Metallic Bonding

Question 1

Why does metallic bonding occur?

Answer 1

Single atoms of metal don’t exist, so they combine in large lattices of atoms that are joined together by chemical bonds (metallic bonds)

Question 2

Explain delocalised electrons

Answer 2

When atoms form a metallic lattice, the valence electrons become delocalised, which means they can move/flow within the lattice.
The atoms become positive ions (cations) and the electrons join the “sea” of electrons that forms around the metal ions

Question 2

How are the metallic lattices held together?

Answer 2

Everything is held together by the attraction of the constantly moving negative electrons and the positive metal ions = metallic bonding

Question 2

Link the properties of metal to metallic bonding

Answer 2

• Shiny because the delocalised electrons reflect light
• High melting and boiling points because the metallic bonds are very strong, so it takes a lot of energy to break them
• Malleable because the lattice can move along and the delocalised electrons can hold the ions together
• Good conductors of heat and electricity because the delocalised electrons have a negative charge and can move

Question 3

Alloys

Answer 3

Metals can be mixed with small amounts of another substance (usually another metal or carbon) to form an alloy