C2.2.3 Metallic Bonding

• The structure of metals involves a regular lattice arrangement of positive metal ions
• What type of attraction holds metal ions and delocalized electrons together in metallic bonding?

  Electrostatic
• Steps to describe the structure of metals

  1️⃣ Regular lattice arrangement of positive metal ions

  2️⃣ Surrounded by a sea of delocalized electrons

  3️⃣ Electrons move freely throughout the lattice
• The delocalized electrons in metals enable high electrical and thermal conductivity.

  True
• The structure of metals involves a regular lattice arrangement of positive metal ions
• The sea of delocalized electrons in metals allows them to conduct heat efficiently.


  True
• What does the Electron Sea Model describe?

  Structure and bonding in metals
• Mobile delocalized electrons in metals carry electric current.
• What are the key features of metallic bonding?

  Regular lattice, delocalized electrons, electrostatic attraction
• Metals are good conductors of heat because delocalized electrons transfer energy.
• Metals have high thermal conductivity because delocalized electrons can efficiently transfer heat energy.


  True
• Why are metals malleable and ductile?

  Regular lattice can slide
• What is the arrangement of positive metal ions in metallic bonding?

  Regular lattice arrangement
• Delocalized electrons in metallic bonding are attracted to positive metal ions.


  True
• The Electron Sea Model describes metals as having a sea of delocalized electrons.
• Why do metals have high electrical conductivity?

  Delocalized electrons can move freely
• Match the bonding type with its description:

  Metallic Bonding ↔️ Regular lattice of positive ions with delocalized electrons

  Ionic Bonding ↔️ Crystal lattice of positive and negative ions

  Covalent Bonding ↔️ Sharing of electrons between atoms
• Metals are used as heat sinks due to their high thermal conductivity.
• Delocalized electrons in metals move freely throughout the lattice.


  True
• Metals have high electrical and thermal conductivity due to mobile electrons
• The electrostatic attraction between positive metal ions and delocalized electrons is called metallic bonding.
• What is the bonding in metals called?

  Metallic bonding
• Why are metals good conductors of electricity?

  Mobile delocalized electrons
• In the electron sea model, positive metal ions are surrounded by delocalized electrons.
• Delocalized electrons in metals are attached to individual atoms.

  False
• Steps to explain the Electron Sea Model

  1️⃣ Delocalized electrons move freely

  2️⃣ Positive metal ions are arranged in a lattice

  3️⃣ Electrical conductivity results from electron mobility

  4️⃣ Thermal conductivity is due to heat transfer by electrons
• Delocalized electrons in metals move freely, resulting in high electrical conductivity.


  True
• What is the role of positive metal ions in the Electron Sea Model?

  Arrange in a regular pattern
• Metals have high electrical conductivity because delocalized electrons in the metallic lattice can move freely.
• Metallic bonding involves a regular lattice of positive metal ions and delocalized electrons.

  True
• Metals have high electrical and thermal conductivity due to their mobile electrons
• What holds the positive metal ions in a metal structure together?

  Electrostatic attraction
• Delocalized electrons in the Electron Sea Model are attached to specific atoms.

  False
• Metals are malleable and ductile because the lattice of metal ions can slide past each other.
• What property of metals makes them suitable for electrical wiring?

  High electrical conductivity