This key facts covers Key Facts to Memorise within Metallic Bonding for GCSE Chemistry. Revise Metallic Bonding in Bonding & Structure for GCSE Chemistry with 20 exam-style questions and 20 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 6 of 11 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 6 of 11
Practice
20 questions
Recall
20 flashcards
📌 Key Facts to Memorise
- Metallic bonding = electrostatic attraction between positive metal ions and delocalised electrons
- Delocalised electrons = electrons free to move throughout the metal (not fixed to one atom)
- Conducts electricity — delocalised electrons can move and carry charge
- Conducts heat — electrons transfer thermal energy rapidly
- Malleable — can be hammered into shape; layers slide, electrons move to maintain bond
- Ductile — can be drawn into wires; same reason as malleable
- High melting point — strong attraction between ions and electron sea
- Can conduct in solid state — unlike ionic compounds!
Quick Check: Predict which would have the higher melting point: sodium (Na) or magnesium (Mg). Give a reason.
Magnesium has the higher melting point. Magnesium atoms release 2 electrons each into the delocalised sea, creating Mg²⁺ ions — higher charge than Na⁺ (1 electron). This creates stronger electrostatic attraction between the ions and the electron sea, requiring more energy to overcome.