Net Ionic Equations and Spectator Ions

This video tutorial guides viewers through writing the balanced net ionic equation for the reaction between nickel(II) bromide and ammonium sulfide. It begins with balancing the molecular equation, followed by determining the solubility and states of the compounds involved. The tutorial then explains how to form the complete ionic equation by splitting strong electrolytes into ions. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring charge conservation and summarizing the process.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

How do you balance the number of bromine atoms in the molecular equation?

• Add a coefficient of 2 in front of ammonium sulfide

• Add a coefficient of 2 in front of ammonium bromide

• Add a coefficient of 2 in front of nickel(II) bromide

• Add a coefficient of 2 in front of nickel(II) sulfide

Which of the following compounds is generally insoluble?

• Ammonium bromide

• Nickel(II) sulfide

• Nickel(II) bromide

• Ammonium sulfide

What is the state of nickel(II) sulfide in the reaction?

• Liquid

• Aqueous

• Solid

• Gas

What is the charge of the bromide ion?

• 2-

• 1-

• 2+

• 1+

What is the charge of the nickel ion in this reaction?

• 2-

• 2+

• 1+

• 1-

Which ion is always 1+ in charge?

• Bromide ion

• Nickel ion

• Ammonium ion

• Sulfide ion

Which ions are considered spectator ions in this reaction?

• Nickel(II) sulfide

• Nickel(II) ions

• Ammonium ions

• Sulfide ions

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

• 2+

• 2-

• 0

• 1+

What happens to spectator ions in the net ionic equation?

• They are included in the final equation

• They are removed from the equation

• They change their charge

• They form a new compound