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Chem > Reactivity Series > Flashcards

Reactivity Series Flashcards

ELEMENT // COMPOUND COLOUR IS DIFFERENT!!!

1
Q

H+ in reactivity series represent

A

acid

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2
Q

which 4 Reactivity Series metals react w/ water? + eqn

A

Potassium, Sodium, Calcium, Magnesium
metal + H2o -> metal hydroxide + H2

i.e. 2K(s) + 2H2o(l) -> 2KOH(aq) + H2(g)

https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 14

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3
Q

which reactivity series metals react w/ steam + eqn

A

Magnesium, Aluminium, Zinc… Iron
metal + steam -> metal oxide + H2

Potassium, Sodium, Calcium
can react, 2 dangerous

i.e. Zn(s) + H2o(g) -> ZnO(s) + H2(g)

https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 14

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4
Q

define displacement in metals

A

more reactive metal
displaces less reactive metal from
salt soln

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5
Q

displacement experiement setup

A

https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 13

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6
Q

why aluminium removed from reactivity series?

A

has protective layer (AlO)
- will not show reactivity immediately

even tho it is high up enf in reactivity series such dat it will react w/ acid

it has protective layer

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7
Q

why aluminium used, food wrapper?

A

has protective layer (AlO)
- will not rust

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8
Q

how cause aluminium react?

A
  1. scrape, sandpaper
  2. Place into acid, long time

  1. AlO -> amphotheric, will react w/ acid, long period time

https://docs.google.com/document/d/1Ep_FO9CxYSFbxmf3Zqg9mgm9NNyt2enpfMDr49gufrU/edit?tab=t.0 page 15

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9
Q

G1 metals/K, Na, Ca displacement why dont use/why bubbling?

A
  1. Soln G1 metal placed in, (aq)
  2. Sodium react w/ water violently, high reactivity
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10
Q

experiments, determine order, reactivity, metals

A
  1. thermal decomposition, carbonate
  2. displacement
  3. reduction w/ (Carbon, H2 gas)
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11
Q

thermal decomposition

which metal easier decompose?

A

Less reactive metal, easier metal carbonate decompose

sulfate, nitrate, carbonate also decompose
not only carbonate

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12
Q

Why Potassium, Sodium, G1 metals formed compounds nvr thermally decompose

A

no reaction
1. K, Na vry reactive
2. (other anion) thermally stable
3. G1 metals dont thermally decompose

  1. K, Na bonds super strong coz vry reactive.
  2. It desperately clings onto other anion
  3. ionic bonds dosent end up breaking and thermally decomposing

sulfate, nitrate, carbonate also decompose
not only carbonate

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13
Q
  1. CaO (s) + C(s) ->
  2. 2CuO (s) + C (s) ->
A
  1. reduction by carbon reaction does not happen, C less reactive, Ca
  2. reduction happens (Co2 (g) + 2Cu (s)), C more reactive, Cu

works the same way, displacement does.
C (s) is always the displacer.

**eqn: ** metal oxide + carbon -> co2 + 2cu(s)

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14
Q
  1. CaO (s) + H2 (g) ->
  2. CuO + H2 (g) ->
A
  1. reduction by hydrogen gas does not happen, H2 less reactive, Ca
  2. reduction happens (H2o (g) + 2Cu (s)), H2 more reactive, Cu

works the same way, displacement does.
H2 (g) is always the displacer.

**eqn: ** metal oxide + h2 -> h2o(l) + metal

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15
Q

does silver carbonate decompose?

A

yez
1. decompose, silver oxide Ag2O + co2

  1. 2Ag2o unstable, decompose further -> 4Ag + o2
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16
Q

.

reactivity series
list out all metals that thermally decompose

form what products?

A
  1. sodium
  2. calcium
  3. magnesium
  4. aluminium
  5. zinc
  6. iron
  7. tin
  8. lead
  9. hydrogen
  10. copper

carbonate decomposes, form metal oxide + co2

metal carbonate -> metal oxide + carbon dioxide

17
Q

top 4 reactive metals in reactivity series…
1. desc how react in water

A

Potassium: explosive, (giving out bright flame)
Sodium: fast
Calcium: readily
Magnesium: slow

18
Q

how determine state symbols if not given

A
  1. look for struct
  2. i.e. SMS = low mp, bp, (g)
  3. i.e. GILS = high mp, bp (s)
19
Q

metal coating
vs
sacrificial protection

advantage, disadvantage

A

metal coating:
nicer finish (aesthetics)
small hole for h2o, o2 enter, ineffective

sacrificial protection:
no need coat entire surface, need replace metal once in a while

20
Q

uses of stainless steel, mild steel, aluminium

A

stainless: surgical instruments/ stainless steel cutlery
mild: car bodies/machinery
aluminium: soft drink cans

21
Q

what does acid rain do?

A

acid rain
1. corrode limestone struct, metal
2. kill aquatic life (acidic rivers)

22
Q

does industry commonly use pure metal? if not wat use?

A

no
use alloy

23
Q

all reaction of metal (s4, not metal + acid or those obv stuff)

A
  • metal + cold/rtp water
  • metal + steam
  • reduction, metal oxide, H2 gas
  • reduction, metal oxide, C
  • displacement, metal, salt soln.
  • thermal decomposition metal carbonates/compounds
24
Q

iron react w/ steam eqn is…? (unique pt)

A

reversible
3Fe (s) + 4h2o (g) -> Fe3O4 + H2 (g)

oxide has to be based on charge of ion bonding w it

25
Q

reduction, metal, C eqn

A

metal oxide + carbon -> Co2 (g) + metal

metal BELOW C reduce

For extraction of pure metal

Metal is reduced.

26
Q

reduction, metal, H2 eqn

A

metal oxide + H2 (g) -> metal + water vapour

metal BELOW H+ reduce

For extraction of pure metal

Metal is reduced.

27
Q

Y reactive metal greater tendency displace less reactive metal

A
  1. more reactive metal, greater tendency lose electrons
  2. than less reactive metal
  3. forming cations
28
Q

explain sacrificial protection

A
  1. more reactive metal attach less reactive metal
  2. more reactive metal oxidise, corrode first
  3. e.g. zinc bars on hull on steel ships
  4. replace regularly
  5. less exp, replace entire steel struct
29
Q

explain galvanising

A

coating less reactive metal w/ zinc
type of sacrificial protection
coating dmg -> still sacrificial protection

30
Q

explain use alloys prevent rusting method

A

contain Nickel, Chromium, rust-resistant alloys i.e. stainless steel

Ni, Cr prevent rusting

31
Q

use protective layer prevent rust

A
  1. apply coat, paint
  2. oil: machinery parts
  3. metal coating: food cans
  4. plastic coating: kitchenware
32
Q

what happens, rusting/corrosion of iron

A

slow oxidation + exposed 2 water, oxygen in air,
iron, form hydrated iron(III) oxide (rust)

33
Q

define rust

A

flaky red-brown substance

34
Q

rusting of iron chem formula

A

4Fe + 3O2 + 2xH2o -> 2Fe2O3.xH2o (s)

iron + oxygen + water -> hydrated iron (III) oxide

35
Q

what increases rate of rusting

A

presence of sodium chloride

36
Q

which metals extracted by what method

A

electrolysis, molten ore: PSCMA

heating metal oxide w/ carbon // reduction w/ carbon: ZITLHCS

physical methods: GT

37
Q

ore

A

compounds, metals
mixed w/ earth, rocks

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