Metallic Bonding

• What type of bonding occurs between metal atoms?

  Metallic bonding
• What characteristic properties arise from metallic bonding?

  Strength, high melting and boiling points
• 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 shared among all atoms
• What do we call electrons that are free to move in metals?

  Delocalized electrons
• What holds the structure of metals together?

  Electrostatic attraction between ions and electrons
• Why are metals good conductors of electricity and heat?

  Delocalized electrons carry current and energy
• What does malleable mean in relation to metals?

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

  Due to their regular structure
• What is an alloy?

  A mixture of two or more different elements
• How do alloys differ from pure metals?

  Alloys have disrupted regular structures
• What is the effect of different sized atoms in alloys?

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

  Iron
• What percentage of carbon is typically in steel?

  One to two percent
• What additional elements can be found in steel?

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

  It provides necessary strength
• What are the properties of metals due to metallic bonding?

  • High melting and boiling points
  • Good conductors of electricity and heat
  • Malleable and ductile
  • Strong due to electrostatic attraction
• What are the differences between pure metals and alloys?

  Pure Metals:

  • Regular structure
  • Malleable and ductile

  
  

  Alloys:

  • Disrupted structure
  • Harder and less malleable