Metallic bonding and delocalised electrons

• How does the strength of metallic bonding compare to ionic and covalent bonding?

  Metallic bonding is strong, ionic is very strong
• What forms the "sea" of electrons in metallic bonding?

  Electrons moving freely between positive ions
• What are the characteristics of ionic bonding?

  • Electrons transferred between ions
  • Involves metal and non-metal ions
  • Strength: Very Strong
• What are delocalized electrons?

  Electrons that can move freely in a lattice
• Which metals commonly form BCC structures?

  Fe, Cr, Nb
• What are the positive ions in metals arranged in?

  Regular lattice pattern
• What do metallic crystals form through the arrangement of metal ions?

  Different crystal structures
• What is the arrangement of atoms in BCC structure?

  Body-centered cubic
• What are the three common metallic lattice types?

  • BCC (Body-centered cubic)
  • FCC (Face-centered cubic)
  • Hexagonal (Close-packed layers)
• What are the characteristics of metallic bonding compared to other types of bonding?

  • Electrons shared among all ions
  • Involves metal ions
  • Strength: Strong
• Which metals commonly form hexagonal structures?

  Ti, Mg, Zn
• Which metals commonly form FCC structures?

  Al, Cu, Ag
• What is metallic bonding compared to?

  Sharing a candy in a group
• How does the delocalized structure affect the stability and reactivity of the molecule?

  Delocalization increases stability and reduces reactivity
• What is the arrangement of atoms in hexagonal structure?

  Close-packed layers
• What is the arrangement of atoms in FCC structure?

  Face-centered cubic
• What are the two molecular structures shown in the image?

  6 p-orbitals and delocalized
• What is the mathematical representation of the delocalized structure shown?

  $H_3C-CH_3$
• How do metallic structures affect metal atoms?

  • Create tightly-packed arrangements
  • Allow sharing of outer electrons
• What are the characteristics of covalent bonding?

  • Electrons shared between atoms
  • Involves non-metal atoms
  • Strength: Varies
• What are the key differences between the 6 p-orbitals and delocalized structures?

  • 6 p-orbitals show localized electrons, delocalized shows shared electrons
  • 6 p-orbitals are less stable, delocalized is more stable
  • 6 p-orbitals are more reactive, delocalized is less reactive
• What creates the strong attraction in metallic bonding?

  The shared sea of electrons among ions
• What is the difference between 6 p-orbitals and delocalized structures?

  • 6 p-orbitals show localized electrons in individual atomic orbitals
  • Delocalized structure shows electrons shared across multiple atoms in a molecule
• What is the analogy used to describe delocalized electrons in metals?

  • They are like a sea of electrons
  • Not fixed to particular atoms
  • Can flow freely throughout the lattice
• Why does iron have a "giant structure" according to the image?

  Because iron has metallic bonding between its ions and delocalized electrons
• How do delocalized electrons explain the conductivity of metals?

  • Electrons can move freely between ions
  • They carry electric charge
• How do atoms behave in metallic bonding?

  They lose electrons and become positive ions
• What does the image of delocalized electrons illustrate?

  How electrons are shared across the metal structure
• How do delocalized electrons contribute to the malleability of metals?

  • Metal layers can slide over each other
  • Bonding is maintained through shared electrons
• What are delocalized electrons in metals?

  Electrons that move freely between ions
• How do delocalized electrons behave in a metallic lattice?

  They flow between positive metal ions
• What is the role of regular arrangement in metal strength?

  It holds ions together through strong attraction
• What is the significance of delocalized electrons in a metal structure?

  They allow movement in all directions
• What other metals also form 2+ ions like iron according to the image?

  Magnesium
• What type of bonding is represented in the image?

  Metallic bonding
• What are the key properties of metallic bonding?

  • Delocalized electrons shared between metal ions
  • High electrical and thermal conductivity
  • Malleable and ductile
  • High melting and boiling points
• What are the key properties of metals explained by delocalized electrons?

  • Conductivity: Free movement of electrons
  • Malleability: Sliding of metal layers
  • Strength: Regular arrangement and strong attraction
• What enables metals' characteristic behavior?

  Free flow of delocalized electrons