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Trials Flashcards

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1
Q

AAS definition and process

A

Using atomic absorption spectrometry (AAS) a sample solution containing an element is vaporised in a hot flame. Radiation from a cathode lamp of a particular wavelength is absorbed by the atom’s electrons. Unabsorbed light is passed through a wavelength selector and a detector. A computer determines the amount of absorbance as a measure of the concentration of the metal ions present in the sample.

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2
Q

Production of alcohol

A

-Substitution reaction of haloalkanes with hydroxide (OH⁻)
-Fermentation of sugar/carbohydrates

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3
Q

Oxidation of alcohols (each degree)
reagent

A

Primary - First to aldehydes then to carboxylic acids
Secondary - Ketones
Tertiary - Don’t Oxidize
H⁺/Cr₂O₇²⁻ (acidified dichromate)
H⁺/MnO₄⁻ (acidified permanganate)

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4
Q

condensation equation

A

Alcohol + Carboxylic Acid→ Ester + Water

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5
Q

4 types of addition reactions

A

Hydration, Hydrogenation, Hydro-halogenation and Halogenation

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6
Q

Common ion effect

A

The solubility of a salt is reduced by the presence of one of its constituent ions (the common ion)
already in the solution. The presence the common ion drives the equilibrium towards
precipitation through Le Châtelier’s principle

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7
Q

Fermentation of alcohols conditions

A
  1. Enzyme zymase (found in yeast)
  2. Warm temp (30-40C)
  3. Anaerobic (absence of oxygen)
  4. Aqueous solution
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8
Q

Fermentation of glucose equation

A

C6H12O6 –> (zymase) 2C2H6O +2CO2

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9
Q

Arrhenius definition and equations

A

Acids: dissociate in water to produce hydrogren ions
HCl(aq)→H+(aq)+Cl−(aq)

Bases: dissociate in water to produce hydroxide ions
NaOH(aq)→Na+(aq)+OH−(aq)

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10
Q

Arrhenius adv with equation

A

Explains neutralisation, proposing hydrogen and hydroxide ions forming water
HCl(aq)+NaOH(aq)→NaCl(aq)+H2O

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11
Q

Arrhenius disadv with equations
(3)

A
  1. Compounds without hydroxide ion displaying basic properties like metal oxides and metal carbonates
    2HCl(aq)+CaCO3(s)→CaCl2(aq)+H2O(l)+CO2(g)
  2. Neutrally charged salts like ZnCl2 being acidic in solution, whilst others are basic like Na2S
  3. Acid-base reactions that do not occur in aquous solution
    NH3(g)+HCl(g) ⇋ NH4Cl(s)
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12
Q

Bronsted Lowry definitions with equations

A

Acids; proton donors
HCl(aq)+H2O(l)→H3O+(aq)+Cl−(aq)

Bases: proton acceptors
NH3(aq)+H2O(l)⇋NH+4(aq)+OH−(aq)

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13
Q

Bronsted Lowry advantages with equations
(4)

A
  1. substances that do not contain hydroxide ions.
  2. role of water as more than just a solvent.
  3. include solvents other than water and reactions in non-aqueous states.
  4. conjugate acid-base pairs.
    HF(aq)+H2O(l)⇋H3O+(aq)+F−(aq)
    NH3(aq)+H2O(l)⇋NH+4(aq)+OH−(aq)
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14
Q

Bronsted Lowry disadv

A
  • not explain the acidity of acidic oxides like SO2 and SO3
  • not explain the basicity of basic oxides like MgO and CaO
  • not explain reactions of acidic and basic oxides not involving proton transfer.
    SO3(g)+CaO(s)→CaSO4(s)
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15
Q

Methyl orange range

A

3.1-4.4

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16
Q

Bromothymyl blue range

A

6.0-7.6

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17
Q

Phenophalein range

A

8.2-11.0

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18
Q

Cobalt chloride equilibrium equation (with colour changes)

H value

A

Co(H2O)6 2+ (aq) + 4Cl- (aq) <–> CoCl4 2- (aq) + 6H2O (l)
pink —————– blue

endothermic

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19
Q

Iron (III) thiocyanate equilibrium equation (with colour changes)

H value

A

Fe3+ (aq) + SCN- (aq) <—-> FeSCN 2+ (aq)
yellow—colourless——blood-red

exothermic

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20
Q

H: -
S: +

A

spontaneous

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21
Q

H: +
S: +

A

spontaneous if T is high

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22
Q

H: -
S: -

A

spontaneous if T is low

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23
Q

H: +
S: -

A

non-spotaneous

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24
Q

What is favoured in terms of collision theory temperature increases

A

If endothermic reaction: reverse favoured
If exothermic: forward favoured
(less energy needed to surpass activation energies)

Endothermic reactions have higher increase in reaction rate due to low value?

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25
Q

VALIDITY

A

Aim
Constant
Equipment
Range

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26
Q

RELIABILITY

A

Repeated
Outliers
Consistent
Aveaged

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27
Q

ACCURACY

A

Scale
equipment
Rrecorded
Close to therorital

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28
Q

Catalyst effect

A

Lower activation energy
Increased reaction rate for fwd and rvs

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29
Q

Inert/unreactive gas effect

A

no effect, lowers rate of rxn for both sides

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30
Q

Detoxyfying cycads

A

Leaching: use of water to dissolve the toxin and remove it from the plant
“When the seeds are soaked in water (e.g. a river or creek), the flowing water reduces the concentration of aqueous cycasin, disturbing the equilibrium. According to Le Chatelier’s principle, the equilibrium will shift right to produce more aqueous cycasin and minimise the disturbance, hence increasing the rate at which cycasin dissolves.”

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31
Q

Buffer region of titration curves (explain)

A

OH- and H+ react
Little change occurs since OH is in excess at the start (or other way around)

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32
Q

strong acid strong base titration curve
(eq point range, indicator to use)

A

4-10
all 3 (or bromothymyl blue)

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33
Q

strong acid weak base titration curve
(eq point range, indicator to use)

A

3-7
methyl orange

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34
Q

weak acid strong base titration curve
(eq point range, indicator to use)

A

7-11
phenophalein

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35
Q

Conductivity rules

A

OH and H have the most mobility and create an electrical current
Curve decreases as OH and H react and conductivity is held by Na which has low conductivity

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36
Q

Which conductive curve is the non-straight round one?

A

Weak acid strong base

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37
Q

Which conductive curve is the one that increases at the start?

A

weak acid weak base

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38
Q

Why is it that in a weak base and weak acid conductivity curve, it increases at the start?

A

Acid and base molecules react to become ions (acid donates H+)
More ions means more conductivity

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39
Q

Carbonic buffer system in blood equation
Why is it there
pH range
Alkalosis and acidosis
Ions it is between

A

H2CO3 (aq) + H2O (l) <—> HCO3 - (aq) + H3O+ (aq)
Controls how much H+ and OH- in cells, tissues
Importance for metabolic processes and enzymes to function
7.35-7.45
Alkalosis: hyperventilation, low levels of CO2
Acidosis: diseases
H2CO3 and HCO3 -

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40
Q

What type of combination do you need for a buffer?

A

WEAK acid/base and conj
Large conc for better capacity
Equal moles/conc

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41
Q

Ketone and aldehyde oxygen placement

A

Ketone: middle
Aldehyyde: end

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42
Q

Hydrocarbons with distinct smells

A

Amine (ammonia, fishy), esters

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43
Q

Polarity rule (lone pairs for amine)

A

The presence of lone pair of electrons causes repulsion, and thus it affects the bond angle. Thus, it can increase or decrease the polarity of a molecule.

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44
Q

Hierarchy of boiling points (lowest to highest)

A

alkane, amine/aldehyde, ketone, alcohol, carboxylic acid, amide

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45
Q

how are esters and amides produced

A

condensation reactions

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46
Q

Reliability

A

the consistency of experimental results over mutiple trials under the same conditions

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47
Q

Validity

A

the extent to which the aim of the experiment is fulfilled fairly

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48
Q

Accuracy

A

the closeness of agreement between an experimental result and the accepted theoretical value

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49
Q

Petrol
How is it produced?
Chemical composition?
Combustion equation?

A

Fractional distillation of crude oil. Catalytic cracking of larger fractions from crude oil.

Hydrocarbons like octane and heptane

C8H18(l) + 25/2 O2(g) –> 8CO2(g) + 9H2O(l)

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50
Q

Petrol
Enthaply of commbustion?
Source?
Renewable or non?
CO2 emissions?
Vehicle modification?

A

48kj/g
Crude oil
Non-renewable
High net release during production and use
None

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51
Q

Petrol
Running costs?
Environmental impacts

A

Depends on the price of petrol at the time! Sometimes more expensive than ethanol, sometimes not

Mining, accidents, net release of CO2 higher than biofuels, oil spills

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52
Q

Ethanol
How is it produced?
Chemical composition?
Combustion equation?

A

Fermentation of glucose from biomass (plant sugars) and/or hydration of ethene

ethanol

C2H5OH(l) + 3O2(g) –> 2CO2(g)+ 3H2O(l)

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53
Q

Ethanol
Enthaply of commbustion?
Source?
Renewable or non?
CO2 emissions?
Vehicle modification?

A

29.6 kj/g

Biomass/sugar cane/ molasses

Renewable

Lower net release during combustion since recently removed from atmosphere through photosynthesis

if under 10% no modification needed

54
Q

Ethanol
Running costs?
Environmental impacts

A

Depends on the price of petrol at the time! Sometimes more expensive than petrol, sometimes not

Growing sugarcane to provide sugar uses a lot of land that could be used for food production. Better if using leftover biomass

55
Q

Biodiesel
How is it produced?
Chemical composition?
Combustion equation?

A

From plant oils such as soybean, corn, palm oils.

Esters made from fatty acids of oils

Ester + oxygen –> CO2 + H2O

56
Q

Biodiesel
Enthaply of commbustion?
Source?
Renewable or non?
CO2 emissions?
Vehicle modification?

A

37.2
Usually from waste oils from restaurants and industry.

Renewable

Some release associated with production

Diesel engine required. Up to 20% biodiesel mixed with ordinary diesel does not require modification

57
Q

Biodiesel
Running costs?
Environmental impacts

A

Cheaper than regular diesel.

Using leftover oils reduces need to plant crops and use arable land specifically for production of biodiesel.

58
Q

Molecular formula for alkane

A

C(n)H(2n+2)

59
Q

Molecular formula for alkene

A

C(n)H(2n)

60
Q

Molecular formula for alkyne

A

C(n)H(2n-2)

61
Q

Molecular formula for alcohols

A

C(n)H(2n+2)O

62
Q

Molecular formula for carboxylic acid

A

C(n)H(2n)O2

63
Q

Molecular formula for aldehyde/ketones

A

C(n)H(2n)O

64
Q

Endpoint

A

The point during a titration when the indicator first produces a permanent colour change and this indicates that equivalence point has been reac

65
Q

What causes each colour change for H+/MnO4-

A

Original: purple (same ion)
MnO2 (s): brown ppt –> aldehyde
Mn2+ : colourless –> carboxylic acid

66
Q

What are the colour changes of H+/CrO4 2-

A

Orange –> green

67
Q

What are the oxidising reagents called

A

ACIDIFIED potassium permanganate
ACIDIFIED Potassium dichromate

68
Q

What do fangs on a IR spec indicate?

A

n-H bonds (number of fangs=number of H’s)
2 fangs: primary amide
1 fang: secondary amide or terminal alkyne

69
Q

If the oxidation colour stays ornage that means…

A

Not a primary/secondary or aldehyde functional group (all oxidisable)

70
Q

Words to use in HNMR spec

A

Terminal: at the end
Non-terminal environment
This hydrgen environment is adjecent to 3 hydrogens
Adjecent to CH2 group capable of this triplet splitting

71
Q

Flame colours of each atom
Barium
Calcium
Copper
Lithium
Pottassium
Sodium

A

Apple green
Brick red
Blue green
Crimson red
Lilac
Yellow

72
Q

Identification test
Cl-

A

Forms a white ppt with acidified Ag+ solution which dissolves in dilute ammonia to form a colourless complex

73
Q

Identification test
Br-

A

Forms a cream ppt with acidified Ag+ solution which dissolves in concetrated ammonia to form a colourless complex

74
Q

Identification test
I-

A

Forms a yellow ppt with acidifed Ag+ solution which does not dissolve in ammonia

75
Q

Identification test
OH-

A

pH greater than 7 (turns litmus blue) or forms a blue ppt with Cu2+

76
Q

Identification test
CH3COO-

A

Forms a red-brown complex when reacted with FeCl3

77
Q

Identification test
CO3 2-

A

Forms bubbles when HNO3 is added and the gas turns limewater milky (CO2)

78
Q

Identification test
SO4 2-

A

Forms a white ppt with either acidified Ba2+ or acidified Pb2+

79
Q

Identification test
PO4 3-

A

Prodcues a yellow ppt with acidified (NH4)MoO4 (ammonium molybdate)

80
Q

Identification test
Ba2+

A

Forms no ppt with F- (add NaF)

81
Q

Identification test
Ca2+

A

Forms a white ppt with F- (add NaF)

82
Q

Identification test
Mg2+

A

Forms a white ppt with OH-

83
Q

Identification test
Pb2+

A

Forms a yellow ppt with I- (add NaI solution)

84
Q

Identification test
Ag+

A

Forms a white ppt with Cl- which will dissolve ammonia, forming a complex

85
Q

Identification test
Cu2+

A

Produced a deep blue complex with ammonia and water

86
Q

Identification test
Fe2+

A

Decolourises acidified potassium permanganate solution

87
Q

Identification test
Fe3+

A

Forms a blood red complex with SCN- (add KSCN)

88
Q

Colourimetry process

A

a light source which produces light that is absorbed by the solution; this is passed through a filter to select a particular colour of light required for the analysis
* a transparent cell to hold the sample
* an electronic detector to measure the intensity of light that passes through the cell
* a recorder or electronic display that shows how much light was absorbed by the sample.

needs various standard solutions of the ion to test for different colourimetry

89
Q

UV Vis spec (quantitative)

A

Colorimeters are cheap and can be used easily in school laboratories.
However, their accuracy is limited.
* UV-Visible spectroscopy is like a colorimeter, but has higher accuracy
* UV-Vis uses a monochromator rather than a filter to select light of an
exact wavelength to be used in the analysis.

90
Q

What do safety precautions for hydrocarbons help do?

A

Prevent the buildup of vapours, reduces risk of fuel igniting

91
Q

As carbon chain length increases…

A

more elecrons, stronger dispersion forces, increases mp/bp, overpowers other intermolecular forces

92
Q

Ketone and aldehyde IMF and solubility

A

dipole-dipole
- as chain length icnreases, more dispersion forces decrease solubility (dipole dipole with water)

93
Q

Special property about tertiary amides

A

Cannot hydrogren bond

94
Q

Petrol
Environmental, eocnomic, social implications

A

Social: provides jobs and income

Economic: oil spills –> economic losses, ruin fisheries and fishing industry, USA Russia and Saudi Arabia have largest reserves, large oil industry

Environmental: mining (land degradation, habitat destruction, deforestation, oil spills, pollution of water ways
Fractional distillation: requires heat input which is burning fossil fuels (CO2 emissions)

95
Q

Disadv of soap

A

Cannot be used in acidic conditions
Cannot be used in hard water -> forms soap scum with Mg and Ca ions

96
Q

Events of removing grease using soap

A

Process
1. The non-polar ends of the soap ions bond to the surface of the grease via dispersion forces.
2. The ionic ends bond to water molecules via H-bonding/ion dipole interaction.
3. The grease on clothing or on skin is loosened by agitation or rubbing.
4. The non-polar ends of the soap ions surround more and more of the grease droplet as it is loosened from the surface by further agitation.
5. The result is a micelle, with a spherical shape -the grease droplet is surrounded by the non-polar ends of many soap ions, with the ionic ends bonding to water.
6. Thus, the grease is dispersed throughout the water in the form of an emulsion - the emulsion is the soap, water and grease mixture.

97
Q

Anionic detergents

A

sulfonate head
uses: shampoos,
dishwashing detergents, washing
powders
forms soluabe complex with hard ions

98
Q

catonic detergents

A

bonds to - charge – reduce static
uses: hair conditioners, fabric
softeners, disinfectants.

99
Q

non ionic detergents

A

not lather much
uses: Dishwashing detergents
Glass Cleaners

100
Q

Esters IMF

A

dipole dipole
unable to hydrogen bond as they have no H directly connected to O

101
Q

Qsp < Ksp

A

no ppt (high conc of ppt, so eq moves to right to produce ions)

102
Q

Qsp > Ksp

A

yes ppt (high conc of ions, so eq moves to left to produce ppt)

103
Q

Neutralisation examples

A

Agriculture: adding powdered lime, CaO, limestone to acidic soils

Industry: acid or base spills, netrualisating acidic emissions from factories or power plants

Heath: treating patients who have indigestion

Home: preventing tooth decay by neutralising acids, using baking powder in food preperation

104
Q

Flame test explanation

A

When atoms are heated, the outer shell electrongs absorb energy and become excited, moving to higher energy levels. The atoms are unstable and the electrongs quickkly move back to a lower energy state, emitting energy as light of a specific wavelength and colour. If in the visible region, the flame appears an characteristic colour.

105
Q

Limit of flame tests

A

Can only identify a few metal unambigously, because many flame colours are similar or are masked by colours of other metals that may be present

106
Q

Complexation reactions

A

Form complex ion, usually involving trasition metals (Fe, Ag)
Consists of central metal cation surrounded by 1-6 bound polar molecules or anions (called ligands)

107
Q

Steps of gravimetric analysis

A
  1. Weight sample
  2. Dissolve in solvent (water)
  3. Add excess reactant to form ppt
  4. Filter ppt and wash filter paper with water
  5. Dry ppt in oven
  6. Weight ppt sample
108
Q

UV visible spec process

A
  1. Standard solutions prepared
  2. A wavelength is selected at which the component absorbs light strongly
  3. Absorbance of the standard solution at that wavelength measured
  4. Calibration curve graphed using conc of standard solutions
109
Q

AAS

A

The sample is atomised in a flame. Electrons in atoms absrob light energy of specfic wavelengths, whih causes the elctrons to jump to higher energy levels. A hallow cathode lamp produces light in specific wavelengths that the metal atom can absorb. Wave length selector and detercter determines concentration by consutrcting calibration curve using absorbance.

110
Q

Mass spectroscopy process

A

Electron beam removes electrons, creating cations. Presence of electric and magnetic field leads to cations moveing in curved paths dependent on mass/charge ratio (m/z)
Cation can be unstable. Some fragment, where one frgamnent is a cation, and other is an uncharged free radical (atom or group)
Cations are accelerated. y electric field and then deflected by magnetic field.

111
Q

Infared spec process

A

Causes bonds to stretch (change distance between atoms) and bend (change angle between bonds), as their polar bonds interact with IR light.
Single bonds absorb less energy

112
Q

NMR progress (nucleur magnetic resonance)

A

Interaction of nuclei of atom in a strong magnetic field with radio wave energy
Flips

113
Q

Aim of chemical synthesis and design

A

Aim for high yield of a pure product that is produced quickly ad efficently at a marketable price, while ensuring the health and safety of employees and minimising damage to the environment

114
Q

Points to talk about in chemical synthesis and design

A

Availability of reagents, reaction conditions, yield and purity, location, env soc econ issues

115
Q

Industrial uses of ammonia (haber process)

A

Production of fertilisers
A cleaning agent
Production of other chemicals such as explosives and synthetic fibres

116
Q

Availaibilty of reagents (haber process)

A

H2 is usually obtained from steam reforming of hydrocarbons
Steam reforming involves a reaction between natural gas and steam
N2 is from air

117
Q

haber process equation
H value

A

N2 (g) + 3H2 (g) <–> 2NH3 (g)
exothermic

118
Q

Reaction conditions of haber process

A

To increase yield:
decrease temperature (LCP favour forward exothermic and Keq increases)
increase pressure (LCP favor fwd)

To increase rate of rxn:
Increase T
Catalyst: porous Fe/Fe3O4

Temp must comprimise at moderate 350-500C, under 250atm (P)

119
Q

Yield of haber process

A

NH3 is liquiefied for easy transport
Unreacted gases are recycled to achieve 98% yeild and reduce emissions

120
Q

Waste management of haber process

A

Wasting energy –> use of hea exchangers, energy reused to preheat and generate steam during plant process –> less costs and more efficent

Production of CO2, NO2, SO2, CO in steam reforming –> liquidefy CO2, selling to food beverage fertiliser companies, monitering of emissiosn –> reduce enhanced greenhouse

Sulfur in natural gas for steam reforming produces SO2 (g) –> desulfurisation, collection of gas, sold as raw material for H2SO4 producution –> minimising acid rain, pollustion, poisining of catalysts

121
Q

Health and safety in haber process

A

Ammonia= toxic gas, fire and explosions are hazards

Wear protective clothing, gloves, face shields, rubber boots, aprons, well ventilaited factories, breathing apparatus available

122
Q

Primary standard conditions

A

High molar mass
Stable
Easily stored
Not reactive with water or atmospheric gases
Known chemical formula
Pure
Easily weighable

123
Q

Why is AAS good for multiple ions

A

Looks at one particular wavelength of one element, in ppm

124
Q

Nylon properties and uses

A

High tensile strength
Strong fribre, resistant to abrasions and moisture

Textiles, machine rubber and parts, rope, thread

125
Q

ester to primary/secondary alchohol

A

NaOH and heat

126
Q

dehydration of alchohol

A

conc H2SO4 and heat

127
Q

Alkyne to ketone

A

H2O + H2SO4 + HgSO4

128
Q

Alkyne or alkene to alkane

A

H2 + Ni

129
Q

Haloalkene or alkene to alkane

A

HX or X2 + Ni

130
Q

Haloakane to alcohol

A

NaOH + heat

131
Q
A

Chemistry (5 decks)

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