This is the reaction betweeen Mg and Br₂.

Electrolytes and Nonelectrolytes:

This video shows a the experiment testing the conductivity of NaCl and sugar. NaCl is an example of a strong electrolyte,

NaCl(s) --H₂O--> Na⁺(aq) + Cl^-(aq)

Sugar does not conduct electricity,

C₁₂H₂₂O₁₁(s) --H₂O--> C₁₂H₂₂O₁₁(aq)

This is an animation of NaCl dissolving in water as viewed from the particulate level.

NaCl is an example of a soluble ionic compound.

Ionic compounds are made up of ions. In this case the ions are Na⁺ and Cl^-.

Some substances that are covalent compounds when dissolved in water are strong electrolytes, or weak electrolytes.

Binary acids, such as HCl, are examples of covalent compounds that completely dissociate when added to water.

HCl(g) --H₂O--> H⁺(aq) + Cl^-(aq)

Some acids, like acetic acid, HC₂H₃O₂, are weak electrolytes. Such substances form a few ions. Since acetic acid is 95% in the molecular form (5% ions) we represent acetic acid as, HC₂H₃O₂(aq) in equations.

Here is an example of two precipitation reactions.

In the first example a solution labeled NaCl(aq) and a solution labeled AgNO₃(aq) are mixed.

In the second example a solution labeled NaI(aq) and a solution labeled AgNO₃(aq) are mixed.

This is an introduction to oxidation-reduction processes and what it means for a substance to lose or gain electrons.

Another example of oxidation-reduction reaction viewed at the particulate level.

Here is an oxidation-reduction reaction at the macroscopic level.

Can you write the reaction that occurs?

This is an example of a single replacement reaction between Cu metal and silver nitrate.

Solution formation by dilution

Solution formation by dissolving a solid