1. Ionic Compounds: Electrolytes are typically ionic compounds, meaning they contain positively charged ions (cations) and negatively charged ions (anions). When these compounds dissolve in water, the ions separate, allowing them to move freely in the solution.
2. Dissociation: When an electrolyte dissolves in water, it undergoes a process called dissociation. During dissociation, the ionic bonds between the cations and anions break, releasing individual ions into the solution.
3. Free Ions: The presence of free ions in the solution is what enables electrolytes to conduct electricity. When an electric current is applied, the positively charged cations move toward the negative electrode (cathode), while the negatively charged anions move toward the positive electrode (anode). This movement of ions constitutes an electric current.
4. Solutions: Electrolytes are substances that conduct electricity only in the form of solutions. In a solid state, electrolytes do not conduct electricity effectively because their ions are fixed in a crystal lattice and cannot move freely.
5. Strong vs. Weak Electrolytes: Electrolytes can be classified into two types: strong electrolytes and weak electrolytes. Strong electrolytes completely dissociate in water, releasing all of their ions, while weak electrolytes only partially dissociate, leaving some of their ions bound together.
Examples of common electrolytes include table salt (sodium chloride), sugar (sucrose), and acids (such as hydrochloric acid) or bases (such as sodium hydroxide) when dissolved in water. These substances contain dissolved ions that can move freely, allowing them to conduct electricity.
