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Alevel Chemistry OCR A > Module 4: Section 1- Basic Concepts And Hydrocarbons > Flashcards

Module 4: Section 1- Basic Concepts And Hydrocarbons Flashcards

1
Q

Organic basics
What are the 6 types of formula

A

General
Empirical
Structural
Displayed
Skeletal
Molecular

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2
Q

Organic basics
What is a general formula

A

Algebraic formula can describe any member of a family of compounds

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3
Q

Organic basics
What does an empirical formula show

A

Simplest whole number ratio of atoms of each element is a compound

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4
Q

What is a molecular formula

A

Actual number of atoms in a molecule

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5
Q

Organic basics
What is the displayed formula

A

Shows how atoms are arranged and all the bonds between them

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6
Q

Organic basics
What is the skeletal formula

A

Shows bonds of carbon skeleton only with any functional groups
Carbon and hydrogen atoms aren’t show
Each point represents a carbon

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7
Q

Organic basics
Define functional group

A

Feature of a molecule which defines its characteristic reactions

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8
Q

Organic basics
Define homologous series

A

Group of organic molecules with the same functional group and same general formula where each successive member increased by CH2

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9
Q

Organic basics
Prefix or suffix for alkanes

A

-ane

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10
Q

Organic basics
Prefix or suffix for branched alkanes

A

Alkyl-(-yl)

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11
Q

Organic basics
Prefix or suffix for alkenes

A

-ene

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12
Q

Organic basics
Prefix or suffix for haloalkanes

A

Chloro-/bromo-/iodo-

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13
Q

Organic basics
Prefix or suffix for alcohols

A

-ol/hydroxy-

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14
Q

Organic basics
Prefix or suffix for aldehydes

A

-al

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15
Q

Organic basics
Prefix or suffix for ketones

A

-one

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16
Q

Organic basics
Prefix or suffix for cycloalkanes

A

Cyclo-…-ane

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17
Q

Organic basics
Prefix or suffix for carboxylic acids

A

-oic acid

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18
Q

Organic basics
Prefix or suffix for esters

A

Alkyl- … -anoate

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19
Q

Organic basics
What’s doe unsaturated mean

A

Prescience of double bonds

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20
Q

Organic basics
What does saturated mean

A

All single bonds

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21
Q

Organic basics
What does aliphatic mean

A

anything with a chain of carbons

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22
Q

Organic basics
What does alicyclic mean

A

Cyclic of carbon

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23
Q

Organic basics
What does aromatic mean

A

Delocalised pi system (mostly in y13)

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24
Q

Organic basics
What is an alkyl group

A

Forage,nt of a molecule with general formula Cn H2n+1

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25
Organic basics What is nomenclature
Naming organic compounds
26
Organic basics What is IUPAC
Naming system for organic compound which was invented as an international language for chemistry and can be sued for any organic compound a systematic name using the rules
27
Organic basics Number of carbon - name stem (1-4
1 is meth- 2 is eth- 3 is prop- 4 is but-
28
Organic basics Number of carbons -stem (5-10
5 is pent- 6 is hex- 7 is hept- 8 is oct- 9 is non- 10 is dec-
29
Organic basics What gives the prefix or suffix
Main functional group usually tell you what homologous series the molecule is is and so the prefix or suffix
30
Organic basics IUPAC rule for numbers
Number the longest carbon chain so that the main functional group has the lowest possible number
31
Organic basics What are side chains or less important functional groups added as
Prefixes in alphabetical order after the number of carbon atom each it’d attached to
32
Organic basics What do you do if there’s more than one side chain or functional group
Use di-(2), tri- (3), or tetra- (4) before that part of the name
33
Isomers What are isomers
Two molecules are isomers if they have the same molecular formula but atoms are arranged differently
34
Isomers What are the two types of isomers
Structural isomers and stereoisomers
35
Isomers What are structural isomers
Compounds with the same molecular formulas but different structural formulae
36
Isomers What’s are the three types of structural isomers
Chain isomers Positional isomers Functional group isomers
37
Isomers What are chain isomers
When the carbon skeleton is arranged differently eg straight chain or branched in different ways
38
Isomers Effect of chain isomers on properties
Isomers have similar chemical properties by their physical properties such as boiling point will be different
39
Isomers Why do chain isomers have different physical properties
Because of the change in the shape of the molecule
40
Isomers What are positional isomers
Skeleton and the functional group could be the same only with the functional group attached to a different carbon atom
41
Isomers Effect of positional isomers on characteristics
Different physical properties and the chemical properties might be different too
42
Isomers What are futnional group isomers
Same atoms can be arranged into different functional groups
43
Isomers Effect of functional group isomers on characteristics
Different physical and chemical properties
44
Isomers What is a functional group isomer of aldehyde
Ketone
45
Isomers What is the functional group isomer of carboxylic acid
Ester
46
Isomers What is the functional group isomer of alkenes
Cycloalkanes
47
Isomers What is the functional group isomer of ketones
Aldehydes
48
Isomers What is the functional group isomer of esters
Carboxylic acids
49
Isomers What is the functional group isomer of cycloalkanes
Alkenes
50
Alkanes What is the general formula of alkanes
CnH2n+2
51
Alkanes What are alkanes
Saturated hydrocarbons
52
Alkanes What shape is around each carbon and bond angle
Tetrahedral 109.5
53
Alkanes What are the bonds called in alkanes
Covalent specifically Sigma bonds
54
Alkanes What are sigma bonds
Overlap of orbitals directly between the bonding atoms
55
Alkanes What are the standard states of alkanes
CH4 to C4H10 aregases C5H12 to C17H36 are liquids C18H38 above are solids
56
Alkanes What are between the molecules
London forces which hold them together
57
Alkanes Why happens to the boiling point as the carbon chain gets longer
Increases
58
Alkanes Why does the boiling point increase as the boiling point gets longer
Longer chain, stronger London forces because of more surface contact so more electrons to interrupt, takes more energy to overcome the imf
59
Alkanes Why does a branched chain alkane have lower boiling point than a straight chain isomer
Can’t pack closely together and they have smaller molecular surface areas so the London forces are reduced
60
Alkanes What happens if you burn alkanes with oxygen and what type of reaction is it
Produce carbon dioxide and water Combustion reaction
61
Alkanes What’s the equation for complete combustion of propane
C3H8 (g) + 5 O2 (g) —> 3 CO2 (g) + 4 H2O (g)
62
Alkanes What state does combustion ave to happen between
Gases
63
Alkanes What has to be done to liquid alkanes before combustion
Have to be vaporised first
64
Alkanes Why doe smaller alkanes burn easier
They turn into gases more easily (more volatile)
65
Alkanes Why do larger alkanes releases more energy per mole
Have more bonds to break
66
Alkanes Why do alkanes make excellent fuels
Because they release so much energy when they burn
67
Alkanes What is a common question for alkanes
Using volumes to work out combustion equations
68
Alkanes How can you workout what hydrocarbon is combusting
All gases at the same temperature and pressure have the same molar volume, which means you can use the ratio of the volumes of gases reacting to calculate molar mass and workout the hydrocarbon
69
Alkanes What does incomplete combustion produce
Carbon monoxide and water
70
Alkanes Equation for burning methane with not enough oxygen
2 CH4 (g) + 3 O2 (g) —> 2 CO (g) + 4 H2O (g)
71
Alkanes What is the problem with incomplete production
It produced carbon monoxide which is poisonous
72
Alkanes Health impacts of carbon monoxide
The oxygen in your bloodstream is carried around by haemoglobin. Carbon monoxide is better at binding to haemoglobin than oxygen is, so it binds to the haemoglobin in your bloodstream before the oxygen can. This means that less oxygen can be carried around your body, leading to oxygen deprivation. At very high concentrations, carbon monoxide can be fatal.
73
Alkanes What are free radicals
Particles that have unpaired electrons
74
Alkanes What do alkanes react with
Free radicals
75
Alkanes What is bond fission
Breaking a covalent bonds
76
Alkanes What are the two types of bond fission
Homolytic and heterolytic
77
Alkane What happens in heterolytic fission
The bond breaks unevenly with one of the bonded atoms receiving both electrons from the bonded pair
78
Alkanes What’s formed from heterolytic fission
Two different substances, a positively charged cation (X+) and a negatively charged anion (Y-)
79
Alkanes Mechanism of heterolytic fission
X—:—Y -> X+ + Y- (Curly arrow from electrons in bond to the Y)
80
Alkanes What does a curly arrow show
The movement of an electron pair
81
Alkanes What happens in homolytic fission
Bond breaks evenly and each binding atom receives one electron from the bonded pair
82
Alkanes What’s formed from homolytic fission
Two electrically uncharged radicals
83
Alkanes What are radicals
Particles that have an unpaired electron
84
Alkanes How are radicals shown in mechanisms
By a big dot next to the molecular formula to represent the unpaired electron
85
Alkanes Mechanism for homolytic fission
X—:—Y -> X• + Y•
86
Alkanes Why are radicals very reactive
Because of the unpaired electron
87
Alkanes What’s formed when halogens react with alkanes
Haloalkanes
88
Alkanes What type of reaction os halogens reacting with alkane
Photochemical reactions
89
Alkanes How are photochemical reactions started
By light
90
Alkanes What is needed in photochemical reaction for halkoalkanes to be formed
Ultraviolet light
91
Alkanes What is substituted in the reaction to form a haloalkane and what is it called
Hydrogen atom is substituted by chlorine or bromine
92
Alkanes What dos the reaction of chlorine and methane form
Chloromethane and hydrochloric acid
93
Alkanes Equation for chlorine and Methane
CH4 + Cl2 —uv-> CH3Cl + HCl
94
Alkanes Whatare the three stages of the reaction mechanism for free radical substitution
Initiation reactions Propagation reactions Termination reactions
95
Alkanes What two halogens are needed to know
Chlorine and bromine (interchangeable
96
Alkanes What happens in the intimation reactions
Sunlight provides enough energy to break the Cl-Cl bond (photodissociation) Cl2 -uv-> 2 Cl• This is through homolytic fission and two highly reactive free radicals are formed Cl• because of its unpaired electron
97
Alkanes What happens in the propagation reactions of free radical substitutions
Cl• attacks a methane molecule: Cl• + CH4 —> •CH3 +HCl The new methyl free radical •CH3 can attack another Cl2 molecule: •CH3 + Cl2 —> CH3Cl + Cl• The new Cl• can attack another CH4 molecules and so on until all the Cl2 or CH4 molecules are wiped out
98
Alkanes What happens in termination of free radical substitution
If two few radicals join together a stable molecule is formed so there are heaps of possible termination reactions such as Cl• + •CH3 —> CH3Cl •CH3 + •CH3 —> C2H6
99
Alkanes What are the two problem of free radical substitution in organic synthesis
-Further substitution produces a mixture of products -substitution can occur at different positions in the carbon chain producing isomers
100
Basics of reactions What’s an addition reaction
When two reactants joint together to form one product
101
Basics of reactions What is a substitution reaction
Atom or group of atoms is replaced by A different atom or group of atoms
102
Alkanes What is thermal decomposition and what is it know as in alkanes
Using heat to break up a substance Cracking
103
Basics of reactions What is produced in thermal decomposition (cracking)
Long chains —> shorter chain alkanes + alkenes
104
Properties of Alkenes What are alkenes
Unsaturated hydrocarbons
105
Properties of Alkenes What is unique about alkenes
Contain at least one carbon carbon double bond in the structure
106
Properties of Alkenes What us the general formula of aliphatic alkenes
CnH2n
107
Properties of Alkenes What can be true of alkenes
They can be branched contain more than one double bond or be cyclic General formula only applied to branched and aliphatic alkenes
108
Properties of Alkenes What is the bonding on the carbon atom of the double bond
Three of the four electrons are used in three sigma bonds, and one of the four electrons in a pi bond
109
Properties of Alkenes How does the double bond structure
First sigma bond between the two carbons formed then one electron left which is in a p orbital. A pi bond is formed by the sideways overlap of the 2 p orbitals one from each carbon atom in the double bond
110
Properties of Alkenes Why is there a high pi electron density in the double bond
Electrons concentrated around the line joining the nuclei of the bonded atoms
111
Properties of Alkenes What is true of pi bond but not sigma bonds
Sigma bonds are freely rotating but pi bonds lock the two carbon atoms in position and restrict rotation around the double bond
112
Properties of Alkenes What is the shape around each of the carbon atoms in the double bond
Trigonal planar
113
Properties of Alkenes What are the bond angles around the a carbon atom in the double bond
120 degrees
114
Properties of Alkenes Why is the shape around the carbon atom in a double bond Trigonal planar
Because there are three regions of electron density around each of the carbon atoms The three regions repel each other as far as possible resulting in the 120 degree bond angle All atoms are on the same plane
115
Properties of alkenes How can you test for alkenes
Using bromine water
116
Properties of alkenes Positive test for alkenes using bromine water
Causes bromine water to chnage from orange-brown colour to colourless
117
Properties of alkenes Why does bromine water go colourless in alkenes
Bromine forms bonds to the carbon atoms removing the double carbon bond causing it to be saturated
118
Alkenes, stereoisomerism What are stereoisomers
Have the same structural formula but different arrangement of atoms in space
119
Alkenes, stereoisomerism What are the two types of stereosisomerism
E/Z isomerism and optical isomerism
120
Alkenes, stereoisomerism When can E/Z isomerism only occur
In compounds with a C=C double bond and different group attached to each carbon in the double bond
121
Alkenes, stereoisomerism When can optical isomerism occur
In a wider range of compound including alkanes with not functional group
122
Alkenes, stereoisomerism Why does stereoisomerism aris around double bonds
Because rotation about the double bond is restricted and the groups attached to each carbon atoms are therefore fixed relative to each other
123
Alkenes, stereoisomerism What two conditions does a molecule have to satisfy to have E/Z isomerisms
-a C=C double bond -different groups attached to each carbon atom of the double bond
124
Alkenes, stereoisomerism What is true of the E isomers
High priority groups are apart (one above one below) of the C=C double bond
125
Alkenes, stereoisomerism What is true of Z isomers
High priority groups are on the same side of the C=C double bond
126
Alkenes, stereoisomerism What is Cis-trains isomerism
a special case of E/Z isomerism where molecules must fit the basic two conditions of E/Z isomers but also one of the attached groups on each carbon of the double bond must be the same
127
Alkenes, stereoisomerism What is the cis isomer
When groups are on the same side of the molecule
128
Alkenes, stereoisomerism What is the trans molecules
When the groups are on opposite sides
129
Alkenes, stereoisomerism What is true when there is a hydrogen on each of the double bonded carbon atoms in cis-trans isomerism
The cis isomer is the Z isomer The trans isomer is the E isomer
130
Alkenes, stereoisomerism What are the Cahn-Ingold-Prelog rules
Naming system to give priority to groups in molecules that display E/Z isomers
131
Alkenes, stereoisomerism How do the CIP rules give priority’s to groups
Atoms or groups with higher Mr have priority
132
Alkenes, stereoisomerism Using the CIP rules to decide on the isomer
On either carbon of the double bond identify the highest priority group and the location of it in comparison to the other carbon atom then use either E/Z or cis-trans isomerism
133
Reactions of Alkenes Why are alkenes more reactive then alkanes
Because of the presence of the pi bond
134
Reactions of Alkenes Why does the pi bond mean alkenes undergo addition reactions relatively easily
Double bond made of a sigma and pi bond so pi electron density concentrated above and below plane of the sigma bond and the electrons are more exposed than the electrons in the sigma bond. Pi bond breaks easily so undergo addition reactions relatively easily
135
Reactions of Alkenes What is the bond enthalpy of a pi bond and what are the ramifications of this
Relatively low bond enthalpy so makes them relatively reactive
136
Reactions of Alkenes What happens in addition reaction
Involved addition of a small molecule across the double bond causing the pi bond to break and new bonds to form
137
Reactions of Alkenes Example of addditon reactions for alkenes
Hydrogen in prescient of nickel catalyst Halogen Hydrogen halides Steam in prescience of an acid catalyst
138
Reactions of Alkenes What is hydrogenation of alkenes
When mixed with hydrogen and passed over a nickel catalyst an addition reaction takes place to form an alkane
139
Reactions of Alkenes What is the definition of hydrogenation
When hydrogen is passed across a double bond and is added
140
Reactions of Alkenes Example fo hydrogenation of propene
CH3CHCH2 + H2 —> CH3CH2CH£
141
Reactions of Alkenes What is halogenation of alkenes
Addition reaction with halogens chlorine or bromine
142
Reactions of Alkenes Reaction for the bromination of propene
CH3CHCH2 + Br2 —> CH3CHBrCH2Br
143
Reactions of Alkenes What is catalytic hydrogenation used to manufacture
Margarine and unsaturated vegetable oils
144
Reactions of Alkenes What is the test for unsaturation
Bromine water added dropwise and turns colourless indicating presence of a C=C double bond
145
Reactions of Alkenes What is the addition reaction of alkenes with hydrogen halides
Alkenes react with gaseous halides at room temperature to form haloalkanes
146
Reactions of Alkenes What happens if the alkene is a gas and hydrogen a gas
Two gases are mixed
147
Reactions of Alkenes What happens if alkene if a liquid with hydrogen halide
Hydrogen halide bubbled throughout
148
Reactions of Alkenes What happens if alkenes react with concentrated hydrochloric or hydrobromic avid
They are solutions of hydrogen halides in water so form haloalkanes
149
Reactions of Alkenes What could happen if an unsymmetrical alkene reacts with an unsymmetrical compound
Two products could be made
150
Reactions of Alkenes What are hydration reactions of alkenes and what are the conditions
Alcohols formed when alkenes react with stream H2O (g) in presence of a pohosphoric acid catalyst
151
Reactions of Alkenes Where does steam add in a hydration reaction
Across the double bond
152
Reactions of Alkenes What is the hydration reaction used widely in
Industry to produce ethanol from ethene
153
Reactions of Alkenes What does the hydration reaction often result in
A mixture of alcohols
154
Reactions of Alkenes What’s the reaction between propene and steam in the presence of a phosphoric acid catalyst
Propene + H2O (g) —> propan-1-ol —> propan-2-ol
155
Electrophilic addition in alkenes What is electrophilic addition
Mechanisms that alkenes usually take part in addition reactions to form saturate compounds
156
Electrophilic addition in alkenes What does the double bond in an alkene represent
A region of high electron density because of the prescence of the pi-electrons
157
Electrophilic addition in alkenes What does the high electron density of the pi-electrons
Attracts electrophiles
158
Electrophilic addition in alkenes What are electrophiles defined as
Electron pair acceptor
159
Electrophilic addition in alkenes What are electrophiles actually
Atom or group of atoms that is attracted to an electron rich centre and accepts and electron pair
160
Electrophilic addition in alkenes What happens in an electrophilic addition reaction
Alkene double bond is an area of high electron density so it more susceptible to attack by electrophiles C=C bond breaks forming a single c-c bond and two new bonds from each of the carbon atom
161
Electrophilic addition in alkenes For hydrogen halides why is it polar
Hydrogen and halogen atoms have different electronegativity so halogen has delta negative charge and H has delta positive charge
162
Electrophilic addition in alkenes Why can hydrogen halide act as electrpphile
Delta positive hydrogen attracted to C=C double bond with high electron density
163
Electrophilic addition in alkenes What happens in an electrophilic addition of a hydrogen Halide
H atom acts as electrophilic by accepting pair of electrons from the C=C bond in the Alkene This results in formation of a carbocation intermediate as the hydrogen forms a bond width a carbon which reacts with the halide ion Halide ion the attracted to positive carbocation forming a bond
164
Electrophilic addition in alkenes For the mechanism of electrophilic addition where does the first curly arrow move from and to
From the C=C double bond to the delta positive atom of the thing which is being added
165
Electrophilic addition in alkenes Where does the second curly arrow go from and two in the mechanism
The bond between the molecule adding and the delta negative
166
Electrophilic addition in alkenes What is important to add to the molecule being added on a mechanism
Dipoles (delta + and delta -)
167
Electrophilic addition in alkenes What is the intermediate
An alkane with the first bond formed and a + on the carbon There will also be a negative ion
168
Electrophilic addition in alkenes What is a carbocation
Positive ion with a positive charge on the carbon
169
Electrophilic addition in alkenes Where is the curly arrow and on the intermediate mechanism
From the negative charge on the negative ion to the positive on the carbocation
170
Electrophilic addition in alkenes What is the last part of a mechanism
An alkane
171
Electrophilic addition in alkenes What is key for the curly arrow on any mechanism
Be double headed to show movement of a pair of electrons Start from lone pair of electrons or area of high electron density eg directly from C=C bond Move towards an electrophilic or positive charge of a carbocation
172
Electrophilic addition in alkenes For halogens whats the dipole
Induced dipole caused by repulsion of the halogens e;extrinsic by the high electron density C=C bond on the Alkene
173
Electrophilic addition in alkenes markownikoff What is a carbocation
Positively charged carbon atom with only three covalent bonds instead of four
174
Electrophilic addition in alkenes markownikoff What are the three types of carbocation
Primary secondary and tertiary
175
Electrophilic addition in alkenes markownikoff What’s a primary carbocation
Only one other carbon bonded to carbon ion
176
Electrophilic addition in alkenes markownikoff What’s a secondary carbocation
Two carbons around the carbon ion
177
Electrophilic addition in alkenes markownikoff What’s a tertiary carbocation
Three carbons around the carbon ion
178
Electrophilic addition in alkenes markownikoff What does markownikoffs rule allow us to predict
Products of electrophilic addition
179
Electrophilic addition in alkenes markownikoff How many different products can be produced from asymmetric electrophiles and what are they ca;led
2 (major and minor)
180
Electrophilic addition in alkenes markownikoff What’s the major product
More likely to be made,most common
181
Electrophilic addition in alkenes markownikoff What’s the minor product
Least likely to be made, less common
182
Electrophilic addition in alkenes markownikoff What allows us to predict the minor or major product
Depending on the stability of the carbocation
183
Electrophilic addition in alkenes markownikoff What happens to the stability of the carbocation as more carbons are added around the con
Increases stability Tertiary most stable Primary least stable
184
Electrophilic addition in alkenes markownikoff What does a carbocation being more stable mean
Less likely to return to original structure More likely to pick up more electronegative
185
Electrophilic addition in alkenes markownikoff What is the major product
When more electronegative atom bonded to most stable carbocation
186
Polymers from alkenes What is addition polymerisation
Many monomers containing at least one C=C double bond form long chain polymers as the only product
187
Polymers from alkenes What is a polymer
Long chain molecule that is made up of many repeating units
188
Polymers from alkenes What are monomers
Small reactive molecules that react together to form polymers
189
Polymers from alkenes What is the general equation
Written for any addition reaction and uses the symbol n to balance it either displayed or general formulas
190
Polymers from alkenes Example of general equation for ethene
nC2H4 —> -[-C2H4-]- n
191
Polymers from alkenes What are repeat units
Specific arrangement of atoms in the polymer molecule that repeats over and over
192
Polymers from alkenes In the gerenal equation what is the repeat unit always shown in
Square brackets
193
Polymers from alkenes Difference between monomer and repeat unit
Repeat unit always drawn in square brackets with a singe carbon bind Monomer has double C=C bond Both have symbol n
194
Waste polymers and alternatives Why are polymers used
Provide readily available cheap alternative to metal glass paper and cardboard materials
195
Waste polymers and alternatives Impact of low reactivity of many polymers
Ideal for certain uses such as packaging food but at Sam time creates problems with their disposal as lots are non biodegradable which creates environmental problems such as killing marine animals
196
Waste polymers and alternatives What are the methods of polymer disposal
Landfill Recycling Combustion for energy Feedstock recycling bio plastics
197
Waste polymers and alternatives Why is using landfill not ideal
Bad for environment
198
Waste polymers and alternatives Why can polymers be recycled
Reduced the amount of waste into landfill Can have recycling point at newer landfill sites
199
Waste polymers and alternatives How does recycling polymers reduce the use of finite resources
Lots of polymer made from products of cracking crude oil
200
Waste polymers and alternatives What’s bad about recycling polymers
Time consuming as have to be sorted into different categories
201
Waste polymers and alternatives What happens after sorting to recycle polymers
Chopped washed dried and melting then cats into pellets ready for use
202
Waste polymers and alternatives Why can certain polymers cause problems when recycling
Due to their chemical composition such as PVC contains lost of toxic chlorine
203
Waste polymers and alternatives Why is combustion used to recycle polymers
When incinerates release large amount of energy which can boil water and turn turbines inside a power station
204
Waste polymers and alternatives Negative of combustion to dispose of polymers
Causes environmental pollution as carbon within polymer can be released as CO2 contributing to global warming Other toxic waste products like Cl2 can be released
205
Waste polymers and alternatives What is feedstock recycling
Where waste polymers are broken down be chemical and thermal processes into monomers gases and oils which are then used as the raw materials in the production of new polymers and organic chemicals
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Waste polymers and alternatives What’s the major benefit of feedstock recycling
Compared to other methods it works with unsorted and unwashed polymers
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Waste polymers and alternatives What are bioplastics
Polymers that are made from plant starch plant oils and plant proteins
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Waste polymers and alternatives Why are bioplastics good
Provide a renewable and sustainable alternative to the current polymers which are bases on finite resources such as crude oil
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Waste polymers and alternatives What are biodegradable polymers
Can be broke down over time by microorganisms
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Waste polymers and alternatives Why are biodegradable polymers good
Degrade amend leave no visible or toxic trace
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Waste polymers and alternatives What are photodegradable polymers
Contain bonds which are weakened by light to start degradation Many are oil based
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Waste polymers and alternatives Benefit of photo degradable polymers
Can be recycled better
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Polymers What polymers might you need to name
Poly(ethene) Poly(chloroethene) Polypropylene Phenylethene / styrene Tetrafluorothene
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Polymers How’s poly(ethene) made
Heating a large number of etehne molecules at a high pressure
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Polymers Monomer of poly(ethene)
Ethene
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Polymers Uses of poly(ethene)
Most commonly used eg supermarket bags and shampoo bottles
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Polymers What is poly(chloroethene) known as
PVC
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Polymers What are the two ways poly(chloroethene) can be made into
Rigid or flexible
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Polymers Monomer of poly(chloroethene)
Chloroethene
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Polymers What is poly(chloroethene) used in
Pipes bottles and flooring
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Polymers Monomer of polypropylene
Propene
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Polymers What is polypropylene used in
Packing material and foood cups
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Polymers Why is polypropylene used in food cups
Has thermal insulating properties
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Polymers Monomer of tetrafluoroethene
Tetrafluoroethene
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Polymers What is poly(tetrafluoroethene) used for
Coating for nonstick pans and cable insulation

Alevel Chemistry OCR A (18 decks)

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