What Is Metallic Bonding and How Does It Enable Conductivity?

TL;DR

Metallic bonding occurs when valence electrons are delocalized and shared among many metal atoms, allowing them to move freely and conduct electricity. This delocalization also accounts for other properties such as malleability, ductility, and thermal conductivity, while metals can appear shiny due to their luster.

Transcript

in this video we're going to talk about metallic bonding and why metals conduct electricity metallic bonds are basically covalent bonds the atoms in the metal share electrons so let me give you a visual illustration so let's say these are some atoms in a piece of metal now the metal cations are surrounded by valence electrons and what you need to u... Read More

Key Insights

• 🥶 Metallic bonding involves the delocalization of valence electrons in metals, allowing for the free movement of electrons and electrical conductivity.
• 🤘 Metals conduct electricity because of the presence of delocalized electrons, which can move throughout the metal.
• ✋ Metals possess physical properties like malleability, ductility, and high thermal conductivity due to the mobility of valence electrons.
• 🤘 The delocalization of electrons in metals differentiates metallic bonding from covalent bonding in molecules.
• 🤘 The movement of electrons in metals is random and not in a specific direction, unless influenced by an electric field.
• 🤘 The shiny appearance of metals is attributed to their luster.

Summary & Key Takeaways

• Metallic bonding involves the sharing of electrons between metal atoms, resulting in the delocalization of valence electrons that are free to move.

• The movement of the delocalized electrons gives metals their ability to conduct electricity.

• Metals possess other physical properties like malleability, ductility, thermal conductivity, and luster.