Metallic bonding

• What is the main characteristic of metallic bonding?


  It involves delocalised electrons.
• How do delocalised electrons contribute to metallic bonding?


  They create strong electrostatic attractions between positive metal ions and shared negative electrons.
• What is the structure of metals in terms of bonding?


  Metals consist of a giant structure held together by metallic bonding.
• What types of substances are held together by metallic bonding?

  Metallic elements and alloys.
• What role do delocalised electrons play in the properties of metals?


  They produce all the properties of metals.
• What state are most metals in at room temperature?

  Solid.
• Why do most metallic compounds have high melting and boiling points?


  Because strong electrostatic forces need lots of energy to be broken.
• What makes metals good conductors of electricity and heat?

  The delocalised electrons carry electric charge and thermal energy.
• What does it mean for metals to be malleable?


  They can be bent, hammered, or rolled into flat sheets.
• Why are alloys harder than pure metals?


  Alloys are mixtures that distort the layers of metal atoms, making them harder.
• What is an alloy?


  A mixture of two or more metals or a metal and another element.
• How do different sized atoms in alloys affect their properties?


  They distort the layers of metal atoms, making it difficult for them to slide over each other.
• What are the properties of metals due to metallic bonding?


  • High melting and boiling points
  • Good conductors of electricity and heat
  • Malleable
  • Ductile
• Why is copper used in electrical circuits?


  Because it has delocalised electrons that carry electric charge effectively.
• What is one use of copper in electrical circuits?


  It is used to make hinges for doors.
• What is the state of metals at room temperature?

  Solid
• What type of bonding occurs between metal atoms?

  Metallic bonding
• What is the structure of metals described as?

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


  In a regular pattern
• What happens to outer shell electrons when metal atoms come together?


  They give up outer shell electrons and share them with other atoms
• What do all the atoms in a metal become when they share electrons?


  Positive ions
• What is the nature of the electrons in metallic bonding?


  They are free to move (delocalised)
• What type of attraction exists between positive ions and delocalised electrons?


  Strong electrostatic attraction
• What does metallic bonding give to metals?


  Strength
• What can metals carry due to their structure?

  Charge
• Why are metals good conductors of electricity and heat?


  Due to delocalised electrons
• What does the delocalised electrons allow metals to do?


  Carry electrical current and thermal energy
• What property allows metals to be easily bent or hammered into shapes?

  Malleability
• Why can pure metals be hammered into thin sheets?

  Because their layers can slide over one another
• What are alloys?


  Mixtures of two or more different metals
• How are alloys made?


  By mixing two different metals
• What effect do different sized atoms in alloys have on the structure?


  They disrupt the regular arrangement of atoms
• What happens to the layers of atoms in alloys compared to pure metals?


  Layers can no longer slide over one another
• Why are alloys generally harder than pure metals?


  Because the disruption of layers makes them harder
• What are the key characteristics of metallic bonding?


  • Involves a giant regular structure
  • Atoms are arranged in a regular pattern
  • Outer shell electrons are delocalised
  • Strong electrostatic attraction between positive ions and delocalised electrons
  • Provides strength and conductivity
• What are the properties of metals due to their structure?

  • Solid at room temperature
  • Good conductors of electricity and heat
  • Malleable and ductile
  • Can carry charge