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Chemistry > Introduction To Organic + Alkanes > Flashcards

Introduction To Organic + Alkanes Flashcards

(53 cards)

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1
Q

Skeletal formula

A

Shows bonds in carbon skeleton only

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2
Q

Homologous series (5)

A

Same functional group
Similar chemical properties
Trend in physical properties
Same general formula
Increase C chain length = +CH2 to formula

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3
Q

Aldehyde functional group and general formula

A

CHO
CnH2n+1OH

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4
Q

Ketone functional group and general formula

A

CO
CnH2nO

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5
Q

Carboxylic acid functional group and general formula

A

COOH
CnH2n-1COOH

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6
Q

Naming compounds priority list

A

Functional group
Alkenes
Alkyl group
Halogens

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7
Q

Name 2 types of isomerism and their subgroups

A

Structural
- positional
- functional group
- chain
Stereo
- geometric
- optical

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8
Q

Positional structural isomerism

A

Eg. 1 chloropropane and 2 chloropropane

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9
Q

Functional group structural isomerism

A

Eg. Propanone and propanal

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10
Q

Chain structural isomerism

A

Eg. Pentane and 2 - methyl butane
(Be careful no. Carbons, some are the same just inverted, not isomers)

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11
Q

Stereo isomer definition

A

Same molecular and structural formula but atoms are arranged in different areas of space

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12
Q

Describe cis/trans relationship

A

trans = same atoms on opposite carbons and opposite sides
cis = same atoms on opposite carbons but same sides

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13
Q

Why does E/Z cis/trans isomerism occur

A

C=C is planar
Alkenes
Pi bonds
Cant rotate

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14
Q

E/Z rules

A

All C attachments are different
Cis/trans = non-applicable
Greatest atomic number = highest priority
If same = go to next attached atom
2 highest priority = same side = Z
2 highest priority = different side = E

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15
Q

Name and describe 2 physical properties of alkanes

A

Low mp/bp
- weak LF only
- less ETO
- more length = higher mp/bp (more e density, stronger LF)
- unbranded = higher mp/bp (more SA, more contact points, more e density, stronger LF)
Water insoluble
- H bonds in water stronger than alkane LF
- Soluble in non polar liquids

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16
Q

Name and describe 2 chemical properties of alkanes

A

Relatively unreactive
- Non-polar bonds
- Strong C-C, C-H cov bonds
- dont react with acids, bases, ox/red agents
- react with halogens
Combust well

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17
Q

Name 6 step fractional distillation process

A

Crude oil heated in furnace
L/g mixture enters fractionating column
Ghost at bottom, cooler at top
HCs rise and condense at tray lower than bp
L piped off
Short HCs collect at top, lower mp/bp, weaker LFs

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18
Q

Fraction

A

Group of HCs with similar bps

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19
Q

Temperatures at top/bottom of fractionating column

A

350K
600K

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20
Q

8 fractions and uses

A

Refinery gases - camping stoves
Petrol - cars
Naphtha - rubber solvent
Kerosene - planes
Diesel - lorries
Lubricating oil - candles
Fuel oil - ships
Bitumin - tarmac roads

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21
Q

Describe fractions at the top of the fractionating column

A

Volatile
Flammable
Not viscous
Short HCs
Low bps

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22
Q

Describe fractions at the bottom of the fractionating column

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A

Not volatile
Not flammable
Viscous
Long HCs
High bps

23
Q

Describe the cracking process

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A

C-C bonds broken in LC HCs
Makes SC HCs (petrol/naphtha)
alkenes (polymers —> plastic)

24
Q

Why is cracking necessary

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A

LC HC over abundant
Less useful, lower demand
Low supply for SC HCs
More useful, high demand
More reactive alkenes made
Monetise off waste products
Supply = demand, prices don’t rocket

25
Name and describe 2 types of cracking
Thermal - 1000*C - 70atm Catalytic - 450*C (lower = cheaper) - slight pressure - zeolite catalyst (sulfur dioxide, aluminium oxide) - catalyst increases ROR, decreases time and increases profit
26
Reforming
Straight chain HCs —> branched/cyclo/aromatic alkanes More efficient engine combustion Catalyst, platinum, aluminium oxide
27
Alkane combustion
Oxygen addition Gases (l vaporised) SC, more volatile, combust easier Exothermic (more energy released forming new than absorbed breaking old) LC, more bonds, more Kj/mol
28
Name 6 pollutants
CO CO2 Unburnt HCs SO2 Nitrous oxides Carbon
29
CO
Poisonous Binds to haemoglobin Lower affinity than O2, not enough O2 —> organs Can be fatal
30
CO2
Greenhouse gas Absorb IR rays Cant reflect Greenhouse effect —. Global warming
31
Unburnt HCs
Greenhouse gas Smog component Irritates eyes/resp system (lung damage)
32
Carbon
Global dimming Carcinogen Asthma
33
SO2
HC sulfur impurities React with O2 and water —> H2SO4 (acid rain) Destroy vegetation, fish, buildings (Remove using CaO/CaCO3)
34
Nitrous oxides
Engines, high temp, N2 and O2 react + water —> HNO3 (acid rain) Toxic, poisonous (asthma)
35
Catalytic converters
Removes nitrous oxides, CO and Unburnt HCs Platinum, rhodium Honeycomb structure (high SA, high efficiency) Products pass catalyst —> less harmful products Make CO2 (gg but less harmful)
36
Fossil fuels
Coal/oil/gas Easily extracted Produce lots of energy Non renewable
37
Biofuels pros and cons
Renewable Make CO2 Car engines modified Land fuel use, cant grow crop food Deforestation
38
3 types of biofuel
Bioethanol - fermentation Biodiesel - refund fats Biogas - break organic waste
39
What is a free radical
Particle with an unpaired electron Very reactive
40
Homolytic fission
Covalent bond splits 1 electron to each species using UV light
41
3 stages of a chain reaction
Initiation Propagation Termination
42
Describe the initiation stage of forming chloroalkanes
Break Cl-Cl bond —> 2X free radicals UV light has more energy than bond (photodissociation) Homolytic fission
43
Describe the propagation stage of forming chloroalkanes
Chlorine free radical takes an H from methane Makes hydrogen chloride and methyl free radical Methyl radical reacts with chlorine molecule Makes chloromethane and chlorine free radical Chain reaction, repeated until CH4 or Cl2 used up Cl free radicals regenerated, catalyst
44
Describe the termination stage of forming chloroalkanes
Free radicals removed 2 free radicals react together Stable compound, no free electrons formed 2 chlorine free radicals makes Cl2 2 methyl free radicals makes C2H6 Chlorine and methyl free radical make chloromethane
45
Haloalkane synthesis conditions (3)
- Dichloromethane can be made prop stage if chlorine radical reacts with chloromethane, excess cl, more substitution reactions - LC HCs = isomers form, excess methane, more branched alkyl groups - Not useful for specific products, unpredictable, made variety of products
46
Describe the ozone layers (4)
O3 Stratosphere Chemical sunscreen Absorbs UV radiation from sun
47
Why can UV radiation be harmful
Suburb, skin cancer
48
Ozone layer equilibrium equations
O3 —> O2 + O* O2 —> 2O* O2 + O* —> O3 + heat
49
Why is the ozone layers depleting
Human activity (CFCs and nitrous oxides) More free radicals Effect ozone natural balance
50
Cl free radical formation from CFCs
CFCs decomposed by UV light CFCl3 —> (UV) CFCl2 + Cl* Cl* + O3 —> ClO* + O2 ClO* + O —> Cl* + O2 Less ozone
51
Nitrous oxide free radical formation
NO —> (UV) NO* NO* + O3 —> NO2* + O2 NO2* + O —> NO* + O2 Less ozone levels
52
Benefits of CFCs
High volatility Non toxic Non flammable No smell Extremely un reactive
53
Uses of CFCs
Refrigerants Aerosols Polystyrene blowing agents

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