Net Ionic Equations and Solubility

This video tutorial explains how to balance net ionic equations, using the example of silver nitrate (AgNO3) and magnesium iodide (MgI2). It covers balancing the molecular equation, determining the states of substances based on solubility rules, forming the complete ionic equation, and identifying spectator ions to derive the net ionic equation. The tutorial emphasizes the importance of charge and atom balance in chemical reactions.

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

• Identify spectator ions

• Balance the molecular equation

• Determine the solubility of compounds

• Write the complete ionic equation

Why is silver iodide considered a solid in the reaction?

• It is a gas

• It is a precipitate

• It is highly soluble

• It is a strong electrolyte

Which of the following ions is always soluble according to the solubility rules?

• Silver ion

• Nitrate ion

• Iodide ion

• Magnesium ion

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

• 2+

• 2-

• 1+

• 1-

In the complete ionic equation, which ions are not split apart?

• Nitrate ions

• Solid compounds

• Magnesium ions

• Silver ions

What are spectator ions?

• Ions that do not change during the reaction

• Ions that are gases

• Ions that participate in the reaction

• Ions that form a precipitate

Which ions are removed to form the net ionic equation?

• All ions

• Only solid ions

• Spectator ions

• All reactant ions

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

• Variable

• Zero

• Negative

• Positive

Why do we not write the coefficient '1' in the final net ionic equation?

• It is too complex

• It is only used for gases

• It is incorrect

• It is unnecessary by convention

What ensures that the net ionic equation is correctly balanced?

• Equal charges only

• Both equal number of atoms and charges

• Neither atoms nor charges matter

• Equal number of atoms only