Structure 2.3
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Is the process of removing valence electrons endothermic or exothermic
Endothermic, however the energy required is relatively low when compared to non-metals.
Metallic bonding
the electrostatic attraction between a lattice of cations and delocalised electrons
Electrical conductivity
The ability to carry electrical charge. Due to the movement of charged particles.
Why are metals good conductors
The delocalised electrons are free to carry the charge. They have low electrical resistance.
Does a chemical change take place when a metal conducts electricity
no
Melting points of metals
They have high melting points which suggests that metallic bonding is quite strong.
What does the strength of a metallic bond depend on?
The number of delocalised electrons, the charge on the cation and the radius of the cation.
How does the size of the cation change the strength of a metallic bond?
The larger the cation the weaker the bond bc the attraction between the cations and electrons decreases.
Strength of a metallic bond down a group
Decreases
Strength of a metallic bond across a period
Increases, as the charge on the cation is increasing and the radius of it is decreasing
Malleable
Can be shaped under pressure
Ductile
Can be drawn into a wire
Why are metals malleable and ductile?
The layers of cations can slide over each other without breaking. The movement of the delocalised electrons is non-directional and random throughout the lattice
Why are metals shiny?
Delocalised electrons in metal crystal structures reflect light
Why are metals good thermal conductors?
The delocalised electrons are free to move and closely packed ions enable efficient transfer of thermal energy.