Metals are useful in everyday life but must be extracted from metal ores through mining. Ores like iron ore and bauxite are the natural sources of metals like iron and aluminum. Extracting metals involves removing the metal from the ore through chemical or electrolytic processes. Some metals are more reactive than others based on their placement in the reactivity series, determining which metals can displace others from their compounds and oxides. Metals have several distinctive physical properties including being solid, malleable, ductile, and good conductors of heat and electricity.
Revision Slides for AQA A-Level Chemistry on the Group Two Elements. Designed for the new Exam Series of June 2017, but relevant for all series and exam boards.
Physical properties of metals and non-metals. Explains different properties of Metals and Non-metals slide by slide(with various exceptions examples) . Example: luster, ductility, heat and electricity conductivity, etc.
Online learning to understand the concept and application of chemicals on the topic of salt. These slides were uploaded to help students understand the basic concepts of chemistry. Independent study in Freestyle.com
Revision Slides for AQA A-Level Chemistry on the Group Two Elements. Designed for the new Exam Series of June 2017, but relevant for all series and exam boards.
Physical properties of metals and non-metals. Explains different properties of Metals and Non-metals slide by slide(with various exceptions examples) . Example: luster, ductility, heat and electricity conductivity, etc.
Online learning to understand the concept and application of chemicals on the topic of salt. These slides were uploaded to help students understand the basic concepts of chemistry. Independent study in Freestyle.com
This slide was prepared by me for I was given project on the course applied electro-chemistry. Am student at Addis Ababa university institute of technology , addis ababa Ethiopia
In this ppt everything is available in a sequence and in a very easy way.... It will be very useful to you for your board exams ...
Many ppt also will be available very soon
Metals and Non-Metals form a fundamental classification of elements, playing a pivotal role in understanding the diverse world of chemistry. In Class 10, students delve into the distinct characteristics, properties, and reactions that define these two broad categories. Metals, with their conductivity and malleability, stand in stark contrast to the non-metals, which exhibit varying physical and chemical traits. These notes provide a concise exploration of the essential attributes of metals and non-metals, offering a foundational understanding for students to navigate the complexities of chemical interactions and classifications in the realm of science.
2. Metals are very useful in our everyday lives. Ores
are naturally occurring rocks that provide an
economic starting point for the manufacture of
metals. Iron ore is used to make iron and steel.
Copper can be easily extracted but copper-rich
ores are becoming scarce so new methods of
extracting copper are being developed. Aluminium
and titanium are useful metals but are expensive
to produce. Metals can be mixed together to make
alloys.
3. Students should be able to:
■ consider and evaluate the social, economic
and environmental impacts of exploiting metal
ores, of using metals and of recycling metals
■ evaluate the benefits, drawbacks and risks of
using metals as structural materials.
4. Key words
Ores
Bauxite
Haematite
Metal
Economical
Extract
Purified
Reduction
Reactivity
Electrolysis
Phytomining
Bioleaching
Displacement
Blast furnace
Alloy
Mixtures
Compounds
Steel
Transition metals
Density
Corrosion
5. a) Ores contain enough metal to make it economical
to extract the metal. The economics of extraction may
change over time.
Two common ores are bauxite (aluminium ore, Al2O3)
and haematite (iron ore Fe2O3)
Bauxite Three different types of
haematite
6. b) Ores are mined and may be concentrated
before the metal is extracted and purified.
c) Unreactive metals such as gold are found
in the Earth as the metal itself but most metals
are found as compounds that require
chemical reactions to extract the metal.
7. Question: Are some metals more reactive
than others?
Hypothesis: Some metals are more
reactive than others
Zn Mg Pb Cu
Hydrochloric acid
8. VARIABLES
Independent
What we changed
Dependent
What’s changed as a result
Controlled
What’s kept the same
9. VARIABLES
Independent
What we changed
The type of metal
Dependent
What’s changed as a result
The rate of reaction:
How long it takes to
dissolve
How many bubbles per
minute or second
Controlled
What’s kept the same
The shape and size of the
metal
The acid – strength, type
and amount
The time
10.
11. The Reactivity Series
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Zinc
Iron
Tin
Lead
Copper
Silver
Gold
Platinum
Most reactive
Least reactive
Carbon
Hydrogen
As well as the above metals you may also find two non metals in the series.
12. Since most metal ores contain the metal oxide, then it is obvious
that oxygen must be removed from the ore in order to produce
the metal itself.
The removal of oxygen from a compound is called reduction.
This is opposite from the addition of oxygen to a substance
which is called oxidation.
Metal oxide – oxygen metal
REDUCTION
Metal + oxygen metal oxide
OXIDATION
The removal of oxygen from the metal ore can be done in a number of ways – it
depends upon the metal’s position in the reactivity series.
13. 3. For each of these – state if the metal will
reduce the oxide
a. Aluminium v magnesium oxide
b. Magnesium oxide v iron
c. Iron oxide v aluminium
d. Carbon v aluminium oxide
e. Iron oxide v carbon
14. 4. Metal X will reduce aluminium
oxide but not calcium oxide.
Use the resistivity series to
identify X.
5. Metal Y will reduce copper
oxide but not iron oxide – which
possible metals could it be?
15. Since carbon is more
reactive than iron,
then it can be used to
reduce iron oxide to
iron. This is done in
the Blast Furnace.
16. Carbon is less reactive than aluminium so cannot
be used to reduce aluminium oxide to aluminium.
Another process called electrolysis must be used.
