2.7 Metallic bonding Flashcards
What is metallic bonding?
Metallic bonding is the electrostatic attraction between the positive metal ions (cations) and a ‘sea’ of delocalised electrons in a giant metallic lattice.
How are metals structured in terms of metallic bonding?
Metals consist of giant structures of atoms arranged in a regular pattern. The outer electrons of metal atoms are delocalised and free to move through the whole structure.
Why are metals good conductors of electricity?
Metals are good conductors of electricity because their delocalised electrons are free to move throughout the structure, allowing the flow of electric charge.
Why are metals malleable and ductile?
Metals are malleable and ductile because the layers of atoms can slide over each other due to the strong metallic bonds, allowing metals to be bent and shaped.
Why are alloys harder than pure metals?
Alloys are harder than pure metals because the different sizes of atoms in alloys distort the regular layers, preventing the layers from sliding past each other easily.
Why do metals have high melting and boiling points?
Metals have high melting and boiling points because of the strong electrostatic attraction between the delocalised electrons and the positive metal ions, which requires a lot of energy to overcome.
