Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

A Level Chemistry > Module 5 Section 2: Energy > Flashcards

Module 5 Section 2: Energy Flashcards

(120 cards)

Start Studying
1
Q

Combine the two half equations

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

Why are transition metals good oxidising and reducing agents

A

They are good at changing oxidation state
So they’ll give out or receive electrons
Also change colour so it’s easy to spot when the reaction is finished

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

How potassium manganate is used as an oxidising agent

A

Contains manganate (VII) ions (MnO4 -) in which manganese has an oxidation state of +7
Can be reduced to Mn2+ ions during a redox reaction

MnO4 - is purple and [Mn(H2O)6]2+ is pale pink, but looks colourless so the colour change in the reaction is purple to colourless

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

How is potassium dichromate used as an oxidising agent

A

Contains dichromate(VI) ions (Cr2O7 2-) in which chromium has an oxidation state of +6
They can be reduced to Cr+3 ions during a redox reaction

Cr2O7 2- is orange and [Cr(H2O)6]3+ looks green so colour change is from orange to green

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

How to work out the concentration of a reducing agent

A

Titrate a known volume of it against an oxidising agent of known concentration
Can work the other way

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

How to carry out redox titration with Fe2+ as a reducing agent and MnO4 - as a oxidising agent

A

Measure out a quantity of the Fe2+ reducing agent
Add dilute sulfuric acid to the flask (this is an excess to make sure there are enough H+ to allow oxidising agent to be reduced)
Gradually add the aqueous MnO4 - to the reducing agent using a burette, swirling the conical flask as you do so
Stop when the mixture in the flask just becomes tainted with the colour of the MnO4 - (end point) and record volume of oxidising agent added
Run more titrations and calculate mean volume of MnO4 -

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q
A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How can iodine - sodium thiosulfate titrations be used

A

They are a way of finding the conc of an oxidising agent
The more concentrated an oxidising agent is, the more ions will be oxidised by a certain volume of it

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

How to prepare for a titration of iodine and sodium thiosulfate

A

Use a sample of oxidising agent to oxidise as much iodide as possible by measuring out 25cm3 of potassium iodate solution (KIO3 and oxidising agent)
Add this to excess acidified potassium iodide solution (KI) where the iodate(V) ions oxidise some of the iodide ions to iodine

Then find out how many moles of iodine have been produced by titrations the solution with a known conc of sodium thiosulfate (Na2S2O3)

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

Method of titration of iodine with sodium thiosulfate

A

Take flask containing solution of oxidised iodide ions (iodine and water)
Add sodium thiosulfate from a burette to the flask drop by drop
Colour fades to pale yellow (hard to see at end point) so add 2cm3 of starch solution to detect presence of iodine so solution goes dark blue showing there still iodine there
Add sodium thiosulfate one drop at a time until blue colour disappears
When this happens, all the iodine has just been reacted
Then calculate number of moles of iodine in the solution

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

How to do titrate calculation to find number of moles of iodine produced

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

How to calculate the concentration of oxidising agent using the original equation (6.6x10-4 moles of iodine and 25cm3 oxidising agent)

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

Definition of lattice enthalpy

A

Lattice enthalpy is the enthalpy chance when 1 mole of an ionic lattice is formed from its gaseous ions under standard conditions of 298K and 100kPa

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

What is lattice enthalpy

A

Ionic compounds can form regular structures called giant ionic lattice
The positive and negative ions are held together by electrostatic attractions
Lattice enthalpy is when gaseous ions combine to make a solid lattice

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

What does lattice enthalpy measure

A

This measures the ionic bond strength
The more negative the lattice enthalpy the stronger the bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What makes the lattice enthalpy more exothermic

A

The higher the charge on the ions the more energy is released when an ionic lattice forms
Due to stronger electrostatic forces between the ions
This means that the lattice enthalpy will be more negative
The smaller the ionic radii of the ions involved, the more exothermic the lattice enthalpy
Smaller ions have a higher charge density and the smaller ionic radii means the ions can sit closer together in the lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is the born Haber cycle used for

A

Lattice enthalpy can’t be measured directly so this cycle is used to calculate the enthalpy change if you took another less direct route

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

Meaning of the born Haber cycle diagram

A

Route 1:
Formation of gaseous atoms
• changing the elements in their standard states into gaseous atoms (endothermic process)
Formation of gaseous ions
• changing gaseous atoms into positive and negative gaseous ions (endothermic)
Lattice formation
• changing gaseous ions into the solid ionic lattice (this is lattice enthalpy and is exothermic)

Route 2
Converts elements in their standard states directly to the ionic lattice
Includes one enthalpy change which is enthalpy or formation and is exothermic

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

Standard enthalpy change of atomisation

A

The enthalpy change that takes place for the formation of one mole of gaseous atoms from the element in it’s standard state under standard conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What sign is in front of the enthalpy of atomisation

A

Standard enthalpy of atomisation is always an endothermic process so + value
Bonds are broken to form gaseous atoms

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

What is electron affinity

A

This is the opposite of ionisation energy
Electron affinity measures the energy to gain electrons
Always exothermic as the electron being added is attracted to nucleus

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

Definition of the first electron affinity

A

The enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions

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

Diagram example of successive electron affinities of oxygen

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Why are second electron affinities endothermic
Second electron affinities are endothermic This is because an electron is being gained by a negative ion which repels the electron away Means that energy must be put in to force the negative electron onto the negative ion
26
27
28
How can electrochemical cells be made
Electrochemical cells can be made from two different metals dipped in salt solutions of their own ions and connected by a wire (the external circuit)
29
What are the two reactions taking place in an electrochemical cell
Oxidation and reduction
30
What happens in a zinc/copper electrochemical cell
Zinc loses electrons more easily than copper. So in the half-cell on the left, zinc (from the zinc electrode) is oxidised to form Zn2+ ions. This releases electrons into the external circuit. In the other half-cell, the same number of electrons are taken from the external circuit, reducing the Cu2+ ions to copper atoms
31
Which way do electrons flow in electrochemical cells
Flow from more reactive metal to least reactive metal
32
What would adding a volt meter into the circuit allow you to find
Shows the voltage between the two half-cells. This is the cell potential or e.m.f. Add a high resistance voltmeter
33
Other types of electrochemical cells
You can also have half-cells involving solutions of two aqueous ions of the same element, such as Fe2+/Fe3+ The conversion from Fe2+ to Fe3+, or vice versa, happens on the surface of a platinum electrode. Electrochemical cells can also be made from non-metals. For systems involving a gas (e.g. chlorine), the gas can be bubbled over a platinum electrode sitting in a solution of its aqueous ions (e.g. Cl-) Platinum used as its inert and conducts electricity
34
What determines what direction the reaction goes in at each electrode
The reversible arrows show that both reactions can go in either direction. Which direction each reaction goes in depends on how easily each metal loses electrons (how easily it's oxidised).
35
What are electrode potentials
This measures how easily a metal is oxidised A metal that's easily oxidised (losing electrons) has a very negative electrode potential One that's harder to oxidise has a less negative or a positive electrode potential.
36
Example of how electrode potentials can determine the direction of the reaction in the cell
The zinc half-cell has a more negative electrode potential, so zinc is oxidised (the reaction goes backwards) Copper is reduced (the reaction goes forwards)
37
What does the Θ symbol mean
The Θ symbol next to the E means it's under standard conditions - 298K and 100 kPa.
38
Shorthand for writing electrochemical cell Use example of Zn/Cu cell
The half-cell with the more negative potential goes on the left. The oxidised forms go in the centre of the cell diagram
39
How to calculate overall cell potential
40
What voltage will the cell potential always be
The cell potential will always be a positive voltage Because the more negative E° value is being subtracted from the more positive E° value. E.g. the cell potential for the Zn/Cu cell - +0.34 - (-0.76) = +1.1 v
41
How do you measure the electrode potential
You measure the electrode potential of a half-cell against a standard hydrogen electrode
42
Definition of the standard electrode potential
The standard electrode potential, E°, of a half-cell is the voltage measured under standard conditions when the half-cell is connected to a standard hydrogen electrode.
43
What are the standard conditions for electrochemical cells
Any solutions must have a concentration of 1.00 mol dm3 or be equimolar (i.e. contain the same number of moles of ions). The temperature must be 298 K (25 °C). The pressure must be 100 kPa
44
What side is the standard hydrogen electrode shown
The standard hydrogen electrode is always shown on the left Doesn't matter whether or not the other half-cell has a more positive value. The standard hydrogen electrode half-cell has a value of 0.00 V.
45
How to work out whole cell potential while using standard hydrogen electrode
Whole cell potential = E°RHS -E°LHS E°LHS is 0V so voltage reading will be equal to E°RHS Reading could be positive or negative depending on the way the electrons flow
46
How can conditions effect the value of the electrode potential
Like regular reversible reactions the equilibrium position in a half-cell is affected by changes in temperature, pressure and concentration. Changing the equilibrium position changes the cell potential. Standard conditions are used to measure electrode potentials Using these conditions means you always get the same value for the electrode potential and you can compare values for different cells Shifting a position of equilibrium can increase or decrease the cell potential depending on whether the position shifts to produce more or less electrons
47
Overall equation for oxidation of iodide to iodine using iodate ions
48
Ionic equation for iodine reacting with sodium thiosulfate
49
What is a salt bridge
This is filter paper soaked in super saturated KNO3 Allows ions to flow through and balance out charges
50
What type of electrode potential do more reactive metals have
The more reactive a metal is the more it wants to lose electrons to form a positive ion More reactive metals have more negative standard electrode potentials
51
What would happen in a cell containing magnesium and zinc
Magnesium is more reactive than zinc so it's more eager to form 2+ ions than zinc is. The list of standard electrode potentials shows that Mg2+/Mg has a more negative value than Zn2+/ Zn In terms of oxidation and reduction, magnesium would reduce Zn2+ (or Zn2+ would oxidise Mg).
52
What type of electrode would a more reactive non metal have
The more reactive a non-metal is, the more it wants to gain electrons to form a negative ion. More reactive non-metals have more positive standard electrode potentials
53
What would happen in a cell containing chlorine and bromine
Chlorine is more reactive than bromine so it's more eager to form a negative ion than bromine is. The list of standard electrode potentials shows that ½Cl2 /Cl- is more positive than ½Br /Br-. In terms of oxidation and reduction, chlorine would oxidise Br (or Br would reduce CI)
54
What does a more positive electrode potential mean on an electrochemical series
The left hand substances are more easily reduced The right hand substance are more stable
55
What does a more negative electrode potential mean on an electrochemical series
The right hand substances are more easily oxidised The left hand substances are more stable
56
Predict whether zinc will react with aqueous copper ions using the half equations in the series
57
Why do you flip one of the equations round when balancing half equations Which one do you flip
Half equations are written as reduction equations (e.g. in electrochemical series) One will always need to switch in the direction of oxidation E.g. Zn/ Zn2+ has a more negative electrode potential than Cu2+/Cu so the zinc will be oxidised (equation flips round)
58
Predict whether copper will react with dilute sulfuric acid using the half equations in the series
59
What do predictions using E° state
This only states if the reaction is possible under standard conditions
60
Why may a prediction of whether two metals will react be wrong if the conditions are not standard
Changing the conc (or temp) of the solution can cause the electrode potential to change E.g:
61
Why may a prediction of whether two metals will react be wrong if the reaction kinetics are not favourable
The rate of reaction may be so slow that the reaction might appear not to happen If a reaction has a high activation energy then this may stop it happening
62
Why are standard conditions required at half cell reactions
The position of the redox equilibrium may change with conditions
63
What will decreasing the conc of Mn+ do to the reaction
Decreasing the concentration of Mn+ shifts equilibrium to the left to make more electrons This makes electrode potential more negative as there is more electrons
64
Diagram of a standard hydrogen electrode
Monoprotic acid is used e.g. HCl or NO3 Electrode made of finely divided pieces of platinum (platinum black) which increases surface area
65
Definition of standard electrode potential
The emf of a half cell connect to a standard hydrogen half cell under standard conditions of 298kPa, solution concentrations of 1.00 mol dm-3 and a pressure of 100kPa
66
What we can tell from the metals using their electrode potential
If electrode potential positive then we know the metal is better at gaining electrons than hydrogen If electrode potential is negative then the metal is better at releasing electrons than hydrogen More reactive metal = more oxidised (better reducing agent) = more negative terminal
67
How do energy storage cells work
Energy storage cells have been around for ages and modern ones work just like an electrochemical cell Other name for a battery
68
What was the nickel-iron cell used for
The nickel-iron cell was developed at the start of the 1900s and is often used as a back-up power supply because it can be repeatedly charged and is very robust
69
How to work out voltage for energy storage cells
You can work out the voltage produced by these cells by using the electrode potentials of the substances used in the cell.
70
Advantages of electrochemical cells
They are more efficient at producing energy than conventional combustion engines. This is because energy is wasted during combustion as heat. They produce a lot less pollution (such as CO2). For hydrogen fuel cells, the only waste product is water.
71
Drawbacks of electrochemical cells
The production of the cells involves the use of toxic chemicals, which need to be disposed of once the cell has reached the end of its life span. The chemicals used to make the cells are also often very flammable. E.g. lithium (commonly used in rechargeable batteries), is highly reactive and will catch fire if a fault causes it to overheat
72
Have to double 2nd equation to the electrons balance those in the first equation
73
Draw diagram for how fuel cells generate electricity from reacting a fuel with an oxidant
74
What are primary cells
These are non rechargeable The electrical charge is produced by oxidation and reductions at the electrodes The reactions cannot be reversed Eventually the chemicals will be used up, voltage will fall and the battery will go flat
75
What are secondary cells
these cells are rechargeable The cell reaction producing electrical energy van be reversed during recharging The chemicals in the cell are then regenerated and the cell can be used again
76
Common examples of secondary cells
Lead acid batteries used in car batteries Lithium ion and lithium ion polymer cells used in appliances like laptops and mobile phones
77
What are fuel cells
A fuel cell uses the energy from the reaction of a fuel with oxygen to create voltage The fuel and oxygen flow into the fuel cell and products flow out, electrolyte remains in the cell Fuels can operate continuously provided that the fuel and oxygen are supplied into the cell Do not have be recharged
78
What happens when an ionic lattice dissolves in water
The bonds between the ions break to give gaseous ions - this is endothermic. The enthalpy change is the opposite of the lattice enthalpy Bonds between the gaseous ions and the water are made - this is exothermic. The enthalpy change here is called the enthalpy change of hydration.
79
Definition of the enthalpy of hydration
Is the enthalpy change when 1 mole of gaseous ions dissolves in water
80
Definition of the enthalpy change of solution
Is the enthalpy change when 1 mole of solute dissolves in water
81
What are the energy changes in order for substances to dissolve
Substances generally only dissolve if the energy released is roughly the same, or greater than the energy taken in. So soluble substances tend to have exothermic enthalpies of solution
82
How to set out a born haber cycle for enthalpy change of solution
Put the ionic lattice and the dissolved ions on the top connect them by the enthalpy change of solution - this is the direct route Connect the ionic lattice to the gaseous ions by the reverse of the lattice enthalpy. The breakdown of the lattice has the opposite enthalpy change to the formation of the lattice Connect the gaseous ions to the dissolved ions by the hydration enthalpies of each ion - this completes the indirect route
83
Work out enthalpy change of solution for NaCl Lattice enthalpy NaCl: -787 kJmol-1 Enthalpy hydration Na+: -406 kJmol-1 Enthalpy hydration Cl-: -364 kJmol-1
84
Work out enthalpy change of solution for AgCl Lattice enthalpy AgCl: -905 kJmol-1 Enthalpy hydration Ag+: -464 kJmol-1 Enthalpy hydration Cl-: -364 kJmol-1
85
Is the enthalpy of hydration more or less for ions with a greater charge
Ions with a greater charge have a greater enthalpy of hydration. lons with a higher charge are better at attracting water molecules than those with lower charges Because the electrostatic attraction between the ion and the water molecules is stronger. This means more energy is released when the bonds are made giving them a more exothermic enthalpy of hydration
86
Is the enthalpy of hydration more or less for ions which are smaller
Smaller ions have a greater enthalpy of hydration. Smaller ions have a higher charge density than bigger ions. They attract the water molecules better and have a more exothermic enthalpy of hydration
87
88
89
Alternative way of setting out born-Haber cycle
90
How does changing ionic size and ionic charge affect lattice enthalpy
As you go down the group the ionic radius increases This means the attraction between ions decreases so lattice is less negative Melting point decreases If ionic charge increases then the attraction between ions increases This means that lattice enthalpy becomes more negative Melting point increases
91
What is entropy
Entropy is a measure of the number of ways that particles can be arranged and the number of ways that the energy can be shared out between the particles.
92
What results in a higher entropy
The more disordered the particles are, the higher the entropy is. A large, positive value of entropy shows a high level of disorder
93
What things can affect entropy
Physical state Number of particles
94
How does physical state affect entropy
Solid particles are fixed in place so there is less randomness and lowest entropy Gas particles are constantly moving and have the most random arrangements of particles so have the highest entropy
95
How does physical state affect entropy
Solid particles are fixed in place so there is less randomness and lowest entropy Gas particles are constantly moving and have the most random arrangements of particles so have the highest entropy
96
How does the number of particles effect entropy
The more particles you've got, the more ways they and their energy can be arranged In the reaction: N2O4(g) -> 2NO2(g) entropy increases because the number of moles increases
97
What sort of state will substances usually react towards
Substances are more energetically stable when there’s more disorder Particles will move to try and increase entropy This is why some reactions are feasible even when the enthalpy change is endothermic
98
Why is the reaction between sodium hydrogencarbonate and hydrochloric acid still feasible even though it is endothermic
This is due to an increase in entropy as the reaction produces CO2 gas and water Liquids and gases are more disordered than solids and so have a higher entropy This increase in entropy overcomes the change in enthalpy Also favoured because it increases the number of moles
99
When is a substance thermodynamically stable
When a substance reaches its maximum entropy state (its lowest energy state), it's said to be thermodynamically stable. This means it won't react any further without the input of energy
100
How to calculate entropy change
Must know the entropies of the products and reactants
101
Units of entropy
J K-1 mol-1
102
What entropy are more feasible reactions
Reactions with a positive value of △S are more likely to be feasible
103
104
Definition of standard entropy
The standard entropy S° of a substance is the entropy of one mole of a substance under standard conditions (100kPa and 298K)
105
What does the tendency for a reaction to happen depend on
The entropy: △S The enthalpy: △H The temperature T These combine to make the free energy change △G
106
What does △G tell you
Says if a reaction is feasible or not The more negative the value of △G the more feasible the reaction
107
Formula for free energy change
108
109
What value does △G have to be in order for the reaction to be just feasible
△G = 0
110
How to calculate the minimum temperature needed to make a reaction feasible
111
112
What are the limitations of predictions made for feasibility
A negative △G does not guarantee a reaction It can indicate thermodynamic feasibility but does not take into account kinetics or rate or reaction It may have a high activation energy so it will happen very slowly
113
114
What value will △G be when △H is negative and △S is positive
△G is always negative and the reaction is feasible
115
What value will △G be when △H is positive and △S is negative
△G will always be positive and the reaction is not feasible
116
117
118
119
What does a reaction being feasible mean
They just happen by themselves without the addition of energy
120
Explain the colour change of MnO4- to Mn2+
The Mn2+ is being made in the reaction and is so pale pink that it looks colourless When the limiting reactant is used up, the MnO4- is not longer reduced to Mn2+ and remains in solution This looks pale pink

A Level Chemistry (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions