Net Ionic Equations and Spectator Ions

This video tutorial explains how to write the net ionic equation for the reaction between silver fluoride (AgF) and potassium bromide (KBr). It begins with balancing the molecular equation, then determining the solubility and states of the compounds involved. The tutorial proceeds to split strong electrolytes into ions to form the complete ionic equation and identifies spectator ions to derive the net ionic equation. The video concludes by ensuring that both charge and atoms are balanced in the final equation.

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

• Write the complete ionic equation

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

Which of the following is generally soluble in water?

• Lead sulfate

• Potassium compounds

• Calcium carbonate

• Silver bromide

What does the 's' symbol indicate in a solubility table?

• Solid

• Soluble

• Saturated

• Suspended

What type of reaction occurs when a solid forms from two aqueous solutions?

• Precipitation reaction

• Redox reaction

• Decomposition reaction

• Combustion reaction

Which ion is not split in the complete ionic equation?

• Silver bromide

• Bromide ion

• Fluoride ion

• Potassium ion

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

• 1+

• 2+

• 1-

• 2-

Which ions are considered spectator ions in this reaction?

• Silver and fluoride ions

• Potassium and fluoride ions

• Potassium and bromide ions

• Silver and bromide ions

What is the net charge of the balanced net ionic equation?

• Zero

• Negative

• Variable

• Positive

What is the final product in the net ionic equation for AgF and KBr?

• AgF

• K+ and F-

• AgBr

• Ag+ and Br-

Why are spectator ions removed in the net ionic equation?

• They change the charge balance

• They form a precipitate

• They do not participate in the reaction

• They are insoluble