Zusammenfassung der Ressource
Bonds
- Ionic Bonding
- Between metals and non-metal atoms
- Atoms gain full outer shells by losing or gaining electrons
- Atoms form positive and negatively charged ions
- Strong electrostatic forces of attraction between ions
- Properties
- High melting and boiling points due to strong attraction
between oppositely charged ions
- Conduct electricity when molten or dissolved in water due
to mobile ions, however does not when a solid
- Covalent bonding
- Between non-metals atoms only
- Atoms gain full outer shell by sharing electrons
- Two types of covalent bonding
- Simple molecular
- Small group of atoms share electrons forming
small molecules
- Each covalent bond is very strong
- Forces attraction between molecules is weak
- Properties
- Low melting and boiling points
- Due to the weak forces between molecules easily overcome
- Do not conduct electricity in any state
- Due to no mobile ions or delocalised electrons
- Giant Macromolecular
- Large number of atoms share electrons forming a giant
macromolecule
- Many strong covalent bonds formed
- Two main examples of Giant Macromolecular bonds are both Carbon
- Diamond
- Each carbon atom form 4 strong covalent bonds
- High melting and boiling point due to many strong covalent bonds
- Very hard and strong
- Does not conduct electricity
- No free-moving ions or delocalised electrons
- Graphite
- Each carbon atom forms 3 strong covalent bonds
- Leaves a 'free' delocalised electron on the outer shell
- Conducts electricity
- Due to delocalised electron
- High melting and boiling point due to many strong covalent bonds
- Lubricant because of layered structure
- Weak forces between layers allow them to slide past each other
- Metallic Bonding
- Metals exist as a lattice of positively charged ions
- Properties
- High melting and boiling points
- Due to strong attraction between ions and electrons
- Conducts electricity
- Due to delocalised outer shell electrons
- Malleable since mobile electrons allow planes of metal ions
to move past each other without breaking apart
- Outer shell electrons are delocalised
- Strong attraction between positive ions and negative electrons