Bonding

• What type of bonding occurs between metal atoms?

  Metallic bonding
• What is formed by metallic bonding?

  A lattice of ions with delocalized electrons
• What does "delocalized" mean in the context of electrons?

  Electrons are not fixed to one atom
• Why do metals make good conductors of electricity and heat?

  Because of the free movement of electrons
• How do metals bond to non-metals?

  Through ionic bonding
• What does a group one metal need to do to bond with a group seven atom?

  Lose an electron
• What happens when a lithium atom bonds with chlorine?

  Lithium donates its outer electron
• What is a DOT and cross diagram used for?

  To show electron distribution in bonding
• What must the charges of ions in an ionic compound do?

  Add up to zero
• What is the chemical formula for lithium chloride?

  LiCl
• What is the chemical formula for beryllium chloride?

  BeCl2
• Why do ionic compounds have high melting and boiling points?

  Due to strong electrostatic forces
• When can ionic compounds conduct electricity?

  When molten or dissolved in solution
• What can any ionic compound be called?

  A salt
• What is the name of the positive ion in an ionic compound?

  Cation
• How are anion names different from their normal names?

  They change to reflect their ionic form
• What type of bonding occurs between non-metals?

  Covalent bonding
• How do non-metals bond to form molecules?

  By sharing electrons
• What is the result of two chlorine atoms bonding?

  Chlorine gas (Cl₂)
• What does a structural formula represent?

  The arrangement of atoms in a molecule
• How many extra electrons does each oxygen need in O₂?

  Two extra electrons
• What is a double covalent bond?

  When two atoms share two pairs of electrons
• What are simple molecular structures characterized by?

  Weak intermolecular forces
• Why can't simple molecular compounds conduct electricity?

  They lack free-moving charged particles
• What is giant covalent bonding similar to?

  The lattice nature of ionic compounds
• Why is diamond hard and has a high melting point?

  Due to strong covalent bonds
• What is graphite made of?

  Layers of carbon atoms in hexagonal structure
• How does graphite conduct electricity?

  Through delocalized electrons between layers
• Why can layers of graphite slide over each other easily?

  Due to weak bonds between the layers
• What are metal alloys stronger than?

  Pure metals
• Why do metal alloys have different sized atoms?

  To disrupt the regular lattice structure
• What is graphene?

  A single layer of graphite
• What is Buckminster fullerene?

  A spherical structure of 60 carbon atoms
• What are carbon nanotubes?

  Tubular structures of carbon atoms
• What is the size range for nanoparticles?

  100 to 2,500 nanometers
• What happens to the surface to volume ratio when the length of a cube's side doubles?

  The ratio halves
• Why is the surface to volume ratio significant for nanoparticles?

  It allows fewer particles to fulfill a purpose
• What are the key characteristics of ionic compounds?

  • High melting and boiling points
  • Conduct electricity when molten or dissolved
  • Form a lattice structure
  • Consist of repeating units of ions
• What are the differences between covalent and ionic bonding?

  Covalent bonding:

  • Involves sharing electrons
  • Forms molecules
  • Low melting points

  
  

  Ionic bonding:

  • Involves transfer of electrons
  • Forms ionic compounds
  • High melting points
• What are the properties of giant covalent structures?

  • Very high melting and boiling points
  • Strong covalent bonds
  • Cannot conduct electricity (except graphite)
  • Form a continuous network of atoms