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metals Flashcards

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1
Q

structure of a metal?

A

metals form a metallic lattice made of rows of positive metal ions and delocalised electrons, which are able to move through the structure

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2
Q

why is the melting point of Mg higher than Na

A
  • Na ions have a +1 charge, mg ions have a +2 charge
  • the electrostatic attraction between the mg ions and delocalised e- is stronger
  • requires more energy to overcome it
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3
Q

why are metals malleable

A

the rows of positive metal ions can slide over each other and the delocalised electrons are able to maintain the attraction

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4
Q

3.5.2 define the term thermal decomposition

A

the breaking down of a substance using heat (thermal energy)

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5
Q

define the term ore

A

a rock containing a metal compound

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6
Q

give one example of a native metal & why it’s found this way

A

gold/silver - too unreactive to have combined with oxygen or sulfur

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7
Q

how do you know if something is a redox reaction

A

both oxidation and reduction occur

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8
Q

what does it mean if a substance has been oxidised

A

it’s lost electrons

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9
Q

what does it mean if a substance is a reducing agent

A

it’s helped another substance be reduced by giving it electrons

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10
Q

what does it mean if a substance has been reduced

A

it’s gained electrons

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11
Q

what is the definition of metallic bonding?

A

the electrostatic attraction between the positive metal ions and the negative delocalised electrons

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12
Q

what are the typical properties of metals?

A
  • high MP: metallic bonding usually very strong, so lots of energy needed to break it
  • conduct electricity: bc delocalised e- are free to move
  • malleable: bc layers of metal ions can slide over each other
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13
Q

3.5.2 what is the formula for thermal decomposition of metal carbonates?

A

metal carbonate —> metal oxide + carbon dioxide

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14
Q

what would you observe during the thermal decomposition of copper carbonate?

A

copper carbonate —> copper oxide + carbon dioxide: green solid —> black solid + colourless gas

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15
Q

3.5.2 what is downward delivery?

A

CO2 denser than air, so often collected using this method. that means it just sinks to bottom of a tube & stays there until it needs to be used

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16
Q

3.5.3 what is the order of the metal reactivity series, from lowest to highest?

A

Au Ag Cu H Pb Fe Zn C Al Mg Ca Li Na K

(H and C non-metals but they’re included bc positions important when considering displacement reactions

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17
Q

3.5.3 what is the general formula for metals reacting with cold water?

A

metal + water —> metal hydroxide + hydrogen

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18
Q

3.5.3 what are the observations for the reaction between magnesium and water?

A
  1. effervescence - due to H gas produced
  2. solid disappears - due to being used up in reaction
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19
Q

3.5.3 what happens with metals less reactive than Mg for the metal + water reaction?

A

they react so slowly with cold water that you can’t actually tell anything’s happening; even with Mg need to wait few mins

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20
Q

3.5.3 what are the metals in group 1 called, & what do they do?

A

the alkali metals; react violently w water to form metal hydroxides & hydrogen

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21
Q

3.5.3 what are the shared observations for the reaction of Li, Na and K with water?

A
  • solid floats - it’s less dense than water
  • effervescence - hydrogen gas produced
  • solid moves - effervescence propels it around surface of water
  • solid disappears - used up in reaction
  • when universal indicator added to water afterwards it turns dark blue
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22
Q

3.5.3 what do you observe when Na is reacted with water?

A

faster than Li, and Na melts

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23
Q

3.5.3 what happens when you react K with water?

A
  • fastest
  • K melts
  • lilac flame
24
Q

3.5.3 what happens to the reactivity of the group 1 metals as you go down the group?

A

increases

25
Q

3.5.3 why does the reactivity increase as you go down the group 1 metals?

A
  • atoms get bigger & have more shells
  • outer electron further from nucleus
  • attraction between nucleus & outer electron is weaker
  • so less energy needed to break the attraction
26
Q

3.5.3 what is the formula for metal reacting with steam?

A

metal + steam —> metal oxide + hydrogen

27
Q

3.5.3 describe how to conduct an experiment for the reaction between metal and steam

A
  • put some wet wool and a Mg ribbon into a horizontal test tube, with a bung on the top and a thingy coming out of the bung
  • heat the test tube: some wet wool is heated to generate steam for the Mg to react with
  • ignite the H2 gas coming out the test tube to safely destroy it
28
Q

3.5.3 why do metals react with cold water and hot steam to produce different products?

A

steam has more energy, so both bonds in the water molecule can break - forming just a metal oxide and a H2, not a metal hydroxide and an H

29
Q

3.5.4 what is the formula for an acid reacting with a metal?

A

acid + metal —> salt + hydrogen

30
Q

what salts are always soluble?

A

Na+, K+, NH ₄+, NO ₃-

31
Q

is Cl- soluble?

A

yes, except with Ag+ and Pb2+

32
Q

is SO ₄2- soluble?

A

yes, except with Ca2+, Ba2+ and Pb2+

33
Q

is CO ₃2- soluble?

A

no, except with Na+, K+ and NH ₄+

34
Q

is OH- soluble?

A

no, except with Na+, K+ and Ca2+

35
Q

is O2- soluble?

A

no, except with Na+, K+, and NH ₄+

36
Q

3.5.4 what are the two important observations in an acid + metal reaction?

A
  • metal disappears because used up in reaction
  • fizzing because gas (H) produced
37
Q

3.5.4 what metals cant/won’t react with H and why?

A
  • Au, Ag and Cu, because they’re less reactive than H so won’t displace it
  • Li, Na and K, because they’re too reactive so reaction with acids is too violent
38
Q

3.5.5 what are the observations for displacement reactions?

A
  • solid colour change
  • solution colour change
39
Q

3.5.6 what are ores?

A

the rocks containing specific metal compounds

40
Q

3.5.6 what are most metals in the earths crust found as?

A

found as compounds with oxygen & sulphur, bc over a long time those metals have reacted w oxygen & sulphur

41
Q

3.5.6 which metals are found ‘native’ in the earth’s crust and why?

A

gold (au) and silver (ag) - too unreactive to have combined with oxygen or sulphur

42
Q

3.5.6 what does ‘native’ mean for metals?

A

means chemically uncombined

43
Q

3.5.6 do native metals need to be chemically extracted?

A

no they already exist on their own

44
Q

3.5.6 how is the method of extraction for metals chosen?

A

it depends on how reactive the metal is

45
Q

3.5.6 what is the electricity method of chemical extraction? (electrolysis)

A
  • metals more reactive than carbon can’t be displaced by carbon
  • instead, have to use electricity to break down their ore compounds
  • don’t need to know how this works
46
Q

3.5.6 what is the carbon extraction method of chemical extraction?

A
  • metals less reaction than carbon can be displaced by carbon
  • for example, copper can be displaced from its ore (copper oxide) by heating with carbon:
    carbon C (s) + copper oxide 2CuO (s) —> carbon dioxide CO2 (g) + copper 2Cu (s)
  • only works bc carbon more reactive than copper
47
Q

3.5.6 what type of reaction is using carbon to displace a metal from its oxide?

A

a redox reaction

48
Q

3.5.7 what are the qualities of iron compared to hydrated iron (III) oxide (rust)?

A

iron: grey shiny malleable
rust: brown dull brittle

49
Q

3.5.7 what two stages does rusting occur in?

A
  1. iron oxidised by oxygen to form iron(iii) oxide:
    4Fe (s) + 3O2 (g) —> 2Fe2O3 (s)

Fe has gained oxygen and also lost e- to form Fe3+ ions. for both reasons, it’s been oxidised

  1. iron(iii) oxide hydrated by water:
    Fe2O3 (s) + xH2O (l) —> Fe2O3•xH2O (s)

the amount of water gained by iron(iii) oxide varies a lot

50
Q

3.5.7 what elements are in steel, brass, and bronze?

A

steel: iron + carbon
brass: copper + zinc
bronze: copper + tin

51
Q

3.5.7 what is the use for iron (alloys)?

A

making steel - steel more useful than iron

52
Q

3.5.7 what elements are in low-carbon steel, and what are its uses?

A

Fe, 0.1% C; ships, cars bridges etc - strong, but low-carbon so can be hammered into various shapes

53
Q

3.5.7 what elements are in high-carbon steel, and what are its uses?

A

Fe, 1% C; tools e.g. knives, screwdrivers - high-carbon so less malleable & stiffer than low-carbon steel

54
Q

3.5.7 what elements are in stainless steel, and what are its uses?

A

Fe, 1% C, 10% Cr; cutlery, cooking utensils, kitchen sinks - Cr forms oxide layer that resists corrosion, so stays shiny & clean

55
Q

3.5.7 what are coppers uses? (alloys)

A
  • wires: excellent conductor of electricity
  • cooking pans: excellent conductor of heat
  • water pipes: unreactive & malleable
56
Q

3.5.7 what are the uses for aluminium (alloys)?

A
  • aircraft bodies: low-density & high strength
  • power cables: low-density & conducts

chemistry (10 decks)

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