4.5 Metallic Bonding Flashcards
Characteristic of metals
Low ionisation energies
Few valency electrons
When they form ionic bonds become positively charged
What is a metallic bond?
The electrostatic attraction between the lattice of cations and delocalised electrons
What does the strength of a bond depend on?
Number of delocalised electrons
Charge on a cation
Radius of cation
What does the strength of a metallic bond depend on?
The strength of a metallic bond decreases down a group because the size of the cation increases which reduces the attraction between the delocalised electrons and the positive charges
Why are metals good electrical conductors?
Delocalised electrons which are highly mobile that can move through the substance and carry charge
Can be used in electrical circuits
Why are metals good thermal conductors?
They have delocalised electrons which can carry charge and closely packed ions which are key for conduction
Can be used for cooking utensils
Why are metals mobile and ductile?
They have delocalised electrons which are non-directional, therefore the bonds remain intact under pressure
Can be used in wires and cables
Why do metals have high melting points?
They have strong metallic bonds
Can be used for high speed tools
Why are metals shiny?
They have delocalised electrons in the crystal which reflect light
Can be used in ornamental structures
How is an alloy formed?
As the mixture of a metal solicits the different ions are scattered orthotic the lattice and bound by delocalised electrons. This is possible because of the non-directional nature of the electrons
Where are metals found in the periodic table?
Left side
