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Chemistry > C6 Chemistry out there > Flashcards

C6 Chemistry out there Flashcards

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1
Q

What is electrolysis?

A

Electrolysis is the decomposition of liquid by passing electricity through it. (Flow of charge by moving ions and the discharge of ions at the electrodes)

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2
Q

What is the anode?

What is the cathode?

A
  • Positive electrode

- Negative electrode

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3
Q

What are cations?

What are anions?

A
  • Positively charged (Loss of electrons)

- Negatively charged (Gain of electrons)

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4
Q

Describe what the term electrolyte means?

A

Electrolyte is the liquid which conducts the electricity and is decomposed or broken down during electrolysis

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5
Q

What apparatus is required for electrolysis?

A
  • DC power supply
  • Anode
  • Cathode
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6
Q

Where are the negative ions and positive ions discharged?

A

Cathode (Positive ions)

Anode (Negative ions)

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7
Q

Describe the chemical test for oxygen and hydrogen

A
  • When hydrogen burns with a lit splint, it makes a ‘pop’ sound
  • Oxygen relights a ‘glowing’ splint
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8
Q

Describe the observations of the electrolysis of Copper(II) Sulfate solution using carbon electrodes

A
  • The cathode gets plated with copper and bubbles are formed at the anode
  • The blue colour will slowly disappear
  • Oxygen is produced at the anode
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9
Q

What factors affect the amount of substance produced during electrolysis?

A
  • Time

- Current

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10
Q

Name the products made during the electrolysis of NaOH

A

Oxygen - anode

Hydrogen - cathode

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11
Q

Name the products made during the electrolysis of H2SO4

A

Hydrogen - Cathode

Oxygen - Anode

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12
Q

Why does the electrolysis of NaOH produce Hydrogen instead of Sodium at the Cathode

A

Because Na is higher in the reactivity series, hence Hydrogen is discharged as a preference

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13
Q

Explain why an ionic solid can not be electrolysed but the molten liquid can be electrolysed

A

The ions in the ionic solid can not move as they vibrate in a fixed position, the ions in a molten liquid can move, hence then can be electrolysed

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14
Q

What type of reaction occurs between hydrogen and oxygen?

A

Exothermic (energy is released into the atmosphere)

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15
Q

Describe what a fuel cell is

A

A fuel cell is a cell supplied with fuel and oxygen that uses the energy released from the reaction between the fuel and oxygen to produce electrical energy efficiently

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16
Q

What fuel is used in a hydrogen-oxygen fuel cell?

A

Hydrogen

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17
Q

Why does a hydrogen-oxygen fuel cell not form a polluting waste product?

A

Unsure

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18
Q

Balanced symbol equation for the reaction between hydrogen and oxygen

A

2H2 +O2 —-> 2H2O

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19
Q

Energy-level diagram

A

2H2 + O2 ——–> 2H2O
Energy
Released

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20
Q

Construct the balanced symbol equation for the overall reaction in a hydrogen-oxygen fuel cell

A

Equation

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21
Q

Advantages of fuel cells

A
  • Provides water for astronauts
  • Lightweight
  • Compact
  • No moving parts
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22
Q

Disadvantages of using fuel cells

A
  • Fuels cells often contain harmful catalysts that have to be disposed at the end of the lifetime of a fuel cell
  • Production of the hydrogen and oxygen will involve the use of energy which may have to come from the burning of fossil fuels
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23
Q

Explain why the car industry is developing fuel cells

A
  • No carbon emissions from the car
  • Fossil fuels currently used are non-renewable
  • Large source of hydrogen is available by decomposing water
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24
Q

What is oxidation and reduction?

A
  • Oxidation is the addition of oxygen

- Reduction is the removal of oxygen

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25
Q

What two conditions are required for rusting of steel and iron?

A
  • Water

- Oxygen

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26
Q

Methods to prevent rusting

A
  • oil and grease
  • paint
  • galvanising
  • sacrificial protection
  • alloying
  • tin plating
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27
Q

How do these methods prevent rusting?

A
  • they prevent oxygen and water reaching the surface of the metal requiring protection
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28
Q

Order of reactivity (most to least)

A

Magnesium
Zinc
Iron
Tin

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29
Q

Temperature change during a displacement reaction

A

Temperature increases because it is an exothermic reaction

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30
Q

Define the terms :

  • oxidation and reduction

- oxidising agent and reducing agent

A

Oxidation is the loss of electrons
Oxidising agent is a substance that can remove electrons from other substances, oxidising them
Reduction is the gain of electrons
Reducing agent is a substance that can give electrons to other substances, reducing them

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31
Q

Why is rusting a redox reaction?

A
  • Iron loses electrons

- Oxygen gains electrons

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32
Q

How does sacrificial protection work and protect the iron underneath it?

A
  • Use of metal such as zinc or magnesium
  • Use of metal which is more reactive than iron
  • Sacrificial metal will lose electrons in preference to the underlying iron
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33
Q

Explain the disadvantage of using tin plating to protect the iron

A
  • Tin acts as a barrier stopping water or oxygen reaching the surface of the iron
  • When the tin layer is scratched, the iron will lose electrons in preference to the tin as it is more reactive than tin and so the iron rust even more quicker than on its own
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34
Q

Rusting word equation

A

Oxygen + Water + Iron —-> Hydrated iron (III) Oxide

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35
Q

Explain how galvanising protects iron from rusting

A
  • Galvanised iron is coated with zinc
  • Layer of zinc stops water and oxygen from reaching the surface of the iron
  • Zinc also acts as a sacrificial metal
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36
Q

Explain displacement reactions in terms of oxidation and reduction

A
  • Metal ion is reduced by gaining electrons

- Metal atom is oxidised by losing electrons

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37
Q

Explain why alcohols aren’t hydrocarbons

A

Because they contain atoms other than hydrogen and carbon

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38
Q

What are the required conditions for fermentation?

A
  • 25 to 50 degrees Celsius
  • Presence of water
  • Yeast
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39
Q

What are the main uses of ethanol?

A
  • Alcoholic beverages
  • Solvent ( industrial methylated spirits)
  • Fuel for care
40
Q

Word equation for fermentation

A

Glucose —-> Carbon dioxide + Ethanol

41
Q

Word equation for Hydration of ethene

A

Ethene + Water —-> Ethanol

42
Q

Describe how ethanol can be made from fermentation

A
  • Glucose solution
  • Reaction catalysed by enzymes in yeast
  • Absence of oxygen
  • Fractional distillation to obtain ethanol
43
Q

Conditions during fermentation

A
  • Temperature too low, enzymes are inactive
  • Temperature too high, enzymes become denatured
  • Absence of oxygen, to prevent ethanoic acid being made
44
Q

Explain why fermentation is a renewable process

A

It’s raw material is sugars from plants

45
Q

Explain why hydration is a non-renewable resource

A

It uses ethene from crude oil as its raw material

46
Q

Evaluate the merits at which the two processes are judged by

A 
Conditions used
Raw materials used
Sustainability 
Batch verses continuous 
Purification 
Atom Economy 
Percentage yield
47
Q

Ethanol is produced for industrial use, how?

A
  • Passing ethene and steam over a heated phosphoric acid catalyst
48
Q

Chlorofluorocarbon is an organic molecule containing carbon, fluorine and chlorine atoms

A

True

49
Q

Give some uses of CFCs

A

Refrigerators
Aerosols propellants
Air conditioning systems

50
Q

Ozone is a form of oxygen p, what is the formula?

A

O3

51
Q

Describe some properties of CFCs

A
  • Chemically inert
  • Insoluble in water
  • Low boiling point
52
Q

Describe the problems increased Ultraviolet light can caus

A
  • Eye cataracts
  • Accelerated ageing of skin
  • Skin cancer
  • Increased chances of sunburn
53
Q

Alternatives to CFCs

A

HFCs
Hydrofluorocarbon
Hydrocarbons provide a safer alternative
Alkanes

54
Q

Explain why the use of CFCs has been banned in the UK

A

Society agrees with scientists’ views that CFCs deplete the ozone layer

55
Q

Describe and explain how scientists’ attitudes towards CFCs have changed

A
  • initial enthusiasm for the use of CFCs based upon their inertness
  • later discovery of ozone depletion and link to CFCs being used
  • acceptance by scientists and the rest of the world community that use of CFCs should be banned
56
Q

Describe how CFCs deplete the ozone layer

A
  • CFCs molecules are broken down in the stratosphere by UV light to give highly reactive chlorine atoms
  • chlorine atoms react with ozone molecules
  • chlorine atoms are regenerated so they can react with more ozone molecules, causing a chain reaction
57
Q

Explain in terms of electrons how a carbon-chlorine bond can break to form highly reactive chlorine atoms

A

Unsure

58
Q

Explain why only a small number of chlorine atoms will destroy a large number of ozone molecules

A

Unsure

59
Q

Explain why CFCs will continue to deplete ozone a long time after their use has been banned

A

Unsure

60
Q

What atom is a chlorine radical

A

Chlorine atom

61
Q

Explain why CFCs are only removed slowly fro the stratosphere

A

Unsure

62
Q

Describe how the depletion of the ozone layer allows more UV light to reach the earth

A

Unsure

63
Q

Explain how ozone absorbs UV light in the stratosphere

A

Unsure

64
Q

Does hard water lather well with soap?

A

No, but soft water does

65
Q

Both hard and soft water lather well with soap less detergents

A

True

66
Q

What ions cause water hardness?

A

Magnesium and Calcium ions

67
Q

What method is used to remove temporary hardness, but can’t be used to remove permanent hardness?

A

Boiling

68
Q

Describe how hardness in water can be removed?

A
  • Passing water through an ion-exchange column

- Adding washing soda (sodium carbonate)

69
Q

Describe the origin of temporary hardness in water. Give the word equation

A

Calcium carbonate in rocks reacts with dissolved carbon dioxide and water to form soluble calcium hydrogen-carbonate

Calcium Carbonate + Water + Carbon Dioxide —->Calcium Hydrogen-carbonate

70
Q

What is temporary hardness caused by?

What is permanent hardness caused by?

A
  • Calcium hydrogen carbonate

- Calcium Sulfate

71
Q

Describe how boiling removes temporary hardness

A
  • Decomposition of calcium hydrogen carbonate to give insoluble calcium carbonate(limescale), water and carbon dioxide
  • Soluble Calcium ions are changed in to insoluble compounds
72
Q

Explain how an ion exchange resin can soften water

A
  • tiny beads are packed in to a plastic column, the water softens as it passes through the column
  • the ions from the resin swap with the ions in the water
  • as the water passes through, the magnesium and calcium ions are attached to the resin and sodium ions leave the resin
  • the water softens because the Mg and Ca ions are gone
  • the resin is regenerated by flushing the resin with sodium chloride solution. The sodium ions are swapped back in to the resin. The other ions are pushed out washed in to waste water
73
Q

What can vegetable oil be used to make, which is an alternative to diesel from crude oil?

A

Bio-diesel

74
Q

At room temperature:

  • oils are_______
  • fats are _______
A
  • liquids

- solids

75
Q

Describe an emulsion

A

In an emulsion, tiny droplets of one of the liquids are dispersed throughout the other liquid. The two liquids in an emulsion will eventually settle out in to separate layers agin.

76
Q

Give an example of a oil-in-water emulsion

A

Milk

77
Q

Give a water-in-oil emulsion

A

Butter

78
Q

Vegetable oil + Sodium Hydroxide —->___________

A

Soap

79
Q

Animals fats, vegetable fats and oils are ____________

A

Esters

80
Q

Explain why unsaturated fats are healthier as a part of balanced diet

A

Reduce the risk of heart disease

…

81
Q

Describe how margarine is manufactured from vegetable oils

A

Unsaturated vegetable oil is turned in to saturated vegetable oils by reacting them with hydrogen. A nickel catalyst may be used

82
Q

Describe how immiscible liquids can form an emulsion

A

If the two liquids have different densities, they will not dissolve in one another. However if they are shaken vigorously, they form an emulsion.

83
Q

Describe an oil-in-water (milk)

A

It contains tiny droplets of oil dispersed in water

84
Q

Describe a water-in-milk emulsion (butter)

A

Consist of tiny droplets of water dispersed in oil

85
Q

Describe how natural fats and oil can be split up by hot sodium hydroxide solution. (Saponification)

A

During saponification, the hydroxide ions from sodium hydroxide solution breakdown the oil or fat molecule. This causes the bonds between fatty acids and glycerol to break.

Fat+Sodium Hydroxide —-> Soap + Glycerol

86
Q

What type of a reaction is saponification?

A

Hydrolysis

87
Q

Ingredients of a washing powder and it’s purpose

A
  • Active detergent: does the cleaning
  • Water softener: to soften hard water
  • Bleaches: to remove coloured stains
  • Optical brighteners: to give a whiter than white appearance
  • Enzymes: used in low temperature washes to remove food stains
88
Q

Describe the term solvent

A

The liquid that does the dissolving

89
Q

Describe the term solute

A

The dissolved substance

90
Q

Describe the term solution

A

If the substance dissolves in the liquid, it forms a solution

91
Q

Ingredients in a washing up liquid and it’s purpose

A
  • Active detergent does the cleaning
  • Water: to thin out detergent so it can be dispensed easily
  • Colouring agent and fragrance: to improve attractiveness to the product
  • Rinse agent: to help drain the water out of the crockery
92
Q

Advantages of washing clothes at low temperature

A
  • Saving energy costs

- A greater range of clothing can be washed

93
Q

Describe the term detergent

A

Detergents are ingredients of washing-up liquid and washing powders. They are substances that can surround fat or oil molecules in stains and remove them from clothing or plates. They have a hydrophobic tail and hydrophilic head.

94
Q

Explain how detergents remove fat or stains

A
  • Hydrophilic end of detergent molecule forms strong intermolecular forces with water molecules
  • Hydrophobic rails of detergent molecule forms strong intermolecular forces with fat or oil molecules
95
Q

Describe dry cleaning

A

Solvent does not involve water

Stain will not dissolve in water

96
Q

Explain in terms of intermolecular forces how dry cleaning works

A
  • There are weak intermolecular forces between grease molecules
  • There are weak intermolecular forces between solvent molecules
  • Solvent molecules form intermolecular forces with molecules of grease and so solvent molecules can surround molecules of grease

Chemistry (4 decks)

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