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mocks Flashcards

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1
Q

Define ionisation energy

A

Energy required to remove one e- from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous ions

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2
Q

What factors affect ionisation energy

A

Shielding
Charge of nucleus
Distance from nucleus

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3
Q

Ionisation energy pattern across periods

A

Increase
Distance from nucleus decreases and nuclear charge is increasing

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4
Q

Ionisation energies pattern down groups

A

Decrease
More shielding and greater distance

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5
Q

Four stages of TofF

A

Ionisation
Acceleration
Ion drift
Detection

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6
Q

What is dative covalent/co-ordinate bonding

A

When both electrons in the shared pair of electrons come from the same atom

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7
Q

Name and angle when co-ord no. is 2

A

180° Linear

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8
Q

Name and angle when co-ord no. is 3

A

120° trigonal planar

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9
Q

Name and angle when co-ord no. is 4

A

109.5° tetrahedral

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10
Q

Name and angle when co-ord no. is 5

A

90° and 120° trigonal bipyradimal

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11
Q

Name and angle when co-ord no. is 6

A

90° octahedral

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12
Q

Why is bonding covalent instead of ionic?

A

Small difference in electronegativity

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13
Q

Why is the m.p of aluminium higher than the m.p of sodium?

A

Al3+ has a greater charge than Na+ so there are more delocalised electrons and therefore a stronger attraction

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14
Q

How does increases charge of nucleus affect IE?

A

increases IE

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15
Q

How does increased distance from the nucleus affect IE?

A

decreased IE

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16
Q

How does increased shielding affect IE?

A

decreases IE

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17
Q

why do covalent macromolecular structures have high m.p?

A

lots of strong covalent bonds which require lots of energy to break

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18
Q

why is graphite slippery?

A

weak vdw forces between layers so layers can slide easily

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19
Q

why does graphite conduct electricity?

A

each carbon atom is bonded to 3 other carbon atoms so there are non-bonded delocalised electrons that can move through structure and conduct electricity

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20
Q

why do molecular covalent molecules have a low m.p?

A

weak vdw forces between molecules so little energy required to overcome them

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21
Q

name and shape of angle when there are 3 bonding pairs and 1 lone pair?

A

107.5 trigonal pyramid

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22
Q

does a bigger molecule have stronger vdw forces?

A

yes - more electrons

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23
Q

Difference between vdw and dipole-dipole forces?

A

vdw are temporary dipoles instead of permeant as there isn’t a big enough difference in electronegativity

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24
Q

why does ice have a greater volume than water?

A

ice has more hydrogen bonds so is arranged in a regular lattice

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25
Q

why does ice float in water?

A

less dense as has a greater volume

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26
Q

enthalpy change defintion?

A

energy change of a reaction under constant pressure

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27
Q

standard enthalpy of combustion?

A

enthalpy change when one mole of a compound is completely burnt in oxygen with all the reactants and products in their standard states

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28
Q

standard enthalpy of formation?

A

enthalpy change when one mole of a substance is formed from its elements in their standard states and under standard conditions

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29
Q

enthalpy of atomisation?

A

enthalpy change when one mole of gaseous monatomic atoms are formed from their elements

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30
Q

first ionisation energy definition?

A

enthalpy change when one mole of gaseous atoms lose one mole of electrons to form one mole of unipositive cations

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31
Q

electron affinity definiton?

A

enthalpy change when one mole of gaseous atoms gains one mole of electrons to form one mole of uni negative anions

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32
Q

lattice enthalpy of disassociation?

A

enthalpy change when one mole of a solid ionic substance is disassociated into its consituent gaseous ions

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33
Q

lattice enthalpy of formation?

A

enthalpy change one mole of a solid ionic substance is formed from its constituent gaseous ions

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34
Q

enthalpy of hydration?

A

enthalpy change when one mole of isolated gaseous ions are hydrated with an infinitely large volume of water to form one mole of aqueous ions

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35
Q

enthalpy of solution?

A

enthalpy change when one mole of an ionic solid is dissolved in an infinitely large volume of water to form its constituent ions

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36
Q

why do we use a copper calorimeter?

A

good conductor of heat and has a low specific heat capacity

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37
Q

how do you calculate heat change (calorimetry)?

A

q = m c ΔT

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38
Q

reasons why value from calorimetry experiment might be less?

A

heat lost to surroundings
incomplete combustions
(faulty thermometer)

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39
Q

what is Hess’s Law?

A

enthalpy change for a reaction is independent of the route taken

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40
Q

Le Chatelier’s principle?

A

when a factor (e.g temp or pressure) is changed, an equilibrium will shift to oppose that change

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41
Q

what are the conditions of equilibria?

A

rate of forward and backward reactions are equal

conc. of reactants and products aren’t changing

must be in a closed system

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42
Q

what happens when temp. decreases (eqm)?

A

exothermic direction is favoured, eqm shifts in that direction

means energy is released to the surroundings causing the temp. to increase

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43
Q

what happens when temp. increases (eqm)?

A

endothermic direction is favoured

energy is absorbed from the surroundings causing the temp. to decrease

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44
Q

what happens when pressure increases (eqm)?

A

eqm shifts to side with fewer moles to oppose change and decrease pressure

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45
Q

what happens when pressure decreases (eqm)?

A

eqm shifts to side with more molecules to oppose change and increase pressure

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46
Q

what is the Haber Process?

A

formation of ammonia (NH3)

N2 + 3 H2 —> 2 NH3
<—

iron catalyst

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47
Q

ammonia?

A

NH3

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48
Q

ammonium?

A

NH4 +

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49
Q

theoretical conditions and actual conditions for max. yield of ammonia?

N2 + 3 H2 —> 2 NH3
<—
(exothermic reaction)

A

theoretical:
high pressure
low temp

actual:
200 atm (expensive and engineeringly difficult)
450 c (faster rate)

compromised conditions

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50
Q

what affect does a catalyst have on the position of eqm?

A

it doesn’t - increases both forward and backward reaction so will reach eqm faster

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51
Q

what is a redox reaction?

A

when reduction and oxidation occur simultaneously

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52
Q

what is oxidation?

A

loss of electrons

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53
Q

what is reduction?

A

gain of electrons

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54
Q

what is the exception for the oxidation state of H?

A

metal hydride e.g NaH

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55
Q

oxidising agent?

A

electron acceptor (it gets reduced)

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56
Q

reducing agent?

A

electron donor (it gets oxidised)

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57
Q

entropy defintion?

A

a measure of disorder
symbol = S

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58
Q

when is a reaction feasible? (ΔS)

A

when change in entropy is positive

ΔS > 0

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59
Q

how do you calculate ΔS?

A

ΣS products - ΣS reactants

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60
Q

Gibbs free energy equation?

A

ΔG = ΔH - TΔS

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61
Q

when is a reaction feasible? (ΔG)

A

ΔG < 0 - negative

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62
Q

at which electrode does oxidation occur?

A

left - negative terminal

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63
Q

at which electrode does reduction occur?

A

right - positive terminal

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64
Q

which electrode goes on the left?

A

the lowest EMF (smallest or most negative)

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65
Q

which half equation is reversed?

A

the more negative one

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66
Q

what is the purpose of the salt bridge?

A

its soaked in ionic solution (eg KNO3) and it completes the circuit to allow electrons to flow

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67
Q

what are the conditions of the standard hydrogen electrode?

A

298 K
100 kPa
conc. of all solutions 1moldm-3

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68
Q

how do you calculate EMF?

A

EMF RHS - EMF LHS

(bigger EMF - smaller EMF)

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69
Q

rules of conventional cell representation?

A

most oxidised species on the inside (closest to salt bridge)

more negative electrode potential on LHS (except H is always on left)

phase boundary whenever you change state

platinum on end if there’s no solid

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70
Q

when and why do we use platinum in an electrochemical cell?

A

when there’s no solid and because its unreactive and a good electrical conductor

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71
Q

properties of more negative EMF?

A

favours oxidation

best reducing agent

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72
Q

properties of more positive EMF?

A

favours reduction

best oxidising agent

73
Q

when is a reaction feasible? (electrochemical cells)

A

EMF > 0

74
Q

What are batteries?

A

types of electrochemical cells which convert chemical energy into electrical energy

75
Q

where are lithium cells used and why?

A

mobiles because they’re rechargeable

76
Q

example of what a lithium cell is made from?

A

lithium cobalt oxide electrode (LiCoO2)

graphite electrode

77
Q

how do batteries recharge?

A

a current is supplied to force electrons to flow in the opposite direction and reverse the reactions

78
Q

advantages of fuel cells?

A

more efficient

only waste product is H2O

don’t need to be recharged

79
Q

disadvantages of fuel cells?

A

need energy to produce a constant supply of hydrogen and oxygen which often comes from fossil fuels

hydrogen is highly flammable

80
Q

example of hydrogen/oxygen fuel cell?

A

alkaline hydrogen - oxygen fuel cell used in vehicles

81
Q

where are the chemicals stored in a fuel cell?

A

stored separately outside cell and fed in when electricity is required

82
Q

what happens to the atomic radius across periods?

A

decreases because they have the same shielding but an increased no. of protons in the nucleus which means there is a stronger attraction

83
Q

what happens to m.p across period 3?

(Na Mg Al Si P S Cl Ar)

A

from Na –> Al increases
(they are all metals so have high m.p due to metallic bonding but increase as nuclear charge increases)

increases to Si (highest m.p)
(macromolecular structure so has lots of strong covalent bonds)

P4 S8 Cl2
(all simple covalent structures but from lowest to highest m.p. Cl2, P4, S8 as more electrons means stronger vdw)

Ar is the lowest as monatomic so very weak vdw

84
Q

what is the trend in reactivity down group 2?

A

reactivity increases as it becomes easier to oxidise atoms

85
Q

group 2 reaction with water?

A

M + 2H2O —> M(OH)2 + H2

86
Q

magnesium reaction with steam?

A

Mg (s) + H2O (g) —> MgO (s) + H2 (g)

87
Q

what is the trend in solubility with OH- ions down group 2?

A

solubility increases down the group

88
Q

what is the trend in solubility with (SO4) 2- ions down group 2?

A

solubility decreases down the group

89
Q

use of Mg(OH)2 (s) ?

A

indigestion tablets

90
Q

use of Ba(SO4) 2- (s) ?

A

barium meal (used in x-rays)

91
Q

use of Ca(OH)2 ?

A

neutralising acidic soil

92
Q

How do you test for (SO4) 2- , sulfate ions?

A

add dilute HCL and then BaCl2
positive result = white ppt (BaSO4)

93
Q

test for CO3 2- ions (carbonate ions) ?

A

add dilute acid and bubble will be given off

94
Q

test for Cl- ?

A

add dilute HNO3 and then dilute silver nitrate (AgNO3)
white ppt

95
Q

test for Br- ?

A

add dilute HNO3 and then dilute silver nitrate (AgNO3)
cream ppt

96
Q

test for I- ?

A

add dilute HNO3 and then dilute silver nitrate (AgNO3)
yellow ppt

97
Q

flame test crimson red?

A

lithium

98
Q

flame test yellow?

A

sodium

99
Q

flame test lilac?

A

potassium

100
Q

flame test blue/green?

A

copper

101
Q

flame test brick red?

A

calcium

102
Q

test for ammonium ions?

A

add warm dilute NaOH
gas given off turns damp red litmus paper blue

103
Q

what happens when you add NH3 to AgCl, AgBr, AgI?

A

AgCl - dissolves in dilute
AgBr - dissolves in conc.
AgI - doesn’t dissolve

104
Q

which halide has the greater oxidising power?

A

Cl-

smallest atomic radius so strongest attraction to electrons

105
Q

which halide has the greatest reducing power?

A

I-

biggest atomic radius so weakest attraction to electrons

106
Q

what is a transition metal?

A

a metal that can form one or more stable ions and has a partially filled d-orbital

107
Q

physical properties of transition metals?

A

high densities
high m.p
ionic radii are all very similar

108
Q

chemical properties of transition metals?

A

can form complex ions
form coloured ions
good catalysts
exist in various oxidation states

109
Q

what is a complex?

A

a complex has a central metal atom/ion surrounded by co-ordinately bonded ligands

110
Q

what is a ligand?

A

an atom, ion or molecule that donates a pair of electrons to a central transiton metal ion to from a co-ordinate bond

111
Q

example of a 6-coordinate bond and shape name complex?

A

[Fe(H2O)6] 2+

octahedral

112
Q

example of a 4-coordinate bond and shape name complex?

A

[Cu Cl4] 2-

tetrahedral

113
Q

example of a 2-coordinate bond and shape name complex?

A

[Ag (NH3)2 ] + Tollens Reagent

linear

114
Q

what must ligands have to form a co-ord. bond?

A

at least one lone pair

115
Q

what is a ligand that can form more than one co-ord. bond and give and example?

A

multi dentate

EDTA 4-

116
Q

example of a bidentate ligand?

A

ethane - 1,2 - diamine

:NH2CH2CH2N:H2

117
Q

what is haemoglobin made from?

A

Fe 2+ central metal ion (hexa- coord)
multidentate ligand which has four N co-ord. bonded to central atom
global which is a protein
and ten either a O2 or H2O which swaps so the complex can transport oxygen

118
Q

what is a saturated hydrocarbon?

A

only has carbon carbon single bonds

119
Q

what is crude oil?

A

a mixture of alkanes

120
Q

why do bigger alkanes have higher m.p/b.p?

A

more atoms and electrons so greater vdw forces

121
Q

what is cracking?

A

the decomposition of long carbon chain alkanes to make lots of more in demand smaller ones

122
Q

what are the conditions for catalytic cracking?

A

450 c
catalyst - silica or alumina

123
Q

what are the conditions for thermal cracking?

A

high temp - 1000C
high pressure

124
Q

test for alkenes?

A

bromine water goes from orange to colourless

125
Q

what is a use of alkenes?

A

used to make plastics

126
Q

what compounds are typically made from catalytic cracking?

A

aromatic compounds and fuels (benzene ring)

127
Q

what compounds are typically made from thermal cracking?

A

alkenes

128
Q

what do we do with fuels?

A

combust them in oxygen

129
Q

products of complete combustion?

A

CO2 and H2O

130
Q

products of incomplete combustion (when there’s not enough O2)?

A

CO (g) and H2O

131
Q

products of incomplete combustion (there’s very little O2)?

A

C (s) and H2O

132
Q

what is the problem with sulphur dioxide?

A

forms acid rain which is a pollutant

133
Q

how can you remove SO2 after a combustion recation?

A

react it with a base e.g CaO

134
Q

what is the process of reacting SO2 with a base called?

A

flue-gas desulphurisation

135
Q

where are nitrogen oxides formed?

A

combustion in car engines due to high heat and pressure

136
Q

what are the three stages of free radical substitution?

A

initiation
propagation
termination

137
Q

conditions for free radical substitution?

A

UV light

138
Q

what do the dots in free radical substitution represent?

A

single unpaired electron

139
Q

what are CFC’s and what’s the problem with them?

A

chloro-fluorocarbons
CFC’s exist in our atmosphere due to aerosols and UV light from the sun causes their bonds to break which creates free radicals that then react with ozone depleting the ozone layer

140
Q

what does the ozone layer do?

A

protects us from UV radiation

141
Q

what type of reaction/mechanism occurs between halogens and alkanes?

A

free radical substitution

142
Q

what is four in IUPAC (as in di, tri, …., penta?

A

tetra

143
Q

what is a nucleophile?

A

a molecule with a lone pair of electrons that has a tendency to donate the elctrons

144
Q

what mechanism allows you to go from haloalkanes to alkenes?

A

elimination

145
Q

what conditions and things do you need in elimination?

A

base/proton acceptor eg OH-
high temp
ethanol as a solvent

146
Q

what is an alkene?

A

an unsaturated hydrocarbon

147
Q

what isomerism do you get from C=C and why?

A

E-Z steroisomerism
restricted oration around the C=C

148
Q

when is it Z?

A

together

149
Q

when is it E?

A

apart (ew)

150
Q

what is an electrophile?

A

electron pair acceptor

151
Q

what is the organic reactant in electrophilic addition and why?

A

alkene - C=C is and electron dense area

152
Q

what is the more stable carbonation and why?

A

the one with more alkyl groups attached as the alkyl groups push electrons onto the carbocation so spread the electrons around the molecule more evenly

153
Q

what two methods can you use to make ethanol?

A

fermentation
hydration of ethene

154
Q

conditions for fermentation?

A

yeast
oxygen free environment
temp 30-40 c

155
Q

what are the advantages of fermentation?

A

sugars renewable
cheap equipment

156
Q

what are the disadvantages of fermentation?

A

ethanol needs distilling
batch process - its not continuous

157
Q

conditions for the hydration of ethene?

A

catalyst - conc. H2SO4
temp 300 c
pressure 70 atm

158
Q

what are the advantages of the hydration of ethene?

A

produces a purer product than fermentation
continuous reaction

159
Q

what are the disadvantages of hydration of ethene?

A

ethene is non-renewable

160
Q

what do we use ethanol for?

A

biofuel so we combust it

161
Q

what do you use to oxidise alcohols? (comparing primary, secondary and tertiary)

A

acidified potassium dichromate
K2Cr2O7

162
Q

conditions when oxidising aldehyde?

A

heat under reflux

163
Q

what do you get when you oxidise aldehydes?

A

carboxylic acids

164
Q

what is the colour change when oxidising primary and secondary alcohols with K2Cr2O7?

A

orange to green

165
Q

what does a primary alcohol turn into when you oxidise it?

A

aldehyde

166
Q

what does a secondary alcohol turn into when you oxidise it?

A

ketone

167
Q

what does a tertiary alcohol turn into when you oxidise it?

A

can’t be oxidised

168
Q

can an aldehyde be oxidised?

A

yes

169
Q

can a ketone be oxidised?

A

no

170
Q

can a ketone be oxidised?

A

no

171
Q

test to distinguish aldehydes and ketones?

A

tollens reagent
aldehyde positive test (silver mirror) Ag+ —> Ag
ketone NVC

fehlings solution
aldehyde positive test (blue solution to red ppt)
Cu 2+ —> Cu +
ketone NVC

172
Q

what is seteroisomerism?

A

same molecular and structural formula but different arrangements in space

173
Q

what does chiral mean?

A

can’t be superimposed

174
Q

what does achiral mean?

A

can be superimposed

175
Q

what is a racemic mixture?

A

a mixture which contains equal quantities of each enantiomer

176
Q

What is the chelate effect?

A

Positive entropy change is always favourable as it means a more stable complex is being formed

177
Q

What will be more acidic M2+ or M3+ and why?

A

M3+ as as it has a higher charge to size ratio so is more polarising so it pulls the electrons towards it which weakens the O-H bonds making it easier to lose a H+

178
Q

What is cisplatin made from and what is it’s shape?

A

Central Pt ion/molecule
2 Cl ligands
2 NH3 ligands

Square planar

Chemistry (3 decks)

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