Net Ionic Equations and Balancing

This video tutorial guides viewers through writing a balanced net ionic equation for the reaction between silver nitrate (AgNO3) and calcium bromide (CaBr2). It begins with balancing the molecular equation, followed by determining the solubility and states of the substances involved. The tutorial then explains how to form the complete ionic equation by splitting strong electrolytes into ions. Next, it demonstrates deriving the net ionic equation by removing spectator ions. Finally, the video concludes with simplifying the coefficients and summarizing the balanced net ionic equation.

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

• Write the complete ionic equation

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

How do you balance the molecular equation for AgNO3 and CaBr2?

• Add more reactants

• Change the products

• Adjust the coefficients

• Remove spectator ions

Which of the following is generally soluble in water?

• Lead sulfate

• Calcium bromide

• Barium carbonate

• Silver bromide

What is the state of silver bromide in the reaction?

• Liquid

• Solid

• Gas

• Aqueous

What is the charge of the nitrate ion?

• 2-

• 1-

• 2+

• 1+

What do you do with spectator ions in a net ionic equation?

• Convert them to solids

• Remove them from the equation

• Include them in the final equation

• Change their charges

Which ions are considered spectator ions in this reaction?

• Nitrate ions

• Silver ions

• Bromide ions

• Calcium ions

What is the final step in simplifying the net ionic equation?

• Change the states of substances

• Include all ions

• Ensure the equation is balanced

• Add more reactants

How can the coefficients in the net ionic equation be simplified?

• By changing the reactants

• By adding more ions

• By reducing them to the lowest terms

• By increasing them

What ensures the neutrality of the final compound in the net ionic equation?

• Equal number of atoms

• Presence of solids

• Removal of all ions

• Balanced charges