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FINISHED > C5.4 > Flashcards

C5.4 Flashcards

1
Q
  1. What are ores?
A
  • rocks that contain varying amounts of minerals

- ores are often oxides of a metal

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2
Q
  1. What can be extracted from ores?
A

-metals

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3
Q
  1. What are examples of ores of metals?
A
  • iron ore= haematite

- copper ore= chalcopyrite

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4
Q
  1. For some valuable minerals (e.g. copper) how much ore must be mined?
A

-for some minerals, large amounts of ore need to be mined to recover small percentages of valuable minerals (for example, in copper mining)

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5
Q
  1. What is an example of mining ores in which large amounts need to be mined to get a small percentage of the mineral?
A

-copper mining

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6
Q
  1. How can the metals zinc, iron and copper be extracted?
A

-by heating their oxides with carbon

reduction with carbon or carbon monoxide

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7
Q
  1. What are examples of metals that can be extracted by reduction with carbon?
A
  • zinc
  • iron
  • copper
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8
Q
  1. What happened when a metal oxide loses oxygen and when the carbon gains oxygen (in the extraction of less reactive metals etc.)?
A
  • metal oxide loses oxygen it is reduced,

- carbon gains oxygen and is oxidised

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9
Q
  1. What metals can be extracted by reduction by heating with carbon? Why?
A
  • metals less reactive than carbon

- because the carbon can take oxygen away (reduce) metals less reactive than itself

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10
Q
  1. How are metals more reactive than carbon extracted?
A

-electrolysis

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11
Q
  1. What are the state symbols?
A
  • (s) solid
  • (l) liquid
  • (g) gas
  • (aq) aqueous- dissolved in water
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12
Q
  1. What does (aq) aqueous mean?
A

-dissolved in water

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13
Q
  1. How do you find relative atomic mass?
A

-the top, bigger number on elements on the periodic table

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14
Q
  1. how do you calculate relative formula mass?
A

-add together the relative atomic masses

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15
Q
  1. What is the gram formula mass?
A

-relative atomic mass but in the units grams

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16
Q
  1. How do you calculate the mass of an element in the gram formula mass of a compound?
A
  • relative formula mass with grams as units

- RAM x number of atoms in element

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17
Q
  1. How do you calculate the mass of the metal that can be extracted from a mineral given its formula or an equation?
A
  • calculate proportion of metal in metal oxide- (ram of metal x number of atoms in metal)/RFM of metal oxide
  • multiply answer by mass of metal oxide
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18
Q
  1. What is electrolysis?
A

-the decomposition of an electrolyte with an electric current
(breaking down a substance using electricity)

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19
Q
  1. What is an electrolyte?
A

-liquid that conducts the electricity

20
Q
  1. What are examples of electrolytes?
A
  • free ions dissolved in water (e.g. dissolved salts)

- molten ionic compounds

21
Q
  1. What happens to the ions when an ionic crystal melts?
A

-the charged ions are free to move

=can conduct electricity

22
Q
  1. Where do metals and non- metals for in electrolysis?
A
  • metals form at the negative electrode

- non-metals form at the positive electrode

23
Q
  1. What is the main ore of aluminium called?
A

-bauxite

24
Q
  1. What is the process of the extraction of aluminium from aluminium oxide by electrolysis?
A
  • electrons are taken away from the ions at the positive electrode= atoms/molecules
  • electrons are given to other ions at the positive electrode= atoms/molecules
25
Q
  1. What is the complete WORD equation for the decomposition of aluminium oxide?
A

Aluminium oxide → aluminium + oxygen

26
Q
  1. What is the complete SYMBOL equation for the decomposition of aluminium oxide?
A

2Al2O3 (l) → 4Al(l)+ 3O2 (g)

27
Q
  1. What happens at the negative electrode during electrolysis of molten aluminium oxide?
A

-positively charged aluminium ions gain 3 electrons from the negative electrode= neutral atoms

28
Q
  1. What process occurs at the negative electrode?
A

-reduction- gain of electrons

29
Q
  1. What is the equation for the negative electrode?
A

Al3+ + 3e- → Al

30
Q
  1. What happens at the positive electrode during electrolysis of molten aluminium oxide?
A

-negatively charged oxide ions each lose 2 electrons to the positive electrode= neutral atoms which then combine to form oxygen molecules

31
Q
  1. What process occurs at the positive electrode?
A

-oxidation- loss of electrons

32
Q
  1. What is the equation for the positive electrode?
A

2O2-→ O2 + 4e-

33
Q
  1. What explains the changes taking place during the electrolysis of a molten salt?
A

-the ionic theory

34
Q
  1. How does ionic theory explain the changes taking place during the electrolysis of a molten salt to account for the conductivity of the molten salt and the changes at the electrodes?
A

-ions free to carry charge
=can conduct electricity
(salts= ions. Molten/dissolved= disassociated ion)
During electrolysis the negative electrode attracts the positive ions. The positive electrode attracts the negative ions.
When the ions reach the electrodes, they lose their charges and turn back into atoms.
Metals form positive ions, and non-metals generally form negative ions.

35
Q
  1. What are the uses of metals related to?
A

-their properties

36
Q
  1. What are examples of properties of metals?
A

-strength, malleability, melting point and electrical conductivity

37
Q
  1. What strength are metals?
A

-high strength
-a giant structure held together by strong metallic bonds
=bonds hard to break

38
Q
  1. What is the melting and boiling points of metals like?
A

-high
-a giant structure held together by strong metallic bonds
=bonds hard to break (need lots of energy)

39
Q
  1. How malleable are metals?
A
  • very

- layers of ions can slide over each other

40
Q
  1. Are metal crystals conductive?
A
  • good conductors of heat and electricity

- free charged electrons in the sea of delocalised electrons

41
Q
  1. What is the structure of metal crystals (metallic bonding)?
A
  • a giant structure

- positively charged ions, held closely together by a sea of delocalised electrons that are free to move

42
Q
  1. What impacts can arise from the extraction of metals?
A

-uses up finite resources
-uses energy= burn fossil fuels= greenhouse gases+acid rain
-destroys landscape/habitats
-expensive
+more jobs= more money= improve services

43
Q
  1. What impacts can arise from the use of metals?
A

+useful products made

44
Q
  1. What environmental impacts can arise from the disposal of metals?
A

-landfill takes up space an pollutes surroundings

45
Q
  1. What can we do to reduce negative impacts of mining metals?
A

-recycle

FINISHED (4 decks)

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