# data[].attributes.body
Double bonds are used to join monomers and only one product forms

# data[].attributes.body
Example- Plastics

A very large molecule made up of many repeating units or blocks

We make polymers by joining up (polymerisation) hundreds or thousands of small reactive molecules called monomers.

Ethene  —> polyethene (polythene)
Conditions : 2000atm, 200 degrees Celsius, trace of oxygen

# data[].attributes.body
Catalytic Hydrogenation
Hydrogenation of Ethane
Reagent : Hydrogen
Catalyst: Nickel (Ni)
Conditions: 140 degrees Celsius temperature
C₂H₄ + H₂ —> C₂H₆
Heterogeneous catalyst: Catalyst and reactants are in different states
Uses - Liquid vegetable oils (polyunsaturates- has multiple bonds) can be made saturated by adding hydrogen. This hardens the oil to make margarine.

# data[].attributes.body
Order of Stability
Most: Tertairy carbocation
Secondary carbocation
Least: Primary carbocation

# data[].attributes.body
A positively charge carbon-containing ion.

# data[].attributes.body
Reagent: Bromine Water
Observation: Colour change from orange/yellow to colourless
OR
Reagent: Acidified potassium manganate (VII)
Observation: Colour change from purple to colourless

# data[].attributes.body
Occurs in alkenes and substituted alkenes due to restricted rotation around the C=C double bond

Identifying E or Z
Look at the atoms/groups at earthier end of the double bond
Rank the atoms/groups, taking. The atoms with higher atomic numbers as the most important
Define the isomer as either
Z isomer - higher priority atoms/groups are on the same side of the double bond
E isomer - Higher priority atoms/ groups are on opposite sides of the double bond.

# data[].attributes.body
Alkenes are much more reactive than alkanes due to the C=C bond in the alkenes being a region of high electron density

# data[].attributes.body
A compound of hydrogen and carbon containing no C to C multiple bonds.

# data[].attributes.body
A compound of hydrogen and carbon containing C to C multiple bonds

# data[].attributes.body
Halogenation
Example - Photochlorination of Chlorine
Stage 1: Initiation - Start the mechanism by making radicals
Stage 2: Propahation- Continue the mechanism
In general: Radical + Molecule —> New molecule + New Radical
Stage 3: Termination - Remove radicals and stop

# data[].attributes.headline
Benefits and Drawbacks of using fossil fules

# data[].attributes.subject
Benefits and Drawbacks of using fossil fules

# data[].attributes.body
Benefits

More reliable- eco friendly methods, eg. wind, solar, aren't alwas available

Produce lots of energy

Provides jobs- in power plants and extracting fuel

Many forms of fossil fuels- can be used for different things

Drawbacks

Non-renewable- will run out eventually

When burnt, they release CO (carbon monoxide) which is toxic to humans

Release CO₂ (carbon dioxide) which has a negative impact on global warming.

Disrupts the natural environment to access fuels

Expensive to get materials and transfer them into energy - powerplants

Can create acid rain which can damage buildings

# data[].attributes.body
If there is enough oxygen we get complete combustion with carbon dioxide and water as products

If there is insufficient oxygen, incomplete combustion occurs and carbon monoxide is made.