Studied by 1 person
state the properties of metals
malleable
electrical conductor
high melting/boiling point
ductile
shiny
dense
explain why metals are malleable
layers of metal cations can slide over each when force is applied
explain why metals are electrical conductors
metal layers contain sea of delocalised electrons
which are capable of moving and carrying charge
explain why metals have high melting/boiling points
large amount of energy needed to overcome
strong electrostatic forces of attraction
between metal cations and delocalised electrons
explain the differences between metals and non-metals
conductivity - metals can conduct and most non-metals can’t
boiling/melting points - metals have high melting points and most non-metals have low melting points
explain what a displacement reaction is
redox reaction
as both oxidation and reduction occur
state what a redox reaction is
a reaction where both oxidation (loss of electrons) and reduction (gain of electrons) occurs
state the metal reactivity series
potassium
sodium
calcium
magnesium
aluminium
carbon
zinc
iron
tin
lead
hydrogen
copper
silver
gold
platinum
state which metals react with water
potassium
sodium
calcium
state which metals react with acids
magnesium
aluminium
zinc
iron
tin
lead
recall how and where metals are found
extracted from ores in the earth’s crust
unreactive metals are found as unreacted elements
explain what oxidation is
gain of oxygen
loss of electrons
explain what reduction is
loss of oxygen
gain of electrons
recall what the extraction of metals involves
reduction of metal ores
state which metals are extracted from their ores by heating with carbon
zinc
iron
tin
lead
state which metals are extracted from their ores by electrolysis
potassium
sodium
calcium
magnesium
aluminium
explain why specific metals are extracted from their ores by heating with carbon based on their relative reactivity
zinc, iron, tin and lead are extracted using carbon
as they are less reactive than carbon
so the carbon can displace the metal from its ore
explain why specific metals are extracted from their ores by heating with carbon based on cost of extraction
this process requires less energy for extraction
keeping costs lower
explain why specific metals are extracted from their ores by electrolysis based on their relative reactivity
potassium, sodium, calcium, magnesium and aluminium are extracted using electrolysis
as they are more reactive than carbon
and therefore carbon cannot displace it from its ore
evaluate bioleaching as a method of metal extraction
avoids significant environmental damage caused by traditional methods including mining
process is very slow
can extract metals from mining waste
evaluate phyto mining as a method of metal extraction
avoids significant environmental damage caused by traditional methods including mining
process is very slow
can extract metals from mining waste
recall what oxidation of metals causes
corrosion
explain how the exclusion of oxygen prevents the rusting of iron
iron, water and oxygen react together to make hydrated iron oxide
iron oxide is rust
without oxygen, iron oxide could not be formed
explain how the exclusion of water prevents the rusting of iron
iron, water and oxygen react together to make hydrated iron oxide
iron oxide is rust
without water, iron oxide could not be formed
explain how sacrificial protection prevents the rusting of iron
if iron is in contact with a more reactive metal, the more reactive metal will oxidise
this means the iron will not rust as it won’t oxidise
evaluate the advantages of recycling metals
less mining for raw materials - preserves environment
preserves supply of raw materials
more economical to recycle instead of mine for new material as it takes up less energy
explain how electroplating can be used to improve the appearance of metal objects
electroplating is when a metal object is covered in a thin layer of another metal
this thin layer of metal can be used to improve the appearance of the object
e.g. make it shiny
explain how electroplating can be used to improve the resistance to corrosion of metal objects
electroplating is when a metal object is covered in a thin layer of another metal
the layer of metal provides a physical barrier to oxygen and water, ensuring iron oxide (rust) cannot form
explain why converting pure metals into alloys increases the strength of the metal
an alloy is when a metal is added to a pure metal in order to increase strength
the added metal disrupts the regular structure and arrangement of metal cations and delocalised electrons
this means the layers of metal cannot slide over each other, increasing the strength of the metal
explain why iron is alloyed with other metals to produce alloy steels
pure iron is a very soft material
when another metal is added, steel alloy is created
the steel alloy is stronger than the pure iron
state the properties of aluminium
corrosion resistant
good conductor
strong (when alloyed)
low density
explain how the properties of aluminium are related to its uses
corrosion resistant - cans and aircrafts
good conductor - pots, pans and power cables
strong (alloy form) - pots and pans
state the properties of copper
malleable
ductile
good conductor
corrosion resistant
attractive colour
explain how the properties of copper are related to its uses
attractive colour - decorative goods
corrosion resistant - water pipes
ductile - electrical wires
state the properties of gold
malleable
attractive colour
corrosion resistant
shiny
explain how the properties of gold are related to its uses
malleable - jewellery
attractive colour - jewellery
shiny - jewellery
corrosion resistant - jewellery
state the properties of magnalium
strong
low density
corrosion resistant
explain how the properties of magnalium are related to its uses
corrosion resistant - aircraft parts
strong - aircraft parts
state the properties of brass
corrosion resistant
malleable
ductile
good conductor
explain how the properties of brass are related to its uses
corrosion resistant - plumbing fittings
good conductor - electrical wires
Note
Flashcard