Honors Chemistry
Name: ____________________________________ Date: ___________________ Mods: _________
Ch. 4.4: Single Replacement Reactions & Oxidation-Reduction
A.
REDOX REACTIONS: AN OVERVIEW

All single replacement reactions can be classified as redox reactions (but not all redox reactions
are single replacement reactions)
o
In a single replacement reaction, one reactant is always an __________________ by itself
and the other reactant is typically an aqueous ionic compound (or an acid or water)

Redox reactions occur when __________________ are transferred between atoms, ions, or
molecules in a reaction

Oxidation (LEO) –
o

Example:
Li (s)
Reduction (GER) –
o
Example:
Au3+ (aq)
“LEO the lions says GER!!!!!!!!”
B.
WHAT IS AN ACTIVITY SERIES?

An activity series is a list of substances ranked in order of relative chemical _____________
(this is related to the ease with which the substance can be oxidized or reduced)

NOTE: There is one activity series for metals and a separate activity series for halogens

Reactivity Series of Metals:
o
Most metals are more likely to be oxidized (LEO) to become _________________ in single
replacement reactions

Active Metals: metals at the ____________ of the activity series are ___________
reactive and more easily oxidized (ex: Lithium, Potassium)

Noble Metals: metals at the _______________ of the activity series which have very
low reactivity and are more likely to be ____________________ in a redox reaction
and are thus ___________ likely to react in a single replacement reaction
o

these noble metals typically include Cu, Ag, Hg, Pt, Au (as well as a few
select others) and are resistant to ____________________ and oxidation in
moist air.
___________________ is the only nonmetal listed on the metal activity series.
This is significant because only metals which are MORE REACTIVE (higher) than
hydrogen react with _____________ and water to produce H2 (g).

Reactivity Series of Halogens:
o
C.
Nonmetal halogens are more likely to be reduced (GER) to become _______________ in
single replacement reactions

the halogens at the top of the series are ____________ reactive and are more
easily reduced (ex: Fluorine, F2)

the halogens at the bottom of the series are ______________ reactive and are
therefore __________ likely to react in single replacement reactions (ex: Iodine, I2)
HOW AND WHY WOULD I USE THE ACTIVITY SERIES?

Before predicting the products of a single replacement reaction, you must consult the activity
series to determine if the chemical reaction can even occur at all…
o In a single replacement reaction, you must look at the element which is by itself in the
reaction and compare its reactivity (position in the activity series) to the element it is trying
to replace within the ionic compound

If it is a metal solid (or H2), it will try to replace the metal cation (or hydrogen) in the
ionic compound

If it is a diatomic halogen, it will try to replace the nonmetal anion in the ionic
compound
o ***Looking at the respective activity series, the element that is by itself must be MORE
REACTIVE (______________ in the activity series) than the ion it is trying to replace in
order for the chemical reaction to occur!!!***

D.
If the element that is by itself is LESS REACTIVE (_____________ in the activity series)
than the ion it is trying to replace, then NO CHEMICAL REACTION can occur  NR
SINGLE REPLACEMENT REACTION EXAMPLES (USING THE ACTIVITY SERIES)

SR w/ metals:
1)
_____Mn (s) + _____Cr(C2H3O2)3 (aq) 
2)
_____KNO3 (aq) + _____Au (s) 
3)
_____H2O (l) + _____Ni (s) 

SR w/ halogens:
4)
_____NH4Br (aq) + _____I2 (s) 
5)
_____Cl2 (g) + _____KI (aq) 
Single Replacement Reactions WS
Directions:
Using the activity series of metals and the activity series of halogens, determine if the following
reactions will occur. If yes, write the balanced chemical equation; if no reaction can occur, write NR.
When specified, write the complete ionic equation (CIE) & net ionic equation (NIE). Remember
that only AQUEOUS reactants/products can be dissociated into their respective ions in the CIE & NIE.
* Note: When you have H2O (l), think of it as H+ and OH–
to help you better predict the reaction products!
1)
_____Zn (s) + _____Sn(NO3)2 (aq) 
2)
_____H2SO4 (aq) + _____Al (s) 
CIE:
NIE:
3)
_____Al (s) + _____ CuCl2 (aq) 
4)
_____Cr (s) + _____NiSO4 (aq) 
5)
_____Cu (s) + _____Al2(SO4)3 (aq) 
6)
_____H2O (l) + _____Na (s) 
7)
_____Pb(NO3)2 (aq) + _____Fe (s) 
8)
_____Cu (s) + _____HBr (aq) 
9)
_____Al (s) + _____Pb(NO3)2 (aq) 
10) _____CaI2 (aq) + _____F2 (g) 
CIE:
NIE:
11) _____H2 (g) + _____K2SO4 (aq) 
12) ____HCl (aq) + ____Pt (s) 
13) _____AgC2H3O2 (aq) + _____Fe (s) 
14) _____Sn (s) + _____HI (aq) 
15) _____Au(NO3)2 (aq) + _____Co (s) 
16) _____SrCl2 (aq) + _____I2 (s) 
17) _____Mg (s) + _____HNO3 (aq) 
18) _____Cu(C2H3O2)2 (aq) + _____H2 (g) 