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organic compounds Flashcards

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1
Q

organic compounds

A

compound containing Carbon
except CO, Co2, H2Co3

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2
Q

alkanes, alkenes
similarities

A

both hydrocarbons
- contain H, C
- mostly colourless

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3
Q

alkanes v alkenes

A

alkanes
general formula: Cn H2n+2, n ≥ 1
functional group: none
saturated hydrocarbons

alkenes
general formula: Cn H2n, n ≥ 2
functional group: C=C
unsaturated hydrocarbons
more reactive, flammable than alkane cuz C=C more reactive, than C-C

prefixes are based on total no. of carbon

alkanes struct formula start w/ n = 1
alkenes struct formula start w/ n = 2

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4
Q

drawing struct formula important

A
  1. 1 carbon can ONLY take 4 bonds (4 sticks)
  2. if diagram ask copy down struct formula must place hydrogen, carbon same place
  3. suffix based on number of other “sticks” that isnt carbon.

I.e. C5h10br2
-ane (C5 and 12 other bonds)

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5
Q

alcohol, carboxylic acid common property

A

not hydrocarbons
hydrocarbons contain C, H ONLY

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6
Q

alcohol properties

A
  1. funct grp —OH (hydroxyl)
  2. usally end w/ -anol (i.e. ethanol)
  3. Cn H2n+1 OH, where n ≥ 1
  4. all alcohol are neutral despite having O-H
  5. DOES NOT IONISE IN WATER.

alcohol slightly polar due to O-H
hence dissolve water (O-H), organic solvent (covalent bonds, other bonds, alcohol)

prefixes are based on total no. of carbon

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7
Q

carboxylic acid properties

A
  1. funct grp carboxyl
  2. usually end w/ -anioc acid
  3. Cn H2n+1 COOH, n ≥ 0
  4. all weak, organic acids
  5. high bp, mp compared, alcohol

carboxylic acid struct formula start w/ n = 0

prefixes are based on total no. of carbon

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8
Q

wat to do w/ funct group

A

most times: add at end, struct formula

prefixes are based on total no. of carbon

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9
Q

homologous series definition

A
  • same general formula
  • same chemical properties
  • bcuz same funct grp

differ from each other, Ch2

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10
Q

how categorise into homologous series

A
  1. funct grp
  2. general form
  3. successive unit differ, Ch2 unit
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11
Q

4 reactions of alkanes

A
  1. incomplete combustion (insufficient o2)
  2. complete combustion (excess/enough o2)
  3. substitution w/ halogens (typically) (2 reactant form 2 products)
  4. Cracking
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12
Q

6 reactions, alkenes

A

combustion
1. incomplete combustion (insufficient o2)
2. complete combustion (excess/enough o2)

addition (2 reactants added, form one product)
3. hydrogenation (add hydrogen)
4. (halogen)nation (add halogen) (i.e. iodinisation)
5. hydration (add steam h2o(g))
6. addition polymerisation

https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 27 chlorinisation

https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 28 hydration

addition req C=C

Most, but not all addition reaction result in formation of alkanes.

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13
Q

hydrogenation reaction condition

A

Nickel as catalyst
200 deg celc

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14
Q

halogenation conditions

A

alkene, no condition for halogenation

alkane, req UV light, substitution

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15
Q

hydration conditions

A

300 deg celc
pressure 60 atm
phosphoric (V) acid as catalyst ( h3po4 (aq) )
steam (must be steam, not h2o (l)!)

300 + 60 + 5

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16
Q

carboxylic acid reactions

A
  1. esterification
  2. Cracking
  3. acid reactions

no combustion.

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17
Q

incomplete combustion typically give out…

complete combustion typically give out…

A

ONLY
incomp
CO, H2o, sometimes Carbon (soot)

comp
h2o, co2

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18
Q

substitution of methane w/ chlorine gas (halogen)
visualise + what needed

A

https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 26

req UV light
one of hydrogen atoms, methane, replace by halogen atom

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19
Q

as molecular mass of
4 homologous series compounds increase,

A

more carbon, stronger intermolecular forces btwn alkane molecules
mp, bp increase
more viscous (resistance to flow)

change of state gas -> liquid -> solid
density increase

flammability decrease EXCEPT
- Carboxylic acid not flammable (acid)
- Alkenes: %tage by mass carbon increase, causes decrease flammability

carboxylic acid does not undergo combustion

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20
Q

what require for cracking reaction

A
  1. porous pot
  2. catalyst: Al2O3/SiO2
  3. high temp: at least 600deg celc
  4. room pressure: 1 atm
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21
Q

cracking definition

A

break down of large alkane -> smaller hydrocarbon,
always producing alkene

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22
Q

3 uses of cracking

A
  1. crack one of the components of fuel oil (mix of hydrocarbons) produce gasoline (petrol)
  2. crack alkenes produce plastic
  3. produce h2 (g)
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23
Q

alkanes properties

A
  1. lowest mp, bp
  2. insoluble in water, soluble in organic solvent

nonpolar

all homologous nonpolar
except alcohol, slightly polar
However, too weak, overcome GILS strong electrostatic forces of attraction

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24
Q

what req for addition polymerisation

A
  1. C=C bond
  2. catalyst, nickel

unsaturated means contain C=C bond

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25
how distinguish saturated from unsaturated hydrocarbon **IMPT**
add Br2 (aq) saturated hydrocarbon/alkane: - Br2 (aq) reddish-brown bromine remain reddish brown. - **substitution reaction, decolourises after very long period time** unsaturated hydrocarbon/alkene/contains C=C bond: - Br2 (aq) reddish-brown bromine decolourised rapidly - **addition reaction**
26
polyunsaturated
many C=C emperical formula: CH2
27
acetic acid
ethanoic acid ## Footnote ethanoate ion Ch3cooh-
28
alcohol reactions
1. combustion 2. esterification (alcohol + carboxylic acid) 3. oxidation (form carboxylic acid) ## Footnote esterification is NOT acid base reaction, even tho react w/ carboxylic acid
29
oxidation of alcohol conditions
**EITHER** use oxidising agent i.e. KMno4/potassium dichromate/g17 heat catalyse reaction **OR** expose to air presence, bacteria ## Footnote usually oxidising agent one: Lab
30
oxidation of alcohol general eqn
**USING OXIDIZING AGENT** 1. alcohol + [O] -> alcohol acid + H2o 2. [O] is [O] from oxidising agent (i.e. KMn**O4** **EXPOSE SURROUNDING AIR** 1. alcohol + o2 -> alcohol acid + h2o ## Footnote i.e. C2h5oh + 2(O) -> Ch3Cooh + h2o c2h5oh + o2 -> Ch3cooh + H2o ethanol + oxidising agent -> ethanol + oxygen ->
31
carboxylic acid usages
ethanoic acid: vinegar
32
how produce ethanol
1. addition w/ steam (hydration, c2h4 + h2o -> c2h5OH) 2. fermentation (glucose -> ethanol + co2, c6h12o6 -> 2c2h5oh + 2co2)
33
fermentation conditions, extra steps if industrial use
**consumption** yeast, catalyst, sugar soln. **37deg celc** absence of o2 **if industrial use i.e. fuels** obtain pure ethanol, fractional distillation, liquid mixture **separate, component, i.e. water** ## Footnote optimum temperature for enzyme-catalysed anaerobic respiration of yeast :>
34
limit of fermentation
1. yeast death, high ethanol conc., toxic 2. 15-20% ethanol
35
hydration, fermentation when to use which
production, ethanol **hydration** 1. industrial solvent 2. 80-90% conc. 3. high conc., toxic **fermentation** 1. typically consumption, low conc.
36
saturated vs unsaturated alcohol
**saturated** 1. w/o C=C bond **unsaturated** 1. w/ C=C bond 2. derive from saturated. i.e. 3. every missing H2 equal one double carbon bond
37
ethanol fuel 2 advantages compared to petrol
1. come from sugarcane, renewable source, energy reduce need, burn non renewable fossil fuels 2. ethanol clea**ner** fuel, nvr produce pollutants i.e. sulfur dioxide ## Footnote ethanol still produce co2 (g)
38
carboxylic acid naming
TAKE NOTE there is 1 extra C, and prefix based on **total no. C**
39
esterification conditions
1. warm 2. conc. H2So4 (aq)
40
esterification
1. carboxylic acid + alcohol react 2. funct grps carboxyl and hydroxyl react w/ each other, form ester linkage C-O || O 3. ethanoic acid + ethanol -> ester + h2o (l) 4. naming (alcohol **yl**) (acid **noate**) ## Footnote https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 30
41
ester properties
sweet, fruity smell
42
C2h6 chemical/molecular formula struct formula
**chem:** C2h6 **struct:** Ch3Ch3 ## Footnote full struct/displayed is drawing
43
Ch3cooh **full struct/displayed formula** **condensed struct formula**
https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 31
44
isomers
compounds with same molecular formula diff struct formula ## Footnote does not have to
45
isomers properties
1. different phys properties 2. sometimes different chem properties (depends on if funct grp is changed) ## Footnote https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 32: **forming** isomers
46
polymers
1. large molecules, smaller molecules, monomers 2. copolymers, 2 or more diff types, monomer units i.e. **nylon** ## Footnote each unit connected to adjacent unit, covalent bonds
47
polymers containing only one type of unit + usage
polyethene polytetraflouroethene (non stick fry pans) polychloroethene (**PVC**) (thin gloves, pipes) polystyrene (disposable containers)
48
different linkages
covalent bonds amide, ester linkages
49
how polyethene formed uses
1. addition polymerisation (**bcoz monomers are unsaturated, join tgt form long chain**) 2. many ethene monomers join tgt, C=C breaking -> **poly**ethene 3. plastic bag, clingfilm
50
define polymerisation
join many monomers tgt, form polymer
51
addition polymerisation
1. only occur, monomers, C=C bonds 2. C=C bonds, monomers breaks, forms bond, adjacent monomer, 3. polymer C-C only 4. **no loss, small molecules** 5. **all identical monomers** ## Footnote https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 33
52
condensation polymerisation
1. small molecules, removed, such as water 2. involve monomers w/ funct grp 3. polyamide/polyesters 4. monomers need 2 funct grp ## Footnote C=C vs 2 funct grp no molecules removed vs small molecules removed involves formation of C-C bonds vs no formation of C-C
53
how is nylon formed condensation polymerisation
**nylon - polyamide - many amide linkage** - monomers dicarboxylic acid, diamine - add OH back, monomer ---CO - add H back, monomer ---NH ## Footnote amine: Nh2 https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 34
54
nylon terylene usages
**nylon** fishing lines ropes sleeping bag **terylene** clothing
55
how terylene formed condensation polymerisation
**terylene - polyester - many ester linkages** - monomers dicarboxylic acid, diol (**start, end w/ 2 --OH groups**)
56
physical method of recycling plastic
**mechanical recycling** - never change chemical composition, plastic waste - melting, cooling, new products/pellets
57
chemical methods of recycling plsatic
**cracking** - plastic waste -> short chain alkanes (**use, fuels**), alkenes (**use, raw materials, industrial product**) **depolymerisation** - polymers -> monomers - monomers -> other product
58
depolymerisation specific e.g.
**polyesters, acid hydrolysis** - polyesters, presence, acid catalyst - break down -> dicarboxylic acids, diols
59
one env, econ., social issue of recycling plastic
**econ.** - recycling plastic waste, expensive, transportation, sorting, cleaning high energy, manpower **social** - unaware proper way recycle plsatic waste, plastic waste, recycling bins, eventually not recycled
60
one env issue of plastic besides burning release cause global warming
made of non-renewable petroleum (naphfta fraction)
61
macromolecules
large molecules made of many smaller molecules, monomers
62
when add ()n
when ask for polymer: YES when repeating unit: no need ## Footnote when repeating unit, add bond connector at both ends of the unit i.e. H H H | | | -C-C-C- https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 36
63
what constitutes as amine? Is ammonia amine?
ammonia not amine, does not contain C.
64
amine vs amide
amine - funct grp (Nh2) amide - amide linkage (COHN) ## Footnote https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 amide vs amine pg 35
65
define biodegradable (chem)
can be decomposed, bacteria, soil
66
non biodegradable plastic waste issues
**disadv** - air pollution, produce toxic gases, burn - land pollution, bury, landfill ## Footnote plastics cheap
67
out of butter, fats, oil, margarine which is most polyunsaturated
oil
68
margarine and vegetable oil which one alkene, which one alkane
alkane: m**a**g**a**rine alkene: v**e**g**e**table oil
69
natural polyester
fats (triester) ## Footnote saturated hydrocarbons (no C=C bond)
70
repeat unit vs monomer
repeat unit: no ()n, disconnected monomer: no ()n, connected to H ## Footnote https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 36
71
are linkages funct grp
amide and ester linkage
72
complete combustion formula
CxHy + (x + y/4) o2 -> xCo2 + (y/2)h2o
73
why polymerisation benefit, catalyst
formation long chain polymers take vry long time w/o catalyst
74
why alkene burn sootier flame
- percentage by mass of carbon, alkene higher - req more moles of o2 for complete combustion - more likely undergo incomplete combustion - produce carbon monoxide, carbon
75
cracking vs catalytic cracking use of cracking
cracking: no need catalyst, slower used break long chain alkanes from not so useful crude oil fractions
76
straight chain vs branched chain isomer
straight chain isomer: longest main carbon chain out of all isomers
77
what is alkyl group
remove one hydrogen from alkane ## Footnote i.e. ethyl ethene but remove one hydrogen
78
how to make margarine. As no. of C=C decrease, mp, bp ____.
hydrogenation, unsaturated vegetable oils mp, bp increase ## Footnote more hydrogen added, less C=C bonds exist, high mp, bp so that it wont melt so easily, more convenient to use
79
define polyunsaturated
hydrocarbon chains, 2 or more C=C
80
high polyunsaturation aka more C=C bonds how affect mp, bp
decrease mp, bp - saturated fats, hydrocarbon chains, stack well, each other - unsaturated fats do not stack as well - C=C cause bends, struct, chains dont come as close, each other, intermolecular FoA weaker ## Footnote melting and boiling points based on **saturation** if **unsaturated** fats e.g. lower mp, bp
81
how trans fat formed
during hydrogenation of unsaturated vegetable oils, may react w/ catalyst
82
partial ionisation of carboxylic acid, water
RCOOH ⇌ RCOO- (aq) + H+ (aq) ## Footnote R represents alkyl COO- carboxylate ion HCOO- methanoate ion Ch3COO- ethanoate ion C2h5Coo- propanoate ion etc.
83
synthetic fibers property
drawn long thin strands w/o break
84
**alkane -> alkene and vice versa** **alkene -> alcohol and vice versa** **alcohol -> carboxylic acid and vice versa**
alkane -> alkene - catalytic cracking/dehydrogenation - **vv**: catalytic cracking/hydrogenation alkene -> alcohol - hydration - **vv**: dehydration alcohol -> carboxylic acid - oxidation - reduction
85
why is higher fraction lower mp,bp
- smaller molecule, surface area - smaller chain - weaker intermolecular FoA
86
addition poly reaction conditions
**add:** catalyst, high heat, high pressure
87
alcohol + acid is condensation reaction?
**condensation reaction** - combination 2 smaller molecules, form larger molecule - removal, small molecules, water
88
different plastic have
diff chemical properties
89
fermenter use
prevent o2 enter, alcohol oxidise -> carboxylic acid
90
cracking products (if not a smaller alkane/alkene)
hydrogen
91
reversible organic reactions
- hydration - esterification
92
metals itself oxidise/reduce g17 itself oxidise/reduce
metals -> oxidises, good R.A. g17 -> reduces, good O.A.
93
alkali and acid can do ppt reaction?
yes - but must form insoluble ppt. - and both starting reagents must be soluble
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