metallic bonding

• What role do delocalized electrons play in metallic bonding?


  They act as the glue holding the positive ions together
• What are the four physical properties of metals mentioned?

  Good conductors of heat, good conductors of electricity, malleable, and ductile
• Why are metals good conductors of heat?


  Atoms are closely arranged in rows, allowing energy to pass through them
• How do free electrons contribute to the conductivity of metals?


  They can move freely and carry energy through the metal
• Why are metals good conductors of electricity?


  Electrons carry a negative charge and their movement creates an electrical current
• Why are metals malleable?

  Atoms can slide over each other when hammered
• What happens to the layers of atoms when a metal is hammered?

  The layers of atoms slide over each other
• What does ductile mean in relation to metals?


  Metals can be drawn into wires
• Why can metals be stretched into wires?

  Layers of atoms slide over each other when stretched
• What is plastic deformation in metals?


  It is the ability of metals to change shape without breaking
• What trend is observed in the melting points of group one metals?

  The melting point decreases as you go down the group
• Why does the melting point decrease in group one metals?


  Atoms get larger with more shells, weakening the forces holding them together
• How does the melting point of group two metals compare to group one metals?


  Group two metals have a higher melting point than group one metals
• Why do group two metals have a higher melting point than group one metals?

  Group two metals have more delocalized electrons and stronger metallic bonding
• What is the relationship between the number of protons in the nucleus and the strength of metallic bonding?

  More protons lead to a stronger positive charge and stronger metallic bonding