Metallic Bonding

• What is metallic bonding?

  Metallic bonding is the electrostatic attraction between a lattice of positive metal ions and a sea of delocalized electrons.
• Why do metals form metallic bonds?

  Metals have loosely held outer electrons that become delocalized, creating a strong bond between the ions and free-moving electrons.
• What is meant by a "sea of electrons"?

  It refers to the delocalized electrons that are free to move throughout the metal structure.
• What type of structure do metals have?

  Metals have a giant metallic lattice structure, where positive ions are arranged in a regular pattern surrounded by delocalized electrons.
• Why do metals have high melting and boiling points?

  Strong electrostatic forces between positive ions and delocalized electrons require a lot of energy to overcome.
• Why are metals good conductors of electricity and heat?

  Delocalized electrons can move freely, allowing them to carry electrical charge and transfer thermal energy.
• Why are metals malleable and ductile?

  The layers of ions in the lattice can slide over each other without breaking the metallic bond, as the delocalized electrons maintain the bond.
• Why are metals malleable and ductile?

  The layers of ions in the lattice can slide over each other without breaking the metallic bond, as the delocalized electrons maintain the bond.
• What is an alloy?

  An alloy is a mixture of two or more elements, where at least one is a metal.
• Why are alloys often harder than pure metals?

  Different-sized atoms in alloys disrupt the regular lattice, making it harder for layers to slide over each other.
• Give an example of a common alloy and its use.

  Example: Steel (iron and carbon). Use: Construction and tools due to its strength.
• How does metallic bonding explain the strength of metals?

  The strong attraction between the positive metal ions and the delocalized electrons creates a strong bond that holds the lattice together.
• What is the relationship between the number of delocalized electrons and the strength of metallic bonding?

  More delocalized electrons per atom result in stronger metallic bonds (e.g., magnesium has stronger bonding than sodium because it provides two delocalized electrons per atom compared to one).
• Why are transition metals often stronger than group 1 metals?

  Transition metals have more delocalized electrons and a smaller ionic radius, leading to stronger metallic bonds.
• Compare metallic bonding with ionic and covalent bonding.

  Metallic: Delocalized electrons bonding positive ions in a lattice. Ionic: Transfer of electrons creating electrostatic attraction between cations and anions. Covalent: Sharing of electrons between non-metals.
• What type of bonding is discussed in this video?

  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?

  Atoms slide over each other when stretched
• Which group of metals is mentioned in the study material?

  Group one and group two
• How does the melting point change down group one metals?

  It decreases as you go down
• Why does the melting point decrease down group one?

  Atoms get larger with more shells
• What happens to the force holding the structure together as you go down group one?

  The force becomes weaker
• How do group two metals compare to group one in terms of melting point?

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

  They have more delocalized electrons
• What is the effect of more positive charge in group two metals?

  Stronger metallic bonding
• How does the number of delocalized electrons affect metallic bonding strength?

  More electrons lead to stronger bonding
• What is the melting point trend in group one metals?

  It decreases down the group
• What is the melting point trend in group two metals?

  It is generally higher than group one
• 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 structure and bonding in metals.

  • Giant lattice of positive ions
  • Delocalized electrons act as glue
  • Metallic bonding holds the structure together
• Explain the reasons for the melting point trends in group one and group two metals.

  • Group one: Melting point decreases due to larger atoms
  • Group two: Higher melting point due to more delocalized electrons and stronger bonding