules- the more carbon atoms, the higher the melting and boiling points.
- Insoluble in water.
How does the double bond affect the reactivity of alkenes?
•It increases the bond enthalpy (consists of sigma (σ) and pi bonds (π))- the C=C forms an electron-rich area in the molecule, which can easily be attacked by positively charged reagents (electrophiles).
What are electrophiles?
•Electron pair acceptors.
Give an example of an electrophile.
•H^+ ion.
What reactions do alkenes undergo? (2)
- Electrophilic additions.
* Combustion.
Explain why the π part of the bond is weaker than the σ part.
•The electron density in the σ^- orbital is connected between the nuclei and holds them together better than the electron density of π-orbital, which is above and below the plane of the molecule.
Draw/write an equation for the combustion reaction of ethene.
(See textbook page 220)
Why are alkenes not usually used as fuels?
•Their reactivity makes them very useful for other purposes.
Why are reactions of alkenes typically electrophilic addition reactions? (2)
- The four electrons in the C=C make it a centre of high electron density.
- Electrophiles are attracted to it and can form a bond by using two of the four electrons in the C=C (of the four electrons, the two that are in a π-bond.
What is the mechanism for electrophilic addition? (4)
- 1). The electrophile is attracted to the double bond.
- 2). Electrophiles are positively charged and accept a pair of electrons from the double bond. The electrophile may be a positively charged ion of have a positively charged area.
- 3). A positive ion (a carbocation) is formed.
- 4). A negatively charged ion forms a bond with the carbocation.
How do alkenes react with hydrogen halides?
•E.g. HCl, HBr and HI add across the double bond to form a halogenoalkane.
Draw and explain the mechanism of the electrophilic addition of ethene with hydrogen bromide. (7)
•Bromine is more electronegative than hydrogen, so the hydrogen bromide molecule is polar, H^𝛿+—Br^𝛿-.
•The electrophile is the H^𝛿+ of the H^𝛿+—Br^𝛿-.
•The H^𝛿+ of HBr is attracted to the C=C bond because of the double bond’s high electron density.
•One of the pairs of electrons from the C=C forms a bond with the H^𝛿+ to form a positive ion (called a carbocation), whilst at the same time the electrons in the H^𝛿+—Br^𝛿- bond are drawn towards the Br^𝛿-.
•The bond in hydrogen bromide breaks heterolytically.
•Both electrons from the shared pair of in the bond fo to the bromine atom because it is more electronegative than hydrogen leaving a Br^- ion.
•The Br^- ion attaches to the positively charged carbon of the carbocation forming a bond with one of its electron pairs.
(See textbook page 220)
What happens during electrophilic addition when there are asymmetrical alkenes?
•When the double bond is not exactly in the middle of the chain there are two possible products- the bromine of the hydrogen bromide could bond to either of the carbon atoms of the double bond.