Student Name:
Year 8 Science Home Learning Booklet
Chemical Reactions
To be handed in on or before: 25th April 2014
The options that I have completed for my Home Learning are (Please tick):
Option Number
Vivomiles
Reversible or irreversible?
3 Vivomiles
Simple Chemical Reactions
5 Vivomiles
Matching reactants to products
3 Vivomiles
Which gases are in air?
3 Vivomiles
Complete the fire triangle
5 Vivomiles
Explosions
5 Vivomiles
More combustion
7 Vivomiles
What is made when a fuel burns?
5 Vivomiles
Word equations
10 Vivomiles
Chemical reactions
7 Vivomiles
Reactivity worksheet
5 Vivomiles
Extension: Corrosion of metals with acid
10 Vivomiles
Displacement reactions
10 Vivomiles
Extraction of metals
10 Vivomiles
Rusting in iron and steel
5 Vivomiles
Completed?
What do I need to do?
In Science you are currently studying Chemical Reactions. In this module you will be learning about chemical
reactions, how to test for different gases, the reactivity of different metals, fire safety and how to represent
reactions as word and symbol equations.
To support the work that you are doing in science, all of the home learning activities below will help you to
further your understanding of chemical reactions.
Check which teaching group you belong to and start to work out which home learning activities you have to
select from. If you are not sure – Ask for help!
Teaching Group
What do I need to do?
8R1 & 8R2
Select home learning activities that total a minimum of 45
Vivomiles*
Select home learning activities that total a minimum of 35
Vivomiles*
Select home learning activities that total a minimum of 20
Vivomiles*
8C1
8S1
* Remember that there is nothing stopping you from completing more home learning activities for more
Vivomiles!
Lesson 1– simple reactions
Recall irreversible or reversible reactions
Describe reactions as physical or chemical.
Reversible or Irreversible?
Use your knowledge to Identify which of the following are Re-
The Reaction
Boiling an egg
Mixing baking
powder, vinegar
And washing up liquid
Striking a match
What it looks How do you know
like at the start a reaction has
taken place
Lesson 2– Combustion
Recall the gases present in air
Describe the chemical process of combustion
Explain how to reduce risks from fire.
Nitrogen Oxygen
Water Vapour
Rare Gases
Carbon Dioxide
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Read the following information and
then answer the questions
An explosion is a chemical reaction that happens really quickly. A lot
of gases are released and usually massive amounts of heat. Chemicals
which are designed to explode are called explosives. However,
everyday chemicals can explode. Natural gas will explode if it is mixed
with the right amount of oxygen. This used to be a big problem for
coal miners in the 18th century. Pockets of natural gas in the mines
were ignited by the miners lamps. In 1815 Sir Humphrey Davy invented
a safer mining lamp to reduce the risk of explosions.
The first explosive available was gunpowder. This was invented in
China about 1200 years ago. Gunpowder is not very powerful and has
to be lit with a flame.
In 1847, an Italian Scientist called Ascanio Sobrero invented
nitroglycerine. This chemical is a liquid and explodes with even the
slightest knock.
In 1865, Alfred Nobel opened a factory to make nitroglycerine. The
factory blew up and killed his brother. Nobel then changed the
nitroglycerine so that it was a little safer. This new material he called
dynamite.
1)
What is an explosion?
………………………………………………………………………….
2)
What do we call a material that can cause an explosion?
………………………………………………………………………….
3) What is needed to make Natural gas explode?
Two identical pieces of magnesium are going to be burned. The first
will be in air. The second one will be in a gas jar of pure oxygen.
Magnesium in
Air
Magnesium in
Pure Oxygen
Will they burn
exactly the
same?
………………………………………………………………………
……………………………………………………………………….
……………………………………………………………………….
……………………………………………………………………….
……………………………………………………………………….
4) What was one of the problems for coal miners in the 18th
century?
……………………………………………………………………
………………………………………………………………………
5) What was the first explosive to be invented?
……………………………………………………………………….
6) Who invented Nitroglycerine?
……………………………………………………………………
7) What is the major problem with nitroglycerine?
………………………………………………………………………
8) What did Alfred Nobel make out of
nitroglycerine?
……………………………………….
………………………………………..
9) Can you think of any uses for
explosions
……………………………………….
………………………………………..
………………………………………………………………………..
10) Try to find out about Humphrey Davy and his safety lamp.
……………………………………………………………………….
………………………………………………………………………..
The apparatus below can be used to collect the gases that are produced
when a fuel burns. All fossil fuels contain the chemicals carbon and
hydrogen. The air is sucked out of the apparatus by the pump. This pulls
the gases from the flame into the funnel and through the boiling tubes.
Funnel
To Suction
Pump
Burning Candle
1)
Limewater
Iced Water
What is the fuel in this experiment?
…………………………………………………………………………….
2) What happens to the limewater?
…………………………………………………………………………….
3) Why is this?
…………………………………………………………………………….
4) What is the job of the iced water?
…………………………………………………………………………….
5) What collects on the inside of the first boiling tube?
…………………………………………………………………………..
6) Which two gases are therefore made when the fuel burns?
………………………………………………………………………….
Chemical Reactions can be summarised as word equations. These show
what you start with (REACTANTS) and what is made (PRODUCTS).
Example
Magnesium + Oxygen —–> Magnesium oxide
(Reactants)
(Product)
Complete the word equations for burning carbon and hydrogen
Carbon + Oxygen ——> ………………………..
Hydrogen + …………………. ——> Water
A piece of shiny copper will turn black when you heat it in a
Bunsen flame. Write a word equation to show what you think is
happening
………………………………………………………………………….
Lesson 3– Word equations
Recall products and reactants
Describe reactions in the form of word equations.
Word equations
When a chemical reaction takes place new chemicals are formed. We can
show what is happening using a word equation. Here are three examples:
Reaction 1: Magnesium burning
magnesium + oxygen → …………………………………………………………….
Reaction 2: Carbon burning
Carbon + oxygen → ………………………………………………………..
Reaction 3: Magnesium is added to hydrochloric acid (hydrogen chloride)
Magnesium + hydrogen chloride →…………………………………………………...
We can see that each word equation has an arrow like this →. This arrow
points to the chemicals produced in the reaction. We call these the products.
What is the product of reaction 1?
What is the product of reaction 2?
What are the two products of reaction 3?
The chemicals on the left of the arrow react together to make the products. These chemicals are called the reactants. Underline the reactants
for reactions I,2 and 3 above.
Note: If a compound has only 2 elements in it we give it a name which
ends in “ide”. Its name usually indicates the elements present. For example carbon dioxide has carbon and oxygen in it.
Chemical Reactions
Take it in turns with your partner answering the following questions:
1. Fill in the missing words from these equations
a
__________________________ + oxygen → carbon dioxide
b
lead + oxygen → __________________________ oxide
c
copper + oxygen → copper __________________________
d
tin + __________________________ →tin chloride
e
sodium + chlorine → __________________________
2Each of the chemicals in the table has a common name as well as a proper
chemical name. Fill in the blanks in this table.
Common name
common salt
Chemical name
Elements in the compound
sodium chloride
sodium, chlorine
water
ammonia
‘rotten egg’ gas
hydrogen, oxygen
nitrogen hydride
hydrogen sulphide
3The table shows the names and chemical formulas of some compounds. Fill
in the blank spaces in this table.
Name of compound
Chemical
formula
Number of elements in the
compound
Names of elements in
the compound
magnesium oxide
MgO
2
magnesium, oxygen
potassium oxide
K2O
FeS
potassium hydroxide
calcium carbonate
KOH
CaCO3
iron, sulphur
3
Reactivity Worksheet
Students set up a practical and record the following observations
Each container has hydrochloric acid in it along with a metal.
1 – magnesium 2 – copper
3 – zinc 4 – iron 5 – aluminium
Tasks
How do you know a reaction is happening in the containers?
Which is the most reactive metal?
Describe one way to make sure the experiment the students completed was fair.
Describe how to test the gas given off.
Write a word equation for each reaction
sodium + iron chloride
sodium chloride + iron
Sodium is more reactive so displaces the compound
Magnesium + Silver Oxide
Platinum + Calcium Bromide
Aluminium + Lead Chloride
Gold Oxide + Zinc
Calcium Carbonate + potassium
Will they react?
Put a tick or cross on the tile if a reaction will happen.
Extraction of Metals
Ores
Most metals are found naturally in rocks called ………………………….. They are in
………………………….., chemically bonded to other elements. Some ………………………….. metals can be
found as …………………………... They are called ………………………….. metals.
The Reactivity Series
Metals above carbon in the reactivity series must be extracted using …………………………...
Metals less reactive than carbon can be extracted from their ores by ………………………….. using carbon, coke or charcoal.
Platinum, gold, silver and copper can occur ………………………….. and do not need to be extracted.
In order to extract a metal, the ore or compound of the metal must undergo
………………………….. to free the metal.
Reduction is the ………………………….. of oxygen or ………………………….. of oxygen from a compound.
Generally speaking the method of extraction depends upon the metals position in the reactivity series.
Metal …………………………..
+
carbon
à
metal
+
carbon …………………………..
Reduction and Oxidation
lead oxide
+ …………………………..
lead +
…………………………..…………………………..
2PbO(s) + C(s)
2Pb(s) + CO2(g)
The blast furnace
Match the raw materials to their uses.
Iron Ore
Is made from coal and is nearly pure carbon.
Limestone
(Usually haematite) is mainly iron oxide, Fe2O3,
Hot air
Coke
mixed with sand.
Blasted in at the bottom of the furnace to provide
heat and oxygen.
Is a common rock consisting mainly of calcium carbonate, CaCO3.
Lesson aim:
To research rusting in iron and steel
Information;
 “Corrosion” means when a metal is “eaten away” or
“weakened” by a chemical reaction.
 The most common form of corrosion in iron objects is rust.
 Iron (and steel) is the only metal that rusts.
Your task: Use the internet and text books to research rusting.
1. State what rusting is.
2. State the substances needed for rusting.
3. Why can steel rust?
Write the word and chemical equations for the process of rusting.
Explain the economic problems associated with rust.
List ways in which we can prevent iron from rusting.
Explain how each method, mentioned above, prevents rust.