giant carbon structures

• What is diamond an allotrope of?

  Carbon
• What type of bonds are present in diamond?

  Covalent bonds
• How many carbon atoms is each carbon atom in diamond bonded to?

  Four
• What structure does diamond create?

  A giant covalent structure
• Why is diamond very hard?

  It has many strong covalent bonds
• Why is diamond used as a cutting tool?

  Because it is very hard
• Does diamond conduct electricity?

  No, it does not conduct electricity
• Why does diamond not conduct electricity?

  There are no delocalised electrons
• What is the melting point characteristic of diamond?

  It has a high melting point
• Why does diamond have a high melting point?

  A lot of energy is needed to break bonds
• What is the thermal conductivity of diamond?

  It is an excellent thermal conductor
• Why is diamond an excellent thermal conductor?

  Vibrations carry heat easily through its structure
• What is graphite an allotrope of?

  Carbon
• What type of bonds are present in graphite?

  Covalent bonds
• How many carbon atoms is each carbon atom in graphite bonded to?

  Three
• What structure does graphite create?

  A giant covalent structure
• What is a property of graphite due to its strong covalent bonds?

  It has a high melting point
• Is graphite soluble in solvents?

  No, it is insoluble in solvents
• Why is graphite considered soft?

  Layers can slide over one another easily
• What makes graphite useful as a lubricant?

  Its layers can slide over one another
• Why is graphite used as pencil 'lead'?

  Because it is very soft
• Does graphite conduct electricity?

  Yes, it conducts electricity
• Why does graphite conduct electricity?

  It has delocalised electrons that move freely