Identifying Types of Chemical Reaction Balance the reactions and
Identifying Types of Chemical Reaction Balance the reactions and indicate which type of chemical reaction is being represented:
1. ____ NaBr + ____ Ca(OH)2 ___ CaBr2 + ____ NaOH
Reaction Type : ______________
2. ____ NH3+ ____ H2SO4 ____ (NH4)2SO4
Reaction Type : ______________
3. ____ C5H9O + ____ O2 ____ CO2 + ____ H2O
Reaction Type : ______________
4. ____ Pb + ____ H3PO4 ____ H2 + ____ Pb3(PO4)2
Reaction Type : ______________
5. ____ Li3N + ____ NH4NO3 ___ LiNO3 + ___ (NH4)3N
Reaction Type : ______________
6. ____ HBr + ___ Al(OH)3 ___ H2O + ___ AlBr3
Reaction Type : ______________
7.
Na3PO4 +
KOH
NaOH +
K3PO4
Reaction Type _______________________
8.
MgCl2 +
Li2CO3
9.
C6H12 +
O2
10.
Pb +
11.
CaCO3
12.
P4 +
MgCO3 +
CO2 +
FeSO4
O2
H2O
PbSO4 +
CaO +
P2O3
LiCl
CO2
Reaction Type _______________________
Reaction Type _______________________
Fe
Reaction Type _______________________
Reaction Type _______________________
Reaction Type _______________________
More About Types of Chemical Reactions Single Replacement Reactions Some Additional Information Types of Single Replacement Reactions Model 2 from homework shows 2 types 1)Replacement of a Metal in a Compound by a Meta l and 2)Replacement of Hydrogen by a Metal There is a 3rd type of Single Replacement Reaction Replacement of Halogens One halogen replaces another halogen in a compound For example: Cl2(g) + 2KBr(aq) 2KCl(aq) + Br2(l) Please write a general form equation for this type of single replacement reaction.
Activity Series and Single Replacement Reactions Not every metal can replace every other metal nor can every halogen replace every other halogen. We use an Activity Series to predict if a replacement reaction will occur.
The most active element, placed at the top in the series, can replace each of the elements below it from a compound in a single replacement reaction. Using the above activity series answer the following questions: Can zinc replace nickel? __________
Can copper replace lead? __________
Predicting Products of Chemical Reactions Follow the Patterns from Types of Chemical Reactions Each reaction that you work with will follow the patterns of the 5 types of chemical reactions Synthesis Decomposition Single Replacement Cation Anion Double Replacement Combustion
Steps to follow 1st Classify the reaction by looking at the reactants. What pattern do they match? 2nd Then write the products *If it is synthesis, write a compound that contains both reactants – remember to write true formulas. *If it is decomposition, then break it into two elements or compounds. *If it is single replacement, then replace the single element with the corresponding type of element in the compound give(cation for cation and anion for anion). Check the activity series – it is possible that the reaction will not go forward. Remember to write true formulas. *If it is double replacement, then the cation and anions switch places. Be careful when switching places. The rules require cation before anion and true formulas using charges. *If it is combustion the products are always water and carbon dioxide
With your group, look for additional patterns that will help you to predict the products. Additional information is in your book section 8-2
For all combustion reactions of hydrocarbons or hydrogen-carbon-oxygen molecules, the products will always be CO2 and H2O (assuming a complete reaction).
a. Combustion:
C6H12
+
9O2
6CO2
+
6H2O
b. Combustion:
2C4H6
+
11O2
8CO2
+
6H2O
c. Combustion:
C6H10O3
+
7O2
6CO2
+
5H2O
+
I2
MgI2
1. Synthesis:
Mg 2+
-
Note that Mg can only form Mg and I can only form I , so the product will must have a 1:2 cation:anion ratio.
2. Double displacement:
CuCl2
+
H2S
CuS
+
2HCl 2+
-
Note that the product is not H2Cl2. It is important to recognize that CuCl2 is made of three ions, Cu and two Cl .
3. Double displacement:
NaOH
+
HClO4
NaClO4 +
-
H2O
-
In this question, you must recognize that perchlorate, ClO4 , and hydroxide, OH , are polyatomic ions and will not break apart. Also, this is an acid-base reaction, so the products should be salt and water.
4. Decomposition:
ZnCO3
+
heat
ZnO
+
CO2
When reactions have heat as a reactant, it is very likely that they will involve decompositions. Carbonate compounds usually decompose to CO2 and a metal oxide.
5. Single replacement:
2HCl
+
Zn
ZnCl2
+
H2
Note that one reactant is in its elemental form; if a single replacement reaction is going to occur, the species NOT in its elemental + form in the reactants (H in this case), will end up in its elemental form in the products (H 2) and the species that IS in its elemental 2+ 2+ form (Zn) will end up ionized (Zn ). Note that zinc can only form a Zn ion, so it will have two chloride ions. Note also that hydrogen in its elemental form is H2, not H.
6. Single replacement
2Na
+
MgCl2
2NaCl
+
Mg 2+
Again notice that one species is in its elemental form (Na). The magnesium in MgCl 2 is an ion (Mg ), but is transformed into its + elemental state (Mg), while the Na is converted into an ion (Na , sodium only forms a +1 ion).
7. Double replacement
CaCl2
+
K2CO3
CaCO3
+
2KCl
2-
2+
+
Recognize that carbonate is a polyatomic ion (CO3 ) and that the cations are already stable ions (Ca and K ).
8. Synthesis
2K
+
Cl2
2KCl +
-
Note that both materials are elemental species, so the only result could be a synthesis reaction. In the product, K and Cl are formed. Note that we would NOT write the product as K2Cl2. Ionic compounds are written in their simplest forms.
9. Double replacement
3BaCl2 +
2K3PO4
Ba3(PO4)2
+
6KCl
3-
Note that phosphate (PO4 ) is a polyatomic ion and will not break apart. Since barium is a +2 ion, the barium phosphate will have a 3:2 ratio of Ba:PO4 in order to balance the charge.
10. Double replacement
H2SO4
+
2KOH
2H2O
+
2-
K2SO4 +
Notice that sulfate (SO4 ) is a polyatomic ion and that potassium exists as a +1 ion (K ). Also, this is an acid-base reaction, so the products should be salt and water.
11. Decomposition
Al2(CO3)3+
heat
Al2O3
+
3CO2 3+
Another decomposition that will generate CO2 and a metal oxide (note that Al forms a +3 ion, Al , and monatomic oxygen will have 2a –2 charge, O ).
12. Decomposition
Mg(OH)2 +
heat
MgO
+
H2O
Fe2O3
+
Hydroxides will often decompose with heat to yield water and an oxide. .
13. Decomposition
2Fe(OH)3
+
heat
3+
3H2O
Similar to the question above. Notice that the metal retains its ionic charge, it is Fe in both the reactants and products.
Single-Replacement Reactions Using the Activity Series Step 1 - Write the formulas of the reactants on the left of the yield sign Step 2 - Look at the Activity Series on page 266 or above to determine if the replacement can happen Step 3 - If the replacement can occur, complete the reaction and balance it. If the reaction cannot happen, write N.R. (no rxn) on the product side.
1. lead + zinc acetate
2. iron + aluminum oxide
3. silver nitrate + nickel
4. sodium bromide + iodine
5. aluminum bromide + chlorine
6. sodium iodide + bromine
7. calcium + hydrochloric acid
8. magnesium + nitric acid
9. silver + sulfuric acid
10. potassium + water
11. sodium + water
1. ____ NaBr + ____ Ca(OH)2 ___ CaBr2 + ____ NaOH
Reaction Type : ______________
2. ____ NH3+ ____ H2SO4 ____ (NH4)2SO4
Reaction Type : ______________
3. ____ C5H9O + ____ O2 ____ CO2 + ____ H2O
Reaction Type : ______________
4. ____ Pb + ____ H3PO4 ____ H2 + ____ Pb3(PO4)2
Reaction Type : ______________
5. ____ Li3N + ____ NH4NO3 ___ LiNO3 + ___ (NH4)3N
Reaction Type : ______________
6. ____ HBr + ___ Al(OH)3 ___ H2O + ___ AlBr3
Reaction Type : ______________
7.
Na3PO4 +
KOH
NaOH +
K3PO4
Reaction Type _______________________
8.
MgCl2 +
Li2CO3
9.
C6H12 +
O2
10.
Pb +
11.
CaCO3
12.
P4 +
MgCO3 +
CO2 +
FeSO4
O2
H2O
PbSO4 +
CaO +
P2O3
LiCl
CO2
Reaction Type _______________________
Reaction Type _______________________
Fe
Reaction Type _______________________
Reaction Type _______________________
Reaction Type _______________________
More About Types of Chemical Reactions Single Replacement Reactions Some Additional Information Types of Single Replacement Reactions Model 2 from homework shows 2 types 1)Replacement of a Metal in a Compound by a Meta l and 2)Replacement of Hydrogen by a Metal There is a 3rd type of Single Replacement Reaction Replacement of Halogens One halogen replaces another halogen in a compound For example: Cl2(g) + 2KBr(aq) 2KCl(aq) + Br2(l) Please write a general form equation for this type of single replacement reaction.
Activity Series and Single Replacement Reactions Not every metal can replace every other metal nor can every halogen replace every other halogen. We use an Activity Series to predict if a replacement reaction will occur.
The most active element, placed at the top in the series, can replace each of the elements below it from a compound in a single replacement reaction. Using the above activity series answer the following questions: Can zinc replace nickel? __________
Can copper replace lead? __________
Predicting Products of Chemical Reactions Follow the Patterns from Types of Chemical Reactions Each reaction that you work with will follow the patterns of the 5 types of chemical reactions Synthesis Decomposition Single Replacement Cation Anion Double Replacement Combustion
Steps to follow 1st Classify the reaction by looking at the reactants. What pattern do they match? 2nd Then write the products *If it is synthesis, write a compound that contains both reactants – remember to write true formulas. *If it is decomposition, then break it into two elements or compounds. *If it is single replacement, then replace the single element with the corresponding type of element in the compound give(cation for cation and anion for anion). Check the activity series – it is possible that the reaction will not go forward. Remember to write true formulas. *If it is double replacement, then the cation and anions switch places. Be careful when switching places. The rules require cation before anion and true formulas using charges. *If it is combustion the products are always water and carbon dioxide
With your group, look for additional patterns that will help you to predict the products. Additional information is in your book section 8-2
For all combustion reactions of hydrocarbons or hydrogen-carbon-oxygen molecules, the products will always be CO2 and H2O (assuming a complete reaction).
a. Combustion:
C6H12
+
9O2
6CO2
+
6H2O
b. Combustion:
2C4H6
+
11O2
8CO2
+
6H2O
c. Combustion:
C6H10O3
+
7O2
6CO2
+
5H2O
+
I2
MgI2
1. Synthesis:
Mg 2+
-
Note that Mg can only form Mg and I can only form I , so the product will must have a 1:2 cation:anion ratio.
2. Double displacement:
CuCl2
+
H2S
CuS
+
2HCl 2+
-
Note that the product is not H2Cl2. It is important to recognize that CuCl2 is made of three ions, Cu and two Cl .
3. Double displacement:
NaOH
+
HClO4
NaClO4 +
-
H2O
-
In this question, you must recognize that perchlorate, ClO4 , and hydroxide, OH , are polyatomic ions and will not break apart. Also, this is an acid-base reaction, so the products should be salt and water.
4. Decomposition:
ZnCO3
+
heat
ZnO
+
CO2
When reactions have heat as a reactant, it is very likely that they will involve decompositions. Carbonate compounds usually decompose to CO2 and a metal oxide.
5. Single replacement:
2HCl
+
Zn
ZnCl2
+
H2
Note that one reactant is in its elemental form; if a single replacement reaction is going to occur, the species NOT in its elemental + form in the reactants (H in this case), will end up in its elemental form in the products (H 2) and the species that IS in its elemental 2+ 2+ form (Zn) will end up ionized (Zn ). Note that zinc can only form a Zn ion, so it will have two chloride ions. Note also that hydrogen in its elemental form is H2, not H.
6. Single replacement
2Na
+
MgCl2
2NaCl
+
Mg 2+
Again notice that one species is in its elemental form (Na). The magnesium in MgCl 2 is an ion (Mg ), but is transformed into its + elemental state (Mg), while the Na is converted into an ion (Na , sodium only forms a +1 ion).
7. Double replacement
CaCl2
+
K2CO3
CaCO3
+
2KCl
2-
2+
+
Recognize that carbonate is a polyatomic ion (CO3 ) and that the cations are already stable ions (Ca and K ).
8. Synthesis
2K
+
Cl2
2KCl +
-
Note that both materials are elemental species, so the only result could be a synthesis reaction. In the product, K and Cl are formed. Note that we would NOT write the product as K2Cl2. Ionic compounds are written in their simplest forms.
9. Double replacement
3BaCl2 +
2K3PO4
Ba3(PO4)2
+
6KCl
3-
Note that phosphate (PO4 ) is a polyatomic ion and will not break apart. Since barium is a +2 ion, the barium phosphate will have a 3:2 ratio of Ba:PO4 in order to balance the charge.
10. Double replacement
H2SO4
+
2KOH
2H2O
+
2-
K2SO4 +
Notice that sulfate (SO4 ) is a polyatomic ion and that potassium exists as a +1 ion (K ). Also, this is an acid-base reaction, so the products should be salt and water.
11. Decomposition
Al2(CO3)3+
heat
Al2O3
+
3CO2 3+
Another decomposition that will generate CO2 and a metal oxide (note that Al forms a +3 ion, Al , and monatomic oxygen will have 2a –2 charge, O ).
12. Decomposition
Mg(OH)2 +
heat
MgO
+
H2O
Fe2O3
+
Hydroxides will often decompose with heat to yield water and an oxide. .
13. Decomposition
2Fe(OH)3
+
heat
3+
3H2O
Similar to the question above. Notice that the metal retains its ionic charge, it is Fe in both the reactants and products.
Single-Replacement Reactions Using the Activity Series Step 1 - Write the formulas of the reactants on the left of the yield sign Step 2 - Look at the Activity Series on page 266 or above to determine if the replacement can happen Step 3 - If the replacement can occur, complete the reaction and balance it. If the reaction cannot happen, write N.R. (no rxn) on the product side.
1. lead + zinc acetate
2. iron + aluminum oxide
3. silver nitrate + nickel
4. sodium bromide + iodine
5. aluminum bromide + chlorine
6. sodium iodide + bromine
7. calcium + hydrochloric acid
8. magnesium + nitric acid
9. silver + sulfuric acid
10. potassium + water
11. sodium + water
