Metallic bonding

• What is the structure of a pure metal in the solid state?

  Giant metallic structure
• How are the atoms arranged in a pure metal?

  In layers
• What happens when a force is applied to a pure metal?

  The layers may slide over each other
• What does a greater force needed to slide layers in a metal indicate?

  The metal is harder and stronger
• Why are many pure metals considered soft?

  Small force needed to slide layers
• What is an alloy?

  A mixture of two or more elements
• How do different sized atoms in an alloy affect its hardness?

  They distort the layers of atoms
• Why is an alloy harder than a pure metal?

  Greater force required for layers to slide
• What is an example of an alloy?

  Steel
• What are the types of steel and their properties?

  • Mild steel: Carbon and iron; easy to bend
  • Tool steel: Tungsten and iron; hard, high temperatures
  • Stainless steel: Chromium and iron; hard, rust-resistant
• Why are pure metals often too soft for many uses?

  They can be made harder by alloys
• What property allows metals to conduct electricity?

  Delocalised electrons
• Why are metals good conductors of thermal energy?

  Delocalised electrons transfer energy
• What causes metals to have high melting and boiling points?

  Strong metallic bonding in giant structure
• What is metallic bonding?

  Delocalised electrons sharing among atoms
• How are atoms arranged in metals?

  In a regular pattern
• What is the result of delocalised electrons in metals?

  Strong metallic bonding
• What is the significance of tungsten in tool steel?

  It makes tool steel harder
• What are the general applications of different types of steel?

  Used in construction, tools, and appliances
• What role do delocalised electrons play in metals?

  They allow electrical conductivity
• How does metallic bonding affect metal properties?

  It results in high melting and boiling points