level: Giant covalent molecules - diamond and graphite
Questions and Answers List
level questions: Giant covalent molecules - diamond and graphite
| Question | Answer |
|---|---|
| What are the properties of giant covalent bonds | - No specific formula because the structure can be any size - High melting points because the covalent bonds between them make them solids - They exist as one large structure with no intermolecular forces between them |
| What is the state of giant covalent molecules at room temperature | Solids - Because they have millions of strong covalent bond which requires great deal of energy to overcome. |
| How is diamond formed | From the element Carbon |
| Why cant diamonds conduct electricity | They have no delocalised electrons that can carry charge |
| The bond of carbon in a diamond atom | Forms 4 covalent bonds to 4 other carbon atoms |
| Why does Diamond have a high melting and boiling point | because of the millions of covalent bonds |
| The bond of carbon in graphite | each carbon atom only bonds covalently to 3 other carbon atoms - because of these strong bonds it has high melting and boiling point |
| How are the hexagonal rings in graphite arranged | In layers |
| Why is graphite slippery | There are no covalent bonds between the layers if hexagonal rings so they can slide |
| Why is graphite a good conducter of heat and electricity | Because of the carbon atom only being covlently bonded to 3 other carbon atoms, it leaves each carbon atom with one electron that is delocalised |