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AS organics Flashcards

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1
Q

homologous series

A

a series of organic compounds containing the same functional group with sucessive members differing by -CH2

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2
Q

functional groups

A

a group of atoms responsible for the characteristic reactions of a compound

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3
Q

alkyl group

A

-CH3

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4
Q

aliphatic

A

carbon joined to each other branched (straight), unbranched or non-aromatic rings

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5
Q

alicyclic

A

carbon joined in rings
(with or without branch)

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6
Q

aromatic

A

some/ all carbons found in a benzene ring

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7
Q

unstaurated

A

contain C=C or C≡C

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8
Q

structural isomers

A

same molecular formula but different displayed formulae

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9
Q

What is the naming system for compounds

A

Nomenclature

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10
Q

Steps to naming organic compounds

A
  1. find longest unbranched backbone
  2. Add suffix for main functional group
  3. Number the functional groups and/or alkyl side chains
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11
Q

prefix of alcohol

A

hydroxy-

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12
Q

suffix of aldehyde

A

-al

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13
Q

suffix of ketone

A

-one

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14
Q

stems (from 0-10)

A
  1. meth-
  2. eth-
  3. pro-
  4. but-
  5. pent-
  6. hex-
  7. hept-
  8. oct-
  9. non-
  10. dec-
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15
Q

Homolytic

A

Each bonding atoms recieves one electronforming 2 radical

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16
Q

Hetrolytic

A

One of the bonding atoms recieves both electrons To form a cation and an anion

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17
Q

Radical

A

a reactive species with an unpaired electron
(but not charged)

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18
Q

Electrophile

A

(+ve) electron-deficient species , accepts electrons to form covalent bonds

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19
Q

Nucleophile

A

(-ve)electron-rich species, provides pair of electron to form covalent bonds

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20
Q

General formula of alkanes

A

CnH2n+2

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21
Q

what is the type of bond in alkanes

A

sigma bonds

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22
Q

How are sigma bonds formed?

A

The overlap of the s-orbitals

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23
Q

Why are alkanes non-polared molecules?

A
  1. electronegativity diff. between C - H are neglegible
  2. bonds are relatively non-polared
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24
Q

Structure of alkanes and its bond angles (why?)

A

Tetrahedral (109.5)

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25
Q

Factors affecting boiling point and (why?)

A
  1. Chain length
    (↑C = ↑ S.A. = ↑ London forces)
    (↑electron = ↑strength of london forces)

2.Branching
↑ branching = ↓ surface contact = ↓ london forces

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26
Q

Why is Alkanes unreactive

A
  1. ↑ bond enthalpy of C-C + H-H
  2. ↓ polarity of sigma bond
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27
Q

What must be present for free-radical substituition

A

UV light

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28
Q

Three steps of free radical substitution

A
  1. initiation
    2.propagation
    3.termination
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29
Q

Describle initiation of free radical substitution

A

Halogen molecules broken down in Homolytic fission, under UV

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30
Q

Describle propagation of free radical substitution

A
  1. radical attacks alkanes
  2. C-H bonds Homolytic fission occurs
  3. alkyl radical formed attacks halogen molecules
  4. forming haloalkane + halogen radical
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31
Q

Describle termination of free radical substitution

A

Two radical reacts together to form a single unreactive molecule

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32
Q

3 limitation of free radical substitution

A
  1. impurities in the product
  2. further substitution (when excess halogen under UV)
  3. substitution on different carbon (cannot control where hetrolytic fission occurs)
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33
Q

Two bonds in alkenes

A

σ and π

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34
Q

one characteristic of π bond

A

Fixed above and below the planar, prevent rotation of the molecule

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35
Q

Bond angles of alkene

A

120 - trigonal planar

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36
Q

How does E/Z isomer work ?

A

E - piority group on EPPOSITE side of plane

Z- piority group on ZAME side of plane

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37
Q

What is the CIP priority rules ?

A
  1. calculate the total atomic no of group
  2. Group with greatest atomic no is the priority group
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38
Q

4 types of alkene reactions

A
  1. hydrogenaton
  2. Halogenation
  3. hydrohalogenation
  4. hydration
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39
Q

what does hydrogenation form

A

alkane

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40
Q

what type of reaction are the reactions of alkene?

A

electrophilic addition

41
Q

Observation of halogenation (Bromine)

A

orange to colourless

42
Q

What does hydration form ?

A

Alcohol

43
Q

Inductive effect

A

↑ C-C bonds
carbocation ↓ +ve charged
↓ reactive

44
Q

What does the Markownikoff’s rule apply to ?

A

Only for assymterical molecules only

45
Q

State Markownikoof’s rule

A

Rules favours **major **product here:

Halogen (HX) / most electronegative halogen
bonds to
MOST SUBSTITUITED CARBON

46
Q

Major product of the reaction (hydrogen halide)

A

halogen to
higher class carboncation

47
Q

Major product of the reaction (interhalogen)

A

↑electronegative halogen to
↑ stable carboncation

48
Q

Minor product of the reaction (interhalogen)

A

less electronegative to
more stable carbocation

49
Q

Define polymers

A

A large chain formed from many thousands of repeat units of smaller molecules

50
Q

Define monomers

A

A small molecule that conbines with many other monomers to form a polymers

51
Q

Repeating units

A

the smallest group of atoms that connected after the other make up the polymer chain

52
Q

3 polymers waste managements

A
  1. recycling
    2.combustion
    3.feedstock recycling
53
Q

What is feedstock recycling ?

A

polymers are broken down by chemical and thermal processes to form gases and fuel

54
Q

4 types of alternative plastic solution

A
  1. Bioplastic - made from cellulose, starch…
  2. Biodegradable - breaks down naturally
  3. Compostable - made from plants + degrade naturally
  4. Photodegradable - break down under visible radiation
55
Q

How are photodegradable polymers made

A
  • Contains bonds that are weakened by absorbing light-
  • can be an additive mixed into polymers to promote degradation
56
Q

General formulae of alcohol

A

CnH2n+1 OH

57
Q

Intermolecular forces involved in alcohol

A
  1. Hydrogen bonding - when oxygen (δ-)from one molecules attracts a hydrogen (δ+) on another alcohol
  2. Temporary D-D forces - ↑ chain = ↑ B.P.
58
Q

Solubility of alcohol

A
  1. Small alcohol dissolves in water
  2. ↑ chain length= ↓ soluble
    (As ↓ polared = ↓ likely to dissolve in polared solvent)
59
Q

4 types of reaction of alcohol

A
  1. Combustion
  2. Oxidation
  3. Dehydration
  4. Substitution
60
Q

Alcohol reactions

What are the three types of oxidation reactions? + reagents?

A

primary in distill = aldehyde
primary in reflux = carboxylic acid
secondary in reflux = ketone

61
Q

What is the colour change of oxidation reaction of alcohol

A

Orange to green

62
Q

2 types of Haloalkane reaction

A
  1. nucleophilic substitution
  2. elimination
63
Q

Reactivity of haloalkane

(3 points)

A

1.↓electronegative down the group
2. ↓Polared bonds
3.↓bond enthalpy
4. ↓energy required to overcome

[↓ chain = more electronegative overall]

64
Q

2 ways of hydrolysis of haloalkane

A
  1. by aq. alkali
  2. by water (with prescence of ethanol)

[both forms alcohol and halide]

65
Q

Purpose of alcohol for hydrolysis by water

A

To enable the haloalkane organic layer to mix with water solvent

(haloalkane=non-polared, water=polared)
so won’t mix

66
Q
  1. How to test for halide ions formation
  2. Explain the reactivity of haloalkane?
    (quickest = iodoalkane)
    (second = bromoalkane)
    (slowest = chloroalkane)
    … to form p.p.
A
  1. Add silver nitrate
    (first to form p.p. = most reactive)
  2. Iodoalkane is the most reactive
    * least electronegative
    * weakest bond C-I
    * requires the least energy to overcome
67
Q

Describle the environmental concern of organohalogens

(2 points)

A
  1. produces halogen radicals under UV
  2. which catalyses the break down of Earth’s protective ozone layer
68
Q

2 example of organohalogens

A

CCl3F, CCl2F2

69
Q

Eq. of halogens radical from organohalogens (which starting molecule = CF2Cl2)

A

CF2Cl2 -> CF2Cl* + *Cl

70
Q

5 main organic techniques

A
  1. distillation
  2. heating under reflux
  3. redistillation
  4. BP determination
  5. Drying
71
Q

Purpose of distillation

A

To seperate liquids with different BP

72
Q

4 steps of distillation

A
  1. heat in round bottom flask
  2. lowest B.P. evaporates first
  3. pass through the condenser
  4. fraction then collected in a seperate flask
73
Q

Purpose of reflux

A

to enable reaction to fully complete

74
Q

Steps to heating under reflux

A
  1. continuously heat content
  2. liebig condenser to ensure all vapour condense
  3. So no reactant can escape via evaporation
75
Q

What is redistillation ?

A

subsequent distillation carried our to obtain purer product

76
Q

Purpose of boiling point determination

A

To compare to databook value as a measure of purity

77
Q

4 steps to boiling point determination

A
  1. tightly pack the substance into capillary tube
  2. place into machine
  3. record the MP and the range
  4. compare to databook value
78
Q

Two examples of drying agents for drying

A

Any anhydrous salt
(e.g. MgSO4 , CaCl2)

79
Q

4 factors to determine synthesis routes

A
  1. type of reaction - % yield
  2. Reagent used - renewable ?
  3. By-product , harmful/ toxic ?
  4. Catalyst - Rates , cost
80
Q

How to test for 1* /2* alcohol ?

A

Add potassium dichromate result: orange -> green

81
Q

How to test for aldehyde ?

A

Add tollen’s reagent Result : colourless -> dark silver p.p) MIRROR EFFECT

82
Q

Test for haloalkane

A

Add silver nitrate and ethanol Result :
white p.p. = chloroalkane
creamy p.p = bromoalkane
yellow p.p = iodoalkane

83
Q

What is Infrared spectrometry ?

A
  1. IR radiation causes covalent bonds to vibrate and abosrb energy
    2.The spectrum of absorption can be used to determine functional groups
84
Q

What + Where is the fingerprint region ?

A

to determine exact molecules
< 1500 cm-1

85
Q

Environmental impact of IR radiation

A
  1. Atomospheric gas (e.g. CO2, H2O , CH4) aborbs IR radition
  2. exacerbates global warming
  3. emission usually from fossil fuel usage
86
Q

Application of IR radiation

A
  1. monitor gases that cause air pollution
  2. modern breathalysers to measure ethanol
87
Q

Define Time of Flight in mass spec

A

time for each ion to reach detector

88
Q

Steps of mass spec

A
  1. Sample is vapourised and pass through high voltage
  2. Accelerated by -ve charged plates
  3. deflected by magnetic field
  4. reach detector to form spectrum
89
Q

3 main peaks to focus on mass spec

A
  1. Molecular peak - second rightmost peak (tells molecualr mass )
  2. M+1 peak - right most peak (mass of compound with Carbon -13 isotopes)
  3. framgent peaks - any peaks < RFM (fragment ions of the molecule detected)
90
Q

Markownikoff’s rule

What does it means by most-substituted carbon

A

carbon where it has the most no. of H replaced by C.

i.e. highest class carbon

91
Q

Markownikoff’s rule

Why does higher class carbocation more stable?

A
  1. carbon bonded to more C
  2. non-polared bonds = more stable
  3. ↓ +ve carbocation
  4. ↑ stable (as ↓ likely to react)
92
Q

Markownikoff’s rule

Why does the more stable carbocation forms major product?

A
  1. more likely form
  2. as ↓ likely to be attacked
  3. less energy needed to form
93
Q

2 eq for the breakdown of ozone

A
94
Q

3 condition of hydrogenation

A
  1. 200 °C
  2. 1000 KPa
  3. Nickel catalyst
95
Q

2 condition for hydration

A
  1. 300 °C - reflux
  2. sulfuric / phosphoric acid
96
Q

What bonds do C in C=C make

A

2 σ with hydrogen
1 σ in C=C
1 π in C=C

97
Q

Where are σ bonds found

A
  1. C-H bond (1)
  2. C-C bond (1)
  3. C=C bond (1)
98
Q

Optical isomerism

A

Non-superimposed mirror image

99
Q

What is the difference between esterification and acid hydrolysis

A

Esterification - conc
Acid hydrolysis - diluted

Chemistry (6 decks)

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