Name:
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Chemistry Theoretical & Assessment Booklet 1
LEARNING INTENTIONS
1. To understand the major points to the scientific method followed in
practical activities.
2. To apply this method to gathering suitable and appropriate data to
describe and explain your reactions.
3. To understand the concept of a Chemical Reaction.
4. To be able to identify different types of Chemical reactions.
5. To be able to write complete Word Equations that describe a Chemical
Reaction.
SUCCESS CRITERIA
1. All required data has been collected and accurately recorded.
2. All questions and the Revision Summary are completed.
3. Be able to identify different types of Chemical Reactions from practical
results and various word equations.
Chemical Reactions
A chemical reaction is a process that causes of one set of chemicals to change
into another.
Chemical reactions are identified by a change to the chemicals that you start
with.
Chemical reactions make one or more products which have properties
different from the reactants.
Example;
Hydrogen: is a colourless/odourless gaseous element that is highly
flammable.
Oxygen is a colourless/odourless gaseous element that supports
combustion.
When these two elements are combined in a chemical reaction one product is
formed.
1. What is the product formed in this chemical reaction?
2. Describe the properties of this product.
3. What is the importance of
the chemical reaction
described in the table?
The following experiments will help you understand more about the nature of
chemical reactions.
Experiment 1 - Burning Magnesium
Aim:
The aim of this experiment is to investigate the reaction of
magnesium as it burns in air.
Materials:
A length of Magnesium ribbon, Crucible and lid, Clay Triangle, Tripod,
Bunsen burner, Baseboard,
Tongs, Matches.
Method:
1. Collect all equipment.
2. Observe the Magnesium
and record your
observations below.
3. Set up the equipment as
in the diagram.
4. Coil up the strip of Magnesium and place it in the crucible (See
Diagram).
5. Strongly heat the bottom of the crucible for 2 to 3 minutes.
6. Use the tongs to lift the lid slightly to let air into the crucible.
7. Observe the Magnesium and record any changes below.
8. If there are no changes to the Magnesium replace the crucible
lid and heat for a further 1 to 2 minutes. Repeat steps 5 to 7
until you notice a significant change to the Magnesium.
9. Record all observations.
Results:
DESCRIPTION
Magnesium
before experiment:
Magnesium
after experiment:
Additional Notes:
Experiment 2 - Magnesium in Hydrochloric Acid (HCl)
Aim:
The aim of this experiment is to investigate the reaction of
Magnesium as it is added to Hydrochloric Acid.
Materials.
Hydrochloric Acid, Magnesium ribbon, Baseboard, Large test-tube,
Test-tube rack, Measuring cylinder.
Method:
1. Collect all equipment.
2. Observe the Magnesium and Hydrochloric Acid before the
experiment and record your observations below.
3. Coil up the strip of Magnesium and place it in the bottom of the
test-tube.
4. Measure out 20 ml of Hydrochloric Acid in the measuring
cylinder.
5. Pour the acid into the test-tube.
Acid
6. Record your observations of the two mixed
substances.
Magnesium
Results:
DESCRIPTION
Magnesium
before experiment:
Hydrochloric Acid
before experiment:
Magnesium
after experiment:
Hydrochloric Acid
before experiment:
Additional Notes:
Experiment 3 – Precipitation Reactions
Aim.
The aim of this experiment is to investigate the formation of a
substance known as a precipitate.
Materials.
3 Test-tubes, Test-tube rack, Baseboard, Dropper bottles with the
following solutions;
 Sodium Hydroxide,
 Copper (II) sulfate,
 Potassium iodide,
 Lead (II) nitrate,
 Silver nitrate,
 Sodium Chloride,
 Potassium carbonate ,
Method.
1. Collect all equipment.
2. Record your observations of the 7 substances in their dropper
bottles.
3. Pour Sodium Hydroxide into a test tube to the level of 1 cm.
4. Now add 1 cm’s worth of Copper Sulfate into the test tube.
5. Shake test tube gently.
6. Record your observations.
7. Clean out the test tube thoroughly.
8. Now repeat steps 1 to 6 using the following combination of
chemicals each time.
a. Potassium iodide + lead nitrate
b. Potassium iodide + silver nitrate
c. Sodium chloride + silver nitrate
d. Copper sulfate + potassium iodide
e. Silver nitrate + potassium carbonate
Results:
CHEMICAL DESCRIPTIONS BEFORE EXPERIMENT
1
2
3
4
5
6
7
Additional Notes:
Results Continued:
CHEMICAL DESCRIPTIONS AFTER EXPERIMENT
1
2
3
4
5
6
7
Experiment 4 – Heating Copper Carbonate
Aim:
The aim of this experiment is to investigate heating of Copper
Carbonate in air.
Materials:
Test- tube, Bunsen burner, Baseboard, Copper carbonate
Method:
1. Collect all equipment.
2. Observe the Copper
Carbonate and record
your observations.
3. Add a spatula of copper
carbonate into a boiling
tube
4. Holding the boiling tube
with a pair of test tube
holders move the boiling
tube into a roaring flame and heat the copper carbonate
strongly.
5. Record your observations.
Results:
DESCRIPTION
Copper Carbonate
before experiment:
Copper Carbonate
after experiment.
Discussion:
1. To fully understand these four experiments you need to use the
following terms. Clearly define them.
a. Reactant
b. Product
c. Precipitate
d. Element
e. Compound
2. Using the results from these four experiments state clearly how in future
you could identify if a Chemical reaction has occurred?
Classifying Chemical Reactions.
Chemical reactions generally involve reactants making products which usually
involves some kind of change in temperature, state, colour etc. However, all
reactions can be classified based upon similarities.
 In Experiment one (Burning Magnesium) you have taken two different
elements and made them join together to make a new substance, in this
case a compound. This type of reaction is called a Combination or
Synthesis Reaction.
In a Combination/Synthesis reaction, two or more simple substances
combine to form a more complex substance. These reactions are in the
general form:
For this experiment you took Magnesium and combined it with the
Oxygen in the air and have made Magnesium Oxide.
This can be shown simply in a Word Equation.
Magnesium + Oxygen
Notes:
Magnesium Oxide
Practice writing Word Equations for Combination/Synthesis reactions by
identifying the products.
1. Calcium + Oxygen
Calcium Oxide
2. Copper + Sulfur
3. Hydrogen + Nitrogen
4. Hydrogen + Chlorine
5. Silver + Sulfur
6. Chromium + Oxygen
7. Aluminum + Bromine
8. Sodium + Iodine
9. Aluminum + Oxygen
10. Aluminum + Bromine + Oxygen
11. Silver + Sulfur + Oxygen
12. Copper + Sulfur + Oxygen
13. Hydrogen + Nitrogen + Oxygen
14.Calcium + Carbon + Oxygen
15. Aluminium + Carbon + Oxygen
Complete the following word equations by identifying the reactants.
1.
2.
3.
4.
5.
6.
7.
8.
Calcium Oxide
Hydrogen Oxide
Sodium Chloride
Zinc Sulfide
Silicon oxide
Calcium Carbonate
Magnesium Sulfate
Hydrogen Sulfate
Calcium + Oxygen
 In Experiment 2 (Magnesium in Hydrochloric Acid) we have taken a
compound and an element and made the three components rearrange
their places.
This type of reaction is called a Single Replacement Reaction.
In a single replacement reaction, a single uncombined element replaces
another in a compound; in other words, one element trades places with
another element in a compound. These reactions come in the general
form of:
For this experiment you took Magnesium and reacted it with
Hydrochloric Acid. This can be shown simply in a Word Equation.
Magnesium + Hydrogen Chloride
Hydrogen + Magnesium Chloride
Notes:
Practice writing Word Equations for Single Replacement reactions by
identifying the products.
1. Lead + Zinc Acetate
2. Iron + Aluminium Oxide
3. Silver Nitrate + Nickel
4. Sodium Bromide + Iodine
5. Aluminium Bromide + Chlorine
6. Sodium Iodide + Bromine
7. Calcium + Hydrogen Chloride
8. Magnesium + Hydrogen Nitrate
9. Silver + Hydrogen Sulphate
10. Potassium + Sodium Bromide
 In Experiment three (Precipitation Reactions) we have taken two
compounds and made them totally rearrange their structure.
This type of reaction is called a Double Replacement reaction.
In a double replacement reaction, components of two the compounds
switch places and form two entirely different compounds. These
reactions are in the general form:
For example, when Sodium Hydroxide and Copper Sulfate react, the
elements switch places giving the compounds Sodium Sulfate and
Copper Hydroxide. This can be shown as;
Sodium Hydroxide + Copper Sulfate
Sodium Sulfate + Copper Hydroxide
Notes:
Practice writing Word Equations for Double Replacement reactions by
identifying the products.
Complete the following word equations.
1. aluminium iodide + mercury (II) chloride
2. silver nitrate + potassium phosphate
3. copper (II) bromide + aluminium chloride
4. calcium acetate + sodium carbonate
5. ammonium chloride + mercury (I) acetate
6. calcium nitrate + hydrogen chloride
7. iron (II) sulfide + hydrogen chloride
8. copper (II) hydroxide + hydrogen acetate
9. calcium hydroxide + hydrogen phosphate
10. calcium bromide + potassium hydroxide �
 In Experiment four (Heating Copper Carbonate) you have taken a
compound and made it separate into separate.
This type of reaction is called a Decomposition reaction.
A decomposition reaction is the opposite of a combination/synthesis
reaction. A decomposition reaction is when a more complex substance
breaks down into its more simple parts. It is thus the opposite of a
synthesis reaction, and can be written as;
For example you took copper carbonate and decomposed it by heating. You
drove carbon dioxide out of the copper carbonate leaving just copper oxide in
the test-tube. This can be shown simply in a Word Equation.
Copper Carbonate
Copper Oxide + Carbon Dioxide
Notes:
Practice writing Word Equations for Decomposition reactions by identifying the
products.
1. Aluminum Oxide
2. Silver Oxide
3. Gold Oxide
4. Barium Sulfide
5. Barium Carbonate
6. Magnesium Carbonate
7. Potassium Sulfate
8. Nickel Chlorate
9. Sodium Chlorate
10. Potassium Chlorate
11. Hydrogen Sulfate
12. Zinc Hydroxide
13. Iron Hydroxide
14. Copper Nitrate
Summary:
Here is a representation of the four basic chemical reactions types that we
have worked on;




synthesis,
decomposition,
single replacement
double replacement.
Experiment 5 – Sodium Thiosulfate and Hydrochloric Acid Reaction.
Aim:
To investigate the reaction between Sodium Thiosulfate and
Hydrochloric Acid.
Apparatus:
Sodium Thiosulfate solution, dilute Hydrochloric Acid of 3 different
concentrations, Measuring cylinder, Stopwatch, Conical flask, White
tile, Texta
Method:
1. Collect all equipment.
2. Place 100 cm3 of the Sodium Thiosulfate solution into a conical
flask.
3. Place the flask onto a white tile marked with a black cross.
4. Add 10 cm3 of
M Hydrochloric Acid to the flask. Swirl the
flask for 1 to 2 seconds while starting the stopwatch at the
same time.
5. Look down on the black cross.
6. Record the time taken for the cross to disappear.
7. Repeat steps 2 to 6 using 10 cm3 of
M hydrochloric acid.
8. Repeat steps 2 to 6 using 10 cm3 of
M hydrochloric acid.
Results:
Concentration of
acid
M
M
M
Reaction time (s)
Discussion:
Draw a graph of Reaction time against Concentration of Acid.
ASSESSMENT TASK – Revision Summary
In this assessment task you must write a Revision Summary about
what these 5 experiments, and the associated tasks, have taught you
about Chemical Reactions.
Assessment Rubric
Criteria
High (3)
Medium (2)
Low (1)
Not Shown
(0)
Result tables
More than 75%
of the tables are
completed
More than 50%
of the tables are
completed
Only a few boxes
are completed
Tables not
attempted
Word Equations
More than 75%
of word
equations are
completed
More than 50%
of word
equations are
completed
Less than 50% of
word equations
are completed
Word
Equations
not
attempted
Criteria
High (9)
Medium (6)
Low (3)
Not Shown
(0)
Revision
Summary
Summary is
comprehensive
and accurate.
Provides
excellent
resource for
exam. revision.
Summary is
reasonably
comprehensive
and mainly
accurate.
Provides good
resource for
exam. revision.
Marks:
TOTAL
/15
Summary is
lacking detail and
Revision
accuracy.
Summary
Provides poor
not
resource for
completed.
exam. revision.