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Year 12 Chemistry > Unit 4 AOS 1 > Flashcards

Unit 4 AOS 1 Flashcards

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1
Q

What is the valency of the Carbon atom

A

4

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2
Q

How many outer shell electrons does carbon have

A

4

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3
Q

Nature of C-C bond

A

strong and stable

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4
Q

Prefixes for halogens

A

chloro, idodo, bromo, fluoro

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5
Q

What is the functional group for ketones

A

carbonyl group

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6
Q

How do you label an alkene/alkyne with more than one bond

A

di, tri, tetra

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7
Q

What can’t C=C bonds do

A

rotate

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8
Q

What are the groups called for trans and cis isomers

A

hetero groups

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9
Q

What does it mean if you can draw a line of symmetry in compound

A

it’s achiral

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10
Q

What reactions can alkenes undergo

A

substitution, photochemical substitution

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11
Q

What is photochemical substitution equation for with Cl

A

alkane + Cl (UV) = haloalkane + HCl

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12
Q

What should be added to hydrocarbon to form amino group

A

ammonia

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13
Q

Formula for ammonia

A

NH3

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14
Q

What happens when you add water to alkene + catalyst

A

OH and H are added into hydrocarbon

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15
Q

What type of catalyst is necessary for addition of water to alkene

A

acidic catalyst

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16
Q

What is needed to react H2 with alkene

A

catalyst, e.g. Pt

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17
Q

What reaction can a secondary alcohol undergo

A

oxidation to form ketone

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18
Q

What reactions can a primary alcohol undergo

A

oxidation to form aldehyde, esterification

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19
Q

What reactions can a carboxylic acid undergo

A

can be reacted with amine to form amide and water, esterification

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20
Q

What can’t tertiary alcohols react to form

A

ketone, aldehyde, carboxylic acid

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21
Q

What is needed for esterification to occur

A

concentrated H2SO4 (liquid) and all of the reactants must be in liquid state

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22
Q

What is necessary for hydrolysis of an ester

A

water, H+

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23
Q

What is organic chemistry

A

study of carbon-containing compounds (usually containing C-H bonds and excluding compounds such as cyanide, carbon oxides and carbonates - as they are inorganic compounds)

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24
Q

What are hydrocarbons

A

compounds containing only carbon and hydrogen atoms

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25
Q

Explanation for covalent bonds in carbon

A

The electronegativity of carbon is too low for a carbon to attract electrons from another element to form a negative ion and it is too high to release electrons to another element to form a positive ion

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26
Q

What are covalent bonds

A

Bonds between two or more non-metal atoms involving the sharing of electron pairs between atoms.

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27
Q

Are carbon compounds relatively stable

A

yes

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28
Q

Why can carbon form double bonds/rings

A

they are of a small size so can get close enough

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29
Q

Why can carbon form bonds and chains of various lengths

A

covalent bonds with self

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30
Q

Second best atom for this

A

silicon

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31
Q

Why are carbon compounds diverse

A

because can form 4 bonds

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32
Q

What is bond energy

A

the measure of the amount of energy needed to break apart 1 mole of covalently bonded molecules in the gaseous state

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33
Q

Why organic chemistry is important

A

drugs/medicine, agriculture, industrial applications

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34
Q

What are natural compounds

A

carbohydrates, protein, fats/oils, hydrocarbons, enzymes, vitamines, alkaloids

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35
Q

What are carbohydrates needed for

A

source of energy in food

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36
Q

What are proteins needed for

A

source of compounds for growth and repair of tissues in body

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37
Q

What are the applications of fats and oils/role in the body

A

source of energy found in food, stored in body, used in cooking, soaps

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38
Q

hat are Hydrocarbons used for

A

fuels, petrol, cooking

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39
Q

What are enzymes

A

complex protein molecules found in plants and animals, catalysis of biochemical reactions

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40
Q

Where are alkaloids found

A

found in variety of compounds including medicines

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41
Q

Synthetic compounds examples

A

soaps/detergents, antibiotics, polymers

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42
Q

What are aliphatic compounds

A

Describes organic compounds in which carbon atoms form open chains.

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43
Q

Aromatic compounds

A

Describes a compound that contains at least one benzene ring and is characterised by the presence of alternating double bonds within the ring.

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44
Q

Alkanes

A

saturated, simple carbon compounds containing only single bonds

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45
Q

General formula for Alkanes

A

CnHn+2

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46
Q

Saturated hydrocarbons

A

Hydrocarbons containing only single carbon–carbon bonds and they cannot take up any more hydrogens.

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47
Q

Unsaturated hydrocarbons

A

Hydrocarbons containing at least one double carbon–carbon bond.

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48
Q

Bond angle of methane

A

109.5 degrees

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49
Q

Homologous series

A

A series of organic compounds that have the same structure but in which the formula of each molecule differs from the next by a CH2 group.

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50
Q

Use of methane

A

fuel

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51
Q

Use of ethane

A

manufacture of ethene

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52
Q

Use of propane

A

fuel, aerosols

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53
Q

Use of butane

A

fuel, aerosols

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54
Q

Formulas in which compounds can be written

A

molecular, empirical, structural, semi-structural/condensed, skeletal, 3D structural

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55
Q

Structural isomers

A

Molecules that have the same molecular formula but different structural formulas.

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56
Q

Alkenes

A

The family of hydrocarbons that contain one carbon–carbon double bond.

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57
Q

What is ethene known as

A

ethylene

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58
Q

Alkynes

A

The family of hydrocarbons with one carbon–carbon triple bond.

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59
Q

Cyclohexane

A

A pungent saturated cyclic hydrocarbon C6H12 found in petroleum.

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60
Q

General formula of cycloalkanes

A

CnH2n.

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61
Q

Aliphatic compound example

A

cycloalkanes

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62
Q

Benzene

A

An aromatic hydrocarbon with the formula C6H6. Lack of reactivity, high stability and same bond lengths between the carbon atoms.

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63
Q

Benzene is used for

A

used to produce food, pharmaceuticals but is carcinogenic

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64
Q

Simplest homologous series

A

alkanes

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65
Q

Functional group

A
  • group of atoms attached to or part of a hydrocarbon chain that influence the physical and chemical properties of the molecule. Determines function of compound.
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66
Q

Is a compound with or without a functional group more stable

A

without as if a functional group is attached, it is more likely to react

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67
Q

Do compounds with functional groups form a homologous series

A

yes

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68
Q

Hydroxyl group

A

OH functional group

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69
Q

Alcohols/alkanols

A

hydrocarbons containing the OH functional group

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70
Q

Carboxyl group

A

the COOH functional group, which has weakly acidic properties.

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71
Q

Carboxylic acids

A

Hydrocarbons containing the COOH functional group

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72
Q

Alcohol functional group

A

hydroxyl

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73
Q

Alcohol suffix

A

ol

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74
Q

Aldehyde functional group

A

aldehyde (HC=O)

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75
Q

Aldehyde suffix

A

al

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76
Q

Ketone functional group

A

carbonyl (C=O)

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77
Q

Ketone suffix

A

one

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78
Q

Carboxylic acid functional group

A

carboxyl (COOH)

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79
Q

Carboxylic acid suffix

A

oic acid

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80
Q

Ester functional group

A

ester (OCO)

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81
Q

Ester suffix

A

alkyl alkanoate (alcohol carboxylic acid)

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82
Q

Ether functional group

A

ether (R-O-R)

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83
Q

Amine functional group

A

amine/amino NH2

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84
Q

Amine suffix

A

amine

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85
Q

Amide functional group

A

amide (O=CNH2)

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86
Q

Amide suffix

A

amide

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87
Q

Primary alcohol

A

C-OH is attached to one other carbon atom

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88
Q

Secondary alcohol

A

C-OH is attached to two other carbon atoms

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89
Q

Tertiary alcohol

A

C-OH is attached to three other carbon atoms

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90
Q

What is a property aldehydes are known for

A

smell

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91
Q

What do the low molecular weight aldehydes smell like

A

unpleasant

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92
Q

What do high molecular weight aldehydes smell like

A

pleasant

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93
Q

Uses of aldehydes

A

perfumes, solvents, manufacture of plastic, dyes, pharmaceuticals

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94
Q

Uses of carboxylic acids

A

making soaps and polyesters, found in foods

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95
Q

Ester

A

An organic compound formed from a condensation reaction between an alcohol and a carboxylic acid.

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96
Q

Ester is used in

A

paints, perfumes, cosmetics, artificial flavourings found in fruits

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97
Q

Primary, secondary and tertiary amines determined by

A

how many C connected to N

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98
Q

Amine called … if high functional group

A

amino if higher functional group

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99
Q

Amide uses

A

solvents in a variety of pharmaceuticals, creating nylon and other polymers, to colour crayons/pencils

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100
Q

Priority for naming scale

A

carboxylic acid > ester > amide > aldehyde > ketone > alcohol > amine > alkyne=alkene > alkane

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101
Q

Organic reactions

A

reactions that take place between organic compounds

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102
Q

Types of organic reactions

A

Addition, decomposition, combination, substitution, rearrangement

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103
Q

3 types of intermolecular forces

A

dispersion forces, dipole-dipole attractions and hydrogen bonding

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104
Q

What are physical properties affected by

A

size, shape structure and degree of polarisation of molecules

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105
Q

Simple organic compounds are generally (what state)

A

gases, volatile liquids or solids with low melting and boiling points (because intermolecular forces are weak)

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106
Q

What is the strength of dispersion forces affected by

A

shape and size of molecules

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107
Q

Isomers

A

two or more compounds with the same molecular formula but different arrangements of atoms

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108
Q

Structural isomers

A

Molecules that have the same molecular formula but different structural formulas.

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109
Q

When do isomers have different physical and chemical properties

A

when different functional group

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110
Q

Why do isomers have different physical and chemical properties when there is a different functional group

A

Functional isomers have different intermolecular forces and distinctly different properties.

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111
Q

Three types of structural isomers

A

chain isomers, positional isomers, functional isomerism.

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112
Q

Chain isomer

A

A type of structural isomer that involves more branching.
In chain isomers, more branched isomers have lower boiling points. Could be because more spherical and has less surface area for the dispersions forces to act.

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113
Q

Positional isomers

A

Isomers where the position of the functional group differentiates the compounds.

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114
Q

What does the position of the functional group affect

A

compactness and polarity

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115
Q

Functional isomers

A

Isomers containing different functional groups.

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116
Q

Stereoisomers

A

Two or more compounds differing only in the spatial arrangements of their atoms. The atoms are connected in the same order but are oriented differently in space

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117
Q

Types of stereoisomers

A

cis and trans isomers, enantiomers or optical isomers

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118
Q

Cis-trans isomers

A

types of stereoisomers that are formed when the same two different groups are bonded to each of the carbon atoms in a carbon-carbon double bond. A cis isomer has identical groups on the same side of the double bond; a trans isomer has the groups on opposite sides.

119
Q

Is cis or trans stronger

A

cis (e.g in trans the dipoles may cancel out)

120
Q

Does trans or case have higher boiling points

A

cis is higher

121
Q

Does trans or cis have a higher melting point

A

trans is higher as they can pack more closely

122
Q

Can trans and cis occur in rings

A

yes

123
Q

Chiral

A

Describes compounds containing an asymmetric carbon atom or chiral centre. The molecule cannot be superimposed upon its mirror image.

124
Q

Chiral centre

A

An asymmetric carbon atom.

125
Q

Enantiomers

A

Chiral molecules that are non-superimposable mirror images of one another.

126
Q

Are enantiomers symmetrical

A

no

127
Q

Are the physical/chemical properties the same for enantiomers

A

physical properties are identical (except for optical activity) and their chemical properties are generally the same, but they react differently with other molecules that have optical properties.

128
Q

What it’s called when it’s not chiral

A

achiral

129
Q

What is necessary for something to be achiral

A

2 or more groups attached to tetrahedral are the same

130
Q

What are the states of alkanes

A

first 4 are gases, because as the size of the molecule increases, so does the influence of the dispersion forces; therefore, the melting and boiling points increase.

131
Q

What affects boiling point

A

dispersion forces, degree of branching

132
Q

Does branching increase or decrease boiling points

A

decrease due to the inability of molecules to get closer to each other; as the dispersion forces operate over a small distance only, the attraction is diminished.

133
Q

What is viscosity

A

A measure of a fluid’s resistance to flow

134
Q

The viscosity of liquid alkanes increases with…

A

the number of carbon atoms

135
Q

What increases viscosity

A

n.o. intermolecular forces, branched molecules becoming tangled

136
Q

What happens to viscosity as temp increases

A

decreases because have enough energy to overcome forces

137
Q

What is flashpoint

A

The temperature at which a particular organic compound gives off sufficient vapour to ignite in air. Of volatile liquid is the lowest temperature at which the liquid gives off enough vapour to start burning at its surface on application of an ignition source. Below the flashpoint, there is not enough vapour available to support combustion.

138
Q

What is a flammable liquid

A

is any liquid with a flashpoint below 38.7 degrees

139
Q

Liquids classified as combustible are (in terms of if they are flammable or not and why)

A

harder to ignite and have a flashpoint of 37.8 and above
At what temperatures do flammable liquids ignite and burn easily - at lower temperatures. Combustible liquids can burn at temperatures that are usually above room temperature. It is not actually the liquid that burns; it is the mixture of its vapours that burns in the oxygen in the air.

140
Q

Do smaller hydrocarbons have high or low flashpoint

A

low, as have weaker bonds and are more flammable

141
Q

Are alkanes or alkenes more reactive

A

alkenes due to double bond

142
Q

Are alkynes generally flammable

A

yes

143
Q

What does adding halogen do to strength/polarity

A

more polar, stronger bonds.

144
Q

Why do alcohols have higher boiling points than alkanes

A

OH group so hydrogen bonding + dipole-dipole

145
Q

Are alcohols soluble in water

A

smaller ones are

146
Q

Does alcohol boiling point increase with n.o. carbons

A

yes because of dispersion forces

147
Q

Does solubility of alcohol increase with n.o. of carbons

A

no due to more non-polar sections of the molecules

148
Q

Are alcohols highly flammable

A

yes

149
Q

Do volatility/flammability decrease as the alcohol molecules increases

A

The flammability of alcohols decreases as the molecules increase in size and mass due to the increased strength of attraction between the molecules. Volatility also decreases as the size of the molecule increases.

150
Q

Are carboxylic acids soluble

A

first are very soluble due to hydrogen bonding,

151
Q

Do carboxylic acids or alcohols have higher boiling points

A

carboxylic acids due to more hydrogen bonding

152
Q

Are carboxylic acids strong/weak acids

A

weak as they only partially ionise

153
Q

Are aldehydes and ketones volatile

A

yes (no hydrogen bonds)

154
Q

Does solubility increase with ketones and aldehydes with n.o carbon

A

no

155
Q

Do esters have a higher booing point than carboxylic acids

A

no as they cannot form hydrogen bonds with each other as there is no OH bond

156
Q

Does solubility increase with carbon n.o.

A

no

157
Q

Are amines weak or strong acids or bases

A

weak base

158
Q

Do amines have a higher boiling point than alcohol

A

no

159
Q

What is states of amine

A

first 2 are gases, rest are liquids

160
Q

Does solubility increase with carbon n.o.

A

no

161
Q

Alkanes are fairly…

A

un-reactive: they do not dissolve in water, nor react with acids/bases

162
Q

Substitution reaction

A

Reactions in which one or more atoms of a molecule are replaced by different atoms.

163
Q

What is cracking

A

The process of breaking down complex chemical compounds by heating them. A process that uses heat and pressure, and sometimes a catalyst, to break larger hydrocarbon molecules into smaller molecules, including an alkene and hydrogen, or an alkane.

164
Q

What are addition reactions

A

Reactions in which one molecule bonds covalently with another molecule without losing any other atoms. In addition reactions for alkenes, the double bond is broken, and new single bonds are formed. This is because the energy required to break the double bond is less than the energy released in the formation of two single bonds.

165
Q

How to test for unsaturation

A

add bromine to alkene

166
Q

What is needed to make ethene into ethanol

A

ethene + steam (H2O) = ethanol

167
Q

What is polymerisation

A

A process of reacting monomer molecules together in a chemical reaction to form polymer chains.

168
Q

What is a monomer

A

A molecule that links with other monomers to form a polymer.

169
Q

How to form polyethene

A

use addition polymerisation of ethene

170
Q

What is addition polymerisation

A

The process in which monomers with at least one double bond react together to form a polymer by addition reactions.

171
Q

What is a polymer

A

Giant molecules formed by repeated monomers that have been joined by covalent bonds.

172
Q

Acidified permanganate formula

A

H+/MNO4- (aq)

173
Q

Acidified dichromate formula

A

H+/Cr2O72- (aq)

174
Q

O2 (with a catalyst) can be added to alcohols to form

A

carboxylic acids and H2O is formed as a product

175
Q

What are condensation reactions

A

Reactions in which molecules react and link together by covalent bonding with the elimination of a small molecule, such as water or hydrogen chloride, from the bond that is formed.

176
Q

Polyesters are formed as a result of

A

ester linkages between monomers to form the polymer. In the formation of a polyesters, water is removed for every monomer (except for one water). Not necessarily ester monomer, just bonding.

177
Q

% yield formlula

A

% yield = mass of product/theoretical mass * 100

178
Q

Atom economy is

A

method for measuring the efficiency of a reaction that takes into account the amount of waste produced. The atom economy of a reaction considers the amount of useful product produced from a particular amount of reactants.

179
Q

% atom economy formula

A

% atom economy = mass of atoms in desired product/mass of atoms in reactants X 100

180
Q

What is chromatography used for

A

to separate the components of a mixture and to identify the components

181
Q

What is qualitative analysis

A

An investigation used to identify the presence or absence of elements, ions or molecules in a sample. (What is in a substance)

182
Q

What is quantitative analysis

A

An investigation used to determine the amount of a given element or compound.

183
Q

What is spectroscopy

A

The investigation and measurement of spectra produced when matter interacts with or emits electromagnetic radiation.

184
Q

Types of spectroscopy

A

mass spectrometry, NMR spectroscopy, IR spectroscopy

185
Q

What is mass spectrometry

A

The investigation and measurement of the masses of isotopes, molecules and molecular fragments by ionising them and determining their trajectories in electric and magnetic fields.

186
Q

What happens in mass spectrometry

A

molecules are bombard with high-energy electrons causing them to fragment and lose electrons, resulting in positive ions formed

187
Q

Base peak

A

The most abundant/common ion in a mass spectrum - assigned a height of 100 - highest on the graph

188
Q

Why is it the most common

A

most stable or can be formed in different ways

189
Q

If there is a mass of 15 what is the fragment likely to be

A

methyl group

190
Q

What is infrared spectroscopy

A

Describes spectroscopy that deals with the infrared region of the electromagnetic spectrum.

191
Q

Do all objects emit IR radiation

A

yes

192
Q

Why is infrared radiation used

A

as it is either emitted or absorbed by molecules when the bonds change their vibrational movements

193
Q

What happens to the vibrational energy during IR spectroscopy

A

goes from the ground state to the excited state. A molecule can move from a lower to a higher vibrational energy level if it absorbs an amount of energy equal to the difference between levels.

194
Q

What happens to the wave number as the wave length increases

A

it decreases

195
Q

The more complicated the region on IR below 1000cm-1…

A

the more complex the molecule

196
Q

Why is there a CH2 group near the OH in ethanol

A

because the OH is pulling it towards itself

197
Q

What does NMR stand for

A

nuclear magnetic resonance

198
Q

What two compounds can be used in NMR

A

13C and 1H

199
Q

What happens when an external magnetic field is applied

A

the spinning nuclei either align with the external field or align against it

200
Q

Which one has the higher energy level (either with or against)

A

against

201
Q

What does applying radio waves do

A

causes the nucleus to flip which releases energy

202
Q

Basis of NMR

A

the amount of energy required to change its spin state depends on the environment type

203
Q

Main types of NMR

A

carbon-13 NMR, low-resolution proton NMR (H1), high-resolution proton NMR (H1)

204
Q

What does TMS stand for

A

tetramethylsilane (CH3)4Si

205
Q

Is NMR quantitative or qualitative

A

qualitative

206
Q

What does the number of peak sets tell us

A

the number of unique environments

207
Q

What does the chemical shift tell us

A

information about the functional groups involved

208
Q

What does the n.o of sub-peaks/area under peak set tell us

A

n.o of H present in neighbouring environments

209
Q

What is the scale for 13CNMR

A

0-250ppm

210
Q

What is the scale for 1HNMR

A

0-13ppm

211
Q

What is it called when you analyse relative area under each peak set

A

integral trace

212
Q

Rule to determine n.o of H in adjacent environment

A

n+1 rule

213
Q

What does HPLC stand for

A

high performance liquid chromatography

214
Q

What is the mobile phase

A

The liquid or gas that flows through a chromatography system, moving the materials to be separated at different rates over the stationary phase.

215
Q

What is the stationary phase -

A

A solid with a high surface area, or a finely divided solid coated with liquid. It shows different affinities for various components of a sample mixture when separating them by chromatography.

216
Q

What is used in paper chromatography

A

usually cellulose or filter paper covered with water or ethanol

217
Q

What is used in thin-layer chromatography

A

finely divided adsorbent material is coated onto either a glass slide or aluminium foil to form stationary phase and liquids are used for mobile phase

218
Q

What is adsorption

A

The adhesion of atoms, ions or molecules from a gas, liquid or dissolved solid to a surface.

219
Q

What is desorption

A

The removal of a substance from or through a surface; the opposite of adsorption.

220
Q

What is generally used as a stationary phase for HPLC

A

narrow column that is packed tightly with a finely divided powder (high SA)

221
Q

Examples of powders used

A

alumina or silica

222
Q

What is an eluent

A

A substance used as a solvent in separating materials.

223
Q

What is a sample

A

what is being analysed

224
Q

What are analytes

A

The components of a sample.

225
Q

What is retention time

A

The time taken for each component of a sample to travel from the injection port to the end of the column.

226
Q

Area under each peak shows…

A

amount/concentration of substance

227
Q

Normal-phase liquid chromatography

A

mobile phase is non-polar and stationary phase is polar

228
Q

Reverse-phase liquid chromatography

A

mobile phase is polar and stationary phase is non-polar

229
Q

What is most commonly used in HPLC

A

reverse-phase

230
Q

What are the axes for calibration curve

A

peak area is the y axis and concentration is the x axis

231
Q

What is likely to be compound if it evolves H2 when mixed with Mg

A

carboxylic acid

232
Q

Volumetric analysis

A

Determination of the concentration, by volume, of a substance in a solution, such as by titration. Quantitative analysis.

233
Q

pH formula

A

pH = -log10[H3O+] concentration

234
Q

Hydronium/OH formula

A

[H3O+][OH-]=Kw where Kw = 1.010^-14

235
Q

What is a pipette

A

instrument used to accurately measure or transfer small quantities of liquid

236
Q

What is the aliquot

A

unknown concentration

237
Q

What is the titrant

A

solution of known concentration

238
Q

What is the burette

A

A graduated glass tube for delivering known volumes of a liquid, especially in titrations.

239
Q

What is titration

A

Process used to determine the concentration of a substance by using a pipette to deliver one substance and a burette to deliver another substance until they have reacted exactly in their mole ratios.

240
Q

What is the titre

A

The volume delivered by a burette.

241
Q

2 types of titration

A

acid-base and redox

242
Q

What is the standard solution

A

A solution that has a precisely known concentration.

243
Q

What are the two methods of determining the concentration

A

reacting it with other solution whose concentration is known accurately (standardisation) or dissolving a primary standard into a known volume of water

244
Q

What is the primary standard

A

A substance used in volumetric analysis that is of such high purity and stability that it can be used to prepare a solution of accurately known concentration.

245
Q

Primary standards must be…

A

abundant, accurately known formula, high state of purity, cheap and readily available, relatively high molar mass,

246
Q

Why shouldn’t NaOH be used

A

absorbs moisture, reacts with CO2

247
Q

Why shouldn’t hydrated sodium carbonate

A

unsuitable as it loses water to atmosphere but can be heated to remove water then used

248
Q

What is the volumetric flask used to contain

A

primary standard

249
Q

What is the equivalence point

A

Where two reactants have reacted in their correct mole proportions in a titration.

250
Q

What is the end point

A

The experimentally determined/approximated equivalence point at which the indicator just changes colour or the pH curve becomes vertical. Occurs after slight excess.

251
Q

Titration curve

A

Curve used to measure the volume of a titrant against pH.

252
Q

Concordant titres

A

Describes titres that are within a defined volume of each other, such as 0.10 mL.

253
Q

Concentration formula using mol and volume

A

n=cV

254
Q

Concentration formula using volumes

A

c1V1=c2v2

255
Q

What is a diprotic acid

A

can donate 2 protons

256
Q

What is a monoprotic acid

A

can donate 1 proton

257
Q

What is a polyprotic acid

A

can donate more than 2 protons

258
Q

What is an amphiprotic acid

A

can donate or accept protons

259
Q

What is the retention time for large molecules

A

higher retention time

260
Q

What is the retention for molecules that are soluble in mobile phase

A

shorter retention time

261
Q

What are the axes for chromatogram

A

y axis is absorbance and x axis is retention time in minutes

262
Q

What does elution rate mean

A

how fast it is passed out of column

263
Q

Order of elution in normal phase in order of first elution to last

A

alkanes/alkenes, esters, alkyl halides, alcohols, carboxylic acids. It also goes shortest chain to longest chain.

264
Q

What is the wavelength symbol

A

ʎ m

265
Q

What is the wavelength in terms of the graph

A

the period of the graph

266
Q

What is wave number proportional to

A

frequency

267
Q

What happens if the frequency increases

A

the wavelength decreases and the energy of a photon increases

268
Q

Formula for wave number

A

wavenumber = 1/wavelengthcm-1

269
Q

What do large wavelengths mean

A

small wave numbers

270
Q

What is the absorbance relative to

A

the concentration

271
Q

Formula for delta E for NMR

A

delta E = hv where hv is radio energy

272
Q

In NMR where is polar and where is shield thickness

A

low energy and polar is the left and left to right is decreasing shield thickness

273
Q

What shape is the titration curve

A

S-shaped

274
Q

Why is no indicator required for redox titration

A

as there is usually a colour change

275
Q

What are the axes for IR

A

the y axis is transmittance and the x axis is the wave number

276
Q

What are the names for the number of sub-peaks in NMR

A

singlet, doublet, triplet, quartet,

277
Q

Formula for Rf

A

Rf=distance travelled by component/distance travelled by solvent

278
Q

What does Rf stand for

A

retardation factor

279
Q

What are the units for Rf

A

no units

280
Q

What will titration curve look life for strong acid-weak base titration

A

fairly spread out titration S-shaped curve

281
Q

What will titration curve look life for weak-acid strong base titration

A

very un-spread out (vertically)

282
Q

What does strong acid and strong base form + pH

A

extremely weak conjugate base and extremely weak conjugate acid - pH of 7

283
Q

What does strong acid and weak base form + pH

A

extremely weak conjugate base and weak conjugate base - pH is over 7

284
Q

What does weak acid and strong base form

A

extremely weak conjugate acid and weak conjugate acid - pH less than 7

285
Q

What is the tallest peak called in mass spectroscopy

A

base peak

286
Q

What does the parent ion/peak tell us in mass spectroscopy

A

the molecular mass

287
Q

What is the charge for all the ions on mass spectrum

A

+ 1

288
Q

What does IR show

A

functional groups

289
Q

Basis of IR

A

amount of IR absorbed depends on type of bond

290
Q

What is the wave length for stronger bonds

A

higher wave length

291
Q

What does the mass spectroscopy tell us

A

molecular formula

292
Q

What is high resolution NMR

A

when it has sub-peaks that tell you n.o of H

293
Q

What is low resolution NMR

A

no sub peaks

Year 12 Chemistry (7 decks)

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