corrosion, standard grade chemistry
TRANSCRIPT
CorrosionStandard Grade Chemistry
Topic 12
WHAT IS CORROSION?
• When the surface of a metal changes from being an element into a compound
• The surface goes from being shiny to dull• Nearly all metals corrode• They don’t all corrode at the same rate• Suggest a metal which does NOT
corrode
Potassium
Iron
Gold
REATIVITY
SERIES
Concept Cartoons: Rusting
CHEMICALS FOR RUSTING
Rusting requires OXYGEN and WATER
Rusting is speeded up by SALT
RUSTING
• The corrosion of iron is called rusting• Iron is the only metal which rusts• View Rusting practical demo
Why did the water rise up the tube?
How would the rate of the water rising compare if the wool had been soaked in water instead of acid?
CHEMISTRY OF RUSTING
• Iron metal reacts with oxygen to produce iron(III) oxide (rust)
• Write a word equation and a chemical equation for this process
Iron + oxygen Iron(III) oxide Fe + O2 Fe2O3
•This is an example of a REDOX reaction
Writing ion-electron equation practice:
Sodium atoms losing electrons to form sodium ions
Sulphur atoms gaining electrons to become sulphur ions
Copper(II) ions being reduced
Bromine atoms being reduced
CHEMISTRY OF RUSTING 2
• Corrosion occurs when metals lose electrons – OXIDATION
• When iron rusts, there are two steps.
Iron atoms into iron(II) ions
Iron(II) ions into iron(III) ions
Write ion-electron equations for both steps
The IRON is OXIDISED
REDOX REACTIONS
• Whenever there is oxidation there must also be reduction
• What two other chemicals are involved in the rusting of iron?Oxygen and water
2H2O + O2 + 4e 4OH-
GAIN of electrons = REDUCTION
The reduction step involves these chemicals:
•Dissolved chemicals in the water called ELECTROLYTES help the electrons to be transferred•Give 2 examples of these dissolved chemicals
DETECTING RUSTING
• Ferroxyl indicator can be used to detect rusting• The chemical changes colour in the presence of
Fe2+ ions• It changes from yellow/green to blue
TUTORIAL QUESTIONSTrue or false:
1. Corrosion is the rusting of iron2. pH indicator should be used to test for rusting3. Rusting takes place in the presence of oxygen only4. Rusting will not take place if water is not present5. Salt is required for rusting to take place6. Rusting will occur faster in sea water than tap water
Problem:
Rusting occurs faster in salt solution than in pure water.
(a)Write an ion-electron equation for the rusting of iron
(b)Why does rusting occur faster in salt solution than pure water?
(c)Suggest why rusting also occurs faster in acid solution than in pure water
Practical
A
Set up the experiment shown bellow, using two metals of your choice.
Use a U-tube instead of a beaker.
TUTORIAL QUESTION
Concentration of dissolved electrolytes
Relative rate of rusting of iron
1. Suggest units for the horizontal axis
2. What is the relationship between the rate of rusting of iron and the concentration of dissolved electrolytes.
3. Suggest why the graph does not start from a rate of zero.
FLOWING ELECTRONS
• A chemical cell can be used to show electrons moving away from iron when it rusts
A
Fe Fe2+ + 2e
Oxidation
Reduction
• Electrons leave the iron atoms when it rusts
MORE REDOX
A
Iron Tin
When a cell is made from two metals, ELECTRONS FLOW FROM THE METAL HIGHEST IN THE ELECTROCHEMICAL SERIES TO THE METAL LOWER IN THE SERIES.
Which metal in this cell loses electrons?
Which metal is oxidised?
Describe what happens to:
a) The colour of the solution around the iron
b) The mass of the iron in the cell
c) Does the iron rust?
MORE REDOX 2
A
Iron Magnesium
When a cell is made from two metals, ELECTRONS FLOW FROM THE METAL HIGHEST IN THE ELECTROCHEMICAL SERIES TO THE METAL LOWER IN THE SERIES.
Which metal in this cell loses electrons?
Which metal is oxidised?
Describe what happens to:
a) The colour of the solution around the iron
b) The mass of the iron in the cell
c) Does the iron rust?
MORE REDOX 3
TUTORIAL QUESTIONS• Write an ion-electron equation to show the rusting of iron.• A cell is made using an iron nail and a carbon rod, in a
solution of ferroxyl indicator. Decide which statements are true:
• SG textbook, p118-119
A
Iron Carbon
Electrons move from the carbon rod to the iron
Electrons flow through the solution
A blue colour appears at the iron electrode
The mass of the iron electrode decreases
The iron is oxidised
Set up an experiment to answer the above
questions.
PREVENTING CORROSIONThere are two types of way to help prevent corrosion:• Physical protection• Chemical protection
PHYSICAL PROTECTIONStops oxygen and water coming into contact with the metal:- Paint- Oil or grease- Plastic coating- Tin plating – covering in molten tin- Galvanising – covering in molten zinc (more expensive)- Cathodic protection- Electroplating
Carry out electroplating practical (7.2)
ELECTROPLATING
Copper Gold
Gold ions, Au+
DC-ve +v
e
The metal to be coated is at the NEGATIVE terminal
POSITIVE ions of the OTHER METAL are in the solution
These ions are attracted to the negative terminal, and when they meet it turn into atoms
So the copper is coated in gold atoms
Write an ion-electron equation for the reaction occurring at the negative electrode
Is this oxidation or reduction? Check-test 12.2 ext.
Cathodic Protection
When a metal corrodes it ………………. electronsIf electrons were forced back to the metal, it would
not corrode
How could these be supplied?- Connecting to NEGATIVE terminal of any
electrical supply- Used in cars
Carry out Nails in Contact practical (7.3
core)
CHEMICAL PROTECTION
• Sacrificial protection
A
Iron Magnesium
A metal high in the electrochemical series is connected to the metal to be protected and is sacrificed
- This is used in underground pipes
Mg
In terms of electrons, explain how sacrificial protection works.
• Galvenising
TUTORIAL QUESTIONS
1. a) Why does coating steel with plastic prevent corrosion? b) Chromium-plated steel corrodes quickly if scratched.
What does this tell you about the reactivity of chromium?2. Explain how zinc gives sacrificial protection to steel.3. a) Why should a copper roof not be held in position with iron
nails? b) Suggest a metal which the nails should be made of.
Why?4. Explain what is meant by “electroplating”5. What name is given to the process where steel is protected
by coating it with zinc?6. Assessment test 12.1 + 12.2
PRACTICE EXAM QUESTIONS
SG textbook, p120-121
Questions for SG textbook, p43-44