Metallic Structures Flashcards
What are metal properties all due to?
The sea of free electrons.
What do metals consist of?
Giant structures.
What do metallic bonds involve?
All important ‘free electrons’.
What do free electrons produce?
All properties of metals.
What is another way of saying free electrons?
Delocalised electrons.
Where do delocalised electrons come from?
Outer shell of every metal atom in the structure.
Electrons are free to move where?
Through the whole structure.
Metals are good…
Conductors of heat and electricity.
What do electrons also hold?
Atoms together in a regular structure.
There is strong forces of what? between what?
Electrostatic attraction.
Positive metal ions and the negative electrons.
Layers of atoms can do what?
Slide over each other.
Layers of atoms sliding over each other allows metals to do what?
Bent and be shaped.
What are alloys harder than?
Pure metals.
Pure metals often aren’t quite right for what?
Certain jobs.
What do scientists do to pure metals?
Mix 2 or more metals together, creating alloy.
Different elements have…
Different sized atoms.
What happens when a metal is mixed with a pure metal?
New metal atoms distort the layers of metal atoms.
Making it more difficult to slide over each other.
How can you identify the structure of a substance?
By its properties.
Most substances behave as either what 4 things?
Giant ionic.
Simple molecular.
Giant covalent.
Giant metallic.
What properties does a simple molecular have?
Low melting/boiling point.
Not a good electrical conductor.
What properties does a giant ionic have?
High melting/boiling point.
Good electrical conductor(molten).
What properties does a giant covalent have?
High melting/boiling point.
Not a good electrical conductor.
What properties does a giant metallic have?
High melting/boiling point.
Good electrical conductor.
