Net Ionic Equations and Spectator Ions

The video tutorial explains how to write a balanced net ionic equation for the reaction between silver nitrate (AgNO3) and sodium chromate (Na2CrO4). It begins by balancing the molecular equation, then assigns states to each substance based on solubility rules. The tutorial proceeds to split strong electrolytes into ions to form the complete ionic equation. Spectator ions are identified and removed to derive the net ionic equation. The video concludes by ensuring the equation is balanced in terms of charge and atoms.

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

• Write the complete ionic equation

• Determine the solubility of compounds

• Balance the molecular equation

• Identify spectator ions

Why is silver chromate considered a solid in the reaction?

• It is highly soluble in water

• It forms a gas

• It is insoluble and forms a precipitate

• It dissolves completely

What is the purpose of writing the states of substances in a chemical equation?

• To calculate the molecular weight

• To identify the phase of each substance

• To predict the reaction speed

• To determine the color of the compounds

What is the charge of a nitrate ion?

• 1+

• 2-

• 1-

• 2+

How many silver ions are present in the complete ionic equation?

• Three

• Two

• One

• Four

What is the charge on the chromate ion?

• 2+

• 1+

• 2-

• 1-

Which ions are considered spectator ions in this reaction?

• Silver chromate

• Sodium ions

• Silver ions

• Chromate ions

What happens to the sodium ions in the net ionic equation?

• They remain unchanged

• They form a solid

• They react with chromate ions

• They are removed as spectator ions

What is the net charge on the reactant side of the net ionic equation?

• 2+

• 1-

• 0

• 2-

Why is it important to ensure that the net ionic equation is balanced?

• To predict the color of the precipitate

• To make the equation look neat

• To satisfy the law of conservation of mass and charge

• To ensure the reaction is spontaneous