electrolytes, non-electrolytes, and weak electrolytes

Strong electrolytes

• conducts electricity well

• completely breaks up = 100% dissociation

• any soluble ionic compounds (metal + non metal) (metal + polyatomic ions)

Strong acids (strong electrolytes)

HCl - hydrochloric acid

HBr - hydrobromic acid

HI - hydroiodic acid

HNO3 - nitric acid

HClO4 - perchloric acid

H2SO4 - sulfuric acid

Strong bases (strong electrolytes)

(group 1 or 2) + hydroxide

ex. LiOH, NaOH, Mg(OH)2

Weak Electrolytes

• weak conductor of electricity

• small amount of the compound dissociates into ions

Weak Electrolyte examples

CH3COOH → CH3COO- + H+(aq)

HF → H+ + F-(aq)

HCN → H(aq) + CN-(aq)

NH3

Non Electrolytes

• molecular compounds — nonmetals

• stay intact in water

Non Electrolyte examples

H2O, C3OH, CH3OH, C6H12O6

Precipitation reactions

• formation of insoluble solid

ex. (aq) + (aq) = (aq) + (s)

• double displacement reactions

Acid-Base Neutralization reaction

formation of a very stable molecular compound (H2O)

• usually ends w/water or an ionic compound (salt)

ex. (aq) + (aq) = (l) + (aq)

Oxidation Reduction Reaction

• decrease in the electrical potential

• transfer of electrons between reaction pairs