properties of metals: malleability, electrical conductivity

• What is the role of delocalized electrons in metals?

  They move freely between the ions
• How does the arrangement of atoms and electrons in metallic bonding contribute to the properties of metals?

  • Delocalized electrons allow metals to be malleable and ductile
  • Delocalized electrons allow metals to conduct electricity and heat
  • Positive metal ions held together by delocalized electrons give metals high melting/boiling points
• What does malleability mean in metals?

  Ability to be hammered or rolled into sheets
• What are the two main components of metallic bonding shown in the image?

  Metal ions and delocalized electrons
• Why does the ability to transport charge make metals ideal for electrical applications?

  It allows efficient conduction of electricity
• What happens to positive ions in metals when they slide past each other?

  They can slide past each other easily
• Why are metals considered excellent conductors of electricity?

  They have delocalized electrons that move freely
• How does the metallic bonding in copper differ from the metallic bonding in sodium?

  Copper has more delocalized electrons per atom than sodium, making its metallic bonds stronger
• What is the role of delocalized electrons in metals?

  They facilitate the movement of electric charge
• How are positive metal ions arranged in metals?

  In a regular lattice structure
• How does the structure of metals relate to their malleability?

  • Regular structure allows movement
  • Free electrons facilitate sliding of ions
  • Prevents cracking when deformed
• Why are metals ductile?

  Delocalized electrons allow metal ions to slide
• What happens to electrons when an electric field is applied?

  They transport charge through the material
• What are the key features of metallic bonding?

  • Metal atoms lose their valence electrons
  • Valence electrons become delocalized and shared among all atoms
  • Positive metal ions are held together by the sea of delocalized electrons
  • Allows metals to conduct electricity and heat
• What happens to metal ions when a metal is deformed?

  They slide over each other like cards
• What are the components of metals?

  Positive metal ions and delocalized electrons
• Why can metals be drawn into wires?

  Delocalized electrons allow metal ions to slide
• How do metal ions behave under pressure?

  They slide past each other
• What prevents metals from cracking when deformed?

  Regular structure and free electrons
• How does ductility differ from malleability in metals?

  • Ductility: Metals can be drawn into wires
  • Malleability: Metals can be hammered into sheets
  • Ductility involves vertical alignment, malleability involves horizontal stacking
• What role do delocalized electrons play in metal malleability?

  They hold the ions together during movement
• What is the reason metals are malleable?

  Their lattice structure allows ions to slide
• What is the relationship between metal ions and delocalized electrons in malleability?

  • Metal ions can slide past each other
  • Delocalized electrons act as a "glue"
  • This allows for movement without breaking bonds
• How can you visualize the movement of electrons in metals when an electric field is applied?

  • Electrons act like vehicles on a highway
  • They transport charge through the metal
• What happens to metal ions during ductility?

  They slide over each other and align
• What are the key features of metal structure?

  • Regular lattice structure of positive metal ions
  • Free-moving delocalized electrons
  • Positive ions can slide past each other
• What does ductility mean in metals?

  Ability to be drawn into thin wires
• How do delocalized electrons contribute to malleability?

  They allow layers of metal ions to slide
• Why can metals carry electrical current effectively?

  They have delocalized electrons that move freely
• How do delocalized electrons contribute to electrical conductivity in metals?

  They move freely between metal ions
• What is the visual representation of metal ions aligning to form a wire?

  Image shows metal ions aligning
• If a metal is heated, how would the metallic bonding be affected?

  The delocalized electrons would gain more kinetic energy, weakening the metallic bonds
• In what way do ductility and malleability relate to the movement of metal ions?

  Ductility involves vertical movement, malleability horizontal
• What are metals excellent conductors of?

  Electricity
• What is the significance of delocalized electrons in metals?

  • Allow layers of metal ions to slide
  • Contribute to malleability
  • Prevent cracking during deformation
• Why can metals be hammered or rolled into thin sheets?

  Delocalized electrons allow metal ions to slide
• How do delocalized electrons contribute to ductility?

  They enable layers of metal ions to align
• How does the alignment of metal ions contribute to ductility?

  It allows them to be drawn into thin wires
• What property of metals allows them to be drawn into wires?

  Ductility
• What does electrical conductivity mean?

  A metal can easily carry electrical current