Net Ionic Equations and Spectator Ions

This video tutorial explains how to write the net ionic equation for the reaction between calcium chloride (CaCl2) and sodium phosphate (Na3PO4). It covers balancing the molecular equation, determining the states of substances using solubility rules, splitting strong electrolytes into ions, and forming the net ionic equation by removing spectator ions. The tutorial emphasizes the importance of checking work for accuracy and provides a step-by-step guide to ensure all charges and atoms are balanced.

What is the first step in writing a net ionic equation?

• Determine the solubility of products

• Write the charges of ions

• Balance the molecular equation

• Identify spectator ions

Which of the following is typically aqueous?

• Lead sulfate

• Silver chloride

• Sodium chloride

• Calcium phosphate

What does the 's' indicate when writing the state of a compound?

• Soluble

• Solid

• Solution

• Sublimation

What charge does a calcium ion typically have?

• 1+

• 3+

• 2+

• 1-

Which ion has a 3- charge?

• Phosphate

• Calcium

• Sodium

• Chloride

Why don't we split solids in net ionic equations?

• They have no charge

• They are always soluble

• They do not dissociate in water

• They are not reactive

What is the purpose of identifying spectator ions?

• To find the limiting reactant

• To determine solubility

• To balance the equation

• To simplify the net ionic equation

Which ions are removed to form the net ionic equation?

• Only anions

• Spectator ions

• Only cations

• All ions

What must be conserved in a net ionic equation?

• Mass only

• Charge only

• Both charge and mass

• Volume

What is the final product in the net ionic equation for CaCl2 and Na3PO4?

• Sodium chloride

• Sodium phosphate

• Calcium phosphate

• Calcium chloride