Chemical Reactions I – Mix and Match
Section IA – Vocabulary
Below is a list of all of the vocabulary terms used in this subnit. By the end of the
subunit, you will be able to write a working definition of each term and correctly
use each term.
activity series of metals
aqueous solution
balanced equation
combustion reaction
complete ionic equation
decomposition reaction
precipitate (↓)
product
reactant
catalyst
double replacement
single replacement
chemical equation
chemical reaction
coefficient
reaction
gas (↑)
gas (g)
law of conservation of
reaction
skeleton equation
solid (s)
spectator ion
energy
combination reaction
net ionic equation
Section IA – Key Concepts
1) Writing and balancing Chemical Equations
2) Types of Chemical Reactions
3) Aqueous Reactions and Precipitates
Section 2 –– Outside Class Assignments
Thoughtfully do each of the following assignments. Include all your reasoning and
show all your work wherever it seems appropriate. Due dates for each assignment
will be given in class. (Please remember - homework that is passed in late is
automatically discounted 15%.)
1) Create a concept map for each of the following groups of terms
a) Reactants, products, chemical reaction, law of conservation of mass,
chemical equation, coefficients, balanced equation
b) Single displacement reaction, double displacement reaction, decomposition,
combustion, combination reaction, reactions of aqueous solution, spectator
ions
c) Catalyst, skeleton equation, complete ionic equation, net ionic equation,
balanced equation.
2) List 5 factors that you might use to determine whether a chemical reaction has
occurred when 2 or more substances are mixed in a container.
3) Write a skeletal equation for each of the following:
a) Carbon dioxide combines with water to form glucose and oxygen gas.
b) Sulfur burns in oxygen gas to form sulfur dioxide.
c) Ammonia reacts with iodine to form nitrogen triodide and hydrogen gas.
d) Propane burns in the presence of oxygen gas to form carbon dioxide and
water
e) Nitric acid reacts with potassium hydroxide to form potassium nitrate and
water.
f) Iron reacts with oxygen gas (rusts) to form iron (III) oxide.
g) Hydrogen peroxide spontaneously decomposes into water and oxygen gas.
4) Examine problem #3a again.
a) Re write the skeletal equation
b) As if you were teaching a fellow chemistry student, write down each of the
steps you took to balance this equation.
c) If you were to generalize the steps for balancing an equation, what would
they be?
d) Are there any exceptions to this order or number of steps?
5) Balance each of the remaining skeletal equations you wrote in #3 above.
6) For more practice writing skeletal equations and balancing them, see Writing
and Balancing Equations Worksheet.
7) For even more practice balancing equations, try #8 on p211.
8) You have just spent time balancing a number of equations.
a) Why do chemists balance equations?
b) How does balancing a chemical equation relate to the law of conservation of
matter? Explain your answer.
9) Now that you are familiar with the five types of chemical reactions, use your
annotated table and other information in your tool kit to determine the reaction
type of each of the following:
a) 2H2C2O4 + O2  4CO2 + 2H2O
b) 2KCl + 3O2  2KClO3
c) 2NaCl  2Na Cl2
d) Ca(OH)2  CaO + H2O
e) Na2O + H2O  2NaOH
f) CaCO3 + HCL  CaCl2 + CO2 + H2O
g) CH4 + 2O2  CO2 + 2H2O
h) AgNO3 + NaCl  AgCl + NaNO3
10) Double displacement reactions will only occur if certain types of products are
produced, what are these types of products?
11) For more practice identifying reaction types and predicting products, try the
Worksheet A Voyage through Equations from Cavalcade Publishing.
12) For even more practice identifying reaction types and predicting products, try
the Worksheet Reaction Type Review I and II.
13) Net ionic equations are used when the reactants are in an aqueous state.
a) Why is a net ionic equation often a simplified version of a single or double
displacement reaction?
b) In looking at an ionic equation, how does one determine whether a
precipitate will form?
c) Write balanced net ionic equations and identify the spectator ion for each
of the following:
i)
HCl(aq) + Ca(OH)2(aq) 
ii)
Ag2SO4(aq) + AlCl3(aq) 
iii) Hg(aq) + Zn(NO3)2(aq) 
iv) H2C2O4(aq) + KOH(aq) 
v)
Iron dissolved in water with sulfuric acid
vi) CdBr2(aq) + Na2S(aq) 
vii) NaCl(aq) + H2SO4(aq) 
viii) Iron (III) nitrate and sodium hydroxide 
14) So far we have been working with reactants and predicting products. In this
problem, write down a chemical reaction that could produce each of these
products.
a) Carbon dioxide
b) Ammonium hydroxide
c) Silver carbonate
d) Acetic acid
e) Calcium phosphate
Section 3 –In Class Activities
1) Lecture / slides
2) Demonstrations
3) Student Labs
a) Modeling Chemical Reactions
b) Reaction Types – Completion and Balancing
c) Activity Series of Metals
d) Precipitation Reactions
Section 4 –Textbook and Further Readings
1) Wilbraham, Staley, Matta, Waterman pp202-223