Metallic bonding

• What is the typical state of metals at room temperature?

  Solid
• What allows metals to conduct electricity?

  Delocalized electrons can move through the metallic lattice, carrying charge.
• What is the typical arrangement of particles in solids?

  Particles are tightly packed in a regular arrangement.
• How do the properties of liquids differ from those of solids?

  Liquids have more energy than solids, allowing particles to move freely and slide over each other.
• What is the typical arrangement of particles in gases?

  Particles are spaced out in a random arrangement.
• What happens to the energy of particles in gases compared to solids and liquids?

  Gases have more energy than both solids and liquids, allowing for free movement.
• What are the main types of bonding and their properties?

  • **Covalent Bonds**:
  • Formed by sharing electrons.
  • Low melting/boiling points.
  • May be polar or non-polar.

  
  

  • **Ionic Bonds**:
  • Formed by transfer of electrons.
  • High melting/boiling points.
  • Conduct electricity when dissolved in water.

  
  

  • **Metallic Bonds**:
  • Formed by delocalized electrons.
  • High melting/boiling points.
  • Conduct electricity in solid and liquid states.
• What are the properties of solids, liquids, and gases in terms of particle arrangement and energy?

  • **Solids**:
  • Tightly packed, regular arrangement.
  • Low energy, vibrate in place.

  
  

  • **Liquids**:
  • Tightly packed but random arrangement.
  • Moderate energy, slide over each other.

  
  

  • **Gases**:
  • Spaced out, random arrangement.
  • High energy, move freely.
• Why do metals conduct electricity?

  Metals conduct electricity due to the presence of delocalized electrons that can move freely through the lattice.
• How does the number of delocalized electrons affect the melting point of metals?

  The more electrons a metal can donate, the higher the melting point due to stronger electrostatic attractions.
• What is the typical arrangement of particles in solids?

  Particles in solids are tightly packed in a regular arrangement.
• How do the properties of liquids differ from those of solids?

  Liquids have more energy than solids, allowing them to move freely and slide over each other.
• What is the arrangement of particles in gases?

  Particles in gases are spaced out in a random arrangement and have very low density.
• What are the main types of bonding and their characteristics?

  • Covalent Bonds: Share electrons, can be polar or non-polar.
  • Ionic Bonds: Formed between metals and non-metals, involve transfer of electrons.
  • Metallic Bonds: Involve a sea of delocalized electrons, conduct electricity and heat.
• What is a metallic bond?

  A metallic bond is the bond present in metals between the positive metal ions and negatively charged electrons.
• What is the structure of metallic bonding?

  A lattice of positively charged ions surrounded by a sea of delocalised electrons
• What does the strength of metallic bonding depend on?

  The charge on the positive ion and the size of the ion
• How does the size of an ion affect metallic bonding?

  Larger ions produce a weaker attraction due to their greater atomic radius
• What is a property of substances with a metallic structure?

  They are good conductors of electricity
• Why are metals malleable?

  The layers of positive ions can slide over one another
• What is the melting point characteristic of metallic substances?

  They have high melting points