reactivity series Flashcards
the order of reactivity of metals can be determined by
their reactions with water and acid
most reactive metals react with water and form
metal hydroxide and hydrogen
metals just below calcium,
react very slowly with water
what metals don’t react at all with water (3)
copper, silver and gold
balanced symbol equation for potassium reacting with water
2K (s) + 2H₂O (l) —— 2KOH (aq) + H₂ (g)
balanced symbol equation for sodium reacting with water
2Na (s) + 2H₂0 (L) -> 2NaOH (ag) + H₂ (g)
balanced symbol equation for lithium when reacting with water
2Li(s) + 2H₂0 (L) ->2LiOH (aq) + H₂ (g)
balanced symbol equation for calcium when reacting with water
Ca (s) + 2H₂0 (L) -> Ca(OH)₂ (aq) + H₂ (g)
order of the reactivity of metals (11)
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Copper
Silver
Gold
people say little children make a zebra, i constantly sniff giraffes
reactions becomes ____ vigorous as you go down the reactivity series
less
only metals above ___ will react with acid
iron ( including iron)
metals react with an acid to form
a salt and hydrogen
MASH = metal + acid —> salt. + hydrogen
symbol of sulfuric acid
H₂SO₄
Symbol of hydrochloric acid
HCl
equation of reaction of magnesium and sulfuric acid
Mg (s) + H₂SO₄ (aq) → MgSO4 (aq) + H₂ (g)
equation of reaction of zinc and sulfuric acid
Zn (s) + H₂SO₄ (aq) → ZnSO4 (aq) + H₂ (g)
equation of reaction of iron and sulfuric acid
Fe (s) + H₂SO₄ (aq) → FeSO4 (aq) + H₂ (g)
equation of reaction of magnesium and hydrochloric acid
Mg (s) + 2HCl (aq) → MgCl₂ (aq) + H₂ (g)
equation of reaction of zinc and hydrochloric acid
Zn (s) + 2HCl (aq) → ZnCl₂(aq) + H₂ (g)
equation of reaction of iron and hydrochloric acid
Fe (s) + 2HCl (aq) → FeCl₂ (aq) + H₂ (g)
what actually/physically happens when a metal reacts with an acid
the metal will disappear, and there will be effervescence as bubbles of hydrogen gas are produced
in the physical reaction, the more reactive the metal (acid reaction), then the
quicker the metal will disappear and the more vigorous the effervescence
a displacement reaction is when
a more reactive element displaces a less reactive element from its compound
in a displacement reaction, what is the reducing agent
the element that displaces
in a displacement reaction, what is the reduced
the element that gets displaced
can a displacement reaction happen in a solution
yes
in a displacement reaction, if a reactant is a solid then it will
disappear
if a product is a solid in a displacement reaction, it will
form
if a product and reactant are aqueous in a displacement reaction, what do you observe
if there is a colour change
displacement reactions happen between (2)
a more reactive metal and the oxide of a less reactive metal
OR
a more reactive metal and a solution of a salt of a less reactive metal
corrosion on the surface of metals happens when
they are exposed to the environment for long periods of time
rusting is a specific type of corrosion which happens when
Iron reacts with water and oxygen
what does the rusting of iron form ( equation)
Iron + water+ oxygen —> hydrated iron (III) oxide
what is the prdouct of rusting or iron
rust, or hydrated iron (III) oxide
are both water and oxygen needed for iron to rust
yes
coating the surface of iron with a barrier does what
prevents water and oxygen from coming into contact with the iron so that rusting doesn’t happen
what are the most common barriers ( 3) for iron
- painting
- greasing or oiling
- coating with plastic
barrier only works if
the iron is completely covered
oxidation is
the loss of electrons ( OIL RIG)
Reduction is
the gain of electrons ( OIL RIG)
WHAT IS SACRIFICIAL PROTECTION
when ( usually zinc) a more reactive metal is attached to a less reactive metal (iron) and so the more reactive metal will be oxidised instead of iron
what is galvanising
when a layer of zinc is put around the iron in order to protect it from rusting
if the zinc coating in galvanising is scratched then what happens
there will be sacrificial protection, so the zinc is the one That will lose electrons and so react and become oxidised instead of the iron
3 main methods of protection for iron against rusting
- Barrier
- sacrificial protection
- galvanising
rusting is a oxidation or reduction reaction
oxidation
an oxidising agent is
a substance that oxidises another substance and becomes reduced in the process
what is a reducing agent
a substance that causes another substance to be reduced
PRACTICAL - Investigate Metals reacting with acids
- wear safety goggles
- add some dilute hydrochloric acid to a small measuring cylinder to 3 test tubes
- to first tube add magnesium ribbon and note down what you see
- then use a lighted splint to see if any gasses were given off
- add iron filings to second test tube and do the same
- add zinc turnings to third and do same
- repeat the experiment with sulfuric acid
