Reactants
Products
SOLID ALUMINUM
HYDROCHLORIC ACID
solution
ALUMINUM CHLORIDE
solution
HYDROGEN GAS
2 Al (s)
6 HCl (aq)
2 AlCl3 (aq)
3 H2(g)
ions
ions
molecules
What kind of particles?
Atoms
H+ ion
# protons in each _13___
# electrons in each _13__
net charge __0__
Arrangement
Atoms held in fixed
positions - solid
Attractions
Metallic bonds –
loose free moving
sea of electrons
shared by all the
atoms
_1_ protons
_0_electrons
_+1_ net chg
Cl- ion
_17_ protons
18_electrons
_-1_ net chg
Al3+ ion
Cl- ion
H atom
H atom
_13_ protons
_17_ protons
_1_ protons
_1_ protons
10_electrons
18_electrons
_1_electrons
_1_electrons
_+3_ net chg
_-1_ net chg
_0_ net chg
_0_ net chg
Ions dissociated in solution
(split up) – free to move
and surrounded by water
molecules
Ions dissociated in
solution (split up) – free
to move and surrounded
by water molecules
Hydrogen molecules are widely
spaced and free to move in the
gas
Ion-dipole attractions –
the positive hydrogen ions
are attracted to negative
end of the water molecules
and the negative chloride
ions are attracted to the
positive hydrogen end of
water molecules
Ion-dipole attractions –
the positive aluminum
ions are attracted to
negative end of the water
molecules and the
negative chloride ions
are attracted to the
positive hydrogen end of
water molecules
Nonpolar covalent bonds hold the
hydrogen atoms together in the
hydrogen molecules.
These nonpolar molecules have no
oppositely charged ends so they are
not attracted to each other and stay
far apart. Weak induced dipoleinduced dipole attractions act
between the hydrogen molecules.
total ionic equation
Al (s) + H+ (aq)
+ Cl- (aq)
Al3+ (aq) +
Cl- (aq)
+
H2 (g)
ANALYSIS OF THE REACTION OF ALUMINUM IN HYDROCHLORIC ACID
THE CHANGES
ALUMINUM
ALUMINUM before
What kind of particle?
ALUMINUM after
What kind of particle?
atoms
ions
How many protons?
13
How many protons?
How many electrons?
13
How many electrons? 10
net charge?
half reaction
0
net charge?
13
+3
Al (s)  Al (aq) + 3e3+
NotesWhat happened to the aluminum?
Aluminum lost three
electrons – went from
atom to ion
Chemistry term for this change
Oxidation
Al was oxidized
CHLORINE
CHLORINE before
What kind of particle?
CHLORINE after
What kind of particle?
ions
ions
NotesWhat happened to the chlorine?
NOTHING
How many protons?
17
How many protons?
How many electrons?
18
How many electrons? 18
net charge?
-1
net charge?
17
-1
Cl- ion attracted to water molecules before and after
Chemistry term for this change
spectator ion
HYDROGEN IONS
HYDROGEN before
What kind of particle?
HYDROGEN after
What kind of particle?
ions
atoms in molecules
1
How many electrons? 0
net charge?
+1
How many protons?
How many protons?
half reaction
1
How many electrons? 1
net charge?
0
2H+ (aq) + 2e-  H2 (g)
NotesWhat happened to the hydrogen?
gained electrons
reduced
Chemistry term for this change
reduced
SINGLE REPLACEMENT REACTIONS.
element + compound
 compound + element
Metal + Metal – Nonmetal
M + MNm

Metal + Metal–Nonmetal
M + MNm
Metal replaces metal (or positive ion)
Nonmetal + Metal – Nonmetal
Nm + M Nm
 Metal – Nonmetal + Nonmetal
MNm + Nm
Nonmetal replaces Nonmetal (or negative ion)
The single (element) doing the replacing must be
more active than the one it is replacing
From the lab Mg (s) + 2 HCl (aq)  MgCl2(aq) + H2(g)
The Mg was more active than the H so it replaced
Zn (s) + 2 HCl (aq)  ZnCl2(aq) + H2(g)
The Zn was more active than the H so it replaced
2 Al (s) + 6 HCl (aq)  2 AlCl3(aq) + 3 H2(g)
The Al was more active than the H so it replaced
Cu (s) + HCl (aq)  does not react!!!!!!
The Cu did not replace the H so it must be less active
An example of a Nonmetal replacing Nonmetal
Cl2(g) + NaI (aq)  I2(g) + NaCl (aq)