the activity series and solubility rules -...
TRANSCRIPT
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The Activity Series
and
Solubility Rules
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We have looked at several single displacement reactions:
Fe(s) + CuSO4 (aq) Cu (s) + Fe2(SO4)3
Li + H2O LiOH + H2
The activity series ranks the relative reactivity of metals.
A metal does NOT always react with metal ions in
aqueous solutions.
The activity series allows us to predict if certain
chemicals will undergo single displacement reactions
when mixed
Metals near the top are most reactive and will
displacing metals near the bottom.
KNaLiCaMgAlZnFeNiSnPbH
CuHgAgAu
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Q: Which of these will react?
Fe + CuSO4
Ni + NaCl
Li + ZnCO3
Al + CuCl2
Cu + Fe2(SO4)3
Yes, Fe is
above Cu
NR (no reaction)
No, Ni is
below Na
Zn + Li2CO3
Cu + AlCl3
Yes, Al is
above Cu
KNaLiCaMgAlZnFeNiSnPbH
CuHgAgAu
Yes, Li is
above Zn
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Other Activity Series Information
All metals will have a specific place in theactivity series. For simplicity, only the mostcommon metals are shown.
The metals near the top of the activity seriesare more reactive because their valenceelectrons are more easily removed.
On tests and exams the activity series mayappear as K, Na, … Ag, Au; you mustremember that K is reactive, Au is not.
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Q: Does a reaction occur between Copper + Silver Nitrate
Cu + AgNO3 Ag + Cu(NO3)2
Yes, Cu is
above Ag
KNaLiCaMgAlZnFeNiSnPbH
CuHgAgAu
Image: McGraw-Hill Ryerson Chemistry 12
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Activity series Practice
1. On the next slide, place a check in the corner of boxes where you think reactions will take place.
2. Write chemical equations for chemicals that react. Write NR where there was no reaction.
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Mg Cu Zn
Mg + AgNO3
Ag+ Mg(NO3)2
NR
NR
NR
Cu + AgNO3
Ag+ Cu(NO3)2
Zn + AgNO3
Ag+ Zn(NO3)2
AgN
O3
H2 S
O4
Fe(N
O3 )
3C
uC
l2
Mg + H2SO4
H2 + MgSO4
Zn + H2SO4
H2 + ZnSO4
Mg+ Fe(NO3)3
Fe+ Mg(NO3)2
Zn+ Fe(NO3)3
Fe+ Zn(NO3)2
Mg + CuCl2
Cu + MgCl2
Zn + CuCl2
Cu + ZnCl2
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Solubility Rules and Precipitation Reactions
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Precipitation Reactions
Precipitation reactions: are double displacement
reactions that produce a precipitate
Not all ionic compounds dissolve!
When a solid doesn’t dissolve it is called
insoluble. A solid that forms when two solutions
are mixed is called a precipitate.
Instead of doing experiments all the time to see
which ones will dissolve, we use The solubility
rules.
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Sodium chloride + Silver nitrate
Both reactants are soluble.
One product is soluble, the other one is
precipitate
Which product is a solid? Use the solubility
rules to find out the precipitate
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Solubility Rules
1) All nitrates (NO3-) are soluble.
2) All ammonium (NH4+) or alkali (Li+, Na+, K+, Rb+, Cs+, Fr+)
compounds are soluble.
3) All carbonates (CO32-), phosphates (PO4
3 -) and hydroxides
(OH-) are insoluble except with the cations in Rule #2.
4) All chlorides (Cl-), bromides (Br-), and iodides (I-), aresoluble except with Ag+, Pb2+, or Hg+.
5) All sulphates (SO42-) are soluble except with Ca2+, Sr2+, Ba2+,
Ra2+, Pb2+,
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Which of the following are soluble in water?
a. SrSO4
b. NaNO3
c. PbCl2
Not soluble
soluble
Not soluble
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Predict the products of the following reaction: (if no solid precipitate is formed, there is no reaction)
Pb(NO3)2(aq) + KI (aq)
Pb(NO3)2(aq) + 2KI (aq) PbI2(s) + 2KNO3 (aq)
We know it is a solidprecipitate because it is insoluble according tothe solubility rules.
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A picture of the reaction:
Because K+ and NO3- remain dissolved, they are called
spectator ions and are not included in the net ionicequation.
Net Ionic Equation
Pb2+ (aq) + 2I-(aq) PbI2(s)
Pb2+ NO3-
NO3-
K+ I-
NO3-
K+
PbI2(s)
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Sodium chloride + Silver nitrate Sodium nitrate + Silver chloride
NaCl (aq) + AgNO3 (aq) NaNO3 (?) +AgCl (?)
Using the solubility rules:
Nitrates are soluble
AgCl is insoluble
(White precipitate)
Identify the precipitate
Image: McGraw-Hill Ryerson Chemistry 12
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Net Ionic Equation
Write the balanced chemical and net ionic equation for:
Na2CO3(aq) + CaCl2(aq)
Step 1: Write the balanced chemical equation
Na2CO3(aq) + CaCl2(aq) CaCO3(s) + 2NaCl (aq)
Insoluble precipitate
Step 2: Remove the spectator ions (those that are soluble).
Ca2+(aq) + CO32-(aq) CaCO3(s)
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Image: McGraw-Hill Ryerson Chemistry 12
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Practice Questions:
1) Does the reaction occur?
2) Yes Predict the products & Write skeleton equations
Single Displacement: using reactivity series
Double Displacement: Use the solubility rules, state if the reaction will occur.
For D.D. Write chemical equations and net ionic
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potassium + water potassium hydroxide + hydrogen
gas
Skeleton equation:
K + H2O KOH + H2
single or double displacement?
Single Displacement Reaction
balanced equation:
__K + __H2O __KOH + __H2
2K + 2H2O 2KOH + H2
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zinc + tin(II)chloride zinc chloride + tin
Skeleton equation:
Zn + SnCl2 ZnCl2+ Sn
single or double displacement?
Single Displacement Reaction
__Zn + __SnCl2 __ZnCl2 + __Sn
Zn + SnCl2 ZnCl2 + Sn (balanced)
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Gold + water
No Reaction
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potassium iodide + lead(II) nitrate potassium nitrate +
lead(II) iodide
skeleton equation:
KI + Pb(NO3)2 K NO3 + PbI2single or double displacement?
Double Displacement Reaction
balanced equation:
__KI + __Pb(NO3)2 __KNO3 + __PbI2
2KI + Pb(NO3)2 2K NO3 + PbI2
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Copper + Aluminum Chloride
skeleton equation:
Cu+ AlCl3 NR
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HW: Predict the products and
write net ionic reactions
MgCl2+ NaOH
KI + NaNO3
Na2SO4 + Sr(OH)2