chapter 3 Flashcards
Metallic ions
electrons are delocalised and free moving around the cations.
They act as a cement holding the cations in place.
Strong electrostatic force of attraction between cations and delocalised electrons
Properties of metal
- high boiling and melting points
- good conductors of electricty
- good confuctors of heat
- high density
- malleable
- ductile
- lustrous (shiny)
- tensile strength
- low ionisation energy
Why do metals have a high boiling point
The forces between the particles is strong
Metals and conductivity of electricity
delocalised electrons allow current to flow
metals are malleable and ductile
the ability of the atoms to roll over each other into new positions without breaking the metallic bond. lattice is not disrupted
why are metals deniser
The particles are closely packed in a metal
why are metals a good conductor for heat
There must be a way of quickly transferring
energy throughout a metal object.
why are metals lustrous
Free electrons are present, so metals can reflect
light and appear shiny.
metals tend to react by losing a electron, why
metals typically have relatively low ionization energies
do metallic elements have a high or low electronegativity
low
reactivity of metals
most reactive as you go down and increase when you go across
How can it conduct heat
when heat is supplied the kinetic energy of the electron will increase.
Since they will be able to move quickly they bump into each other increasing the number of collision therefore transferring energy throughout the metal.
density
metal lattice are tightly packed therefore will have a high tensile strength
conduct electricity
delocalised electrons are able to move and transfer current.
