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Chemistry

GCSE · Edexcel

QuestionsFlashcards

Group 1
- Group 1 (Alkali Metals)
  6
- Group 1: Reactivity & Electronic Configurations
  6
Group 7
Group 0

Qualitative Analysis: Tests for Ions
Hydrocarbons
Polymers
Alcohols & Carboxylic Acids
Bulk & Surface Properties of Matter Including Nanoparticles
- Nanoparticles
  7
- Ceramics, Polymers, Composites & Metals
  5

Metals Flashcards

All 6 cards in this deck

Describe the structure and bonding in a metal.: A giant lattice of positive metal ions surrounded by a sea of delocalised electrons.
Why do metals conduct electricity?: They contain delocalised (free) electrons that can move through the structure.
Why are metals malleable?: The layers of metal ions can slide over each other without breaking the metallic bonding.
Why do metals have high melting points?: There are strong forces of attraction between the metal ions and the delocalised electrons, needing lots of energy to break.
State the typical physical properties of most metals.: Shiny solids with high melting points, high density and good electrical conductivity.
True or false? Most non-metals have low boiling points and conduct electricity poorly.: True. Most non-metals are simple molecular with weak intermolecular forces and no free charged particles.