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.