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Chapter 8 Notes Packet
Reactions and Aqueous Solutions
8.1
Predicting Whether a Reaction Will Occur
What are the forces that tend to make reactions go in the direction of the arrow or
towards products?
1.
2.
3.
4.
8.2
Reactions in Which a Solid Forms
Precipitation Reaction –
Soluble Solid–
Insoluble Solid –
Slightly Soluble Solid –
Strong Electrolyte –
Weak Electrolyte –
When working with aqueous solutions, it is helpful to understand a few concerning
which substances are soluble in water and which will form precipitates. The more
common solubility rules are listed below:
1. All common salts of ____________ metals and the ammonium_________ ion
are soluble.
2. All common acetates _________and nitrates _________are soluble
3. All binary (two element) compounds of halogens (other than F) with metals
are soluble, except those of silver, mercury I, and lead.
4. All sulfates ________are soluble except those of barium, strontium, lead,
calcium, silver, and mercury I.
5. Except for those in Rule #1, carbonates_________, hydroxides______,
oxides_______, and phosphates _______are insoluble.
Decide if the following compounds are soluble (S) or insoluble (I) in water.
1. NaOH
5. AgCl
2. KCl
6. ( NH4)2O
3. NaNO3
7. K3(PO4)
4. BaCO3
8. MgO
Predict what will happen when the following solutions are mixed. Write the balanced
equation for any reaction that occurs. Make sure you label the product that will
precipitate and the product that will be dissolved in water.
1. Ba(NO3)2(aq)
+
K3PO4(aq)

2. Pb(NO3)2(aq)
+
KI(aq)

3. (NH4)2S(aq)
+
CoCl2(aq)

4. CaCl2(aq)
+
K2CO3(aq)

5. Na3PO4(aq)
+
CrCl3(aq)

8.3
Describing Reactions in Aqueous Solutions
NaCl(aq)
+

AgNO3(aq)
AgCl(s) +
NaNO3(aq)
Molecular Equation –
Complete Ionic Equation –
Spectator Ions –
Net Ionic Equation –
Write net ionic equations for the following chemical reactions
Example
Molecularequation: Pb(NO3)2
+
2 NaI

PbI2
+
2 NaNO3
Ionic equation: Pb2+(aq) + 2 NO3-(aq) + 2 Na+(aq) + 2I-(aq)  PbI2(s) + 2 Na+(aq) + 2
NO3-(aq)
Net ionic equation: Pb2+(aq) + 2I-(aq)  PbI2(s)
1. 2 NaF(aq)
+ Ca(OH)2(aq) 
2. 2 HNO3(aq)
3. Pb(NO3)2(aq)
+ Mg(OH)2(s) 
+ Na2SO4(aq) 
CaF2(aq)
+ 2 NaOH(aq)
2 H2O(l) + Mg(NO3)2(aq)
PbSO4(s) + 2 NaNO3(aq)
4. Na2CO3(aq)
5. KCl(aq)
8.4

+ 2 HCl(aq)
+ AgNO3(aq)

2 NaCl(aq)
KNO3(aq)
+ H2O(l)
+
+ CO2(g)
AgCl(s)
Reactions That Form Water: Acids and Bases
Acid –
Base –
Strong Acid –
Strong Base –
Salt –
What happens when acids and bases react together?
In a typical acid-base reaction, the products are generally a ________________ and
________________.
Look at the example of an acid-base reaction below.
HCl
+
NaOH

For the reactants, HCl and NaOH, to recombine and form products, they must first come
apart and form ions. What ions do they form?
Once these compounds have formed ions, recombinations can occur. The positive ions of
one compound attract the negative ions of the other compound. What products are
formed? Label the salt.
This is a neutralization reaction.
Predict the products, balance the equations and label the acid, base, salt and water in the
equation.
1. H2SO4
+
KOH 
2. Mg(OH)2
+
H3PO4 
3. HF
+
Ca(OH)2

4. LiOH
+
HNO3

5. Carbonic Acid
+
Barium Hydroxide
8.5

- 8.7 Ways to Classify Reactions
Acid-Base Reaction (Neutralization Reaction) –
Double Displacement or Double Replacement (Precipitation Reactions) –
Single Replacement Reactions -
Combustion Reactions –
Synthesis (Combination) Reactions –
Decomposition Reactions –
Classify the reactions below as synthesis, decomposition, single replacement, double
replacement, combustion or neutralization. Balance the chemical equation.
1.
Fe
+
H2SO4

Fe3(SO4)2
+
H2
2.
HClO4 +
RbOH

RbClO4
+
H2O
3.
K2SO4 +
CaCl2

KCl
+
CaSO4
4.
Ni
+
Cl2

NiCl2
5.
H2O

H2
6.
CH4
+
O2
+
H2O
+
O2

CO2
Identify the type of reaction, predict the products and balance the chemical equation for
the following reactions.
1. Al +
Cl2

2. BaCl2
+
Na2SO4

3. KOH
+
HCl

4. PbO2

5. C3H8
+
6. K
MgCl2
+
O2


Write correct chemical formulas, balance the atoms and label the reactions as one of four
types.
1. Silver nitrate + potassium chloride 
2. Iron (III) chloride 
3. Chlorine + lithium iodide 
ACTIVITY SERIES OF THE ELEMENTS
The ability of an element to react is referred to as the _______________ of the element.
The more readily an element reacts with other substances, the _______________ its
activity. An _______________ _______________ is a list of elements organized
according to the ease with which they undergo certain chemical reactions. The
__________ active element at the top of the series can replace every element below it.
A metal will replace another metal in a compound if it is _______________ on the
activity list.
Activity Series of the elements
Li
Rb
Can react with cold H2O and acids replacing Hydrogen
K
Ba
Sr
Ca
Na___________________________________________________________
Mg
Al
Mn
Can react with steam and acids, replacing Hydrogen
Zn
Cr
Fe
Cd___________________________________________________________
Co
Ni
Can react with acids, replacing Hydrogen
Sn
Pb
H2
Sb
React with oxygen, forming oxides
Bi
Cu
Hg___________________________________________________________
Ag
Pt
Fairly unreactive
Au___________________________________________________________
Demonstration
Will the following reaction take place?
What is the balanced chemical equation?
What type of reaction is this?
Based on the activity series, will this reaction occur?
Record your observations in the space provided below.
Predict whether or not each of the following reactions will occur. If the reactions occur,
predict the products and balance the chemical equations.
+
CuCl2 
2. Zn +
Pb(NO3)2

3. Cu +
FeSO4

1. K