3.1.3.3 Metallic Bonding
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What is the structure of a metal?
A lattice of positive ions in a sea of delocalised electrons Ions sit within the dimples of the recent layer, called a close structure
What does the strength of a metallic bond depend on?
Charge of ion: greater the ion, the stronger the electrostatic attraction Size of ion: smaller the ion, closer the electrons are to the nucleus so the stronger the bond
In a metallic bond, how many electrons are lost?
It depends on how many are lost by each atom
What are the properties of metals? (No explanation)
Conduct electricity Have high thermal conductivity Malleable High melting/boiling points Ductile Mostly insoluble
Why do metals conduct electricity?
Delocalised electrons can move through the structure so they’re good conductors of electricity
Why do metals have high thermal conductivity?
Because energy is spread via the ions vibrating
Why are metals malleable and ductile?
Because the lattice can shift along the layers
Why do metals have high melting/boiling points?
Because of the giant structure and the strong attractive force
Why are alloys stronger than pure metals?
The particles are different sizes which disrupts the layes and stops them from sliding over eachother
What causes an electrostatic force of attraction?
Opposing charges
Is a metal held together by chemical bonds?
No
Why is solid carbon strong?
Because of the macromolecular structure