Chapter 13 Alkenes Flashcards

1
Q

Alkenes

A
  • Unsaturated hydrocarbons (at least 1 C=C bond)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

General formula of alkenes

A
  • CnH2n
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

The nature of the C=C bond

A
  • C has 4 electrons and 3 are used in sigma bonds (1 to the other C and the other 2 for other atoms)
  • The remaining electron is a pi bond
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

pi bond formation

A

Formed by the sideways overlap of 2 electrons in the p-orbitals (one from each C of the C=C bond)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Where is the pi-electron density concentrated

A

above and below the line joining the nuclei of the bonding atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What does the pi bond do to the C atoms

A

Locks the C atoms in positions and prevents them from rotating around the C=C bond -> geometry of alkenes is different to that of alkanes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Alkenes in the natural world

A
  • Carotene = makes flamingos pink
  • Limonene = causes scent of oranges and lemon
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Stereoisomers

A

Have the same structural formula but a different arrangement of the atoms in space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Types of stereoisomerism

A
  • E/Z isomerism
  • Optical isomerism
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why does stereoisomerism occur?

A

The rotation around the C=C bond is restricted so the groups attached to those Cs are therefore fixed relative to eachother

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

When will a molecule have E/Z isomerism

A

When the molecule has:
* A C=C bond (restricted rotation)
* 2 different groups attached to each C atom of C=C bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Cis-trans isomerism

A
  • Special case of E/Z isomerism
  • Same requirements as E/Z isomerism but one of the attached groups on each C atom of the C=Cmust be the same
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Relationship between cis/trans isomerism and E/Z isomerism

A

When there is a H on each C=C bond
* Cis isomer = Z isomer
* Trans isomer = E isomer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Cahn-Ingold-Prelog Rules

A
  • Z isomer: If the groups of highest priority are on the same side of the C=C bond
  • E isomer: If the groups of highest priority are diagonally places across the C=C bond
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

How to assign priority

A
  • As atomic number increases, priority increases
  • If it is a large atom, find the first point of difference and use this to compare priority
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Why are alkenes much more reactive than alkanes

A

pi bond -> the electrons in the pi bond are more exposed than the electrons in the sigma bond. The pi bond readily breaks and alkenes undergo addition reactions relatively easily

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Addition reactions of the alkenes

A
  • hydrogen in the presence of a nickel catalyst
  • halogens
  • hydrogen halides
  • steam in the presence of an acid catalyst
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Hydrogenation of alkenes

A

Alkene + hydrogen -> alkane

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is the product of an addition reaction?

A

Always saturated

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Halogenation of alkenes

A

Alkene + bromine -> dihaloalkane

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Test for unsaturation (C=C bond)

A

Add bromine water
orange -> colourless

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Hydrogen halides

A

Hydrogen + halogen
e.g. HCl

23
Q

Alkenes + hydrogen halides

A

haloalkane

24
Q

Hydration of alkenes

A

Alkene + Water -> alcohol

25
Electrophilic addition
Reaction mechanism for addition reactions of alkenes
26
Electrophile
* Electron pair acceptor (attracted to an electron-rich centre) * Usually a positive ion, or a molecule containing an atom with a δ+ charge
27
Reaction between but-2-ene + hydrogen bromide
1. Bromine is more electronegative than hydrogen, so hydrogen bromide is polar (contains dipole Hδ+ - Brδ-) 2. The electron pair in the pi bond is attracted to the Hδ+ -> causes the double bond to break 3. A bond forms between the H of the H-Br and a C that was part of the C=C bond 4. The H-Br bond breaks by heterolytic fission, with the electron pair going to the bromine atom 5. A Br- ion and carbocation are formed. These react together to form the addition product
28
How does polarisation of bromine occur (bromine is a non-polar molecule)
The pi electrons interact with the electrons in the Br-Br bond -> causes Brδ+ -Brδ-
29
Markownikoff's rule
When a hydrogen halide reacts with an unsymmetrical alkene, the hydrogen from the hydrogen halide attaches to the carbon with more hydrogen and less carbon
30
Steps of electrophilic addition
Sometimes, 3 different carbocations can be produced: * Primary carbocation (has 1 alkyl group) * Secondary carbocation (has 2 alkyl groups) * Tertiary carbocation (has 3 alkyl groups)
31
R
Alkyl group
32
Polymers
Extremely large molecules from many repeat units (monomers)
33
What polymerisation do alkenes undergo?
Addition polymerisation -> produces long chains of saturated chains with no C=C bonds
34
Characteristics of addition polymers
* High molecular masses * Have prefix poly-
35
Examples of synthetic addition polymers
* Poly(ethene) * Poly(chloroethene) * Poly(propene) * Poly(styrene) * Poly(tetrafluoroethene)
36
Environmental concerns of polymers
* Disposing of waste polymers * Recycling * PVC recycling * Using waste polymers as fuel * Feedstock recycling
37
Biodegradable and photodegradable polymers
* Biodegradable polymers * Photodegradable polymers
38
Environmental concerns of polymers: Recycling
Reduces environmental impact by conserving finite fossil fuels and decreasing amount of waste going to landfill
39
Environmental concerns of polymers: PVC recycling
Disposal and recycling of PVC is hazardous due to high chlorine and additive content * New technology uses solvents to dissolve the polymer
40
Environmental concerns of polymers: Using waste polymers as fuel
As polymers are derived from natural gas, they have a high stored energy value -> so can be incinerated to produce heat -> electricity
41
Environmental concerns of polymers: Feedstock recycling
Describes the chemical + thermal processes that can reclaim monomers, gases or oil from waste polymers
42
Advantage of feedstock recycling
Can handle unsorted and unwashed polymers
43
Bioplastics
* Produced from plant starch, cellulose, plant oils and proteins * Offer a renewable + sustainable alternative to oil-based product, and protects our environment and conserves our valuable oil reserves
44
Biodegradable polymers
* Broken down by microorganisms into water, carbon dioxide and biological compounds
45
What are compostable polymers
Based on poly(lactic acid)
46
Photodegradable polymers
Contain bonds that are weakened by absorbing light to start the degradation
47
Catalyst for hydration of alkenes
Phosphoric acid
48
Differences between sigma bonds and pi bonds
* pi bond is weaker than sigma bonds * pi bond is above and below the bonding atoms whereas sigma bond is between bonding atoms
49
When there is a possibility for different haloalkanes to be produced in a reaction, which one will be produced in greater quantity?
The tertiary haloalkane because it is more stable than the secondary and primary haloalkane
50
Advantages of combusting polymers
Produces electricity
51
Disadvantages of combusting polymers
Produces Hcl or chlorine (however this can be neutralised using an alkali)
52
Bonding angle around addition polymer
Tetrahedral 109.5
53