Describe the key features of metallic bonding that explain the high electrical conductivity of metals.
Understand the Problem
The question asks for an explanation of how metallic bonding contributes to the high electrical conductivity observed in metals. This requires understanding the nature of metallic bonding and how it facilitates the movement of electrons, which is essential for electrical conductivity.
Answer
Delocalized electrons in metallic bonds can freely move and carry electrical charge, leading to high conductivity.
Metallic bonding involves a 'sea' of delocalized electrons that are free to move throughout the metal's structure. These mobile electrons can easily carry an electrical charge, resulting in high electrical conductivity.
Answer for screen readers
Metallic bonding involves a 'sea' of delocalized electrons that are free to move throughout the metal's structure. These mobile electrons can easily carry an electrical charge, resulting in high electrical conductivity.
More Information
Metals are also known for their high thermal conductivity due to the ability of these electrons to transfer heat. The 'sea of electrons' model helps explain many of the unique properties of metals.
Tips
A common mistake is to confuse metallic bonding with ionic or covalent bonding. Metallic bonding involves a 'sea' of delocalized electrons, whereas ionic bonding involves the transfer of electrons and covalent bonding involves the sharing of electrons between specific atoms.
Sources
- Metallic Bonding - Chemistry LibreTexts - chem.libretexts.org
- Properties, Examples, & Explanation of Metallic Bonds - BYJU'S - byjus.com
- Metallic Bonding and the Electron Sea Model, Electrical Conductivity - youtube.com
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