Bonding, Structure and Properties of Matter

• What does the term aqueous mean?

  It means a substance that can be dissolved in water
• What does the melting point mean?

  The temperature a pure substance will melt and freeze at
• What does the boiling point mean?

  The temperature a pure substance will boil and condense at
• Complete the sentence

  The stronger the forces of attraction between the particles, the higher the melting and boiling points will be.
• How are ions formed?

  When atoms gain or lose electrons
• Where do ionic bonds occur?

  Between positive and negative ions
• What are ionic bonds?

  Strong electrostatic forces of attraction between a positive metal ion and a negative non metal ion
• Why do ionic compounds conduct electricity when molten or in solution?

  Because the charged ions are free to move and carry charge.
• What is a metallic bond?

  The attraction between the positive ions and the delocalised negatively charged electrons.
• What does delocalised mean?

  It is not bound to one atom
• Describe the structure of metals

  Metals have a giant structure in which electrons are delocalised. This produces a lattice of positive ions held together by electrostatic attraction to delocalised electrons.
• Describe the particle arrangement of pure metals

  Particles in pure metals have a regular arrangement
• What are alloys?

  Mixtures that contain a metal and at least one other element
• Why might someone use alloys over pure metals?

  Alloys have an extra element which disturbs the regular arrangement of the metal atoms, making alloys stronger and harder.
• Define ductile and malleable

  The ability to bend or shape metals without them breaking
• Define brittle

  Delicate and easy to break
• Define corrosion

  When a refined metal naturally converts into a more chemically stable oxide.
• Why are metals good conductors of electricity?

  The delocalised electrons can move around freely and transfer energy
• What are covalent bonds?

  A shared pair of electrons between atoms, typically between non - metals
• Describe the structure of simple molecules

  Simple molecules contain a relatively small number of non-metal atoms joined together by covalent bonds.
• What are the typical substances that consist of intermolecular forces?

  Liquids and gases with low melting and boiling points
• Define intermolecular forces

  Forces of attraction between the molecules
• How does the size of a simple molecule affect the strength of the intermolecular forces between molecules?

  The larger the molecule, the stronger the intermolecular forces between molecules become
• Describe the structure of diamond

  Diamond is a form of carbon that has a lattice structure. Diamond has no charged particles so it does not conduct electricity.
• Describe the structure of Graphite

  Graphite is a form of carbon that has a lattice structure. One electron from each carbon atom in graphite becomes delocalised allowing graphite to conduct electricity.
• Describe the structure of Silica

  Silica has a lattice structure similar to diamond.
• Describe the structure of graphene

  Graphene is a form of carbon. It is a single layer of graphite. Graphene can conduct electricity, heat and is nearly transparent.
• What are fullerenes?

  Molecules formed from carbon which contain different numbers of carbon atoms.
• What is the most stable fullerene?

  Buckminsterfullerene
• What is graphene used in?

  Graphene is used in electronics
• What are fullerenes used for?

  Fullerenes are used to deliver drugs into the body and reinforcing the frames in tennis rackets
• How big are nanoparticles?

  Nanoparticles have a diameter between 1 nm and 100 nm
• What potential problems could nanoparticles cause?

  They are so small that they could get into human cells and damage them.