Properties

Question 1

Alkanes

Answer 1

They have covalent sigma bonds
Boiling point increases as chain increases (Due to increased SA, so more London forces)
Generally insoluble
Fairly unreactive (C-C and C-H are strong, C-C bonds are strong and electronegativity between C and H are similar, so they aren’t polar)
If you branch your alkanes, boiling point decreases
Combustible
Can form haloalkanes (Free radical substitution)

Question 2

Alkenes

Answer 2

Unsaturated hyrdocarbons with C=C bond which is electron dense
They have Sigma + Pi bonds - Shaped like a “Hot dog”
Can undergo electrophilic addition with hydrogen, halogens and hydrogen halides
To test for alkenes, using bromine water will become discoloured if alkene is present, proving a C=C bond is present
Carbocation stability depends on how many alkyl groups are attached to the carbocation, the more alkyl groups, the more spread out the charge is
They can form polymers - A long chain of subsequent repeated units of monomers

Question 3

Alcohols

Answer 3

Polar due to OH functional group, can form hydrogen bonds with other alcohols
They are soluble, solubility decreases as chain increases
Have a relatively low volatility - they are likely to turn into a gas, as boiling points increase, volatility decreases
Can be primary, secondary, tertiary alcohols: Primary - attached to 1 alkyl group and 2/3 H, secondary - attached to 2 alkyl groups and 1 H, tertiary - attached to no H and 3 alkyl groups
They combust and can be oxidized with acidified K2Cr207*H2SO4
Primary = Aldehydes/Carboxylic (Distil)
Secondary = Ketones (Reflux)
Dehydration - Concentrated H3PO4/H2SO4
Form haloalkanes with hydrogen halides (nucleo.)

Question 4

Haloalkane

Answer 4

Become more reactive as you descend down group
Hydrolyse more quickly as you descend down group
Reactivity is determined by bond strength ie C-F is stronger than C-Cl
Have polar bonds
Forms compunds through nucleophilic substitution