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Flashcards

Chemistry: Chapter 10: Metals

HRYN red GCSE Science English 35 cards

Give the order of the Reactivity series 13

Cards in this deck (35)

  1. 1General Physical properties of MetalsHigh melting point and boiling point
    good conductor of heat and electricity
    shiny
    ductile
    malleable
    high density
  2. 2General Chemical Properties of MetalsForm Basis oxides
    form positive ions
    React with oxygen and dilute acid
  3. 3Why do metals have high melting points?They have strong electrostatic forces holding ions together - takes a lot of energy to break apart
  4. 4Why do metals conduct electricity?Have delocalised electrons that are free to move
  5. 5Why are pure metals soft?Layers of ions can slide over one another.
  6. 6What is an alloy? Why are they used2 or more metals, or a metal and non-metal which have been made molten and then mixed together
    used because they have improved qualities for a particular job over the pure metals.
    Stronger than pure metals - harder for layers to slide - atoms having different sizes
  7. 7What is brass made from, what is its special properties and what is its uses?Copper and zinc
    stronger and more resistant to corrosion
    Electrical fittings, car radiators
  8. 8What is Bronze made from, what is its special properties and what is its uses?Copper and tin
    Harder, stronger and sonorous (produce sound)
    Statues, springs, coins
  9. 9What is Stainless Steel made from, what is its special properties and what is its uses?Iron, chromium and nickel
    Doesn't rust
    Kitchen sinks, cutlery, chemical plant
  10. 10What does copper and graphite not react with?acid
  11. 11Give the order of the Reactivity series 13Give the order of the Reactivity series 13
  12. 12group 1 metal + water -?metal hydroxide + hydrogen
  13. 13metal + water + calcium - ?metal hydroxide + hydrogen
  14. 14Metal + acid - ?salt + hydrogen
  15. 15HCl sulphric acid ntirc acid ethanoic acids say what will give and the equation for each ie HCL - HCLHCL - chlorides
    H2SO4 - sulphates
    HNO3 - nitrates
    CH3COOH - ethanoates
  16. 16What is reactivity related to?The tenancy of an atom to become an ion.
    The more reactive an element, the more likely it is to lose or gain electrons and form ions.
  17. 17What do carbonates decompose into? what are the 2 exceptions group 2, lithium and transition metals give an example with lithium carbonatean oxide and carbon dioxide
    exceptions: potassium and sodium carbonate
    ie lithium carbonate - lithium oxide + carbon dioxide
    lLi2CO3
  18. 18What do Nitrates decompose into? group 2, lithium and transition metals give an example with lithium nitrateoxide + nitrogen dioxide + oxygen
    exceptions: potassium, sodium and silver nitrate
    ie lithium nitrate - lithium oxide + nitrogen dioxide + oxygen
    liNO3
  19. 19What do Nitrates of sodium and potassium decompose into? give an examplea nitrite and oxygen
    ie potassium nitrate - potassium nitrite and oxygen
  20. 20What does Silver nitrate decompose into?Silver + nitrogen dioxide + oxygen
    2AgNO3 - 2Ag + 2NO2 + O2
  21. 21What do Hydroxides decompose into? What are the exceptionsOxide + water
    exceptions: potassium and sodium hydroxide
  22. 22In the reactivity series how do you extract each metal?Potassium - aluminum - electrolysis
    zinc - lead - heating with carbon
    copper - gold - occur naturally
  23. 23What is the chemical name and formula for iron ore?Iron oxide
    Hematite
    Fe2O3
  24. 24What is the reducing agent in a Blast Furnace?Carbon/
    Coke
  25. 25What are the raw materials used to extract iron?iron oxide
    coke
    limestone
  26. 26Give a diagram of a blast furnaceGive a diagram of a blast furnace
  27. 27What is the processes that happen in a blast furnace? 8 stages How do you extract iron?1. mixture of limestone, coke and hematite is added at the top of the blast furnace. 2. hot air is blasted into the blast furnace. 3. code reacts with the hot air to form carbon dioxide. 4. code reacts with the co2 to form carbon monoxide. 5. carbon monoxide reduces the iron ore to form iron and carbon dioxide. 6. iron (pig iron) collects at bottom of blast furnace to be tapped off. 7. impurities collect at bottom in a layer (slag) and can be tapped off. 8. waste gases are removed from the blast furnace.
  28. 28Reaction of Oxygen and coke word and symbolC(s) + O2(g) - CO2(g)
    carbon + oxygen - carbon dioxide
  29. 29Reaction of carbon dioxide and coke word and symbolcarbon dioxide + coke - carbon monoxide
    CO2(g) + C(s) - 2CO(g)
  30. 30Reaction of carbon monoxide reducing iron oxide word and symbolIron oxide + carbon monoxide - iron + carbon dioxide
    Fe2O3(s) + 3CO(g) - 2Fe(I) + 3CO2(g)
  31. 31What is the role of the limestone?To remove impurities - reacts with impurities to form slag
  32. 32Give an acid/base reactioncalcium oxide + silica - calcium silicate
    CaO(s) + SiO2 - CaSiO3(i)
  33. 33How do you produce calcium oxide from limestone?Calcium carbonate - calcium oxide + carbon dioxide
  34. 34What are the impurities in iron?Carbon
    Sulfur
    Silica
    Phosphorous
  35. 35How are the impurities removed? 2Oxygen convert to oxides. Carbon and sulfur form gas oxides so will leave as waste gases.
    2. Oxide of phosphorous and silica are acidic so will react with lime to form slag which can be tapped off.

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GCSE Science (Chemistry) Flashcards on Chemistry: Chapter 10: Metals, created by HRYN red on 02/01/2021.
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