Metallic Bonding Flashcards

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What is metallic bonding?

Metallic bonding is the strong attraction between positive metal ions and a ‘sea’ of delocalised electrons.

What happens to the outer electrons of metal atoms when metallic bonding forms?

The atoms lose their outer electrons to become positive ions. The lost electrons become delocalised and can move freely through the metal.

How are the particles arranged in a metal with metallic bonding?

The metal has a giant lattice of positive ions in a regular, closely packed pattern, surrounded by delocalised electrons.

Why do metals usually have high melting points?

The metallic bonds are strong, so a lot of energy is needed to break the attractions between the ions and the delocalised electrons.

Why can metals conduct electricity?

Metals can conduct electricity because their delocalised electrons are free to move and carry charge through the whole structure.

Why can metals conduct heat?

Delocalised electrons move and transfer energy, and the closely packed ions pass vibrations on quickly, so heat flows through the metal.

Why are most pure metals malleable (easy to bend and shape)?

The metal ions are in layers that can slide over each other while the delocalised electrons still hold the structure together.

What does ‘delocalised electrons’ mean in metallic bonding?

They are electrons that are not tied to one atom. They can move anywhere through the metal lattice.

What is the overall charge of a piece of metal, and why?

It is neutral because the total positive charge of the ions is balanced by the total negative charge of the delocalised electrons.

In metallic bonding, are there small molecules or a giant structure?

There is a giant structure made of many metal ions and delocalised electrons, not separate molecules.