Edexcel International A Level Chemistry
Edexcel International A Level Chemistry Metallic Bonding Exam Questions
Free Edexcel International A Level Chemistry exam questions for Metallic Bonding, with a mark scheme for every pack. Covers metallic bonding, delocalised electrons, properties of metals, giant lattice structures, diamond, graphite, graphene and comparing structure types.
Metallic Bonding exam questions
1 question pack of real past exam questions, each with its mark scheme. Do not stop after a few: answer as many as you can without notes, then mark every answer with the mark scheme. The more questions you do, the more quickly you will spot how examiners ask about each idea.
StemUp mark scheme flashcards
A-Level Chemistry Flashcards for 2027 Onwards
Every answer is written in mark scheme wording, so you learn exactly what examiners give marks for. Then test yourself with the questions on this page.
From £10.99View flashcards
About Edexcel International A Level Chemistry Metallic Bonding
Metallic bonding in Unit 1 of Edexcel International A Level Chemistry explains the structure and properties of metals using a lattice of positive ions in a sea of delocalised electrons. It sits alongside ionic and covalent bonding so that you can compare the four structure types: giant metallic, giant ionic, giant covalent and simple molecular. You also study giant covalent carbon allotropes such as diamond, graphite and graphene. Examiners commonly ask you to define metallic bonding, explain electrical conductivity and malleability, account for trends in metal melting temperatures, and predict properties from a given structure.
What you need to know
- Metallic bonding Metallic bonding is the strong electrostatic attraction between a lattice of positive metal ions and a sea of delocalised electrons.
- Electrical conductivity Metals conduct electricity in solid and liquid states because delocalised electrons can move through the structure when a potential difference is applied.
- Malleability and ductility Layers of metal ions can slide over each other while the delocalised electrons keep holding the structure together, so metals can be hammered into shape or drawn into wires.
- Melting temperature trends Melting temperature increases from Na to Mg to Al because the ions have a larger charge, there are more delocalised electrons per atom and the ions are smaller, so the attraction is stronger.
- Giant covalent structures Diamond has each carbon bonded to four others tetrahedrally, so it is very hard and does not conduct. Graphite has layers of hexagonal rings with one delocalised electron per carbon, so it conducts along the layers and the layers slide. Graphene is a single layer of graphite.
- Comparing structures Use melting temperature, solubility and conductivity data to identify whether a substance is giant metallic, giant ionic, giant covalent or simple molecular.
Common mistakes in Metallic Bonding
- Writing that metals contain free electrons without mentioning the electrostatic attraction to positive ions. The definition needs both.
- Calling metal particles atoms in the lattice. The lattice is made of positive ions.
- Saying graphite conducts because of free ions. It conducts because of delocalised electrons.
- Explaining graphite's softness by weak covalent bonds. The covalent bonds within layers are strong; the forces between layers are weak.
- Explaining melting temperature trends with charge alone. Mention the number of delocalised electrons per atom and the ionic radius as well.
Try three Metallic Bonding exam-style questions
1. Describe the structure and bonding in a metal such as magnesium. (2 marks)
Show the mark scheme answer
Lattice of positive ions (Mg2+); surrounded by delocalised electrons; strong electrostatic attraction between them.
2. Explain why aluminium has a higher melting temperature than sodium. (3 marks)
Show the mark scheme answer
Al3+ has a higher charge than Na+ and is smaller; aluminium provides three delocalised electrons per atom compared with one for sodium; so the metallic bonding is stronger and needs more energy to break.
3. Explain why graphite conducts electricity but diamond does not. (2 marks)
Show the mark scheme answer
In graphite each carbon forms three covalent bonds, leaving one delocalised electron per atom that can move along the layers; in diamond all four outer electrons are used in covalent bonds so there are no mobile charge carriers.
Metallic Bonding FAQs
What does Edexcel International A Level Chemistry Metallic bonding cover?
It covers the metallic bonding model, the properties of metals and how they arise, melting temperature trends, giant covalent structures of carbon and how to compare different structure types.
Which unit is Metallic bonding examined in?
Metallic bonding is part of Unit 1, and the structure and properties comparisons often appear in longer bonding questions.
How do I answer 'explain the properties' questions on structures?
Always link the property to the particles present, the type of bonding or force, and whether it is strong or weak, then say whether charged particles are free to move.
