Reaction Types Lab 2015
Objectives:
1. Observe changes in chemical and physical properties during a variety of chemical reactions.
2. Predict the type of reaction carried out based on Reactants and Products involved.
Background:
A chemical reaction consists of reactants and products. The reactants are what you start with (also
called starting materials) and the products are the new compounds that form during the reaction. Most
reactions can be classified into six general categories: (1) Synthesis (Combination) (2) Decomposition (3)
Single displacement (4) Double displacement (5) Acid/Base and (6) Combustion. These reaction types
can be represented by generic chemical equations as follows:
Synthesis: A + B → AB
Decomposition: AB → B + A
Single-displacement: A + BC → AC +B
Double-displacement: AB + CD → AD+ CB
Acid/Base: “H”A + B”OH” → H(OH) + BA
Combustion: Hydrocarbon (CxHy) + O2 → CO2 + H2O
During a precipitation reaction (double-displacement), an insoluble solid (precipitate) is formed as a
product. In addition, reactions can be classified as exothermic (releasing heat) or endothermic (consuming
heat).
In this lab you will carry out various reactions and make careful observations about what you see. In
a final report you will be expected to construct a series of Cl-Ev-R statements claiming which type of
reaction was observed at each station based on evidence and reasoning.
Procedure:
Perform Reactions #1 through #9c. For each reaction record the following information in your Chemistry
Journal BEFORE you do the experiment. See sample data table.
1) Write the reactants half of the formula equation (use key to help identify formulas)
Example: Na + Cl2 
2) Predict the Type of Reaction based on the Reactants described above
Example: (A + B ) = Synthesis
NOW …..Conduct the Experiment !!! Then…….
3) Write the Complete Word Equation based on the type of reaction you identified above (use key)
Example: Sodium reacts with Chlorine to produce Sodium Chloride
4) Write a complete Formula Equation based on the word equation formed above (use key)
Example: Na + Cl2  NaCl
The Reactions: dump waste into appropriate waste containers and CLEAN lab station!
First reaction: Light a Bunsen burner. The methane gas in the line reacts with the oxygen in the air. Put
matches in “matches waste”.
Second reaction: Burn a Mg strip by holding it with tongs and lighting it with a Bunsen burner. The
magnesium ribbon reacts with the oxygen in the air. DO NOT LOOK DIRECTLY AT THE REACTION!
The product should be placed in the solid waste container.
Third reaction: Place a piece of Zinc in a test tube containing Hydrochloric Acid filled to the line. The
zinc reacts with the hydrochloric acid. Cork the top of the test tube for no more than 15 seconds and then
quickly place a lit splint over the opening to TEST for the type of gas produced in this reaction. Pour the
solution into the liquid waste when finished. Place expired match in “match” waste.
Fourth reaction: React 10 drops of 1.0 M HCl and 1 drop of 1.0 M Ag(NO3). When you are finished pour
the solution into the liquid waste.
Fifth reaction: Measure the pH of 0.1 M HCl and 0.1 M NaOH by dropping one drop of each on different spots
on a small piece of pH paper. Do not dip the paper into the solution! Compare the color of the spots to the
chart with the pH paper to determine pH. Then mix 10 drops of each solution in a small beaker and stir well
with a stirring rod. Use the stirring rod to place a drop of the new mixture on a fresh area on the pH paper and
record the pH. When you are finished, pour the solution into the liquid waste and throw away the pH paper.
Sixth reaction: Add a small amount of the crushed limestone Ca(CO3) to a test tube containing 1.0 M HCl.
When you are finished, pour the solution into the liquid waste.
Seventh reaction: Place a small strip of Aluminum in a test tube about 1/3 full of 0.5 M CuCl2. When you
are finished, pour the solution into the liquid waste.
Eighth reaction: Scrub a small paperclip (Fe) with a piece of steel wool and then place into a test tube. Fill
the test tube until ½ of paper clip is covered with 1.0 M Cu(SO4). When you are finished, pour the solution
into the liquid waste.
Ninth Reaction: Using the micro-well plate see what happens when each of the following sets of reactions
take place. Please use no more than two drops of each and DO NOT MIX pipettes. Clean up properly.
a) BaCl2 reacts with
b) Cu(SO4) reacts with
c) KI reacts with
Mg(SO4)
Na2(CO3)
Pb(NO3) 2
Reactants:
Na(OH) – Sodium Hydroxide
Mg(SO4) – Magnesium Sulfate
CaCO3 – Calcium Carbonate
BaCl2 – Barium Chloride
CuCl2 – Copper (II) Chloride
CH4 – Methane Gas
Ag(NO3) – Silver Nitrate
Pb(NO3)2 – Lead (II) Nitrate
KI – Potassium Iodide
Cu(SO4) – Copper (II) Sulfate
Zn - Zinc
Fe – Iron
Mg – Magnesium
Al - Aluminum
HCl – Hydrochloric Acid
Na2(CO3) – Sodium Carbonate
O2 – Oxygen gas
Products:
Magnesium Oxide – MgO
Carbon Dioxide – CO2
Nitric Acid – HNO3
Magnesium Chloride – MgCl2
Aluminum Chloride – AlCl3
Sodium Chloride – NaCl
Silver Chloride – AgCl
Calcium Chloride - CaCl2
Water – H20
Copper metal - Cu
Carbonic Acid - H2CO3
Iron (II) Sulfate – Fe(SO4)
Iron (III) Chloride - FeCl3
Barium Sulfate – Ba(SO4)
Zinc Chloride – ZnCl2
Sodium Sulfate – Na2(SO4)
Copper – Cu
Silver Sulfate – Ag2(SO4)
More Products!
Potassium Nitrate – K(NO3)
Copper (II) Carbonate – Cu(CO3)
Lead (II) Iodide – PbI2
Potassium Nitrate – K(NO3)
Hydrogen gas – H2