Topic 2 - Bonding, Structure and the Properties of Matter

• 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 conduct electricity and heat well?

  Due to free-moving delocalized 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
• How do ionic compounds form crystals?

  Through repeating units of ions in a lattice
• 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 is an example of a molecular ion?

  Hydroxide ion (OH⁻)
• How many hydroxide ions are needed for magnesium hydroxide?

  Two hydroxide ions
• What is the spelling of sulfate according to the author?

  With a "pH" instead of "F"
• What can any ionic compound be called?

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

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

  They change to reflect ionic form
• How do non-metals bond with each other?

  Through covalent bonding
• What do non-metals do in covalent bonding?

  Share electrons to gain full outer shells
• What is the molecular formula for chlorine gas?

  Cl₂
• What does a structural formula represent?

  Molecular structure using symbols and lines
• How many extra electrons does each oxygen need in O₂?

  Two extra electrons
• What type of bond is formed in O₂?

  A double covalent bond
• What is unique about nitrogen (N₂) bonding?

  It has a triple bond
• How do simple molecular structures behave?

  They have low boiling points
• What type of forces exist between simple molecular structures?

  Weak intermolecular forces
• Can simple molecular structures conduct electricity?

  No, they cannot conduct electricity
• What is giant covalent bonding similar to?

  The lattice nature of ionic compounds
• What is diamond an example of?

  A giant covalent structure
• 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 graphite layers slide over each other?

  Weak bonds between layers allow sliding
• What are metal alloys stronger than?

  Pure metals
• Why are metal alloys stronger?

  Different size atoms disrupt regular lattice
• What is graphene?

  A single layer of graphite
• What is Buckminsterfullerene?

  A spherical structure of 60 carbon atoms