Metallic Bonding Flashcards
Metallic Bonding
A lattice of closely packed positive ions in a sea of delocalised electrons
Metal elements structures
Giant Metallic Lattice Structure
Describe structure of metallic bonding
The outermost shell of electrons of a metal atom is delocalised- the electrons are free to move about the metal leaving a positive metal ion.
The positive metal ions are attracted to the delocalised negative electrons
Explain why metals have high melting points
Because of the strong electrostatic attractions between the positive metal ions and the delocalised sea of electrons
Explain why the number of delocalised electrons per atom affects the melting point
The more delocalised electrons there are, the stronger the bonding will be and the higher the melting point
Explain why metals are good thermal conductors
The delocalised electrons can pass kinetic energy to each other
Explain why metals are good electrical conductors
The delocalised electrons can move and carry a current
Explain why metals are insoluble
Because of the strength of the metallic bonds
except in liquid metals
