Active series of metal

practical of Active Series Metal performs in Corrosion Lab In PU, CEET

1. Background
Active Series:
The activity series of metals is an empirical tool used to predict products in
displacement reactions and reactivity of metals with water and acids in replacement
reactions and ore extraction. It can be used to predict the products in similar reactions
involving a different metal.
The relative reactivity of metals can be used to organize them into an activity series.
Once organized, an activity series helps us to predict if a reaction will occur when a
piece of elemental metal is placed in water, an acid solution, or a solution containing the
ion of another metal. Activity series are generally listed in order of decreasing reactivity.
This means that in a metal activity series we would find the most reactive metals at the
top.
 Only a few of the most reactive metals are able to displace hydrogen from water
while a larger number will displace H
+
from an acid.
 The least reactive metals are not able to displace hydrogen from either of these
and are therefore found at the bottom of the series.
 Organizing the metals in this fashion also allows us to predict how the metals will
react with each other. In a solution or compound, an elemental metal will displace
any metal lower than it on the activity series.

An Example Activity Series
From the activity series, we can predict that Metal (aluminum) will not displace H from
water. However, it will displace H
+
from an acid by the following single displacement
reaction.


2 Al(s) + 6 HCl(aq) 3 H2(g) + 2 AlCl3(aq) (molecular equation)
2 Al(s) + 6 H
+
(aq) 3 H2(g) + 2 Al
+3
(aq) (net ionic equation)

From the activity series, we can predict that Metal (Sodium) will displace H from water.
2Na(S) + 2H2O (L) 2NaOH (aq) + H2 (g)

2. Significance and usage of reactivity series of metals:
 By using the reactivity series of metals, one can predict the products of
displacement reaction. Each element in the reactivity series can be replaced from
a compound by any of the elements above it. For example, magnesium metal
can displace zinc ions in a solution.

Mg(s) + Zn
2+
→→ Zn(s) + Mg
2+

 The interval between metals in the reactivity series of metals represents the
reactivity of those metals towards each other. If the interval between elements is
larger, they will react more vigorously. The topmost five elements, form lithium to
sodium are known as very active metals; hence they react with cold water to
produce the hydroxide and hydrogen gas. For example, sodium forms sodium
hydroxide and hydrogen gas with cold water.


2Na + 2H2O →→ 2NaOH + H2
 From magnesium to chromium, elements are considered as active metals and
they will react with very hot water or steam and form the oxide and hydrogen gas.
For example, aluminum reacts with steam to form aluminum oxide and hydrogen
gas.


2Al + 3H2O →→ Al2O3 + 3H2

 From iron to lead, metals can replace hydrogen from various acids like
hydrochloric acid, dilute sulfuric and nitric acids. Oxides of these metals undergo
reduction when heated with hydrogen gas, carbon, or carbon monoxide. Till
copper, metals can combine directly with oxygen and form a metal oxide.
Elements present at the bottom from mercury to gold are often found in the
native form in nature and their oxides show thermal decomposition under mild
conditions.

3. Reactivity of Metal Chart


 Silver, gold, and platinum are metals with the least reactivity. They are found in
nature.
 A metal with high reactive series in the above table also indicates that reverse
reaction is a bit tough process.
 Reactions are mostly Exothermic in case of highly reactive metals.
 The reaction takes place fast in highly reactive metals.
 Metals which are present above the carbon are extracted using electrolysis
method.

4.  Carbon and hydrogen plays and plays vital role in terms of a method that
involves metal extraction.
Objective:
Develop an activity series based on their own lab observations will use it to predict and
explain single replacement reactions and oxidation-reduction.

Principal:
Reactive metal displace the less reactive metal from the solution.

Chemistry of Analysis:
Active metal is a good reducing agent, it easily oxides the noble metal.

Chemical Required:
 Copper Sulphate (CuSO4)
 Iron Sulphate (FeSO4)
 Aluminum Sulphate (Al2(SO4))
 Silver Sulphate (AgNO3)
 Magnesium Sulphate (MgSO4)
 Lead Sulphate (PbSO4)


Material Required
 Iron Strip
 Copper Strip
 Lead Strip
 Silver strip
 Magnesium Strip
 Nickel Strip
 Zinc Strip
 Tin Strip
 Test tube

5.  Test tube stand
 Tongs
 Grinding paper

Procedure:
1. Take metal strip and clean it with the help of grinding paper.
2. Then put it in the test tube in a particular solution.
3. Check will it react or not with the help of series.
4. Change the metal strip and then put it in the test in a particular solution.

Observation:
Observe the
 Bubbles gas produced
 Temperature
 Precipitate form (new solid appears)
 Solid Disintegrates (is “eaten” away as opposed to dissolved)
 Color change
 Odor produced
 Light emitted

Metal Solution Reaction Activity





Zn
Al2SO4 Zn + Al2SO4 = No
reaction
No
Cu2SO4 2Zn + Cu2SO4
=2Cu + Zn2SO4
Black Layer
ZnSO4 Zn + ZnSO4 = No
reaction
NO
NiSO4 Zn + NiSO4 = Ni +
ZnSO4
Fumes, Bubbles,
Color Change
PbSO4 Zn + PbSO4 = Pb
+ ZnSO4
Bubbles, Gas
Evolved
Fe2SO4 Zn + Fe2SO4 = No
reaction
NO

6. Metal Solution Reaction Activity






Cu
Al2SO4 2Cu + Al2SO4 =
No reaction
No
Cu2SO4 Cu + Cu2SO4 = No
reaction
No
ZnSO4 Cu + ZnSO4 = No
reaction
No
NiSO4 Cu + NiSO4 = No
reaction
No
PbSO4 Cu + PbSO4 = No
reaction
No
Fe2SO4 Cu + Fe2SO4 = No
reaction
No




Metal Solution Reaction Activity






Ni
Al2SO4

2Ni + Al2SO4 = No
reaction
No
Cu2SO4

2Ni + Cu2SO4 =
Ni2SO4 + 2Cu
Fumes, Color
change
ZnSO4

Ni + ZnSO4 = No
reaction
No
NiSO4

Ni + NiSO4 = No
reaction
No
PbSO4

Ni + PbSO4 =
NiSO4 + Pb
Bubble,
Exothermic
Fe2SO4

2Cu + Fe2SO4 =
Cu2SO4 + 2Fe
Exothermic

7. Metal Solution Reaction Activity






Al
Al2SO4

2Al + Al2SO4 = No
reaction
No
Cu2SO4

2Al + Cu2SO4 =
Al2SO4 + 2Cu
Reddish Brown,
Fumes
ZnSO4

Al + ZnSO4 = No
reaction
No
NiSO4

Al + NiSO4 =
AlSO4 + Ni
Bubbles
PbSO4

Al + PbSO4 = No
reaction
No
Fe2SO4

2Al + Fe2SO4 = No
reaction
No



Metal Solution Reaction Activity






Fe
Al2SO4

2Fe+ Al2SO4 = No
reaction
No
Cu2SO4

2Fe + Cu2SO4 =
Fe2SO4 + 2Cu
Brick Red layer
ZnSO4

Fe + ZnSO4 = No
reaction
No
NiSO4

2Fe + NiSO4 =
Fe2SO4 + Ni
Fumes
PbSO4

Fe + PbSO4 = Pb
+ FeSO4
Bubbles, exo,
ppt., Dark color
Fe2SO4

2Al + Fe2SO4 = No
reaction
No

8. Metal Solution Reaction Activity





Sn
Al2SO4

2Sn+ Al2SO4 = No
reaction
No
Cu2SO4

2Sn + Cu2SO4 =
Sn2SO4 + 2Cu
Bubbles, Fumes
ZnSO4

Sn + ZnSO4 = No
reaction
No
NiSO4

2Sn + NiSO4 =
Sn2SO4 + Ni
Bubbles,
exothermic
PbSO4

Sn+ PbSO4 = Pb +
SnSO4
Bubbles
Fe2SO4

2Sn + Fe2SO4 =
No reaction
No


Metal Solution Reaction Activity





Pb
Al2SO4

Pb + Al2SO4 = No
reaction
No
Cu2SO4

Pb + Cu2SO4 =
PbSO4 + 2Cu
Reddish brown
layer
ZnSO4

Pb + ZnSO4 = No
reaction
No
NiSO4

Pb + NiSO4 = No
reaction
No
PbSO4

Pb + PbSO4 = No
reaction
No
Fe2SO4

Pb + Fe2SO4 = No
reaction
No