1.3.3 Metallic Bonding

• In metallic bonding, the valence electrons are delocalized
• Metallic bonding involves the sharing of valence electrons between metal atoms.

  False
• Match the property of metallic structures with its explanation:

  Regular lattice arrangement ↔️ Atoms form repeating patterns

  Delocalized electrons ↔️ Free-moving electrons contribute to conductivity

  Strength of bonds ↔️ Requires energy to disrupt, high melting points
• How is metallic bonding different from ionic and covalent bonding in terms of electron behavior?

  Electrons are delocalized
• Metal atoms form repeating patterns for stability in a regular lattice arrangement
• In the electron sea model, the valence electrons of metal atoms are delocalized
• What allows metals to have good electrical and thermal conductivity?

  Delocalized electrons
• Metallic bonding involves a delocalized electron sea, whereas ionic and covalent bonding have more localized electron configurations.


  True
• What is metallic bonding?

  Bonding between metal atoms
• How is metallic bonding different from ionic and covalent bonding?

  Electrons are delocalized
• The "sea of electrons" in metals is responsible for their high conductivity.


  True
• Why are metals good conductors of electricity and heat according to the electron sea model?

  Delocalized electrons move freely
• Valence electrons in metals are delocalized and form a "sea of electrons."

  True
• Metals have high melting and boiling points due to the strength of metallic bonds.

  True
• Ionic and covalent bonding involve more localized electrons compared to metallic bonding.
• Which type of bonding results in good electrical and thermal conductivity?

  Metallic Bonding
• Match the property of metallic bonding with its explanation:

  High melting/boiling points ↔️ Strong metallic bonds require energy to break

  Good conductors of electricity and heat ↔️ Delocalized electrons move through the metal
• Metal atoms are arranged in a regular lattice
• In the electron sea model, valence electrons are attached to individual atoms.

  False
• What type of structure do metal atoms form in metals?

  Regular lattice
• The delocalized electron sea in metals allows them to conduct electricity and heat efficiently.


  True
• Match the type of bonding with its electron configuration:

  Metallic Bonding ↔️ Delocalized valence electrons

  Ionic Bonding ↔️ Localized transfer of electrons

  Covalent Bonding ↔️ Shared localized pairs of electrons
• Delocalized electrons in metallic bonding allow metals to conduct electricity and heat.


  True
• Why do metals have high melting and boiling points in terms of metallic bonding?

  Strong metallic bonds
• What does the electron sea model describe?

  Metallic bonding structure
• Delocalized electrons in metals contribute to high conductivity
• What property do delocalized electrons contribute to in metals?

  High conductivity
• Why do metals have high melting and boiling points according to the electron sea model?

  Strong metallic bonds
• Ionic and covalent bonds involve localized electrons and do not exhibit the same conductive properties as metallic bonds.


  True
• Ionic bonds result in high melting and boiling points due to the strong electrostatic forces between ions.