Properties of Metallic Bonds

• Why do metals conduct heat well?

  Because of the free movement of electrons
• What is created by metallic bonds?

  A "sea" of delocalized electrons
• What forms metallic bonds?

  Metal atoms sharing their outermost electrons
• What is the role of delocalized electrons in metallic bonds?

  They create a shared sea among metal ions
• What are positive ions formed from metal atoms called?

  Cations
• What happens to valence electrons in metal atoms?

  They easily lose to form positive ions
• How do metals differ from non-metals at room temperature?

  Metals are typically solid at room temperature
• How does the Electron Sea Model differ from the ionic bonding model?

  • Ionic bonding involves the complete transfer of electrons between atoms, forming positively and negatively charged ions.
  • Metallic bonding in the Electron Sea Model involves the delocalization of valence electrons, forming a "sea" of electrons around the positively charged metal ions.
• How does the Electron Sea Model explain the malleability and ductility of metals?

  • The delocalized electrons in the "electron sea" allow the positively charged metal ions to slide past each other easily, enabling metals to be shaped and formed.
  • This explains the high malleability and ductility of metals.
• What binds metal ions together in a solid state?

  Metallic bonds involving delocalized electrons
• Why do metals conduct electricity well?

  Due to the movement of delocalized electrons
• What surrounds the positive metal ions in the electron sea model?

  A sea of delocalized electrons
• How do delocalized electrons behave in metallic bonds?

  They move freely between positive metal ions
• If a molecule has delocalized electrons, how would this affect its chemical properties compared to a molecule with localized electrons?

  Delocalized electrons make the molecule more stable and reactive
• What do metals form in the electron sea model?

  A lattice of positive metal ions
• How do delocalized electrons behave in the electron sea model?

  They can move freely between the ions
• What is the significance of delocalized electrons in a molecule?

  • Delocalized electrons are not confined to a single bond or atom
  • They can move freely throughout the molecule
  • This allows for increased stability and reactivity
• What is the electron sea model in metals?

  • Metals form a lattice of positive ions
  • Surrounded by delocalized electrons
  • Electrons move freely, binding the structure
• What is the key concept behind the Electron Sea Model?

  • In metallic bonding, the valence electrons of metal atoms are delocalized and form an "electron sea" around the positively charged metal ions.
  • This allows the electrons to move freely and conduct electricity.
• What role do delocalized electrons play in the structure of metals?

  They create a network that binds the structure
• What do metal atoms have in their outermost shell?

  One or more valence electrons
• What does the continuous electron cloud allow for?

  Free movement of electrons between all atoms
• How do metal ions and delocalized electrons interact?

  They attract each other through electrostatic forces
• What type of bonding is represented by the arrangement of positive metal ions and delocalised electrons?

  • Metallic bonding
• Why aren't electrons in metals stuck in one place?

  They form an "electron sea" that allows movement
• According to the image, what are the negatively charged particles shown in the structure?

  Delocalised electrons
• How does the Electron Sea Model explain the high electrical conductivity of metals?

  The delocalized electrons in the "electron sea" can move freely and conduct electricity
• What type of charge do metal ions have?

  Positive
• What allows electrons to move freely in the metal structure?

  The attraction to fixed metal ions
• What is the relationship between metal ions and delocalized electrons in metals?

  • Metal ions are positively charged
  • Delocalized electrons form an electron sea
  • They attract each other through electrostatic forces
  • This attraction maintains the structure of metals
• How are delocalized electrons formed?

  By merging parallel p-orbitals from multiple atoms
• What are delocalized electrons?

  Electrons that can move freely between atoms
• What type of charge does the electron sea have?

  Negative
• What effect does the attraction between metal ions and delocalized electrons have on the structure?

  It keeps metal ions in fixed positions
• What is represented by the "electron sea" in metals?

  • A shared cloud of free-flowing electrons
  • Electrons move freely between multiple atoms
  • Contributes to metallic properties like conductivity
• How do metals conduct electricity?

  Free electrons carry charge
• What is the "sea of delocalised electrons" in the image?

  • The free-flowing electrons in the metal that are not bound to individual atoms
  • These electrons can move freely and conduct electricity through the metal
• What does it mean for a metal to be ductile?

  It can be drawn into wires
• What is the significance of the image showing layers of positive ions in metals?

  • Illustrates how layers slide over each other
  • Explains why metals are bendable and workable
• Why are metals considered malleable?

  Layers can slide past each other