Metallic Bonding
This lesson covers:
- How metallic bonding works in metals
- The differences between alloys and pure metals
tight / metallic / special / ionic / covalent
Metals can bind to non-metals via bonding, whereby particles with opposite charges are attracted to each other.
Non-metals can bind to other non-metals via bonding, whereby electrons are shared.
Metal atoms can bind to other metals using bonding.
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Which of the following are properties of metals?
(Select all that apply)
Low strength
High strength
Malleable
High melting points
Unable to conduct electricity
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positive / negative / localised / delocalised
In metallic bonding, each metal atom becomes an ion with a charge.
It does this by giving up its outer shell electrons.
These electrons are said to be '', and are shared across all the ions in the structure.
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heat / electricity / thermal / chemical
In metallic bonding, electrons are delocalised from the lattice of metal ions.
These electrons can carry charge, and so metal acts as a conductor of .
These electrons can also carry energy, meaning metals are good conductors of heat.
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Metals are malleable. What does this mean?
They are brittle and are easily cut
They conduct heat and electricity
They are shiny in texture
They can be bent or hammered into shape
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Which of these describes an alloy?
A metal combined with one or more other elements
A non-metal combined with one or more other elements
A pure metal
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lower / higher / charges / sizes / slide / jump
Alloys tend to have a strength than pure metals.
This is because the atoms/ions of the different elements are different , which disrupts the regular layered structure and so means the layers can no longer over one another.
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Which of these is an alloy?
Iron
Steel
Vanadium
Water
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