Reactions
Unit 7 Assignment list Chemistry Chapter 9
Wed Oct 28 Begin writing reactions / Write from word equations
Thursday Oct 29 Retakes~Graphic Org./Enrichment due
Friday October 30 Teach balancing
Monday Nov 2 Practice balancing equations
Tuesday Nov 3 Single replacement reactions / SR minilab
Wednesday Nov 4 Double replacement reactions
Thursday Nov 5 Quiz on balancing / Workday
Friday Nov 6 DR minilab
Monday Nov 9 Workday
Tuesday Nov 10 Combo/Decomp reactions
Wednesday Nov 11 Veterans Day Holiday !
Thursday Nov 12 Lab on reaction types
Friday Nov 13 Quiz over SR & DR / combustion practice
Monday Nov 16 Workday
Tuesday Nov 17 Review
Wednesday Nov 18 TEST/ NB check
EQ Why are reactions balanced?
KQ How are reactions balanced?
EQ How can products of reactions be predicted?
KQ What are the distinguishing characteristics of the 5 reaction types?
What has to happen for a single or double replacement reaction to proceed?
GPS SC2 a & b Identify and balance 5 different types of reactions.
Experimentally determine indicators of chemical reactions.
Do you feel lost?
Don’t forget you can come for help before or after school most days. Also try these very good tutorials on
balancing equations:
http://www.bozemanscience.com/beginners-guide-balancing-equations
https://www.khanacademy.org/science/chemistry/chemical-reactionsstoichiometry/e/balancing_chemical_equations
(Brightstorm) https://www.youtube.com/watch?v=XJwADOk8DTQ
(Mr Causey) https://www.youtube.com/watch?v=Nu-wXCY0nnI
http://www.chemteam.info/Equations/Equations.html
Checklist of things to know:
1) Identify reactants and products in a chemical equation.
2) Convert word equations to formula equations.
3) List four indicators of a chemical change.
4) Identify and use symbols to indicate solids, liquids, gases, aqueous solutions, heat,
and the use of a catalyst in a chemical equation.
5) Explain the purpose of coefficients in a chemical equation.
6) Balance chemical equations.
7) Classify a reaction as one of the following
types: synthesis, decomposition, combustion,
single displacement, double displacement
8) Predict products of reactions.
Vocabulary:
Chemical equation
Coefficient
Law of conservation of mass
Precipitate
Notebook includes:
Vocabulary
Balancing handout
Word equations handout
Intro note guide
5 types notes & handout
SR minilab
SD minilab
Graphic Organizer 5 types
Synthesis
Combustion
Decomposition
Single displacement
Double displacement
Lab due separately on Tues Nov 17
– no written report, just complete
the handout
Activity series of metals
Notes on Chemical Reactions:
Name_________________ Date_______
Chemical equations are like sentences that show ________________________.
Chemical equations all contain ____________. On the left of the __________ are the
_____________. These are the substances you __________________.
On the right of the ____________ are the __________ which are substances you
_________________.
Some reactions contain the following symbols:
+ _________________________
(aq) ________________________
(g) or ______________________
(s) or ______________________

______________________
x
______________________
______________________________
FYI: Seven elements are diatomic which means they won’t exist as a single atom. These are:
________, ________, _________, __________, ________, ________. ________
Skeleton reactions show ___________________ and ___________________ but are
________________________.
Examples –
Underline the reactants and circle the products and then write the following
skeleton reactions . . .
1)
Hydrogen Peroxide decomposes in the presence of the catalyst Manganese Dioxide to form water
and Oxygen gas.
2)
Calcium metal reacts with water to form calcium hydroxide and hydrogen gas.
3)
Copper metal reacts with aqueous nitric acid to form nitrogen dioxide gas, aqueous copper (II)
nitrate and water.
4)
Aqueous Lead (II) Nitrate reacts with aqueous Potassium Iodide to form solid Lead (II) Iodide
and aqueous Potassium Nitrate.
5) Carbon dioxide and water are formed when Propane gas (C3H8) reacts with oxygen in the presence
of heat.
Balancing equations handout
NAME ___________________________
Add coefficients to balance each reaction. Use pencil so you can erase!
1.
H2 + O2  H2O
2. S8
+ O2  SO3
3. HgO  Hg + O2
4. Zn + HCl  ZnCl2
+ H2
 NaOH
5. Na + H2O
6. C10H16
+ Cl2
 C
7. Si2H3
+ O2
 SiO2
8. Fe + O2
 Fe2O3
9. C7H6O2
+ O2
10. FeS2
11. Fe2O3
+ O2
+ H2
+ HCl
+ H2O
 CO2

Fe2O3
+ H2  Fe
+ H2O
+ SO2
+ H2O
12. K + Br2  KBr
13. C2H2 + O2  CO2 + H2O
14. H2O2  H2O + O2
15. C7H16
+ O2  CO2 + H2O
16. SiO2 + HF  SiF4
17. KClO3
+ H2O
 KCl + O2
18. KClO3  KClO4 + KCl
19. P4O10
+ H2O
 H3PO4
20. Sb + O2  Sb4O6
21. C3H8 + O2  CO2 + H2O
22. Fe2O3
23. PCl5
CO  Fe
+
 HCl
+ H2O
+
25. N2
+ O2  N2O
 C6H12O6
+ H2O
+ O2
+ H2O  H4SiO4
27. SiCl4
28. H3PO4 
29. CO2
+ H3PO4
H2  NH3
24. N2
26. CO2
+ CO2
H4P2O7

+ NH3
+ HCl
+ H2O
OC(NH2)2
+
H2O
30. Al(OH)3
+ H2SO4  Al2(SO4)3
31. Fe2(SO4)3
+ KOH 
+ HI  H2S
32. H2SO4

33. Al + FeO
34. Na2CO3
35. P4
+
I2
+ Fe(OH)3
+ H2 O
+ Fe
 NaCl
+ HCl
+ H2O
+ CO2
 P2O5
+ O2
36. K2O
Al2O3
K2SO4
+ H2O
+ H2O  KOH
37. Al + O2  Al2O3
38. Na2O2
+ H2 O 
39. C + H2O  CO

40. H3AsO4
41. Al2(SO4)3
42. FeCl3
NaOH + O2
+ H2
As2O5 + H2O
+ Ca(OH)2  Al(OH)3
+ CaSO4
+ NH4OH  Fe(OH)3 + NH4Cl
43. Ca3(PO4)2 + SiO2
44. N2O5 + H2O
 P4O10
 HNO3
+ CaSiO3
Notes on 5 reaction types:
1)
Combination –
General format: _______________________________________________
How do you know it works?
Example(s):
2)
Decomposition – Reverse of Combination
3)
Single Replacement –
General format - _______________________________________________
Only works if _________________________Use: ____________________
Example(s):
4)
Double Replacement –
General format - ______________________________________________
Only works if __________________________________________________
Example(s):
5)
Combustion –
General format –
Does it work? __________________________________________________
Reaction types practice
1) Predict and balance the following combination (synthesis) reactions:
a) Ba + O2 
b) Mg
+ F2 
c) Al +
d) Ca
S 
+
P 
2) Predict and balance the following decomposition reactions:
a) HgO 
b) CuCl2 
c) Al2O3 
d) NaCl 
e) K3N 
3. Use the activity series of metals to predict the products of SR reactions:
(Balance)
a) Zn + CuSO4 
b) Ag + FeSO4 
c) Al + H2SO4 
d) Fe + H2O 
e) Na + H2O 
4. Write the products (and balance) the following double replacement
reactions:
a) Ag2SO4
+ AlCl3 
b) H2C2O4
+ KOH 
c) BaCl2
+
Na3PO4 
d) HCl + Ca(OH)2
e) CaS
f)
+

HCl 
NaCl + Ca(NO3)2 
5) Write the products for the following combustion reactions. (Balance)
a) C6H12O6 +
O2 
b) C2H5OH +
O2 
c) C7H16 +
d) C2H2
e) C3H8O
O2 
+ O2

+ O2 