Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between cadmium nitrate and ammonium sulfide. It covers balancing the molecular equation, determining the states of substances using solubility rules, and splitting strong electrolytes into ions to form the complete ionic equation. The tutorial also discusses identifying and removing spectator ions to derive the net ionic equation, ensuring charge and atom balance.

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

• Assign states to each substance

• Balance the molecular equation

• Identify spectator ions

• Write the complete ionic equation

How do you balance the molecular equation for the reaction between cadmium nitrate and ammonium sulfide?

• Add a coefficient of 3 to cadmium nitrate

• Add a coefficient of 2 to ammonium nitrate

• Add a coefficient of 2 to ammonium sulfide

• Add a coefficient of 3 to ammonium nitrate

Which of the following is generally insoluble in water?

• Chlorides

• Ammonium compounds

• Nitrates

• Sulfides

What type of reaction occurs when cadmium sulfide forms?

• Acid-base reaction

• Redox reaction

• Precipitation reaction

• Combustion reaction

In the complete ionic equation, which ion is not split into its components?

• Cadmium sulfide

• Ammonium ion

• Nitrate ion

• Cadmium ion

What is the charge of the cadmium ion in the complete ionic equation?

• 1+

• 2+

• 1-

• 2-

Which ions are considered spectator ions in this reaction?

• Cadmium ions

• Sulfide ions

• Cadmium sulfide

• Nitrate ions

What is the net charge on both sides of the net ionic equation?

• 2-

• 1+

• 2+

• 0

Why is it important to remove spectator ions when writing a net ionic equation?

• To identify the precipitate

• To balance the equation

• To determine the reaction type

• To simplify the equation

What ensures that the net ionic equation is correctly balanced?

• Equal number of molecules

• Equal number of compounds

• Equal number of atoms and charges

• Equal number of ions