Topic 4 - Metals Flashcards
Properties of metals
- Conductivity
- Shiny
- Malleable
- Solid (mostly)
- High melting point and boiling point
- High density
- low ionisation energies
- low electronegativities
Cations
Metals, lose electrons so they have a positive charge
Transition metals
harder, higher density, higher melting points, strong magnetic properties, bright coloured
Alloys
- metals are mixed with small amounts of another substance usually another metal or carbon. They are melted together, mixed and then allowed to cool. An alloy is harder and melts at a lower temperature than a pure metal.
- Steel = Transition metals + carbon
- Copper is one of the few metals that s mainly used in pure form.
In what order do you write the number and charge of an ion
Number then charge
Metals are usually hard and tend to have high boiling points
the forces between the particles must be strong
Metals are usually hard and tend to have high boiling points
the forces between the particles must be strong
Metals conduct electricity in the solid state and in the modern liquid state
metals have charged particles that are free to move
metals are malleable and ductile
the attractive forces between the particles must be stronger than the repulsive forces between the particles when the layers of particles are moved
Metals generally have high densities
The particles are closely packed in a metal
Metals are good conductors of heat
there must be a way of quickly transferring energy throughout a metal object
Metals are lustrous or reflective
free electrons are present, so metals can reflect light and appear shiny
Metals tend to react by losing electrons
electrons must be relatively easily removed from metal atoms.
The metallic bonding model must include:
charged particles that are free to move and conduct electricity
strong forces of attraction between particles throughout the metal structure
some electrons that are relatively easily removed
A metal crystal:
a region of solid where the particles
are arranged regularly.
Lattice:
Tightly packed regular arrangement.
The reactivity of a metal depends
on how easily electrons can be removed from their atoms.
Metals can react with
water, oxygen, acids
what is the trend of reactivity to water, oxygen and acids
Group 1, group 2, transition metals
Metals are normally more reactive with
acids than with water. More metals react with acids and
the reactions tend to be more energetic.
Gold and platinum are essentially unreactive and are described as
inert.
The Reactivity Series
- Please
- Send
- Charlie’s
- Monkey
- And
- Zebras
- In
- Lead
- Cages
- Securely
- Guarded
Potassium
Sodium
Calcium
Magnesium
Aluminium
zinc
iron
lead
copper
Silver
gold
potassium highest, gold lowest
Atoms of metals
are generally larger than the atoms of non-metallic elements within a period.
have lower effective nuclear charge (core charge)
have lower ionisation energy (it takes less energy to remove electrons from an outer shell)
Metals tend to lose their outer shell electrons to form positive ions, called ions
The reactivity of a metal depends on how…
easily electrons can be removed from its atoms
Circular economy
a continuous cycle where the extracted material is reused after initial use, waste is minimum and can be recycled, or re-purposed
sustainable
most metals in the earths crust form…
oxides, sulphides or silicates
when the concentration of mineral in rock is high enough to be extracted it is called…
an ore
Mining
the first step in metal production from ores
involves the removal of surface vegetation, soil and bedrock to reach the ore deposits. Underground mining - digging a vertical shafts into the group then tunnels are dug to reach the ore
in-situ leaching, injecting solutions into holes to resolve the minerals and then pumping them to the surface where the minerals can be recovered, cheaper.
Ore processing
the second step in metal production from ores
processed to separate the valuable minerals from the waste rock.
metal extraction
the thirds step in metal production from ores
the method to extract the metals changes based on the reactivity. All metals can be extracted by passing an electric current through the liquid compound, electrolysis. Uses lots of energy. expensive, only used for very reactive elements
iron can be extracted by heating it at a high temperature with carbon, and smelting.
environmental issues
land, water, air, biodiversity.
Linear Economies
you use it then dispose of it. take make dispose
metal recycling…
save up to 20 times the energy needed to extract metals
avoids using metals as landfill
reduces CO2 emmisons
Recycling process
collection
preparation for recovery
smelting
purification
haematite
Fe 2 O 3
extraction of iron
materials used = iron ore, coke, limestone and air
To extract iron, blast furnace
- different reactions in different temperature zones
part 1
- coke reacts with oxygen to produce carbon dioxide which reacts with carbon to form carbon monoxide
Part 2
- carbon monoxide reacts with iron ore
- carbon monoxide + iron oxide = iron + carbon dioxide
limestone
- limestone breaks down, to form calcium oxide and carbon dioxide with reacts with the unwanted materials to form slag
collection of iron
- holes at the base of the furnace are opened and the molten iron and slag are drained out and separated.
