Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry aqa > Organic 1st yr > Flashcards

Organic 1st yr Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Functional group

A

is an atom or group of atoms which when present in different molecules causes them to have similar chemical properties

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Homologous series

A

Homologous series are families of organic compounds with the same functional group and the same general formula.

  • They show a gradual change in physical properties (e.g. boiling point).
  • Each member differs by CH2 from the last.
  • same chemical properties
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Order of priority highest first:

CA, ALD, KET,halo, alke,alc

A

Carboxylic acids >aldehydes>ketones>alcohols>alkenes>halogenoalkanes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

HOMOLYTIC FISSION

A

each atom gets one electron from the covalent bond

When a bond breaks by homolytic fission it forms two Free Radicals. Free Radicals do not have a charge and are represented by a

A Free Radical is a reactive species which possess an unpaired electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

HETEROLYTIC FISSION

A

one atom gets both electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Structural isomers

A

same molecular formula different structures (or structural formulae)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Chain isomers

A

Compounds with the same molecular formula but different structures of the carbon skeleton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

position isomers

A

Compounds with the same molecular formula but different structures due to different positions of the same functional group on the same carbon skeleton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Functional group isomers

A

Compounds with the same molecular formula but with atoms arranged to give different functional groups

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Stereoisomerism

A

Stereoisomers have the same structural formulae but have a different spatial arrangement of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

E-Z stereoisomers arise when:

ab

A

(a) There is restricted rotation around the C=C double bond.
(b) There are two different groups/atoms attached both ends of the double bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Cahn–Ingold–Prelog (CIP) priority rules

A
  1. Compare the atomic number of the atoms directly attached to each side of the double bond; the atom of higher atomic number is given priority
  2. If the atoms are the same, consider the atoms at distance 2 from the double bond. Make a list of each atom bonded to the one directly attached to the double bond. Arrange list in order of decreasing atomic number. Compare the lists atom by atom; at the earliest difference, the group containing the atom of higher atomic number is given priority
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Priority Group:

A

The atom with the bigger atomic number is classed as the priority atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Petroleum fraction

A

mixture of hydrocarbons with a similar chain length and boiling point range

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Draw fractional destillation mechanism

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Key points to learn

about fractional distillation

A
  • Oil is pre-heated
  • then passed into the column.
  • The fractions condense at different heights
  • The temperature of the column decreases upwards
  • The separation depends on the boiling point.
  • Boiling point depends on the size of molecules.
  • The larger the molecule the larger the van der Waals forces
  • Similar molecules (size, bp, mass) condense together
  • Small molecules condense at the top at lower temperatures
  • and big molecules condense at the bottom at higher temperatures
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Vacuum distillation unit

A
  • Heavy residues from the fractionating column are distilled again under a vacuum.
  • Lowering the pressure over a liquid will lower its boiling point.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Fractional Distillation: In the laboratory

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Cracking:

A

conversion of large hydrocarbons to smaller hydrocarbon molecules by breakage of C-C bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Economic reasons for cracking

A
  • The petroleum fractions with shorter C chains (e.g. petrol and naphtha) are in more demand than larger fractions.
  • To make use of excess larger hydrocarbons and to supply demand for shorter ones, longer hydrocarbons are cracked.
  • The products of cracking are more valuable than the starting materials (e.g. ethene used to make poly(ethene), branched alkanes for motor fuels, etc.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

There are two main types of cracking:

A

thermal and catalytic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Thermal Cracking

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Catalytic Cracking

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Fuel :

A

releases heat energy when burnt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Complete Combustion

A

In excess oxygen, alkanes will burn with complete combustion

The products of complete combustion are CO2 and H2O

C8H18(g) + 12.5 O2 (g) —– 8CO2 (g) + 9 H2O(l)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Incomplete Combustion

A

If there is a limited amount of oxygen then incomplete combustion occurs, producing CO (which is very toxic) and/or C (producing a sooty flame)

CH4 (g) + 3 /2 O2 (g) —-CO(g) + 2 H2O(l)

CH4 (g) + O2 (g)—– - C(s) + 2 H2O(l)

Incomplete combustion produces less energy per mole than complete combustion

Carbon (soot) can cause global dimming- reflection of the sun’s light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Pollution from Combustion

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Nitrogen Oxides NOx

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Catalytic converters

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Global warming

A

Carbon dioxide (CO2 ), methane (CH4 ) and water vapour (H2O) are all greenhouse gases.

Water is the main greenhouse gas (but is natural), followed by carbon dioxide and methane

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Mechanism of the greenhouse effect

A

UV wavelength radiation passes through the atmosphere to the Earth’s surface and heats up Earth’s surface.

The Earth radiates out infrared long-wavelength radiation.

The C=O Bonds in CO2 absorb infrared radiation so the IR radiation does not escape from the atmosphere.

This energy is transferred to other molecules in the atmosphere by collisions so the atmosphere is warmed

Carbon dioxide levels have risen significantly in recent years due to the increased burning of fossil fuels.

Carbon dioxide is a particularly effective greenhouse gas and its increase is thought to be largely responsible for global warming

The Earth is thought to be getting warmer, and many scientists believe it is due to increasing amounts of greenhouse gases in the atmosphere

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

The reaction of alkanes with bromine/chlorine in UV light

A

Overall Reaction

CH4 + Cl2 —-CH3Cl + HCl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Example: Write mechanism of Br2 and propane

A
34
Q

Primary halogenoalkane

A

One carbon attached to the carbon atom adjoining the halogen

35
Q

Secondary halogenoalkane

A

Two carbons attached to the carbon atom adjoining the halogen

36
Q

Tertiary halogenoalkane

A

Three carbons attached to the carbon atom adjoining the halogen

37
Q

Haloalkanes

Nucleophilic substitution reactions

A
38
Q

Comparing the rate of hydrolysis reactions

A
39
Q

Nucleophilic substitution with aqueous hydroxide ions

A
40
Q

Alternative mechanism for tertiary halogenoalkanes

A
41
Q

Nucleophilic substitution with cyanide ions

A
42
Q

Naming Nitriles

A
43
Q

Nucleophilic substitution with ammonia

A
44
Q

Elimination reaction of halogenoalkanes

Elimination with alcoholic hydroxide ions

A
45
Q

The structure of the halogenoalkane also has an effect on the degree to which substitution or elimination occurs in this reaction

A

Primary tends towards substitution

Tertiary tends towards elimination

46
Q

Uses of Halogenoalkanes

A

Chloroalkanes and chlorofluoroalkanes can be used as solvents

Halogenoalkanes have also been used as refrigerants, pesticides and aerosol propellants CH3CCl3 was used as the solvent in dry cleaning Many of these uses have now been stopped due to the toxicity of halogenoalkanes and also their detrimental effect on the atmosphere

47
Q

ozone

A

The naturally occurring ozone (O3 ) layer in the upper atmosphere is beneficial as it filters out much of the sun’s harmful UV radiation

Ozone in the lower atmosphere is a pollutant and contributes towards the formation of smog

Man-made chlorofluorocarbons (CFC’s) caused a hole to form in the ozone layer. Chlorine radicals are formed in the upper atmosphere when energy from ultra-violet radiation causes C–Cl bonds in chlorofluorocarbons (CFCs) to break

CF2Cl2 —- CF2Cl. + Cl.

48
Q

Cl radicals + ozone depletion equation+ description

A
49
Q

Alkenes

A

unsaturated hydrocarbons

50
Q

Alkenes bonds

A

C=C double covalent bond consists of one sigma (σ) bond and one pi (π) bond

π bonds are exposed and have high electron density. They are therefore vulnerable to attack by species which ‘like’ electrons: these species are called electrophiles

51
Q

Reaction of Bromine with Alkenes

A
52
Q

Reaction of Hydrogen Bromide with Alkenes

A
53
Q

Reaction of Sulfuric acid with Alkenes

A
54
Q

Direct industrial hydration of alkenes to form alcohols

A
55
Q

Testing for Alkenes with Bromine water

A

Bromine water decolourises in the presence of a double bond. This can be used as a test for the presence of an double bond in a molecule. It can be used quantitatively to show the presence of multiple double bonds in compounds like polyunsaturated oils

56
Q

Poly(chloroethene)

draw + describe

A

Poly(chloroethene) is a polymer that is waterproof, an electrical insulator, and doesn’t react with acids

In its pure form, it is a rigid plastic due to the strong intermolecular bonding between polymer chains that prevents them from moving over each other.

In this un-plasticized form it is used to make uPVC window frame coverings and guttering.

If a plasticizer is added the intermolecular forces are weakened which allows the chains to move more easily, resulting in more flexibility in the polymer.

In this form, PVC is used to make insulation on electrical wires, and waterproof clothing

57
Q

Bond angles in Alcohols

A

All the H-C-H bonds and C- C-O are 109.5o (tetrahedral shape), because there are 4 bonding pairs of electrons repelling to a position of minimum repulsion

The H-O- C bond is 104.5o (bent line shape), because there are 2 bonding pairs of electrons and 2 lone pairs repelling to a position of minimum repulsion. Lone pairs repel more than bonding pairs so the bond angle is reduced

58
Q

Boiling point

A

The alcohols have relatively low volatility and high boiling points due to their ability to form hydrogen bond between alcohol molecules

59
Q

Partial Oxidation of Primary Alcohols

A
60
Q

Distillation of an alcohol

A
61
Q

Full Oxidation of Primary Alcohols

A
62
Q

Reflux

A
63
Q

Oxidation of Secondary Alcohols

A
64
Q

Tollens’ Reagent

A
65
Q

Fehling’s solution

A
66
Q

Reaction of Alcohols with Dehydrating agents

A
67
Q

Forming ethanol

fermentation

A
68
Q

Forming ethanol

From ethene

A
69
Q

Acid catalysed addition mechanism for hydration of ethene

A
70
Q

Ethanol as biofuel

A

A biofuel is a fuel produced from plants

Ethanol produced from fermentation is a biofuel. It can be argued that ethanol produced from this method is classed as carbon–neutral because any carbon dioxide given off when the biofuel is burnt would have been extracted from the air by photosynthesis when the plant grew. There would be no net CO2 emission into the atmosphere

71
Q

Equations to show no net contribution to CO2

A
72
Q

Identification of functional groups by test-tube reactions

Alkene

Functional group

Reagent

Result

A

Bromine water

Orange colour decolourises

73
Q

Aldehyde

Reagent

Result

A

Fehling’s solution

Blue solution to red precipitate

Tollens’ reagent

Silver mirror formed

74
Q

Carboxylic acid

Reagent

Result

A

Sodium carbonate

Effervescence of CO2 evolved

75
Q

1 o 2 o alcohol and aldehyde

Reagent

Result

A

Sodium dichromate and sulfuric acid

Orange to green colour change

76
Q

chloroalkane

Reagent

Result

A

Warm with silver nitrate

Slow formation of white precipitate of AgCl

77
Q

Optical Isomerism

A

Type of a stereoisomerism

Optical isomerism occurs in carbon compounds with 4 different groups of atoms attached to carbon (called an asymmetric carbon

Two compounds that are optical isomers of each other are called enantiomers

A carbon atom that has four different groups attached is called a chiral

Non-superimposable images of each other

Rotate plane-polarized light

A mixture containing a 50/50 mixture of the two isomers (enantiomers) is described as being a racemate or racemic mixture.

Many naturally occurring molecules contain chiral C atoms but are usually found in nature as a pure enantiomer

Optical isomers have similar physical and chemical properties, but they rotate plane polarised light in different directions.

One enantiomer rotates it in one direction and the other enantiomer rotates it by the same amount in the opposite direction

A racemic mixture (a mixture of equal amounts of the two optical isomers) will not rotate plane-polarised light.

78
Q

Chemical Reactions and Optical Isomers

Formation of a racemate

A

A racemate will be formed in a reaction mechanism when a reactant or intermediate has a trigonal planar group in the molecule is approached from both sides by an attacking species

79
Q

Nucleophilic addition of HCN to aldehydes and ketones (unsymmetrical)

A
80
Q
A

Chemistry aqa (21 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions