Covalent Bonding
- Created by: Rebeccaellis17
- Created on: 03-04-15 12:34
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- Covalent Bonding
- 2 Non-Metals
- The atoms/single elements share electrons
- Each shared pair of electrons strongly attract the atoms together - A Covalent Bond
- However atoms of some elements can form several covalent bonds
- Called Giant Covalent Structures
- There ae no intermolecular forces just covalent bonds
- So they have a very high melting and boiling point. A lot of energy is needed to break down the lattice
- Diamond
- Each carbon atom forms four covalent bonds
- Very hard
- 3-D so is transparent
- Each carbon atom forms four covalent bonds
- Silicon Doxide (Similar properties to diamond)
- Diamond
- Each carbon atom forms four covalent bonds
- Very hard
- 3-D so is transparent
- Each carbon atom forms four covalent bonds
- Diamond
- Graphite
- Covalently bonded to three other carbon atoms
- Flat 2-D layers that slide
- No covalent bonds between layers: Weak intermolecular
- They slide over each other
- Used in pencils as layers slide to leave a mark and in lubricants
- They slide over each other
- No covalent bonds between layers: Weak intermolecular
- Has one delocalised electron so can conduct heat and electricity
- This is because it bonds covalently 3 times so has a spare electron (delocalised) to carry a charge
- Fullerenes
- Large molecules formed from £-D hexagonal rings of carbon
- Some are nano-sized and used for drug delivery in the body, lubricants, reinforcing metals
- Large molecules formed from £-D hexagonal rings of carbon
- There ae no intermolecular forces just covalent bonds
- Called Giant Covalent Structures
- However atoms of some elements can form several covalent bonds
- Each shared pair of electrons strongly attract the atoms together - A Covalent Bond
- The atoms/single elements share electrons
- 2 Non-Metals
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