Net Ionic Equations and Spectator Ions

The video tutorial explains how to write the balanced net ionic equation for the reaction between strontium hydroxide and iron(II) sulfate. It begins with balancing the molecular equation and identifying the states of each substance. The tutorial then discusses the solubility rules, particularly for strontium sulfate and iron(II) hydroxide, which form precipitates. The complete ionic equation is formed by splitting strong electrolytes into ions, and the net ionic equation is derived by ensuring charge balance and identifying spectator ions. The tutorial concludes with a review of the balanced net ionic equation.

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

• Identify spectator ions

• Write the complete ionic equation

• Balance the molecular equation

• Determine the states of substances

Which of the following is considered a strong base?

• Iron(II) sulfate

• Strontium hydroxide

• Strontium sulfate

• Iron(II) hydroxide

What is the state of strontium sulfate in the reaction?

• Gas

• Aqueous

• Solid

• Liquid

What type of product is formed when strontium hydroxide reacts with iron(II) sulfate?

• Gas

• Precipitate

• Aqueous solution

• Liquid

Which ion is not split in the net ionic equation?

• Strontium sulfate

• Sulfate ion

• Hydroxide ion

• Strontium ion

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

• 1-

• 2-

• 2+

• 1+

Why can't spectator ions be crossed out in this reaction?

• They are not ions

• They are different in reactants and products

• They are not present in the reactants

• They are not present in the products

What is the net charge of the products in the net ionic equation?

• 2-

• 1+

• 2+

• 0

What is the role of spectator ions in a chemical reaction?

• They participate in the reaction

• They change the state of the reaction

• They remain unchanged

• They form new compounds

What ensures that the net ionic equation is correctly balanced?

• Equal number of compounds

• Equal number of ions

• Equal number of atoms and charges

• Equal number of molecules