2.3.2 Properties of Metals

• The metallic structure consists of positive metal ions arranged in a lattice
• Delocalized electrons in metals act as carriers of electrical and thermal energy
• What are the key properties of metals influenced by their metallic structure?

  Hardness, conductivity, malleability
• Match the property with its explanation:

  Hardness ↔️ Positive metal ions are closely packed in the lattice

  Conductivity ↔️ Delocalized electrons carry charge and thermal energy

  Malleability ↔️ Metal ions slide past each other without breaking metallic bonds
• Delocalized electrons in metals are responsible for their high electrical conductivity.
• Why do metals conduct electricity when an electric field is applied?

  Delocalized electrons flow freely
• Steps in thermal conductivity of metals

  1️⃣ Delocalized electrons gain kinetic energy when heated

  2️⃣ Energized electrons collide with other particles in the lattice

  3️⃣ Heat energy spreads throughout the metal
• Why does copper have higher thermal conductivity than iron?

  More delocalized electrons
• The malleability and ductility of metals are due to the ability of metal ions to slide past each other.
• Delocalized electrons allow metal ions to slide past each other without disrupting the overall structure
• What factors influence the melting and boiling points of metals?

  Charge density and ionic radius
• Metals possess a metallic structure with delocalized electrons
• Which metal has the highest melting point?

  Tungsten
• Tungsten has a high melting point due to its strong metallic bonds
• Sodium has a higher melting point than tungsten.

  False
• What is the structure of metals called?

  Metallic structure
• Metals consist of positive metal ions arranged in a lattice
• What carries charge and thermal energy in metals?

  Delocalized electrons
• Match the property of metals with its explanation:

  Hardness ↔️ Positive ions are closely packed

  Conductivity ↔️ Delocalized electrons carry energy

  Malleability ↔️ Metal ions slide past each other

  Ductility ↔️ Metal ions rearrange under stress
• Metals are malleable because their metallic bonds break easily when hammered.

  False
• Steps involved in the thermal conductivity of metals:

  1️⃣ Delocalized electrons gain kinetic energy

  2️⃣ Energized electrons collide with ions

  3️⃣ Heat energy is transferred throughout
• Which metal is commonly used in cooking pans due to its high thermal conductivity?

  Copper
• The malleability of metals is due to the ability of metal ions to slide past each other without breaking bonds.
• What are the two factors that influence the melting and boiling points of metals?

  Charge density and ionic radius
• A higher charge density increases the strength of metallic bonds
• What causes the lustrous appearance of metals?

  Delocalized electrons
• Metals appear shiny because their delocalized electrons absorb and re-emit light at the same frequency.