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GCSE Chemistry OCR A > paper4 > Flashcards

paper4 Flashcards

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1
Q

Describe the group 1 physical & chemical properties:

A

1️⃣shiny when freshly cut
1️⃣solid state at RT
1️⃣soft
1️⃣ conducts of electricity

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2
Q

What is the trend of group 1 metals going down the group?

A

1️⃣ density increases
1️⃣ melting point decreases
1️⃣ reactivity increases (fizzes —> flames)

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3
Q

Why do group 1 elements get more reactive down the group?

A

Want to loose 1 electron
Larger Atomic radius = weaker force of attraction
Shielding (more electron shells in way) = weaker force

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4
Q

What do group 1 metals produce when they react with water?

A

Hydrogen and an alkali (metal hydroxide)

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5
Q

What are some chemical and physical properties of group 7 elements?

A

7️⃣brittle
7️⃣poor conductors
7️⃣DIATOMIC

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6
Q

How does fluorine appear in RT?

A

A pale yellow gas (F2)

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7
Q

How does chlorine appear in RT?

A

Cl2
A green gas

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8
Q

How does bromine appear in RT?

A

An orange / brown liquid (Br2)
Vaporises easily

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9
Q

How does Iodine (I2) appear at RT?

A

A shiny grey- black crystalline solid

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10
Q

What are the trend of group 7 , going down the group?

A

7️⃣density increases
7️⃣MP/BP increase
7️⃣ reactivity decreases

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11
Q

What do halogens produce when reacting with metals?

A

Salt

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12
Q

Why does the reactivity decrease when going down the group?

A

Must gain 2 electrons
More atomic radius = weaker forces of attraction
More shielding = weaker forces of attraction
More shells , makes it harder to attract 2 electrons

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13
Q

Why do halogens displace other halogens?

A

If they are more reactive (more higher on in the group) then they kick the other out

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14
Q

What are some chemical and physical properties of group 0 elements

A

0️⃣all gasses at RT
0️⃣so un reactive (full outer shells)
0️⃣non metals
0️⃣monatomic
0️⃣low BPs

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15
Q

What is the trend of group 0 going down the group?

A

Boiling point increases (attractive forces between atoms are stronger)
Boiling point increases

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16
Q

What are some properties of transition metals?

A

Shiny when freshly cut
Good conductors of electricity
Strong
Malleable

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17
Q

Describe the transition metals in comparison to group 1

A

More dense
More stronger /harder
Higher melting points
Also less reactive

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18
Q

What are some chemical properties of transition metals?

A

💚Less reactive than group 1
💚Produce coloured ionic compounds
💚Can have multiple charges
💚Good catalyst
💚 resistant to corrosion (not so reactive)

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19
Q

What is the reactivity series?

A

Potassium
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Tin
Lead

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20
Q

What does the rate of reaction tell you?

A

The order of reactivity
More reactive = greater rate of hydrogen production

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21
Q

Do group 0 react?

A

NOPE
Full outer shell and so won’t easily give up or gain electrons

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22
Q

Which are least reactive out of group 1, group 2 and transition metals

A

Transition metals

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23
Q

How do you test for oxygen?

A

Place a glowing splint near the mouth of the container of gas
If oxygen is present the splint should relight

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24
Q

How do you test for hydrogen?

A

Place a lighted splint near the mouth of the container.
If hydrogen is present it should ignite with a squeaky pop

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25
Q

How do you test for carbon dioxide ?

A

Use limewater (calcium hydroxide).
If it turns cloudy when carbon dioxide is bubbled through then it is present.
White precipitate = calcium carbonate

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26
Q

How do you test for chlorine?

A
  1. Dampen the blue litmus paper
  2. Put it near, should turn red then white(bleeches )
    Chlorine + water =acidic solution
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27
Q

What colour is lithium in the flame test?

A

Red

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28
Q

What colour is sodium in the flame test?

A

Yellow

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29
Q

What colour is potassium in the flame test?

A

Lilac

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30
Q

What colour is calcium in the flame test?

A

Orange-red

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31
Q

What colour is copper in the flame test?

A

Green-blue

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32
Q

Why do metal ions create a colour when heated?(excitation)

A

Energy is transferred to the electrons
They move to higher shells , and then move back down
As they do radiation is emitted in the form of visible light

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33
Q

How do you carry out a flame test?

A
  1. Clean Nichrome wire loop in HCL, hold it in the flame until it stops changing colour.
    2.dip the loop into the test powder.
  2. Hold it in the roaring flame and note the colour
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34
Q

Why is sodium hydroxide solution used in experiments?

A

Group 1 hydroxides are soluable in water

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35
Q

What colour does iron (ll) make in the sodium hydroxide tests?

A

Green

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36
Q

What colour does iron (lll) make in the sodium hydroxide tests?

A

Orange - brown

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37
Q

What colour does copper(ll) make in the sodium hydroxide tests?

A

Blue

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38
Q

What colour does calcium make in the sodium hydroxide tests?

A

A white precipitate that does NOT a dissolve in excess
*remains white

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39
Q

What colour does zinc make in the sodium hydroxide tests?

A

A white precipitate that DOES dissolve in excess.
Goes from white to colourless

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40
Q

How do you detect sulfate ions?

A

Add HCL
Add barium chloride

If present then should get an insoluble white precipitate (barium sulphate)

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41
Q

How do you detect carbonate ions?

A

Add a few drops of dilute hydrochloric acid
*should produce bubbles

If present there should be bubbling of carbon dioxide being released

2H+ (aq) + CO3 2-(aq) —> CO2 (g) + H2O (l)

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42
Q

How do you detect halide ions?

A

Add a few drops of nitric acids
Then add a few drops of silver nitrate solution

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43
Q

What colour Is the precipitate of silver chloride?

A

Whitw

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44
Q

What is the colour of silver bromide?

A

Cream

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45
Q

What is the colour of silver iodide precipitate ?

A

Yellow

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46
Q

What is the reaction for the copper hydroxide(product)?

A

CuSo4 (aq) + 2NaOH(aq) —> Cu(OH)2 (s) + Na2SO4 (aq)

Net ionic equation:
Cu 2+ (aq) + OH- (aq) —> cu(OH)2 (s)

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47
Q

What are the advantages of instrumental methods of analysis?

A

🟢speed
🟢accuracy : more decimal points
🟢sensitivity: a small amount can be used

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48
Q

How do you interpret a mass spectrometer?

A

The x axis (mass to charge ratio) is just the mr
1. Look at the last peak on the graph, this is the relative formula of the entire substance

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49
Q

What is formed when a metal and water react?

A

Metal + water —> metal hydroxide + hydrogen

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50
Q

Why might a precipitate reaction occur really fast?

A

The collision frequency is high

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51
Q

What would you observe if a Grp 1 metal is added to water?

A

🟣floats on surface
🟣fizzing
🟣the flame of hydrogen ignites
🟣melts as reacts

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52
Q

What is a metal and steam form?

A

🤨
Metal+ steam —> metal oxide + hydrogen
Metal + H20–> metalO + H2

Weird coz it’s water but no hydroxide

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53
Q

Why might some experiments be made in a fume cupboard?

A

The gas produced could be TOXIC

¥toxic by Britney Spears 💋

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54
Q

Why does the reactivity increase going down group 1 (2marks)?

A

🟢more shielding
🟢’outer electron’ is lost more easily

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55
Q

Why is nitric acid added before silver nitrate?

A

To make sure there are no carbonate ions present

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56
Q

What is a yield of a product?

A

The mass of the product that is made in a chemical process

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57
Q

What is theoretical yield?

A

The maximum amount of mass that is possible to be made from the given mass of reactants

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58
Q

How do you calculate theoretical yield?

A

Basically a reacting masses question:
1. From mass find mols
2. Find mols of desired thing through stoichometry
3. Convert back from mols to mass

Will be answered in grams

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59
Q

How do you calculate percentage Yield?

A

(Actual yield ➗theoretical yield)✖️100

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60
Q

What affects percentage yield? (!100%)

A

🟢transfer loss of substance
🟢reaction may not go to completion
🟢reaction may react in a different way than planned

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61
Q

What is atom economy?

A

How many atoms in the reactants form a desired product

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62
Q

How do you calculate atom economy?

A

(Sum of Mr of desired products➗sum of Mr of all products)✖️100

BALANCING NUMBERS ARE INCLUDED

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63
Q

What factors affect the reaction pathway?

A

🟡percentage yield
🟡atom economy
🟡rate of reaction
🟡usefulness of by products
🟡wether it is a reversible reaction

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64
Q

How do you convert between dm and cm cubed?

A

Cm^3: dm^3
1000:1

10cm =1dm

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65
Q

How do you calculate the concentration of a solution

A

Concentration (mol/dm^3 ) = amount in mass/mols➗volume in dm^3

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66
Q

How do you convert between g/dm^3 and mol/dm^3?

A

➗molar mass

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67
Q

How do you carry out a titration?

A

🔶biruete clamped using a glass clamp
🔶volumetric pipette to measure alkali
🔶Then put into a conical flask
🔶using a funnel put the acid in the biruette, read the bottom of the minniscous and place the set up on the floor to get at eye level
🔶take out the funnel and add indicator (phenolphthalein)in the conical flask, should be pink
🔶add the acid while swirling when it turns colourless , stop the tap. Repeat 3 times -Dripwise
🔶initial - final = titre

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68
Q

What is the point of a titration?

A

To find the concentration of the acid or alkali

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69
Q

How do you calculate titration questions?

A

1) find mols
2) do the stoichemetry
3) convert back to concentration

Mols = volume ✖️concentration

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70
Q

What is the rate of reaction?

A

How quickly products are formed/reactants used.

Amount of products are formed/reactants used.➗time taken

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71
Q

How do you measure the rate of reaction from a gas syringe? With different concentration

A

(A conical flask with a rubber bung attached to the gas syringe)
🔹measure a known volume of acid
🔹add known mass of other solute
🔹measure the volume of gas every 30s
🔹repeat with different concentrations of acid
🔹repeat using the same temperature

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72
Q

How do you read a volume time line graph?

A

At the beginning a steep gradient because more reactant particles means more successful collisions.
A flat line towards the end means that the reaction has stopped.
The gradient measures the rate of reaction

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73
Q

How do you calculate the mean rate of reaction (2 values)?

A

Do change in y ➗ change in x for

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74
Q

How do you calculate the instantaneous rate of reaction?

A

At the point draw a tanget.
Then calculate the gradient of this tangent.

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75
Q

How does temperature affect the rate of reaction?

A

🟡increases rate of reaction as particles hold move more quickly and so would collide more frequently.
🟡 these colliding particles would also have the activation energy or more
🟡therefore leading to successful collisions

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76
Q

Describe the disappearing cross experiment

A

Draw a black cross on a piece of paper and place beneath a transparent beaker. Place the reactants in the beaker and start timing , stop it when the black cross is no longer visible. Calculate the rate by doing
1➗time

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77
Q

How does increased concentration affect the rate of reaction?

A

Concentration =how much solute is dissolved in the solvent

🟣 more crowded particles
🟣 more collisions per second
🟣due to rate of collisions increasing , the rate of successful collisions increases

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78
Q

How does increasing pressure affect the rate of reaction?

A

🟣more particles per unit of volume (in the gas state the particles become more crowded )
🟣more collisions per second
🟣as rate of collisions increases the rate of successful collisions increases

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79
Q

HOw does the size of the reactants affect the rate of reaction.

A

🟣smaller the pieces, the larger the surface area
🟣more particles are exposed (more reactant particles are available for collisions)
🟣higher frequency of collisions.
🟣due to increased frequency of collisions, there is an increased frequency of successful collisions

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80
Q

How would you use the mass balance experiment to measure the rate of reaction?

A

NOT WHEN USING HYDROGEN AS TOO LIGHT
Place conical a flask with a cotton wool to avoid spitting on a mass nance and record the mass at regular intervals.

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81
Q

What is the effect of a catalyst on the rate of reaction?

A

It increases the rate of reaction without using up any of it’s own energy

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82
Q

How do catalysts affect the activation energy?

A

They provide an alternative reaction pathway , with a lower activation energy. So the particles have enough energy for their collisions to be successful.
A greater proportion of the colliding particles then have the activation energy or more.

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83
Q

What is dynamic equilibrium?

A

A reversible reaction in a closed system, when the rate of the forward reaction is equal to the rate of the reverse reaction.
The concentration of the reactants an products must be stable.

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84
Q

What is a reversible reaction?

A

A reaction where the products of the reaction can react to produce the original reactants.

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85
Q

What does a ‘shift in the position of equilibrium’ mean?

A

The side to where it shifts has a larger percentage yield (more is made).
Eg: a shift to the left makes more reactants
A shift to the right makes more products

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86
Q

How does pressure change the position of Equilibrium?

A

Increasing the pressure will cause a shift to the side with less GAS mols. Because a higher pressure means less area.

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87
Q

How does temperature shift the position the equilibrium ?

A

Then through Le chatilers principal, the system will try to counteract this change as it wants to go back to before.

If there is an increase in temperature.
The system will want to get rid of this extra heat and so will perform an endothermic reaction, as it absorbs heat from the surroundings.

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88
Q

How does concentration shift the position of equilibrium?

A

Then through Le chatilers principal, the system will try to counteract this change as it wants to go back to
If the concentration of a substance has been increased then the position of equilibrium will be moved to the opposite side away from it.

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89
Q

What effect do catalyst have on the position of equilibrium ?

A

They don’t have any effect. They only increase the rate and make it a more efficient process

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90
Q

Why might a manufacturer compromise on temperature?

A

Cannot make to low because of activation energy and rate of reaction.
Cannot make too high because it’s expensive

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91
Q

Why might a manufacturer compromise on pressure ?

A

High pressure requires tough reaction vessels which can be quiet expensive
Low pressure is cheaper to generate

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92
Q

What are concordat titres?

A

Titres that are within 0.1of each other

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93
Q

When do gases occupy the same volume?

A

When they are all at room temperature and pressure

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94
Q

How do you handle gas calculations?

A

Volume = 24 (concentration) ✖️mols

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95
Q

Why do to measure the bottom of a minniscous ?

A

To avoid a parallax error

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96
Q

Why are indicators such as phenolphthalein used?

A

There is a sudden colour change as opposed to a gradual change

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97
Q

Why should industrial process have the highest atom economy possible?

A

To the reduce the production of unwanted products.
To make the process more sustainable

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98
Q

What does it mean for the particles to have successful collisions?

A

The particles have the activation energy

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99
Q

What is the cotton wool used for in the mass scale rate of reaction experiment?

A

The cotton wool prevents spitting. BUT allows the gases to escape from the flask , no worry

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100
Q

How could titrations be improved

A

🔵swirling flask, ensures mixing
🔵use a white tile underneath to see end point clearly
🔵 add drop-wise, to see colour change in one drop

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101
Q

How do data loggers and ph probes affect titrations?

A

They are more accurate as you can predict the endpoint more accurately

102
Q

What is the very first titration results accounted for?

A

They are seen as a rough test, more of an anomaly and are not used in the results data

103
Q

How does surface area affect rate of reaction?

A

The higher the SA the higher the rate of reaction

104
Q

What do the following prefixes mean?
Meth
Eth
Prop
Bute

A
105
Q

Draw propene
(Alkene)

A
106
Q

Why are alkanes a homologous series?

A
107
Q

What does it mean to be saturated?

A

(Basically all single bonds. Nothing can be added by breaking new bonds)

greatest possible number of hydrogen atoms, without carbon–carbon double or triple bonds.

108
Q

What is the difference between complete and incomplete combustion?

A
109
Q

What are hydrocarbons?

A

Compounds that only contain hydrogen and carbon

110
Q

Draw ethane

A
111
Q

Why are alkenes a homologous series?

A
112
Q

Describe the addition reaction alkenes undergo with bromine

A
113
Q

Describe an experiment to tell apart alkenes and alkanes
*With safety precautions

A
114
Q

Why are alcohols a homologous series?

A
115
Q

Draw methanol

A
116
Q

What is an organic compound?

A

A compound that contains oxygen

117
Q

Draw methanol

A
118
Q

Draw the incomplete and complete reactions of ethanol

A
119
Q

Draw and describe an amine

A
120
Q

Draw and describe ester

A
121
Q

Draw and describe amide

A
122
Q

What is condensation polymerisation?

A

Reactions in which monomers join together and lose
small molecules, such as water. These reactions involve monomers with two
functional groups.

123
Q

What is a dicarboxylic acid?

A

The COOH on either side

124
Q

What is a diol?

A

Two hydroxyl (OH) groups on either side

125
Q

How is polyester formed?

A
126
Q

How is polyamide formed?

A
127
Q

How does crude oil separated into hydrocarbons?

A
  • crude oil is mostly made up from alkanes
128
Q

What is the renewable method of making ethanol?

A

fermentation

129
Q

What is the structure of a chemical cell ?

A
130
Q

why do chemical cells have a salt bridge , and what do they consist of ?

A

The salt bridge is basically just filter paper soaked in potassium nitrate solution.
It completes the circle by allowing IONS to move

131
Q

What happens when a cell goes flat?

A

One of the reactants is used up, so it can no longer provide a potential difference

132
Q

Why happens at the negative terminal of a chemical cell?

A

Oxidation happens , so electrons are lost

133
Q

What happens at the positive terminal of a chemical cell?

A

Reduction , gain of electrons

134
Q

How do you identify the negative terminal of a chemical cell?

A

The more reactive metal (reactivity series) becomes the negative terminal

135
Q

describe a hydrogen oxygen electrical fuel cell

A
  1. The hydrogen is turned into hydrogen ions at the anode
  2. The hydrogen ions pass through the proton exchange membrane
  3. Into the cathode , where the hydrogen ions combine with oxygen to make water
136
Q

what conditions are needed for addition polymerisation?

A

🟢high pressure
🟢catalyst
* the monomers must have a carbon carbon double bond

137
Q

What is the difference between complete and incomplete combustion?

A

complete combustion, makes the products of carbon dioxide and water
Incomplete combustion, makes the product of carbon monoxide and water .(toxic)

138
Q

What are the requirements of cracking ?

A

🟣high temperature
🟣catalyst (alumina /silica)

139
Q

What is cracking and why is it needed ?

A

Turn large hydrocarbons into small hydrocarbons ( higher demand )

140
Q

Why are carboxylic acids a homologous series ?

A
141
Q

Draw propanoic acid

A
142
Q

How are carboxylic acids made?

A
143
Q

describe the process of hydration

A
144
Q

what reactions do carboxylic acids participate in ?

A

All the usual reactions that acids participate in:

145
Q

describe the broken pot experiment used to exemplify cracking

A
146
Q

What are some names / orders of fractions from cracking

A
147
Q

Why is cracking of crude oil used ?

A

Crude oil is a main source of hydrocarbons and is a feedstock for the petrochemical industry

148
Q

Why is crude oil a finite source?

A

Non renewable as , It is being used up much faster than it is formed .

149
Q

How does the size of the hydrocarbon molecule affect the flammability and cleanses of the flame ?

A

The larger the hydro carbon ,
The less flammable it gets
The dirtier flame (more soot because of more carbons )

150
Q

What happens when an alcohol is oxidised?

A

With the addition of an oxidising Agent (potassium magnate VII), the corresponding carboxylic acid is produced

151
Q

What does it mean to be unsaturated?

A

Have a double bond

152
Q

describe addition polymerisation

A
153
Q

How does the monomer propene become a polymer ?

A
154
Q

How many polymer strands make up a DNA molecule

A

2 anti parallel polymer strands

155
Q

What is an electrolyte ?

A

A solution where ions are free to move

156
Q

What is the difference between wet and dry cells

A

Wet cells have the solutions , whereas dry cells have the paste /powder

157
Q

What is a fuel cell

A

Something that can produce electricity through the reaction of fuel and oxygen

158
Q

what is the definition of addition polymerisation?

A

The reaction in which many small molecule monomers bond
together to form a long chain polymer

159
Q

what is the definition of a chemical cell?

A

A cell which converts chemical energy to electrical energy. They are made
up of two metal electrodes connected by an electrolyte. The cell produces a voltage until one
of the reactants is used up

160
Q

what is the definition of a fuel cell?

A

An electrochemical cell which continuously produces a voltage when supplied
with a fuel and oxygen. The fuel donates electrons at one electrode and oxygen gains
electrons at the other electrode.

161
Q

what is the definition of a ‘functional group’ ?

A

The group of atoms responsible for how a particular compound reacts.
All compounds in the same homologous series have the same functional group.

162
Q

What is the definition of a polymer ?

A

Large long-chain molecule made up of lots of small monomers joined together by
covalent bonds.

163
Q

What is the phosphate ion?

A
164
Q

What is phosphoric acid?

A
165
Q

What happens when ammonia reacts with an acid?

A

Instead of salt + water ,
Only salt
With ammonium ion (NH4+)

166
Q

Why are fertilsers needed?

A

They contain NPK (essential elements)needed by plants to grow. The fertilisers will increase yield and replace the elements used up when growing the previous crop.

167
Q

What is the deficiency of NPK in farming ?

A
168
Q

Why is the haber process important in agriculture?

A
169
Q

The Haber Process

A
170
Q

How do you make potassium sulfate ? ( a needed fertiliser)

A
171
Q

How do you make ammonium sulfate? ( a fertilster )

A
172
Q

what is the difference between a batch process and a continuous process?

A

The batch process is in labs, whereas the continuous process happens in factories and on a larger scale (much more automated)

173
Q

What are the conditions needed for the haber process?

A
174
Q

What are the conditions needed for the contact process?

A
175
Q

Stage 1 of the contact process

A
176
Q

Stage 2 of the contact process

A
177
Q

Stage 3 contact process

A
178
Q

What are the certain conditions needed for stage 2 and why? (Of contact process )

A
179
Q

Catalyst for the contact process

A
180
Q

Reactivity series with carbon

A

Extracting with carbon is a lot more cheaper

181
Q

How do you extract copper (practical method) with safety?

A

Wear eye protection

182
Q

How can copper be extracted from copper(II) sulfide?

A
183
Q

What are the two methods for making ethanol ?

A

🟢fermentation
🟢flash /hydration method

184
Q

Describe the fermentation method for making ethanol

A
185
Q

Describe the flash /hydration method for making ethanol

A
186
Q

Compare the flash method with the fermentation method for making ethanol.

A

Cost
Availability of raw materials
Rate of reaction
Yield of ethanol

187
Q

Which ore is iron extracted from ?

A

Haematite (contains iron (III) oxide)

188
Q

What are the 4 raw material used within the blast furnace ?

A
189
Q

describe the extraction of iron (with equations)

A
190
Q

What are the two equations for removing the impurities from the blast furnace ?

A
191
Q

What are the equations for the iron extraction from the blast furnace

A
192
Q

What is stage 3 for the contact process and why ?

A

Hydrate the oleum instead

193
Q

What are the conditions needed for the haber process

A
194
Q

What are the conditions for stage 2 of contact process

A
195
Q

describe the process for the extraction of aluminium

A
196
Q

What ore is aluminium oxide present in ?

A

Bauxite

197
Q

What are the equations for extracting copper from copper sulphide?

A
198
Q

What are the biological methods for extracting metal

A

Bio leaching
Phytoextraction

199
Q

Describe the process of bio leaching

A
200
Q

What is a low - grade ore ?

A

An ode where there is a few small percentage of actual metal. So to conduct large processes on it would be unprofitable

201
Q

What are the advantages and disadvantages of bio leaching compared to normal metal extraction

A
202
Q

describe the process of phytoextraction

A
203
Q

describe the advantages and disadvantages of phytoextrction compared to other methods of metal extraction

A
204
Q

What is the definition of an alloy ?

A

Mixture of at two or more elements , one of which is at least a metal.

205
Q

What is the main metal in the alloy steel , and it’s use?

A

MM =Iron
Uses : buildings 🏥 , bridges 🌉, cars 🚘

206
Q

what is the main metal in the alloy duralumin, and it’s main uses ?

A

MM: Aluminium
* also a little bit of copper
Uses: aircraft parts ✈️🛩

207
Q

What is the main metal in the alloy solder, and it’s main uses ?

A

MM =tin
*also a bit of copper
Uses : joints electrical components and copper pipes (motherboard)

208
Q

What is the main metal in the alloy brass, and it’s main uses ?

A

MM: copper
* a bit of zinc
Uses : musical instruments 🎺 , coins 🪙

209
Q

What is the main metal in the alloy bronze and it’s uses ?

A

MM= copper
*a little bit of tin
Uses : 🔔bells , propellers for ships 🚢

210
Q

Describe solder

A
211
Q

Describe the chemical structure of an alloy compared to metals

A

🔵larger atoms , distort the regular arrangement of metal atoms
🔵this means that layers can no longer slider over each other
🔵making the alloy stronger

212
Q

Define corrosion

A

The reaction of a metal with it’s surroundings (such as air or water ).

213
Q

Define rusting ?

A

A form form of corrosion whereby iron or steel react withy oxygen and water for a hydrated Fe(III)O or rust

214
Q

Rusting reaction (iron )

A
215
Q

What are the results for these reactions

A
216
Q

What are the ways to reduce corrosion ?

A

🟡Physical barrier (coating )
🟡Sacrificial protection
🟡Galvanising

217
Q

Describe how coating works

A

Supplies a physical barrier between air and water
Coating with oil / grease / painting
However if the layer is damaged, rusting starts on the exposed metal and continues underneath the layer

218
Q

Describe sacrificial protection

A

A metal more reactive than iron (magnesium or zinc ). This will corrode first. However will eventually corrode away and will have to be replaced.

As those metals are more reactive than iron they loose electrons more easily and so are “more readily oxidised than iron “

219
Q

How does galvanising work ?

A

Dipping the object in molten zinc ,
Acts as a physical barrier , stopping contact of metal with oxygen and water and when it chips away , becomes a sacrificial barrier

220
Q

What’s a disadvantage of tin plating ?

A

Although acts as a physical barrier k when chips away actually speeds up the rusting process instead of acting as a sacrificial barrier

221
Q

Describe ceramics typical properties

A

Hard , non -metallic structures, brittle
🟣high MP; (giant ionic lattices or giant covalent structures )
🟣hard and stiff , and brittle
🟣poor conductors of electricity and heat

Compounds in ceramics mostly oxides and so are unreactive .

222
Q

Describe glass

A

Made by melting sand
🟣irregular giant structure, no crystals , and so can see through making it transparent
🟣

223
Q

What is a composite material ?

A

A metrical made from two or more different materials , each with different properties

224
Q

What is tensile strength

A

A measure of how strong a material is when stretched

225
Q

What is compressive strength

A

A measure of how strong a material is when squashed

226
Q

What does density refer to in tables ?

A

Strength

227
Q

What are the 4 types of ceramics ?

A

Glass , porcelain , brick and China

228
Q

What is a life - cycle assessment?

A

An analysis of the making using and disposing of a manufactured product 

229
Q

Why is the life cycle assessment performed?

A

Helps identify stages that could be improved , or alternate materials that may do the same job

230
Q

Why should materials be recycled?

A

🟣conserving limited raw materials and energy resources
🟣reducing the real sense of harmful substances into the environment
🟣reducing waste

231
Q

What factors decide whether a product can be recycled or not ?

A

🟢how easily the waste can be collected and stored 🟢the amount and type of by products released
🟢the cost of recycling, compared to disposal
🟢the amount of energy involved at each stage

232
Q

How are metals and glass processed and polymers ?

A

Melted by heating and moulded to produce new ingot s/ glass objects

*plastics must be carefully separated

233
Q

How is paper recycled ?

A

Mixed with water , cleaned and rolled and heated to make new paper

234
Q

What are the main gases in the atmosphere today, and their percentage ?

A

Nitrogen = 78%
Oxygen = 21%
Argon = 0.9%
Carbon dioxide =0.04%

235
Q

How did the atmosphere form originally ?

A

Substances realised as gas from volcanic eruptions.
During volcanic activity carbon dioxide and water were produced.
Carbon dioxide = left in the atmosphere
Water = condensed into oceans

236
Q

What was the original atmosphere?

A

Mostly carbon diode and water, with every little oxygen.

237
Q

How did an oxygen-rich atmosphere develop overtime ?

A

Plants do photosynthesis, taking in carbon dioxide and releasing oxygen .
Initially oxygen reacted with rocks to form as many metal oxides as possible, and then all the rest of free oxygen remained in the atmosphere

238
Q

What are the atmosphere pollutants ?

A

🟣carbon monoxide
🟣sulfur dioxide
🟣particulates
🟣nitrate oxides

239
Q

Where most of the atmospheric pollutants come from?

A

🟣burning fossil fuels
🟣vehicle engines
🟣metal extractions

240
Q

What problems can carbon monoxide as an atmospheric pollutants cause?

A

Combines to haemoglobin in red blood cells, so they can no longer carry oxygen into the bloodstream. This now causes : dizziness, breathing issues and death because is (toxic)

241
Q

Why do particulates as an atmospheric pollutant cause problems?

A

“Particulates “ are small particles.
When breathed in they go deep into the lungs , causing breathing problems or diseases such as bronchitis , and increases risk of heart disease

242
Q

What are PM 10 Particles ?

A

Are 10 micro meters in diameter or less

243
Q

Why do nitrate oxides as atmospheric gases cause issues?

A

Dissolve in the moisture in the clouds, forming acidic solutions, which eventually form as acidic rain

244
Q

Why is acidic rain bad?

A

🟣kills trees
🟣kills living things in lakes/rivers
🟣 erodes stonework , and corrodes metal

245
Q

Why is sulfur dioxide a problem as an atmospheric pollutant?

A

Fossil fuels Contain small amounts of sulfur compounds. When they are burnt they form sulfur dioxide, which a,so causes acid rain and can cause breathing difficulties

246
Q

Examples of some green house gases?

A

Methane & carbon dioxide

247
Q

What is the green house effect?

A
  1. Energy transferred by radiation from the sun reaches the Earth’s surface.
  2. This radiation warms up the Easth’s surface
  3. The Earth’s Surface also emits Infrared radiation, some goes into space, but the rest is absorbed by greenhouse gasses in the atmospheres
  4. The greenhouse gases emit radiation in all directions , war,img the Earth’s surface and atmosphere
248
Q

What problems are causes by the greenhouse effect?

A

The greenhouse effect leads to an increase in the Earth’s atmosphere, leading to global warming :
🟢melting ice caps
🟢rising sea levels
Climate change:
🟢flooding
🟢altered weather patterns
🟢problems with framing and pest control

249
Q

How can green house emissions be reduced ?

A

🟢reducing consumption of fossil fuels (using biofuels)
🟢renewable nervy resources (wind and solar to generate electricity
🟢stop carbon dioxide escaping by using carbon capture

250
Q

Ways to protect against global warming ?

A

Buildings to withstand higher pressure
Flood barriers
Planting different crops

251
Q

Describe the process of fresh water being treated?

A
  1. Water passed through a screen (greed of metal rods), removing large objects
  2. Then water put into settlement tanks, where sand and soils particles sink to the bottom of the water.
  3. Then aluminium sulfate and lime is further added to clump smaller, more fine particles together , making them sink from the water into sludge aswell.
  4. Then a sand filter removes any finer particles
  5. Lastly, chlorine is added to kill harmful bacteria and organisms (not enough to affect humans)
  6. The pH may be ausgeredete but then is shipped of for use to buildings and people

GCSE Chemistry OCR A (10 decks)

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