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Edexcel GCSE Chemistry Higher > Topic 5 (lots of questions) > Flashcards

Topic 5 (lots of questions) Flashcards

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1
Q

Examples of transition metals

A

Iron, copper, nickel, silver, and gold

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2
Q

Typical properties of transition metals

A

Malleability, high melting point, good conductor of electricity and heat ,hard,strong,shiny

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3
Q

Which transition metal is liquid at room temperature?

A

Mercury

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4
Q

Transition metals have high

A

densities

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5
Q

What is a catalyst

A

substance that speeds up the rate of a chemical reaction without being changed or used up

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6
Q

Catalyst in haber process

A

iron to make ammonia

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7
Q

Catalyst in contact process

A

Vanadium(V) oxide to make sulfuric acid

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8
Q

Transition metals make great

A

Catalysts

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9
Q

compounds of transition metals are…

A

colourful. The colour they are depends on the ions they contain

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10
Q

Pure metals are

A

Malleable due to the regular arrangement so layers can slide over each other. They aren’t useful so some used due to this

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11
Q

What is an alloy

A

mixture of metals or with a non metal

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12
Q

Why are alloys harder than pure metals?

A

the different sized atoms of the metals distort the layers in the structure, making it more difficult for them to slide over each other

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13
Q

Steel is…than iron

A

Harder and stronger as long as carbon is less than 1%

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14
Q

Properties of low carbon steel

A

easily shaped

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15
Q

Properties of high carbon steel

A

strong but brittle

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16
Q

Properties of stainless steel

A

Resistant to corrosion

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17
Q

On its own iron will

A

Rust/corrode quickly so adding steel helps

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18
Q

Bronze

A

copper and tin

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19
Q

Brass

A

copper and zinc

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20
Q

Gold alloys

A

combining gold with other metals creates the hardness required for an indirect restoration

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21
Q

Aluminium alloys

A

Used in aircraft as it has the low density of aluminium but is stronger.

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22
Q

Magnalium

A

aluminium and magnesium

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23
Q

What is a redox reaction?

A

an oxidation reaction paired with a reduction reaction

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24
Q

Metals can corrode in the presence of

A

Oxygen and water to form their metal oxides

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25
Q

Corrosion of metals is caused by

A

Redox reaction s the metal loses electrons so it’s oxidised whilst the oxygen gains electrons when it reacts

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26
Q

Rusting

A

The corrosion of iron

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27
Q

Experiment for corrosion

A

Add nail to boiling tube with water and it won’t rust as the boiling water will remove oxygen and oil can be used to stop air getting in. Calcium chloride can be used to absorb any water from the air

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28
Q

How to prevent rusting

A

Coat the iron with a barrier to keep the water or oxygen out. Eg painting

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29
Q

Preventing rusting on moving parts

A

Oiling or greasing

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30
Q

Sacrificial protection

A

Process where a metal is coated with another metal which is more reactive than it,More reactive metal will react with water or oxygen in preference to the less reactive metal

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31
Q

galvanizing

A

a process in which steel is coated with zinc to prevent corrosion

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32
Q

Electroplating

A

Coating the surface of a metal with another metal using electrolysis

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33
Q

In electroplating, the cathode is

A

The object to be plated.

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34
Q

In electroplating, The anode is

A

Metal sued for plating

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35
Q

Electrolyte in electroplating

A

A solution containing ions of the coating metal.

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36
Q

Why is electroplating useful?

A

Household objects like cutlery and cooking utensils are electroplated with metals to stop them corroding. Jewellery is electroplated to improve appearance

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37
Q

Optimum temperature for haber process

A

450°

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38
Q

Optimum pressure for the haber process

A

200 atmosphere

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39
Q

Disadvantages of recycling

A

-can cost more than burying in areas with ample landfill space

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40
Q

Advantages of recycling

A

Environmentally friendly. Saves money and energy.

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41
Q

equation for haber process

A

N2 + 3H2 –> 2NH3

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42
Q

Properties of copper

A

Good electrical and thermal conductor, flexible so used for wiring and pans

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43
Q

Properties of gold

A

Unreactive so used for jewellery and coins

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44
Q

Uses of aluminium

A

-Airplane manufacture (light)

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45
Q

What is titration used for?

A

Finding exactly how much acid is needed to neutralise a given quantity of alkali or vise versa

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46
Q

Titration method

A
  1. add set volume of alkali to flask with indicator
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47
Q

unit for concentration

A

moles/dm3

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48
Q

Formula for concentration

A

Number of moles (mol) / volume (dm3)

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49
Q

How to convert mol/dm3 to g/dm3

A

mol/dm3 x Mr of substance = g/dm3

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50
Q

How to find the Mr (relative formula mass) of a substance

A

Sum of atomic numbers in substance

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51
Q

empirical forumla

A

a chemical formula giving the simplest whole-number mole ratios of atoms in a compound; also called simplest formula

52
Q

Yield

A

The amount of product you get from a reaction. More reactants you start with the more yield you get

53
Q

Percentage yield formula

A

actual yield/theoretical yield x 100

54
Q

What is the theoretical yield

A

The mass of product you’d make of all reactants were converted to products

55
Q

How to calculate theoretical yield

A

-Balance equation

56
Q

Percentage yield is always

A

Between 1 and 100. 100 means that all product was delivered but 0 is that none is

57
Q

In a reaction with a low percentage yield

A

A lot of reactants are wasted. In industry, we want high yield to limit costs

58
Q

Ways of not getting 100% yield

A

Incomplete reactions, practical losses, unwanted reactions

59
Q

incomplete reaction

A

If not all of the reactants are converted to product, the reaction id incomplete and the yield will be less

60
Q

Practical losses

A

You always lose a bit when you transfer chemicals between containers. Imagine pouring a liquid into a new container - some is always left on the inside of the old one

61
Q

Unwanted reactions

A

If unexpected reactions happen, the yield of the intended product goes down, these can be caused by impurities in the reactants or by the change to reaction conditions

62
Q

A lot of reactions make

A

More than one product

63
Q

Some products are

A

Useful but some are watse

64
Q

Atom economy

A

Tells you wha percentage of the mass of the reactants has been converted into your desired product when manufacturing a chemical

65
Q

Atom Economy Formula

A

Mr of Desired Product / Mr of All Products x 100

66
Q

100% atom economy means that…

A

All the atoms in the reactants have been turned into useful products.

67
Q

Reactions with low atom economies

A

Use up resources very quickly. At the same time, they make lots of waste products that have to be disposed which makes the reaction unsustainable because the waste has to go somewhere

68
Q

Low atom economies aren’t usually

A

Profitable because materials are expensive and waste is expensive ti remove and dispose responsibly

69
Q

Way around sustainability of low atom economy reactions

A

Use the waste products instead of disposing of them so make a reaction that produces by products that could be useful

70
Q

Atom economy isn the only factor to consider in industry. What else?

A

Percentage yield, rate of reaction, reaction conditions to move equilibrium for favourable amount of products

71
Q

Factors to consider when designing an industrial process

A
  • cost of refining and extracting the raw materials will affect whether the process is economically viable to make profit
72
Q

Haber process equation

A

N2 + 3H2 –> 2NH3 + heat

73
Q

Higher pressures in the haber process

A

Favour the forward reaction because there are gas molecules on the left. The pressure is set to the highest it can be for the haber process to get the best yield but it can’t be too high as it’s too expensive.

74
Q

Optimum pressure for the haber process

A

200 atmospheres

75
Q

Forward reaction in haber process

A

exothermic so increasing the temperatures decreases the yield of ammonia

76
Q

Temperature used in the Haber process?

A

450° because decreasing the temperature decreases the rate of reaction so temperature is increased to have a fast reaction

77
Q

Catalysts: Haber process

A

Iron catalyst is used to increase the rate of reaction and so it reaches equilibrium fast too. The catalysts doesn’t affect the % yield or position of equilibrium

78
Q

3 main elements for a fertiliser

A

Nitrogen,phosphorous and potassium

79
Q

Plants absorb

A

Nutrients from the fertiliser in the soil

80
Q

If plants don’t get enough essential elements

A

Their growth and life processes are affected

81
Q

What do fertilisers do

A

Supply plants with essential elements that there missing form the soil to increase crop yield by helping the crops grow bigger and faster

82
Q

advantages of ammonia fertilisers

A

You can control the compositions of chemicals in them as well as how much is made. Ammonia fertilisers are soluble so all chemicals can dissolve down into the soil to reach the plants.

83
Q

Ammonia can be reacted with oxygen and water to make

A

nitric acid

84
Q

Reacting ammonia with acids

A

Makes ammonium salts

85
Q

Ammonia + nitric acid

A

ammonium nitrate (fertiliser)

86
Q

How to make ammonium sulfate

A

Mix ammonia and sulfuric acid in a titration experiment

87
Q

Ammonium sulfate method

A
  1. Set up titration equipment using methyl orange in the ammonia
88
Q

Industrial production of ammonium sulfate

A

Ammonia is made using the haber process and and sulfuric acid is made using the contact process. They sue a large reaction chamber filled with ammonia gas and sukfuric acid is sprayed onto the chamber where they produce ammonium sulfate powder

89
Q

Molar volume

A

the volume occupied by 1 mole of a gas at standard temperature and pressure (STP); 22.4 L

90
Q

Molar volume units

A

dm3 mol-1

91
Q

Molar Volume Formula

A

gas volume / number of moles

92
Q

Avagadro’s Law

A

under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules.

93
Q

at RTP, all gases have the

A

Same molar volume - 24dm3 mol-1

94
Q

Molar volume at RTP

A

Moles x 24

95
Q

You can use Avogadro’s number to find

A

Volume of gas a reaction will produce

96
Q

Chemical cells produce

A

A voltage across the cell,until all of one of the reactants has been used up

97
Q

What is a fuel cell?

A

A type of chemical cell that’s supplied with a fuel and oxygen and uses energy from the reaction between them to produce electrical energy efficiently.

98
Q

The reaction between hydrogen and oxygen releases

A

Energy

99
Q

In a hydrogen oxygen fuel cell

A

You can produce a voltage (electrical energy) by reacting hydrogen and oxygen and it doesn’t release any nasty pollutants so clean. Releases water

100
Q

Reaction of a hydrogen-oxygen fuel cell

A

Hydrogen + oxygen -> water 2H2 + 02 = 2H20

101
Q

Advantages of hydrogen-oxygen fuel cells

A

-more efficient

102
Q

Hydrogen-oxygen fuel cells could replace

A

Batteries which are highly toxic so dangerous to dispose of

103
Q

Why won’t hydrogen-oxygen fuel cells take over power stations?

A
  • hydrogen is a gas so takes up more space to store than liquids
104
Q

What is a mole

A

the relative formula mass of a substance in grams (6.02 x 10^23)

105
Q

Number of particles

A

moles x Avogadro’s constant (6.02 x 10^23)

106
Q

How to work out molecular formula

A

Work out the Mr of empirical formula

107
Q

advantages of hydrogen fuel cells

A
  • do not need to be electrically recharged
108
Q

Advantages of chemical fuel cells

A

High emissions

109
Q

Disadvantages of hydrogen fuel cells

A
  • hydrogen is highly flammable
110
Q

Advantages of chemical fuel cells

A

Cheaper

111
Q

Scale of fertiliser industrial production

A

Large scale

112
Q

Starting materials of fertiliser industrial production

A

Raw materials for ammonia and sulfuric acid (haber and contact process)

113
Q

Stages of fertiliser industrial production

A

Several stages

114
Q

Type of process of fertiliser industrial production

A

Continuous

115
Q

Scale of fertiliser lab production

A

Small scale

116
Q

Starting materials of fertiliser lab producing

A

Ammonia solution and sulfuric acid

117
Q

Stages of lab fertiliser

A

Titration then crystallisation

118
Q

Type of process of lab fertiliser

A

Batch

119
Q

why is universal indicator not used in titrations?

A

you want to see a sudden colour change at the end point; U.I turns a variety of colour which indicators a narrow range of pH and is made from a mixture of indicators - it’s a gradual colour change

120
Q

What is meant by molar volume

A

Volume that one mole of chemical occupies

121
Q

How does greasing prevent rusting?

A

Oil forms a barrier protecting the metal from moisture so it cant rust

122
Q

What substance prevents corrosion of nail in experiment

A

Calcium chloride

123
Q

Why might yield be higher than theoretical

A

Not all water has been evaporated

124
Q

How to work out empirical formula from percentages

A

Moles = mass/mr with mass = the percentages

125
Q

Explain why a cathode gains mass but anode loses mass

A

Copper atoms are oxidised at the anode to from positive ions attracted to the cathode but copper ions are reduced at cathode to be attracted to solution

126
Q

What happens in electrolysis with copper electrolysis

A

Cations leave the anode and move toward the cathode to be reduced. Anode loses mass and cathode gains mass.

127
Q

What needs to be remembered about volume for titration

A

Must be to two decimal places

Edexcel GCSE Chemistry Higher (12 decks)

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