Net Ionic Equations, Electrolytes, and Ionization

Net Ionic Equations, Electrolytes, and Ionization

Net ionic equation

• Not all compounds and ions undergo a chemical change in a reaction in an aqueous solution.

• Those ions are called spectator ions, and can be found in the solution both before and after the reaction

• Cd²⁺(aq) + 2NO^-₃(aq) + 2NH₄⁺(aq) + S^2-(aq) → CdS(s) + 2NO₃^-(aq) +2NH₄⁺(aq)

Ionization

• Molecular compounds ionize in a polar solvent

• Contrary to what we have Learned about molecules. They actually undergo a process called ionization

• Ionization depends on the strength of the covalent bond, and the strength of attractive forces between the solute and solvent

• Ionization is the forming of ions when there previously were none

•  $HCl\rightarrow^{H2O^{ }}H^+\left(aq\right)+Cl^-\left(aq\right)$  
  

Hydronium Ions

• In atoms that contain hydrogen atoms covalently bonded to a high electronegative ion (F,Cl,O) can ionize and release a H⁺. This is basically the donation of a proton

•  $H_2O\left(l\right)+HCl\left(g\right)\rightarrow H_3O^+\left(aq\right)+Cl^-\left(aq\right)$  

• H30+ is known as the hydronium atom

• the reaction creating the hydronium atom produces most of the energy needed to ionize a molecular solute

Weak vs Strong Electrolytes

• Strong electrolyte- dilute aqeuous solution that has most or all of the compound in the from of ions: it can conduct electricity well

• some acids, and all soluble ionic compounds

• Weak electrolytes- compound that has a small presence of ions made from its dissolved compound: it conducts electricity poorly.

• Hydrogen flouride, acetic acid