Metallic bonding (Edexcel IGCSE Chemistry (Modular): Unit 2): Flashcards

A metallic bond is the strong force of attraction between positive metal ions and a 'sea' of delocalised electrons in a metal lattice.

False.

In a metal, the outer electrons leave their original atoms and become delocalised, meaning they can move freely throughout the metal lattice.

Metals have high melting and boiling points because of the strong electrostatic attraction between the positive metal ions and the delocalised electrons. A large amount of energy is needed to overcome these forces.

In a metal, atoms lose their outer electrons and become positively charged metal ions. The released electrons are said to be delocalised and form a 'sea of electrons'.

Delocalised electrons are electrons that have been released from their atoms and are free to move throughout the metal lattice, not belonging to any specific atom.

Metals can conduct electricity because they have delocalised electrons that are free to move through the lattice. These electrons carry charge when a potential difference is applied.

True.

The atoms (or ions) in a metal are arranged in regular layers. When a force is applied, these layers can slide over each other, allowing the metal to be bent or hammered into shape.

Complete the table linking each property of metals to its explanation.

Saying a metal is malleable means it can be hammered or bent into shape without breaking. This is possible because the layers of atoms or ions in the lattice can slide over each other when a force is applied.