covalent bonding

• diamond is very hard due to strong covalent bonds
• diamond has high melting and boiling points as covalent bonds are strong so need large amounts of energy to overcome the forces
• diamond is insoluble as covalent bonds are strong
• diamond is a poor conductor of electricity as there are no free electrons as one carbon atom is bonded to four other carbon atoms
• diamonds have a tetrahedral structure
• graphite is slippery as it contains layers that slide over each other
• graphite has a high melting and boiling point as strong covalent bonds need high amounts of energy to overcome the forces
• graphite is insoluble as the attraction between carbon atoms are strong
• graphite is a good conductor of electricity due to one delocolised electron as carbon atoms bond to three other carbon atoms
• graphene is strong due to the strong covalent bonds between carbon atoms
• graphene can conduct electricity due to the delocolised electrons which are free to move and electrons carry charge
• graphene are single layered rings
• simple covalent have low melting and boiling points as they have weak intermolecular forces
• simple covalent cannot conduct electricity as they are not charged particles
• simple covalent are often soluble is non polar solvents as they are held together by weak intermolecular forces
• dative bonding 


  pair of shared electrons where both electrons come from the same atom