Question

Why do non-metals not have delocalised electrons, whilst metals do have delocalised electrons? I understand that delocalised electrons is defined as "electrons that are not bound in place to a single atom or a single bond between two atoms", and I think that delocalised electrons are necessary for the bonding of two elements. If I am correct about my latter statement, shouldn’t both metals and non-metals have delocalised electrons (because they form ionic bonds)?

Answer 1

Metals have delocalized electrons because their outer energy level electrons can drift from one atom to another, creating a sea of mobile valence electrons. Non-metals, on the other hand, have covalent bonds and the electrons are localized in these bonds.

Step-by-step explanation:

Metals have delocalized electrons because the electrons in the outer energy levels of a metal are mobile and capable of drifting from one metal atom to another.

This creates a sea of mobile valence electrons surrounding the positively charged metal ions. The delocalized electrons are not bound in place and are free to move throughout the metal lattice.

On the other hand, non-metals do not have delocalized electrons because their atomic structures are different. Nonmetals have covalent bonds and individual molecules. The electrons in nonmetals are localized in these covalent bonds and are not free to move throughout the entire substance.