Electrolytes

Electrolytes: substances that when dissolved in water split apart, or dissociate, forming ions. When a substance ionizes in a solution, those ions or charges can conduct electricity.

Therefore, an electrolyte can also be said to have electrical conductive properties.

But not all electrolytes are created equally! They can be classified as strong or weak electrolytes, depending on how well they conduct electricity.

Strong Electrolytes:

Ionize 100%, therefore generating the maximum amount of ions
Conduct electricity very well
Types of Compounds: soluble salts (ionic compounds made of a metal—or ammonia NH4 – and nonmetal) and strong acids and bases.
Examples: NaCl, MgCl₂, HCl, NaOH, NH₄Cl
Chemical Equation: unidirectional, non-reversible

Weak Electrolytes:

Only partially ionize (<<<100%), therefore creating fewer ions and not as many charges
Poor electrical conductors
Type of Compounds: weak acids and bases, molecular compounds
Examples: HF, NH₃, NH₄⁺, H₃PO₄, CH₃COOH
Chemical Equation: bidirectional, reversible (so ions can rejoin and reform molecule)

Non-Electrolytes:

Do not ionize; generate no ions
No electrical conduction
Type of Compounds: alcohols (contain OH, names end in “ol”), sugars (CH₂O type formula, names end in “ose”), biological compounds.
Examples: C₆H₁₂O₆ (glucose), C₂H₅OH (ethanol), CO(NH₂)₂ (urea)