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Title: 1. O Level Chemistry Metals Notes PDF 2.Reactivity Series Cheat Sheet for Students 3.Metal Reactions Summary for Exam Preparation 4.Download PowerPoint on Extraction of Metals 5.Comparison of Properties of Metals and Non-Metals 6.Rusting of Iron Expe
Description: This PDF provides comprehensive notes on metals tailored for O Level Chemistry students. It begins by outlining the general physical properties of metals and contrasts them with non-metals, highlighting characteristics like conductivity, malleability, ductility, and ion formation. The document then details various metal reactions—specifically with acids, cold water, steam, and oxygen—along with balanced chemical equations and key observations such as fizzing, temperature change, and color or state changes. The concept of reactivity is clearly explained using the reactivity series, supported by tables and common mnemonics to aid memorization. Displacement reactions are discussed in depth, demonstrating how more reactive metals displace less reactive ones from salt solutions. The uses of common metals like aluminium and copper are linked directly to their properties, and the section on alloys explains their formation, advantages, and examples like brass and stainless steel. Rusting of iron is covered with experimental setups, observations, and methods of prevention using barrier methods and sacrificial protection. Galvanising is explained as both a physical barrier and an electrochemical defense using zinc. The final sections cover the extraction of metals, describing methods such as electrolysis and blast furnace reduction, with full chemical equations and process explanations. The extraction of aluminium from bauxite and iron from hematite are presented in detail with supporting diagrams and electrode reactions. Overall, the notes serve as a complete, exam-focused summary ideal for revision and concept reinforcement.
Description: This PDF provides comprehensive notes on metals tailored for O Level Chemistry students. It begins by outlining the general physical properties of metals and contrasts them with non-metals, highlighting characteristics like conductivity, malleability, ductility, and ion formation. The document then details various metal reactions—specifically with acids, cold water, steam, and oxygen—along with balanced chemical equations and key observations such as fizzing, temperature change, and color or state changes. The concept of reactivity is clearly explained using the reactivity series, supported by tables and common mnemonics to aid memorization. Displacement reactions are discussed in depth, demonstrating how more reactive metals displace less reactive ones from salt solutions. The uses of common metals like aluminium and copper are linked directly to their properties, and the section on alloys explains their formation, advantages, and examples like brass and stainless steel. Rusting of iron is covered with experimental setups, observations, and methods of prevention using barrier methods and sacrificial protection. Galvanising is explained as both a physical barrier and an electrochemical defense using zinc. The final sections cover the extraction of metals, describing methods such as electrolysis and blast furnace reduction, with full chemical equations and process explanations. The extraction of aluminium from bauxite and iron from hematite are presented in detail with supporting diagrams and electrode reactions. Overall, the notes serve as a complete, exam-focused summary ideal for revision and concept reinforcement.
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Metals
O levels Chemistry(5070)
Learning Outcomes
• Properties of Metals and Non-Metals
...
• Uses Of Metals
...
• Reactivity series
...
• Extraction Of Metals
...
• When acids and metals react , the hydrogen atom in the
acid is replaced by the metal atom to produce a salt and
hydrogen gas,for example iron:
metal + acid → salt + hydrogen
Fe (s) + 2HCl (aq) → FeCl2 (aq) + H2 (g)
• Metals below Hydrogen in reactivity series can not react
with acids because they are not able to displace
hydrogen from solution
Metal reaction with Acid
•
•
•
•
•
•
•
•
•
Observations During the Reaction:
Fizzing/Bubbling: Due to the release of hydrogen gas
...
Metal dissolves gradually: As it reacts to form a salt
...
Important Notes:
Not all metals react with acids
...
More reactive metals (like Mg, Zn, and Fe) react quickly and vigorously
...
Flames or sparks may be seen, depending on the metal
...
Properties of Metal Oxides:
Usually basic in nature
...
• Some are amphoteric (e
...
, aluminum oxide)
...
Metals that react with cold water:
Potassium (K)
Sodium (Na)
Calcium (Ca)
General reaction:
Metal + Cold water → Metal hydroxide +Hydrogen gas
2Na+2H2O→2NaOH+H2↑
Metal reaction with Steam
• Some moderately reactive metals
(that do not react with cold water) can react with steam
...
• General reaction:
• Metal+Steam→Metal oxide+Hydrogen gas
• Example:
• Mg+H2O(g)→MgO+H2↑
Willingness of Metals to react
with Cold water/Steam
Metal
Cold Water
Steam
Potassium
Reacts violently
Reacts violently
Sodium
Reacts violently
Reacts violently
Calcium
Reacts steadily
Reacts violently
Magnesium
No reaction
Reacts
Zinc
No reaction
Reacts slowly
Iron
No reaction
Reacts slowly
Copper/Silver
No reaction
No reaction
Key Observation made during
reaction of metals with cold
water/steam
Metal
Water Type
Observations
Potassium
Cold water
Violent fizzing, lilac
flame, floats, alkaline
solution
Sodium
Cold water
Fizzing, melts, may
catch fire, yellow flame
Cold water
Steady fizzing, cloudy
solution (Ca(OH)₂), sinks
then rises
Magnesium
Steam
Bright white flame,
white solid (MgO), fast
reaction
Zinc
Steam
Yellow (hot) → white
(cool) ZnO, slow fizzing
Iron
Steam
Black solid (Fe₃O₄), slow
fizzing, red-hot iron
Calcium
Uses
of
metals
Describe the uses of metals in terms of their physical properties, including:
Aluminum in the manufacture of aircraft because
of its low density
Aluminum in the manufacture of overhead
electrical cables because of its low density and
good electrical conductivity
Copper in electrical wiring because of its good
electrical conductivity and ductility
Aluminum in food containers because of its
resistance to corrosion
Properties & Uses of Alloys
• An alloy is a mixture of two or more metals or metal with
a non-metal such as carbon
...
• These enhanced properties can make alloys more useful
than pure metals
Structure of Alloy
Common alloys and their uses
• Brass is an alloy of copper and zinc and is much stronger than
either metal
• It is used in musical instruments, ornaments and door knobs
• Stainless steel is a mixture of iron and other elements, for
example, chromium, nickel and carbon
• It is used in cutlery because of its hardness and resistance to
corrosion
• Alloys of iron with tungsten are extremely hard and resistant
to high temperatures
• Alloys of iron mixed with chromium or nickel are resistant to
corrosion
• Aluminum is mixed with copper, manganese and silicon for
aircraft body production as the alloy is stronger but still has a
low density
Explaining the Properties of
Alloys
• Alloys contain atoms of different sizes, which distorts the
normally regular arrangements of atoms in metals
• This makes it more difficult for the layers to slide over
each other, so alloys are usually much harder than the
pure metal
Common Misconception about
Alloys
Alloys are mixtures of substances,
they are not chemically combined and
an alloy is not a compound
...
• Based on these reactions a reactivity series of metals
can be produced
...
• The non-metals hydrogen and carbon are also included
in the reactivity series as they are used to extract metals
from their oxides
Table Of Metal Reactions part1
Table Of Metal Reactions part2
Deduced reactivity Series
Po
ta
ssi
u
m
So
di
u
m
MOST
REACTIVE
Ca M
lli ag
ng ne
siu
m
Al Ca Zi
u
rb nc
mi on
nu
m
Ir Ti
on n
Le
ad
Hy Co Sil
dr pp ve
og er r
en
Go
ld
LEAST
REACTIVE
Helpful Mnemonics
Please Stop CALling ME A CAReless
Zebra Instead Try LEArning How
COPPER Saves GOLD
Displacement Reaction And
Reactivity Series
• Reactivity of Metals: Basic Idea
• More reactive metals lose electrons more easily to form
positive ions (cations)
...
• Displacement Reaction Rule
• A more reactive metal can displace a less reactive metal
ion from its salt solution
...
However
in part C dilute hydrochloric acid does not react with
copper, silver and gold because Hydrogen can not be
displaced during reaction
...
Aluminium is actually a reactive metal, but
...
• 4Al+3O2→2Al2O3
• This oxide layer is:
•
Tightly bonded
•
Hard and tough
•
Insoluble in water
•
Chemically unreactive
What the Oxide Layer Does:
• It acts as a protective barrier between the aluminium and the environment
...
• As a result, aluminium appears to be unreactive, even though it is highly reactive just
beneath the surface
...
• Oxygen and water must be present for rust to occur
...
If any other metal
oxidises in air causing the metal to
break down, you should say that the
metal has corroded
...
Explanation Using Reactivity Series:
• More reactive metals lose electrons more easily (they are oxidized more readily)
...
• Reactive metal→ 𝑚𝑒𝑡𝑎𝑙
oxidizing (rusting)
...
Zinc in Galvanising: Barrier +
Sacrificial Protection
• Galvanizing: Galvanizing is the process of coating iron or steel with a layer of zinc
...
Barrier Method:
• The zinc coating physically blocks air and moisture from reaching the iron
...
• As long as the coating is intact, iron is safe
...
Sacrificial Protection (if coating is damaged):
• If the zinc coating is scratched or damaged, exposing the iron:
• Zinc is more reactive than iron (higher in reactivity series)
...
• Zinc acts as a sacrificial anode
...
Summary
Protection Method
Description
Zinc Role
Barrier Method
Prevents water/oxygen
contact
Coating blocks exposure
Sacrificial Protection
Zinc corrodes in place of
iron
Donates electrons to
protect iron
Extraction Of Metals
• The Earth’s crust contains metals and metal compounds such
as gold, copper, iron oxide and aluminium oxide
• Useful metals are often chemically combined with other
substances forming ores
• A metal ore is a rock that contains enough of the metal to
make it worthwhile extracting
• They have to be extracted from their ores through processes
such as electrolysis, using a blast furnace or by reacting
with more reactive material
• In many cases the ore is an oxide of the metal, therefore the
extraction of these metals is a reduction process since oxygen
is being removed
• Common examples of oxide ores are iron and aluminium ores
which are called hematite and bauxite respectively
Extraction Of Metals
• Unreactive metals do not have to be extracted chemically as
they are often found as the uncombined element
• This occurs as they do not easily react with other substances
due to their chemical stability
• They are known as native metals and examples
include gold and platinum which can both be mined directly
from the Earth’s crust
• The position of the metal on the reactivity series influences
the method of extraction
• Those metals placed higher up on the series (above carbon)
have to be extracted using electrolysis
• Metals lower down on the series can be extracted by heating
with carbon
Reactivity Series and extraction of
Metals
The Extraction Method Depends on the Position of a Metal in the Reactivity
Series
Extraction of Iron from
Hematite
• Iron is extracted in a large container called a blast
furnace from its ore, hematite
• Modern blast furnaces produce approximately 10,000
tonnes of iron per day
Diagram Of Blast Furnace
The diagram is rotated 90degree anti clockwise to give better view
...
• The calcium carbonate in the limestone thermally decomposes to
form calcium oxide
calcium carbonate → calcium oxide + carbon dioxide
• The calcium oxide formed reacts with the silicon dioxide, which is an
impurity in the iron ore, to form calcium silicate
• This melts and collects as a molten slag floating on top of the
molten iron, which is tapped off separately
calcium oxide + silicon dioxide → calcium silicate
Equations for Extraction of Iron
from Hematite
You must learn each of these equations!
Extraction of Aluminium from
Bauxite
• Aluminium is a reactive metal, above carbon in the
reactivity series
• Its main ore, is bauxite, which contains aluminium oxide
• Aluminium is higher in the reactivity series than carbon,
so it cannot be extracted by reduction using carbon
• Instead, aluminium is extracted by electrolysis
Electrolysis of Bauxite to extract
Aluminum
You should study it carefully
Extraction of Aluminium from
Bauxite
• Bauxite is first purified to produce aluminium oxide, Al2O3
• Aluminium oxide is then dissolved in molten cryolite
• This is because aluminium oxide has a melting point of
over 2000°C which would use a lot of energy and be
very expensive
• The resulting mixture has a lower melting point without
interfering with the reaction The mixture is placed in an
electrolysis cell, made from steel, lined with graphite
• The graphite lining acts as the negative electrode, with
several large graphite blocks as the positive electrodes
At the cathode (negative
electrode)
At the cathode (negative electrode):
• Aluminium ions gain electrons (reduction)
• Molten aluminium forms at the bottom of the cell
• The molten aluminium is siphoned off from time to time
and fresh aluminium oxide is added to the cell
+ 3
→ Al
At the anode (positive
electrode)
At the anode (positive electrode):
• Oxide ions lose electrons (oxidation)
• Oxygen is produced at the anode:
2
→ O2 + 4
• The overall equation for the reaction is:
2Al2O3 → 4Al + 3O2
• The carbon in the graphite anodes reacts with the oxygen
produced to produce
C(s) + O2(g) → CO2(g)
• As a result, the anode wears away and has to be replaced
regularly
• A lot of electricity is required for this process of extraction,
this is a major expense
Thank You!
Title: 1. O Level Chemistry Metals Notes PDF 2.Reactivity Series Cheat Sheet for Students 3.Metal Reactions Summary for Exam Preparation 4.Download PowerPoint on Extraction of Metals 5.Comparison of Properties of Metals and Non-Metals 6.Rusting of Iron Expe
Description: This PDF provides comprehensive notes on metals tailored for O Level Chemistry students. It begins by outlining the general physical properties of metals and contrasts them with non-metals, highlighting characteristics like conductivity, malleability, ductility, and ion formation. The document then details various metal reactions—specifically with acids, cold water, steam, and oxygen—along with balanced chemical equations and key observations such as fizzing, temperature change, and color or state changes. The concept of reactivity is clearly explained using the reactivity series, supported by tables and common mnemonics to aid memorization. Displacement reactions are discussed in depth, demonstrating how more reactive metals displace less reactive ones from salt solutions. The uses of common metals like aluminium and copper are linked directly to their properties, and the section on alloys explains their formation, advantages, and examples like brass and stainless steel. Rusting of iron is covered with experimental setups, observations, and methods of prevention using barrier methods and sacrificial protection. Galvanising is explained as both a physical barrier and an electrochemical defense using zinc. The final sections cover the extraction of metals, describing methods such as electrolysis and blast furnace reduction, with full chemical equations and process explanations. The extraction of aluminium from bauxite and iron from hematite are presented in detail with supporting diagrams and electrode reactions. Overall, the notes serve as a complete, exam-focused summary ideal for revision and concept reinforcement.
Description: This PDF provides comprehensive notes on metals tailored for O Level Chemistry students. It begins by outlining the general physical properties of metals and contrasts them with non-metals, highlighting characteristics like conductivity, malleability, ductility, and ion formation. The document then details various metal reactions—specifically with acids, cold water, steam, and oxygen—along with balanced chemical equations and key observations such as fizzing, temperature change, and color or state changes. The concept of reactivity is clearly explained using the reactivity series, supported by tables and common mnemonics to aid memorization. Displacement reactions are discussed in depth, demonstrating how more reactive metals displace less reactive ones from salt solutions. The uses of common metals like aluminium and copper are linked directly to their properties, and the section on alloys explains their formation, advantages, and examples like brass and stainless steel. Rusting of iron is covered with experimental setups, observations, and methods of prevention using barrier methods and sacrificial protection. Galvanising is explained as both a physical barrier and an electrochemical defense using zinc. The final sections cover the extraction of metals, describing methods such as electrolysis and blast furnace reduction, with full chemical equations and process explanations. The extraction of aluminium from bauxite and iron from hematite are presented in detail with supporting diagrams and electrode reactions. Overall, the notes serve as a complete, exam-focused summary ideal for revision and concept reinforcement.