Transcript The Activity Series Text Reference: 3.3 (pg. 125 - 128) We have looked at several reactions: Fe + CuSO4  Cu +

The Activity Series
Text Reference: 3.3 (pg. 125 - 128)
We have looked at several reactions:
Fe + CuSO4  Cu + Fe2(SO4)3
Li + H2O  LiOH + H2
No, Ni is
Yes,
Li is
Such experiments reveal trends.
The
activity
below
Na
above
series ranks the relative reactivity
of Zn
metals.
It allows us to predict if certain chemicals will
Al is when
undergo single displacement Yes,
reactions
above
mixed: metals near the top are
mostCu
reactive
and will displacing metals near the bottom.
Q: Which of these will react? Yes, Fe is
Fe + CuSO4  Cu + Fe2above
(SO4)3Cu
Ni + NaCl
 NR (no reaction)
Li + ZnCO3  Zn + Li2CO3
Al + CuCl2  Cu + AlCl3
K
Na
Li
Ca
Mg
Al
Zn
Fe
Ni
Sn
Pb
H
Cu
Hg
Ag
Au
H is the only nonmetal listed. H2 may
cold
be displaced from acids or can be
given off when a metal reacts with
H 2O
H2O (producing H2 + metal hydroxide).
The reaction with H2O depends on hot H O
2
metal reactivity & water temp.
Q: will Mg react with H2O?
steam
A: No for cold, yes if it is hot/steam
Mg + H2O  H2 + Mg(OH)2 acid
Q: Zn + HCl  H2 + ZnCl2
Complete these reactions:
Al + H2O(steam)  H2 + Al(OH)3
Cu + H2O  NR
Ca + H2SO4  H2 + CaSO4
Na + H2O  H2 + NaOH
K
Na
Li
Ca
Mg
Al
Zn
Fe
Ni
Sn
Pb
H
Cu
Hg
Ag
Au
Other Activity Series Information
• All metals will have a specific place in the
activity series. For simplicity, only the most
common metals are shown.
• The metals near the top of the activity series
are more reactive because their valence
electrons are more easily removed.
• On tests and exams the activity series may
appear as K, Na, … Ag, Au; you must
remember that K is reactive, Au is not.
• If the valence of a metal is not indicated in
the question, use its most common valence
(in bold on your periodic table) to determine
the correct chemical formula.
Activity series lab
1. On the next slide, place a check in the corner of
boxes where you think reactions will take place.
2. Get a plastic spot plate.
3. Combine chemicals specified in the chart.
Figure out a way to keep track of the chemicals.
Use a ¼ scoop for solids (the less, the better).
Use 1 squeeze of an eyedropper for solutions.
4. Write chemical equations for chemicals that
reacted. Write NR where there was no reaction.
5. Dump used chemicals into the large funnel at
the front of the room (use a squirt bottle to rinse
remaining chemicals into the funnel). Wash the
spot plate and glass rod very well. Dry & return.
Mg
Cu
Zn
AgNO3



Mg + AgNO3 Cu + AgNO3 Zn + AgNO3



Ag+ Mg(NO3)2 Ag+ Cu(NO3)2 Ag+ Zn(NO3)2
H2SO4 Fe(NO3)3 CuCl2

Mg + H2SO4

H2 + MgSO4

Zn + H2SO4
NR

Mg+ Fe(NO3)3

Fe+ Mg(NO3)2
Mg + CuCl2 

Cu + MgCl2
NR
NR

H2 + ZnSO4

Zn+ Fe(NO3)3

Fe+ Zn(NO3)2
Zn + CuCl2 

Cu + ZnCl2
Oxides
The formation
Oxides form via the
and behavior of
addition of oxygen:
oxides can also
K + O2  K2O
be predicted via
the activity series. Oxides plus H2 (with
heat) will change to
Complete these
metal and H2O:
reactions:
heat
Ca + O2  CaO NiO + H2  Ni + H2O
Au + O2  NR
Oxides decompose
with heat:
heat
Fe2O3+ H2 
heat
HgO

Hg
+
O
2
Fe + H2O
K
Na
Li
Ca
Mg
Al
Zn
Fe
Ni
Sn
Pb
H
Cu
Hg
Ag
Au