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Karteikarten

Metals

fiery Barbarian Chemistry Year 10 Englisch 39 Karten

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  1. 1Physical properties of metals- Thermal and Electrical conductors
    - High melting and boiling points
    - Malleable
    - Ductile
    - Sonourous
    - Lustrous (Shiny)
    - High density
  2. 2Metallic bonding- For metal atoms to become atoms it loses electrons. These delocalised electrons then surround the the metal atoms creating a sea of electrons. This allows for the metal to stay intact and is why it is a good conductor and malleable.
    - Delocalised electrons are electrons that are no associated with 1 atom rather multiple atoms.
    - This is why metals have an electrostatic force of attraction between the cations and the electrons.
  3. 3Explanations of metal's physical properties - Conduction of thermal and electrical energy- Metals are thermal conductors because the electrons can carry thermal energy. Also, the vibration between particles moves along the heat.
    - It conducts electricity as it has delocalised electrons
  4. 4Explanations of metal's physical properties - High MP, Lustrous, Sonorous and High density- It has high MP and BP as the electrostatic force is very strong
    - It generally has high density due to the tightly packed atoms.
  5. 5Metal + Oxide -->Metal oxide
  6. 6Metal + Acid -->Salt + Hydrogen
  7. 7Alloy- An alloy is made up of metals mixed with other metals, or a metal mixed with a non metal.
  8. 8Differences between Alloy and Pure metal structure and properties- In general properties of an alloy and pure metal do differ.
    - Generally a pure metal can be forced to slide over each other as the bonds are maintained, hence not being so strong.
    - An alloy on the other hand has difference sizes atoms which stop the layers from sliding over as easily. This makes the alloy stronger, yet brittle.
  9. 9Common alloys- Stainless steel
    - Mild steel
    - Aluminium alloy
    - Brass
    - Bronze
  10. 10How to put metals in the reactivity order- We can put metals in the reactivity order by reacting metal oxides with carbon. Carbon is a reducing agent here. We can list those that aren't displaced and those that are.
    - Another way is reacting metals with cold water or steam. Only very reactive metals have reactions with cold water and lower reactivity has it with steam. The more vigorous the reaction the more reactive the metal.
  11. 11Reactivity series- Potassium
    - Sodium
    - Calcium
    - Magnesium
    - Aluminium
    - CARBON
    - Zinc
    - Iron
    - Lead
    - HYDROGEN
    - Copper
    - Silver
    - Gold
  12. 12Reactivity series extra info- Most reactive metals are in Group 1 and 2
    - The lesser reactive metals from zinc downwards are transitional metals.
  13. 13Metal + WaterMetal hydroxide + hydrogen
  14. 14Thermal decomposition- The breaking down of a compound by heat is thermal decomposition
    - The lower a metal is in the reactivity series the more readiliy its compounds decompose with heat
  15. 15Thermal decompositions exceptions and examples of hydroxide, nitrate and carbonate- All metal nitrates, carbonates and hydroxides can decompose with exception of sodium and potassium
    - Metal carbonates break down into metal oxide and carbon dioxide
    - Metal hydroxides break down into metal oxide and water
    - Metal nitrate break down into Metal oxide, Nitrogen dioxide and oxygen
  16. 16Basics of extraction of metals- A rock that contains enough metal to make it worth mining is called an ore
    - Apart from gold and silver most metals are found in compounds from which they have to be extracted from
  17. 17Methods of extracting- The more reactive a metal the better it is at hanging on to the element in its compound
    - Therefore, for all the metals that are above carbon in the reactivity series electrolysis is used to extract them
    - For those under carbon, a blast furnace and reduction using carbon or carbon monoxide is used.
    - Gold and silver are found naturally in there pure forms
  18. 18Extracting Ironhttps://www.youtube.com/watch?v=JC3jf7DFbJc
    - Iron is extracted using a blast furnace
    - Inputs -- haematite, coke and limestone and air is blasted from beneath the furnace
    - Process = Coke burning with oxygen from the air, giving CO2. The excess coke reduces CO2 to 2CO. The iron ore is reduced by carbon monoxide to Iron and carbon dioxide.
    - Impurities are removed by reacting calcium oxide with it. This results in Slag.
    - Two wasted gases are Carbon dioxide and Nitrogen.
  19. 19Formulas to remember for extraction of Iron- Coke burning with air to form CO2. ----- C + O2 --> CO2
    - Excess coke reducing carbon dioxide
    CO2 + C --> 2CO
    - Iron ore reduced to iron by CO ---
    Fe2O3 + 3CO --> 2Fe + 3CO2
    - Decomposition of calcium carbonate
    CaCO3 --> HEAT --> CaO + CO2
    - Sand and impurties reacting with CaO
    - CaO + SiO2 --> CaSiO3 (Slag) (Calcium silicate)
  20. 20OILRIG- Oxygen
    - IS
    - Loss of electrons
    - Reduction
    - IS
    - Gain of electrons
  21. 21Extraction of Zinc- Ore = Zinc Blende
    - After breaking the ore and using froth flotation we get zinc sulphide
    - The zinc sulphide is then roasted in the furnace with oxygen resulting in zinc oxide and sulphur dioxide.
    - Zinc oxide then reacts with carbon monoxide in a blast furnace giving us Zinc and carbon dioxide
    - Zinc, coke and limestone
    - We then purify the many impurities from the smelted zinc through fractional distillation or electrolysis
    - Wasted gases: Sulfur dioxide, nitrogen and carbon dioxide.
  22. 22Equations of extraction of Zinc- Roasting : 2ZnS + 3O2 --> 2ZnO + 2SO2
    - Coke burns with oxygen: C + O2 --> CO2
    - CO2 burns with excess coke: C + CO2 --> 2CO
    - Zinc oxide is reduced to zinc: ZnO + CO --> Zn + CO2
    - Decomposition of limestone: CaCO3 --> CaO + CO2
    - CaO reacts reacts with sand to give slag --> CaO + SiO2 --> CaSiO3
  23. 23Uses of aluminium, copper and zinc- Aluminium: Aircraft bodies and food containers
    - Copper: Electrical wires and saucepans
    - Zinc: Galvanising Iron and for making brass.
  24. 24Amphoteric oxide- This is an metal oxide that can neutralise a base or/and acid. Aluminium oxide is the only one
  25. 25Why is aluminium resistive to corrosion- When aluminium reacts with oxygen or water it forms aluminium oxide. This is a layer that coats the aluminium and is impermeable which means it stops the pure aluminium from corrosion.
  26. 26Bauxite formulaAl2O3
  27. 27Extraction of pure Aluminium oxide- First we mix the alumina (aluminium oxide) into molten cryolite (a compound of alumina). This is done to reduce the MP of alumina, increase conductivity and act as a solvent for alumina.
    - This saves money as the operating temperature of electrolysis reduces.
    - In the electrolysis reacction alumina sinks to the bottom as at 1000 degrees celcius it is denser than cryolite.
    - The aluminium ions go to the cathode and the oxygen ions go to the anode.
    - Due to the high temperature the oxygen reacts with the graphite anode producing carbon dioxide
  28. 28Extraction of aluminium reactions- First half equation: Al^3+ + 3e- --> Al
    - Second half equation: 2O^2- --> O2 + 4e-
    - C + O2 --> CO2
  29. 29Displacement- Displacement is the when a lesser reactive metal compound reacts with a more reactive metal and therefore becomes replaced.
    - I.e Mg + CuSO4 --> MgSO4 + Cu
  30. 30Protecting metals methods- Painting
    - Oiling
    - Galvanising
    - Cathodic protection
    - Sacrificial protection
  31. 31What is galvanising- Galvanising is where we coat a metal in molten zinc
    - Zinc prevents the metal from corrosion as it creates a protective layer of Zinc oxide to stop oxygen reacting with the metal
    - When the zinc coating is chinked oxygen will react with the metal underneath however the zinc coating will give the metal electrons preventing it from oxidisation.
  32. 32Cathodic protection- This is where a current is used and powered into the structure
    - The gist of it is that electrons are pushed into the metal object so any lost through oxidation are replaced and the metal doesn't rust.
  33. 33Sacrificial protection- This where we put more reactive metal blocks in front of a metal object. E.g magnesium block on a ship's hull
    - More reactive corrode instead and have to be replaced every now and then.
  34. 34Properties of Transitional metals- High MP and BP
    - Coloured when in compounds
    - High density
    - Shiny
    - Malleable
    - Strong
    - Good conductors of heat and electricity
  35. 35Properties of group 1 metals- Soft
    - Highly reactive
    - Colourless compounds
    - Low MP/ BP
    - Low density
    - good conductors of heat and electricity
    - Malleable, ductile and lustrous
  36. 36Properties of group 2 metals- Low density
    - Low MP/ BP
    - Some soft and some strong
    - Lustrous
    - Malleable
    - Ductile
  37. 37How to remove carbon from iron- Blast oxygen into the furnace and react it with the carbon to remove it from the iron alloy
    - This produces carbon dioxide
  38. 38What is a redox reaction- Where in a reaction one element is reduced and the other is oxidised
  39. 39—

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Year 10 Chemistry Karteikarten am Metals , erstellt von fiery Barbarian am 20/03/2022.
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