Ions

Atoms held together with an Ionic bond present all the characteristics listed for this discussion. Let’s dig a little deeper though and look at why these ionic bonds have these characteristics.

We have read in our text that an ionic bond happens when there is a transfer of one or more electrons from one atom to another during a chemical reaction (Simon, Reese, and Dickey 27). What are left are atoms that have a charge, either positive or negative, because they either have more protons than electrons, or less. The result is a positively charged atom being attracted to a negatively charged atom, an ionic bond. Compounds created by ionic bonds have high melting points because “it takes a lot of energy to overcome this attraction in order to allow the ions to move more freely and form a liquid” (AUS-e-TUTE).

Ions need to be able to move freely to conduct electricity as well. “Solid ionic compounds do not conduct electricity because the ions are locked into a rigid lattice or array. The ions cannot move out of the lattice, so the solid cannot conduct electricity” (AUS-e-TUTE). This is why an ionic compound in a molten state can conduct electricity while one in a solid state cannot. The ions can also move more freely when dissolved in water.

This brings us to the ionic bonds crystalline nature at a solid state. Like mentioned before, ionic bonds form a lattice like structure with positive atoms surrounded by negative atoms. “When a stress is applied to the ionic lattice, the layers shift slightly” (AUS-e-TUTE). When a shift occurs, “ions of the same charge will be brought closer together [and] repel each other” (AUS-e-TUTE). This is why ionic bonds have a brittle characteristic and a crystalline appearance.

Simon, Reese, and Dickey. Campbell Essential Biology, 4th Ed. Benjamin Cummings: Boston, 2010. Print.

AUS-e-TUTE n.d. “Chemistry Tutorial.” Ausetute. Date Unknown. Web. 21 August 2012.