Extracion and uses of Metals Flashcards

1
Q

where are most metals found?

A
  • in ores
  • and have to be separated
  • metals that are unreactive don’t tend to form compounds with other elements. unreactive metals such as gold are found uncombined, so you have to find them and dig them up.
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2
Q

what happens with metals that do react with other element to form compounds?

A
  • most metals do react with other element to form compounds, which can be found naturally in the earth’s crust.
  • if a compound contains enough of the metal to make it worthwhile extracting, the compound is called a metal ore.
  • there are limited amounts of metal ores, they’re “finite resources”
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3
Q

what happens the more reactive a metal is?

A

the harder it is to extract it from a compound

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4
Q

what do lots of common metal oxides form?

A
  • lots of common metals like iron and aluminium form metal oxides
  • the metal can be separated from its oxide by a REDUCTION reaction
  • the most common type of reduction reaction uses carbon as a reducing agent to separate the oxygen from the metal
  • but carbon can’t be used for all metals.
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5
Q

what are methods of extractions linked to?

A
  • order of reactivity
  • only metals that are LESS REACTIVE than carbon can be extracted by a reduction reaction with carbon, this is done by heating the ore with carbon monoxide. (e.g. iron oxide is reduced in a blast furnace to make iron)
  • this is because more reactive elements form compounds more readily. carbon is more reactive than iron, so carbon “steals” oxygen from iron oxide
  • in other words, carbon can only take the oxygen away from metals which are LESS REACTIVE THAN THE CARBON ITSELF
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6
Q

what do very reactive metals form?

A
  • very reactive metals form very stable ores
  • i.e. its difficult to get the metal out of its compound
  • so metals that are more reactive than carbon (higher in the reactivity series) have to be extracted using electrolysis
  • electrolysis uses electricity to separate the metal from the other elements in the compound.
  • for example, aluminium is extracted from aluminium oxide using electrolysis.
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7
Q

what similarities do aluminium, iron and copper have?

A
  • they are dense and shiny and have high melting points
  • they have high tensile strength (strong and hard to break)
  • they can also be hammered into a different shape (malleable)
  • they are good conductors of electricity and heat energy
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8
Q

what are the properties of iron and therefore what are its uses?

A
  • iron has all the properties you’d expect of a metal. adding other materials can change its properties though
  • wrought iron is almost completely pure iron.
  • its malleable, so its used to make gates and railings
  • the main problem is that it corrodes easily/rusts.
  • alloys of iron called steels are often used instead of pure iron. steels are made by adding small amounts of carbon and sometimes other metals to iron.
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9
Q

what are the properties of aluminium and therefore what are its uses?

A
  • aluminium is also a typical metal. however, unlike iron it doesn’t corrode easily
  • aluminium reacts very quickly with oxygen in the air to form aluminium oxide. a nice protective layer of aluminium oxide sticks firmly to the aluminium below and stops any further reaction taking place
  • because aluminium doesn’t corrode its useful for products that come in contact with water e.g. drinks cans
  • aluminium is also much less dense than iron, which makes it lighter
  • this makes it useful when the weight of the metal is important, e.g. bicycle frame and aeroplanes
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10
Q

what are the properties of copper and therefore what are its uses?

A
  • copper is an especially good conductor of heat and electricity
  • its used in electrical components and wiring as it has low resistance and so is efficient at transferring energy.
  • its also used in heating systems, such as underfloor heating, as it allows speedy transfer of heat to the surroundings.
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11
Q

why and how are alloys used?

A
  • pure metals don’t always have the properties needed
  • the regular structure of pure metals makes them soft, often too soft for use in everyday life
  • alloys are made by adding other elements to the metal (usually other metals and/or carbon)
  • different elements have different sized atoms. so when another element is mixed with a pure metal, the new atoms will distort the layers of metal atoms, making it difficult for them to slide over each other. this makes alloys HARDER than pure metals.
  • alloys of iron called steels are often used instead of pure iron. steels are made by adding small amounts of carbon and sometimes other metals to iron.
  • many other alloys are used in everyday life, e.g. brass (copper and zinc) and bronze (copper and tin)
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12
Q

why are alloys harder than pure metals?

A
  • different elements have different sized atoms.
  • so when another element is mixed with a pure metal, the new atoms will distort the layers of metal atoms, making it difficult for them to slide over each other.
  • this makes alloys HARDER than pure metals.
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13
Q

what are the properties and uses of each type of steel?

A
  1. LOW CARBON STEEL:
    - easily shaped
    - car bodies
  2. HIGH CARBON STEEL:
    - very strong, inflexible, brittle
    - bridges
  3. STAINLESS STEEL
    - corrosion resistant, hard
    - cutlery
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