bonding

• How are ions formed?

  Ions are formed when atoms lose or gain electrons.
• What types of elements typically form ionic bonds?

  Ionic bonds typically form between metals and non-metals.
• What is a characteristic of ionic bonds?

  Ionic bonds are very strong.
• Why are metal and non-metal ions attracted to each other?

  They are attracted to each other by electrostatic forces due to opposite charges.
• What determines the high melting and boiling points of ionic compounds?

  The strength of the bonds holding the ions together determines their high melting and boiling points.
• What are the properties of ionic compounds?

  • Form a regular lattice structure
  • Have high melting and boiling points due to strong ionic bonds
  • Conduct electricity when melted or dissolved in water
• Under what conditions can ionic compounds conduct electricity?

  Ionic compounds can conduct electricity when melted or dissolved in water.
• How are electrons involved in covalent bonding?

  Electrons are shared between non-metallic atoms in covalent bonding.
• What is a simple molecule in terms of covalent bonding?

  A simple molecule has multiple atoms covalently bonded together.
• Why are simple molecules easily separated from each other?

  The electrostatic attraction between separate molecules are weak.
• What is the melting and boiling point characteristic of simple covalent substances?

  They have low melting and boiling points due to weak intermolecular forces.
• What are the characteristics of simple covalent substances?

  • Contain only a few atoms
  • Low boiling and melting points
  • Usually gases at room temperature
  • Unable to conduct electricity
• What is an allotrope?

  An allotrope is a different structural form of the same element in the same physical state.
• What are the characteristics of giant covalent structures?

  • Contain millions of atoms
  • High melting and boiling points due to strong covalent bonds
  • No weak intermolecular forces
  • Cannot conduct electricity unless it is graphite
• Why does diamond have a high melting point?

  Diamond has a high melting point because a lot of energy is needed to break the strong covalent bonds.
• How is diamond structured in terms of covalent bonding?

  Diamond has a regular lattice of covalently bonded atoms, with each carbon atom bonded to four others.
• Why doesn't diamond conduct electricity?

  Diamond doesn't conduct electricity because it has no free electrons.
• How is graphite structured in terms of covalent bonding?

  Graphite has a regular lattice of covalently bonded atoms, with each carbon atom bonded to three others in hexagonal layers.
• Why can graphite conduct electricity?

  Graphite can conduct electricity because it has delocalised electrons from the spare electron of each three carbons.
• What is graphene and its properties?

  Graphene is one layer of graphite, strong and can conduct electricity due to delocalised electrons.
• What are some uses of graphene?

  • Strengthens other materials
  • Acts as a cage around drugs
  • Used as a catalyst
  • Applications in nanotechnology
• What are fullerenes?

  • Made from graphene
  • Can be formed into spheres and tubes
  • Allotropes of carbon that are hollow
• What is metallic bonding?

  Metallic bonding occurs between two metals.
• What are the characteristics of solid metals?

  • Giant structure of atoms arranged in a regular pattern
  • Outer shell electrons are shared among all atoms
  • Many delocalised electrons
  • Strong electrostatic attraction between positive metal ions and delocalised electrons
• Why do metals have high melting and boiling points?

  Metals have high melting and boiling points due to strong electrostatic attraction in metallic bonding.
• What makes metals good conductors of electricity and heat?

  Metals are good conductors due to the presence of delocalised electrons.
• Why are pure metals malleable?

  Pure metals are malleable because their regular structure allows layers to slide over each other.
• What are the properties of alloys?

  • Composed of two or more different elements
  • Different sized atoms disrupt the regular structure
  • Layers cannot slide over each other
  • Alloys are harder than pure metals