Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
41 Cards in this Set
- Front
- Back
Homologous series definition |
A family of organic compounds with the same function group, in which each successive member increases by a CH₂ unit |
|
Alkyl functional group |
CₓH₂ₓ₊₁ |
|
What is the functional group responsible for? |
A compound’s reactivity |
|
Methyl |
CH₃ |
|
Ethyl |
C₂H₅ |
|
Saturated definition |
Doesn’t contain a C=C |
|
Unsaturated definition |
Contains a C=C |
|
Aliphatic definition |
Hydrocarbon where the carbons are joined in straight unbranched or branched chains |
|
Alicyclic definition |
Hydrocarbons where the carbon atoms are joined together in a non-aromatic ring structure |
|
aromatic definition |
Hydrocarbons with a benzene (C₆H₆) ring structure |
|
general formula of alkenes |
CnH2n |
|
functional group of alkenes |
C=C |
|
are alkenes saturated or unsaturated |
unsaturated |
|
what does the C=C do to the atoms the carbons are bonded with? |
holds the atoms in a fixed position - no rotation around the double bond |
|
sigma (σ) bond |
covalent bonds formed by the head-on overlapping of two orbitals - increased electron density between the nuclei - the strongest type of covalent bond |
|
pi (π) bond |
a covalent bond formed by the sideways overlapping of two p orbitals - increased electron density above and below the plane of carbon atoms |
|
how does the C=C form in alkenes? |
- each carbon forms 3 σ bonds (with two hydrogens and another carbon) - the last electron in the outer shell of each carbon is in a p orbital - these p orbitals form a π bond as the second bond in the C=C |
|
why are alkenes more reactive than alkanes? |
the pi bond in the C=C is weaker than the sigma bonds so it beaks easier to react |
|
heterolytic fission |
when a bond breaks and one atom takes both electrons - forms a negative ion and a positive ion |
|
homolytic fission |
when a bond breaks and each atom takes one of the electrons in the pair - forms two radicals |
|
radical definition |
a species with an unpaired electron |
|
electrophile definition |
an atom/group of atoms which is attracted to an electron dense centre/atom where it accepts a pair of electrons to form a covalent bond |
|
electrophilic addition definition |
an addition reaction where the first step is attack by an electrophile on a region of high electron density |
|
which molecules undergo electrophilic addition reactions |
alkenes |
|
electrophilic addition reactions of alkenes |
- hydrogenation - hydration - alkene + hydrogen halide - halogenation |
|
hydrogenation of alkenes |
alkene + H₂ → alkane - needs a nickel catalyst and 423K |
|
kelvin to celcius |
OK = -273°C |
|
halogenation of alkenes |
alkene + halogen → haloalkane - needs RTP |
|
addition definition |
when molecules are added to an unsaturated molecule to make one saturated product |
|
hydration of alkenes |
alkene + water (g) → alcohol - needs phosphoric acid catalyst and steam |
|
addition polymerisation of alkenes |
- pi bond breaks so the electrons can bond with a neighbouring carbon atom - draw alkene with the C=C in the centre and alkyl groups around monomer → poly(monomer) |
|
how many carbon atoms are in a repeat unit of a polymer |
2 in the middle (not part of alkyl groups) |
|
carbocation stability |
the carbon with the most alkyl groups around it is the most stable and will form a carbocation - forms the major product e.g. propene + bromine - can have 1-bromopropane or 2-bromopropane - the 2nd carbon has 2 methyl groups but the 1st only has 1 ethyl - secondary carbocation is more stable so 2-bromopropane is the major product |
|
incineration of polymers |
Polymers that cannot be recycled (made from petroleum or natural gas - high energy level) are incinerated and used to produce heat and electricity |
|
pros of recycling polymers |
conserves finite resources and reduces the amount in landfill |
|
what are alkene polymers derived from? |
usually crude oil which is finite |
|
why are alkene-based polymers used |
unreactive so it's suitable for storing food and medicines |
|
cons of alkene-based polymers |
non-biodegradable kill marine life |
|
feedstock |
breaking down polymers into starting materials to form new polymers - can use unsorted or unwashed ones unlike with recycling |
|
bioplastics and biodegradable polymers |
polymers made from plant starch, cellulose, oils - renewable - sustainable - break down so environment isn't damaged |
|
photodegradable polymers |
adding UV light to polymers breaks bonds and starts the degradation process |