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Metallic and Giant Covelant Bonding (Properties (Generally high melting…
Metallic and Giant Covelant Bonding
[METALLIC] Made as a giant metallic lattice structure
Giant Lattice= repeating pattern of atoms in a fixed structure
Metal atoms lose the electrons in the outermost shell to become a positive metal ion. The lost electrons are delocalised, which means they're free to move. The positively charged metal ions are held together packed closely together in a sea of delocalised electrons
Properties
Generally high melting point
Due to strong metallic bonding - the number of delocalised electrons per atom affects the melting point, the more there are the stronger the bonding and therefore the higher the melting point. E.g Mg2+ has two delocalised electrons per atoms, so will have a higher melting point than Na+ which only has one
The size of the metal ion as well as the lattice struture also affects the melting point
Malleable (can be bent into a shape)
This is due the fact there are no bonds holding the atoms together, so the atoms can easily slide over each other in the lattice structure
Good thermal Conductors
The delocalised electrons can pass kinetic energy to each other
Good electrical conductors
The delocalised electrons are free to move so can carry a current. Any impurities can reduce the electrical conductivity as there are less electrons to carry the charge
Insoluble (except in liquid metals)
Due to the strength of the metallic bonds
[COVELANT] Made from covalent bonds (where atoms share electrons) but in massive lattices - containing billions of atoms)
E.g. Carbon and Silicon
Properties
Very high melting points
lots of strong bonds need to be broken to melt - lot of energy required
Very hard
due to strong bonds in lattice arrangement
Good thermal Conductors
vibrations easily travel through stiff laticces
Insoluble
The covelant bonds cause the atoms to be more attracted to the neighbouring atoms than the molecules in the solvents
Can't conduct electricity
There are no charged ions or free electrons
