Metallic bonds are the force of attraction between valence electrons and the metal ions. They are strong, allowing metals to conduct electricity and heat.
Think of metallic bonds like a sea full of fish (the electrons) that move freely around islands (the metal ions). This allows for the high conductivity seen in metals.
Conductivity: The measure of a material's ability to conduct electricity. Metals have high conductivity due to their metallic bonding.
Malleability: The property of a substance that allows it to be hammered or rolled into sheets without breaking. This is another characteristic feature of metals due to their unique bonding.
Delocalized Electrons: These are electrons in a molecule, ion or solid metal that are not associated with a single atom or one covalent bond. In metallic bonds, these delocalized electrons allow for properties such as electrical conductivity and malleability.
Study guides for the entire semester
200k practice questions
Glossary of 50k key terms - memorize important vocab
© 2024 Fiveable Inc. All rights reserved.
AP® and SAT® are trademarks registered by the College Board, which is not affiliated with, and does not endorse this website.