metallic bonding

• What is the structure of a metal?

  A giant lattice of positive ions
• What role do delocalized electrons play in metals?

  They hold positive ions together
• What are the four physical properties of metals?

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

  Atoms are closely arranged in rows
• How do free electrons contribute to heat conduction in metals?

  They carry energy through the metal
• Why are metals good conductors of electricity?

  Electrons carry a negative charge
• What happens to electrons when they move through a metal?

  They create an electrical current
• Why are metals malleable?

  Atoms can slide over each other
• What occurs when a metal is hammered?

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

  Can be drawn into wire
• What is plastic deformation in metals?

  Permanent change in shape under stress
• What elements are in Group 1?

  Lithium, sodium, potassium, rubidium, cesium
• How does the melting point change down Group 1?

  It decreases as you go down
• Why does the melting point decrease down Group 1?

  • Atoms get larger with more shells
  • distance between nucleus and delocalised electron is bigger
  • forces holding structure together are weaker
• What happens to the force holding the structure together as you go down Group 1?

  The force becomes weaker
• How do Group 2 metals compare to Group 1 in terms of melting points?

  Group 2 has higher melting points
• Why do Group 2 metals have higher melting points?

  More delocalized electrons per atom
• What effect does a higher positive charge in metal ions have?

  Stronger metallic bonding
• Why does magnesium have a higher melting point than sodium?

  Magnesium has more protons than sodium
• What are the key properties of metals?

  • Good conductors of heat
  • Good conductors of electricity
  • Malleable (can be hammered into shape)
  • Ductile (can be drawn into wire)
• Describe the differences in melting points between Group 1 and Group 2 metals.

  • Group 1: Lower melting points
  • Group 2: Higher melting points
  • Group 2 has more delocalized electrons
  • Group 2 has more positive charge in ions
• What are the reasons for the melting point trends in Group 1 and Group 2 metals?

  • Group 1: Larger atoms, weaker forces
  • Group 2: More delocalized electrons, stronger forces