Metals and non-metals

• What are the two main categories of elements in the periodic table?

  Metals and non-metals
• How can the properties of metals be explained?

  In terms of metallic structure and bonding
• What are the typical properties of metals and non-metals?

  Metals:

  • Shiny
  • High melting points
  • Good conductors of electricity and heat
  • High density
  • Malleable

  
  

  Non-metals:

  • Dull
  • Low melting points
  • Poor conductors of electricity and heat
  • Low density
  • Brittle
• What is a characteristic of metals regarding their appearance?

  Metals are shiny
• What is a characteristic of non-metals regarding their appearance?

  Non-metals are dull
• What is the melting point comparison between metals and non-metals?

  Metals have high melting points, non-metals low
• How do metals and non-metals differ in electrical conductivity?

  Metals are good conductors, non-metals are poor
• How do metals and non-metals differ in thermal conductivity?

  Metals are good conductors, non-metals are poor
• What is the density comparison between metals and non-metals?

  Metals have high density, non-metals low
• What does malleable mean in relation to metals?

  Malleable means they can be shaped without breaking
• What does brittle mean in relation to non-metals?

  Brittle means they shatter when bent or hit
• What is an example of a metal with a low melting point?

  Mercury
• What is an example of a non-metal that conducts electricity?

  Graphite
• What is the definition of density?

  Density is mass per unit volume
• What is the structure of metals in terms of atoms?

  Metals consist of closely packed metal ions
• What is metallic bonding?

  It is the attraction between metal ions and delocalised electrons
• Why are metals malleable?

  Layers of ions can slide over each other
• How do delocalised electrons contribute to electrical conductivity in metals?

  They move through the lattice structure when voltage is applied
• What is an electric current?

  The movement of electrically charged particles
• What happens when a voltage is applied to a metal?

  Delocalised electrons travel through the lattice
• How does the structure of metals contribute to their properties?

  The metallic lattice allows for malleability and conductivity
• What are the four kinds of bonding types?

  Ionic, simple covalent, giant covalent, metallic
• How does ionic bonding occur?

  Electrons are transferred between atoms
• What forms as a result of ionic bonding?

  A positive-negative ion pair
• What is the structure of simple covalent molecular substances?

  Small groups of atoms held together
• What is the structure of giant covalent network substances?

  Billions of atoms are held together
• What is a characteristic of metallic bonding?

  Outer electrons are free to move
• What is the ionic lattice structure?

  A regular arrangement of oppositely charged ions
• What is a limitation of the metallic lattice model?

  It does not show multiple layers of ions
• What is an ionic compound?

  Formed by positive and negative ions
• What are the forces holding simple molecular substances together?

  Weak intermolecular forces
• What happens when a simple molecular substance melts?

  Intermolecular forces are broken
• What is an example of a simple molecular substance?

  Water
• What are the typical properties of ionic, simple covalent, giant covalent, and metallic bonding types?

  • Ionic: Loss and gain of electrons, strong attraction
  • Simple covalent: Share pairs of electrons, small groups
  • Giant covalent: Share pairs of electrons, billions of atoms
  • Metallic: Free-moving outer electrons, billions of positive ions
• What are the limitations of different bonding models?

  • Do not show all layers of ions
  • Do not represent electron movement accurately
  • May oversimplify the structure of substances
• How do ionic compounds form their structure?

  • Regular lattice structure
  • Oppositely charged ions attract each other
  • Example: Sodium chloride
• What distinguishes simple molecular substances from giant covalent substances?

  • Simple: Small groups of atoms, weak forces
  • Giant: Billions of atoms, strong covalent bonds
• What is the difference between covalent bonds and intermolecular forces?

  • Covalent bonds: Strong, within molecules
  • Intermolecular forces: Weak, between molecules