Chapter 6: Chemical Reactions
 Identify and predict single displacement
reactions.
The reactivity series is a series of
metals, in order of reactivity from highest
to lowest. It is used to determine the
products of single displacement reactions,
whereby metal A will replace another
metal B in a solution if A is higher in the
series. Activity series of some of the more
common metals, listed in descending
order of reactivity.
The reactivity of metals is due to the
difference in stability of their electron
configurations as atoms and as ions. As they
are all metals they will form positive ions
when they react.
Potassium has a single outer shell electron to
lose to obtain a stable "Noble gas" electron
configuration; the precious metals which exist
in
the d-block cannot form structures which are
much more stable than their elemental state
with the loss of just a few electrons. Metals
that require the loss of only one electron to
form stable ions are more reactive than
similar metals which require the loss of more
than one electron. Group 1 metals are the
most reactive for that reason.
Metals with a greater total number of
electrons tend to be more reactive as
their outermost electrons (the ones
which will be lost) exist further from
the positive nucleus and therefore
they are held less strongly.
 In a single-displacement reaction, one
element displaces another in a
compound.

Single displacement reactions follow this
general equation:
 A + BC  AC + B
 In single-displacement reactions, one
metal can replace hydrogen or another
metal.
 A metal will not always replace a metal
in a compound dissolved in water
because of differing reactivities.
 An activity series can be used to predict if
reactions will occur.
 Halogens frequently replace other
halogens in replacement reactions.
 Halogens also have different reactivities
and do not always replace each other.
 An activity series can be used to predict if
reactions will occur.
 Identify which two elements would be
likely to swap.
 Consult the activity series to see which
element is more reactive.
 If the free element is more reactive, it will
trade places with the element in the
compound.
 If the free element is less reactive, no reaction
will take place.

Predict whether the following single displacement
reactions will occur. If a reaction occurs, write a
balanced equation for the reaction.

K(s) +
ZnCl2(aq) 
HF(aq) 

Cl2(g) +

Fe(s) +
Na3PO4(aq) 

Al(s) +
Pb(NO3)2(aq) 
Metals
Metal Ion
Reactivity
K
Na
Li
Ba
Sr
Ca
Mg
Al
Mn
Zn
Cr
Fe
Cd
Co
Ni
Sn
Pb
H2
Sb
Bi
Cu
Hg
Ag
Au
Pt
K
Na+
Li+
Ba2+
Sr2+
Ca2+
Mg2+
Al3+
Mn2+
Zn2+
Cr2+
Fe2+
Cd2+
Co2+
Ni2+
Sn2+
Pb2+
H+
Sb2+
Bi2+
Cu2+
Hg2+
Ag+
Au3+
Pt+
reacts with water
reacts with water
reacts with water
reacts with water
reacts with water
reacts with water
reacts with acids
reacts with acids
reacts with acids
reacts with acids
reacts with acids
reacts with acids
reacts with acids
reacts with acids
reacts with acids
reacts with acids
reacts with acids
included for comparison
highly unreactive
highly unreactive
highly unreactive
highly unreactive
highly unreactive
highly unreactive
highly unreactive
+