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metals Flashcards

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?

25
3.5.3 why does the reactivity increase as you go down the group 1 metals?
- 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
3.5.3 what is the formula for metal reacting with steam?
metal + steam —> metal oxide + hydrogen
27
3.5.3 describe how to conduct an experiment for the reaction between metal and steam
- 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
3.5.3 why do metals react with cold water and hot steam to produce different products?
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
3.5.4 what is the formula for an acid reacting with a metal?
acid + metal —> salt + hydrogen
30
what salts are always soluble?
Na+, K+, NH ₄+, NO ₃-
31
is Cl- soluble?
yes, except with Ag+ and Pb2+
32
is SO ₄2- soluble?
yes, except with Ca2+, Ba2+ and Pb2+
33
is CO ₃2- soluble?
no, except with Na+, K+ and NH ₄+
34
is OH- soluble?
no, except with Na+, K+ and Ca2+
35
is O2- soluble?
no, except with Na+, K+, and NH ₄+
36
3.5.4 what are the two important observations in an acid + metal reaction?
- metal disappears because used up in reaction - fizzing because gas (H) produced
37
3.5.4 what metals cant/won’t react with H and why?
- 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
3.5.5 what are the observations for displacement reactions?
- solid colour change - solution colour change
39
3.5.6 what are ores?
the rocks containing specific metal compounds
40
3.5.6 what are most metals in the earths crust found as?
found as **compounds with oxygen & sulphur**, bc over a long time **those metals have reacted** w oxygen & sulphur
41
3.5.6 which metals are found ‘native’ in the earth’s crust and why?
gold (au) and silver (ag) - too unreactive to have combined with oxygen or sulphur
42
3.5.6 what does ‘native’ mean for metals?
means chemically uncombined
43
3.5.6 do native metals need to be chemically extracted?
no they already exist on their own
44
3.5.6 how is the method of extraction for metals chosen?
it depends on how reactive the metal is
45
3.5.6 what is the electricity method of chemical extraction? (electrolysis)
- 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
3.5.6 what is the carbon extraction method of chemical extraction?
- 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
3.5.6 what type of reaction is using carbon to displace a metal from its oxide?
a redox reaction
48
3.5.7 what are the qualities of iron compared to hydrated iron (III) oxide (rust)?
iron: grey shiny malleable rust: brown dull brittle
49
3.5.7 what two stages does rusting occur in?
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** 2. **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
3.5.7 what elements are in steel, brass, and bronze?
steel: iron + carbon brass: copper + zinc bronze: copper + tin
51
3.5.7 what is the use for iron (alloys)?
making steel - steel more useful than iron
52
3.5.7 what elements are in low-carbon steel, and what are its uses?
Fe, 0.1% C; ships, cars bridges etc - strong, but low-carbon so can be hammered into various shapes
53
3.5.7 what elements are in high-carbon steel, and what are its uses?
Fe, 1% C; tools e.g. knives, screwdrivers - high-carbon so less malleable & stiffer than low-carbon steel
54
3.5.7 what elements are in stainless steel, and what are its uses?
Fe, 1% C, 10% Cr; cutlery, cooking utensils, kitchen sinks - Cr forms oxide layer that resists corrosion, so stays shiny & clean
55
3.5.7 what are coppers uses? (alloys)
- wires: excellent conductor of electricity - cooking pans: excellent conductor of heat - water pipes: unreactive & malleable
56
3.5.7 what are the uses for aluminium (alloys)?
- aircraft bodies: low-density & high strength - power cables: low-density & conducts

chemistry (12 decks)

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