2.3.1 Structure of Metals

• What is metallic bonding defined as?

  Electrostatic attraction between positive ions and a sea of electrons
• In metallic bonding, metal atoms lose valence electrons to become positive ions
• Delocalized electrons in metallic bonding provide electrical conductivity.
• What is the key property of metals due to metallic bonding?

  High electrical conductivity
• What does the electron sea model describe?

  Metallic bonding as an electrostatic attraction
• In the electron sea model, the outer valence electrons of metal atoms become delocalized
• The electron sea allows metals to have high electrical conductivity.
• Match the bonding type with its characteristics:

  Ionic ↔️ Localized electron arrangement

  Covalent ↔️ Shared electron pairs

  Metallic ↔️ Delocalized electron sea
• What is the arrangement of metal atoms in a lattice structure?

  Highly ordered three-dimensional arrangement
• Metal atoms in a lattice are densely packed in arrangements like FCC, BCC, or HCP
• Metals have high electrical conductivity because of delocalized electrons.
• What is the definition of metallic bonding?

  Electrostatic attraction between ions and electrons
• In metallic bonding, metal atoms lose valence electrons to become positive ions
• What is the role of delocalized electrons in metallic bonding?

  High electrical conductivity
• The metallic lattice structure consists of a regular arrangement of metal ions.
• The electron sea model describes metallic bonding as an electrostatic attraction between positive metal ions and a sea of delocalized electrons
• What happens to the outer valence electrons in the electron sea model?

  They become delocalized
• The delocalized electron sea in metals allows for high electrical conductivity.
• Metallic bonding results in properties such as high conductivity, malleability, and ductility
• What are the key characteristics of metal lattice structures?

  Ordered, 3D arrangement
• Match the type of metal packing with its description:

  FCC ↔️ Atoms in cube faces

  BCC ↔️ Atoms in cube center

  HCP ↔️ Hexagonal close-packed
• Why are delocalized electrons essential for thermal conductivity in metals?

  They move freely
• The strong electrostatic attraction between ions and the electron sea maintains lattice stability.
• Metal atoms are densely packed in specific arrangements like FCC, BCC, or HCP
• What is the arrangement of atoms in a metal lattice structure?

  Three-dimensional ordered array
• Metals are densely packed in arrangements like FCC, BCC, or HCP
• What is the role of delocalized electrons in metals?

  Electrical and thermal conductivity
• Strong electrostatic attraction between positive ions and delocalized electrons maintains lattice stability in metals.
• Match the structure with its bond formers:

  Metal ↔️ Positive ions & electron sea

  Ionic ↔️ Positive & negative ions

  Covalent ↔️ Shared electron pairs
• What type of electrical conductivity do covalent compounds typically have?

  Generally poor
• The delocalized electrons in metals contribute to their high electrical conductivity
• What two factors contribute to the properties of metals?

  Metallic lattice and delocalized electrons
• Why are metals malleable and ductile?

  Delocalized electrons allow ions to slide
• Metals generally have low melting and boiling points compared to ionic compounds.