Chapter 3: Bonding

• What is ionic bonding?

  Transfer of electrons from metal to non metal.
• What is covalent bonding?

  Sharing of electrons between non metals.
• What's the physical properties of Ionic compound?

  #1. Solids at room temperature.

  #2. Non volatile.

  #3. High melting and boiling point

  #4.

  (B): Contains ionic bondings.

  (S): It is arranged in a giant lattice structure.

  (A): Strong electrostatic forces of attraction between.

  (P): Opposite charged ions.

  (E): More energy is needed to overcome these forces.
• What's the physical properties of Covalent compound?

  #1. Usually exist as gases or liquids at room temperature.

  #2. Volatile.

  #3. Low melting and boiling point.

  #4.

  (B) Contains covalent bondings.

  (S) It is arranged in a simple molecular structure.

  (A) Weak intermolecular forces of attraction between.

  (P) Molecules.

  (E) Less energy is needed to break these forces.
• What's the physical properties of diamond?

  #1.

  (B) Strong covalent bonds.

  (S) Giant molecular and tetrahedral structure.

  (A) Held by strong covalent bonds.

  (P) Within each layer, every carbon atom is joined to three other carbon atoms,

  (E) A lot of energy is needed to overcome these strong bonds.

  #2. Insoluble.

  #3. Soft & Slippery.

  #4. Conducts electricity.
• Why does graphite conduct electricity while diamond does not?

  #Graphite:

  Only 3 out of 4 valance electrons from each carbon atoms, are usd for bonding, leaving one electron delocalised to move along the layers, carrying electric current.

  #Diamond:

  All the valence electrons of the atoms are used for bonding. Thus, there are no free moving electrons to carry electric current.
• Explain why diamond can be used as a drill?

  Diamond has a giant molecular structure with every carbon atom joined to 4 other carbon atoms by strong covalent bond. A lot of energy is needed to overcome these bonds. Therefore, diamond is very hard amd can be used as drill tip.
• Explain why graphite can be used as a lubricant?

  Graphite has a parallel layered structure with weak intermolecular forces of attraction between the layers of carbon atoms. The layers of carbon aroms can slide over each other when force is applied. Therefore, graphite is very soft and slippery and can be used as lubricant.