Metallic bonding

• What type of bonding occurs between metal atoms?

  Metallic bonding
• What are the characteristic properties of metals attributed to?

  Metallic bonding
• How do metals bond to non-metals?

  Through ionic bonding
• How do non-metals bond to other non-metals?

  Through covalent bonding
• What happens to outer shell electrons in metallic bonding?

  They are given up and shared among all atoms
• What do we call the electrons that are free to move in metallic bonding?

  Delocalized electrons
• What type of attraction holds the structure of metals together?

  Strong electrostatic attraction
• Why do most metallic structures have high melting and boiling points?

  Due to the strong forces of attraction in metallic bonding
• What is a key property of metals regarding electricity and heat?

  They are good conductors
• What allows metals to conduct electricity and heat?

  The movement of delocalized electrons
• What does it mean for metals to be malleable?

  They can be bent or hammered into shapes
• Why can different layers of metal atoms slide over one another?

  Because of their regular structure
• What is the purpose of creating alloys?

  To make a harder metal that won't bend easily
• How are alloys typically made?

  By mixing two different metals or a metal and a non-metal
• Why do different sized atoms in alloys help improve hardness?

  They disrupt the regular structure of metals
• What is steel primarily made of?

  Iron
• What percentage of carbon is typically found in steel?

  1 to 2 percent
• What additional elements can be found in steel to enhance its properties?

  Chromium, manganese, or vanadium
• Why is steel used in cars and planes?

  Because of its strength
• What are the key properties of metals due to metallic bonding?

  • High melting and boiling points
  • Good conductors of electricity and heat
  • Malleable (can be bent or hammered)
• How do alloys differ from pure metals?

  • Alloys contain two or more different elements
  • Alloys have disrupted regular structures
  • Alloys are generally harder than pure metals
• Electrons carry charge, so the metal can conduct electricity.
• The electrons can carry thermal energy meaning they are good conducters of heat.