5. Metallic bonding

Question 1

what is metallic bonding?

Answer 1

a strong electrostatic attraction between cations and delocalised electrons

Question 2

physical properties: melting and boiling points.

Answer 2

-number of delocalised electrons per atom afftect the melting and boiling points.
-the more there are the stronger the bonding will be and the higher the melting and boiling points.

e.g. Mg2+ has two delocalised electrons per atom compared to Na+ which only has one and so Mg2+ has a higher melting and boiling point.

• the size of the metal ion and the lattice structure also affect melting and boiling points, a smaller ionic radius will hold the delocalised electrons closer to the nuclei.

Question 3

physical properties: Conductivity.

Answer 3

-the delocalised electrons can pass kinetic energy to eachother,making metals good thermal conductors.
-metals are good electrical conductors because the delocalised electrons can carry a charge.

Question 4

physical properties: solubility.

Answer 4

Metals are insoluble, except in liquid metals, because of the strength of the metallic bonds.

Question 5

physical properties: ability to be shaped.

Answer 5

metals are malleable and ductile- no bonds holding specific ions together, the metal ions can slide over each other when the structure is pulled.