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Compare the bond energy between atoms of Ca in a piece of solid Ca metal and...

Compare the bond energy between atoms of Ca in a piece of solid Ca metal and the lattice energy between ions of Ca^2+ and O^2- in a piece of solid CaO. Assume that bond energies and lattice energies are equivalent concepts, explain how these energy values give us an indication as to which of these two materials is stronger.

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Answer #1

Metallic Bonding: It is the electrostatic attraction between positively charged atomic nuclei with negatively charge sea of electrons. The strength of metallic bonding is dependent on the attractive force as we go along K to Ca to Sc the electron sea gets more negative and bond become stronger.

Ionic Bonding: When a positively charged ions form a bond with negatively charged ions then the bond is known as ionic bonding.

Formation of ionic materials occurs via formation of lattice where the negatively charged species and positively charged species arranged in a symmetrical fashion. The stability of the material depends on the energy liberated or stored in the material due to the formation of lattice and this is known as lattice energy.

This quite analogical to the bond energy which is defined as the energy stored in the material during the bond formation.

Ca^2+ and O^2- forms CaO which is ionic material and Ca is a metal. So the CaO will have lattice energy as stability determining factor and for Ca it is metallic bond energy.

If the lattice energy < metal bond energy then Ca is more stable than CaO.

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