C2new Hard Flashcards
Why do small covalent structures have poor electrical conductivity
Because molecules are neutral
Why do diamonds have a high melting a boiling point
Needs lots of energy to overcome strong covalent bonds
Why are diamonds very hard
Giant structure of strong covalent bonds so layers cannot slide
Why do diamonds not conduct electricity
No delocalised electrons
Why do diamonds have a crystal structure
4 covalent bonds to each atom in tetrahedral structure
Why does graphite have a high melting point
Need lots of energy to overcome strong covalent bonds
Why is graphite soft
Layers of atoms can slide past each other because weak intermolecular forces between layers
Why is graphite a good electrical conductor
Delocalised electrons move and carry charge
Why does graphite rub off into paper
3 covalent bonds to each atom in hexagonal layers
Why does silicone have a crystal structure
4 covalent bonds in a tetrahedral structure
Why does silicone have a high melting and boiling point
Needs a lot of energy to overcome strong covalent bonds
Why does silicone have a poor electrical conductivity
No delocalised electrons
