Spectator Ions and Ionic Reactions

The video tutorial explains how to write a balanced net ionic equation for the reaction between nickel(II) chloride and ammonium sulfide. It begins with balancing the molecular equation, then discusses the solubility of the reactants and products, and how to write their states. The tutorial proceeds to split strong electrolytes into ions for the complete ionic equation, identifies spectator ions, and finally writes the net ionic equation. The video emphasizes the importance of conserving charge and atoms in the equation.

What is the chemical formula for nickel(II) chloride?

• Ni2Cl

• NiCl2

• Ni2Cl2

• NiCl

Why do we write 'AQ' next to chlorides in the reaction?

• They are gases

• They are insoluble

• They are very soluble

• They are solids

Why is it important to balance the molecular equation first?

• To make the reaction faster

• To conserve mass and charge

• To ensure the reaction is endothermic

• To determine the color of the solution

What is the role of solubility rules in this reaction?

• To predict the color change

• To determine the state of compounds

• To calculate the reaction rate

• To find the temperature of the reaction

What is the charge on the nickel ion in nickel(II) chloride?

• 0

• 3+

• 1+

• 2+

Which of the following is a spectator ion in the reaction?

• Ammonium ion

• Nickel sulfide

• Nickel ion

• Sulfide ion

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

• They form a solid

• They form a gas

• They remain as spectator ions

• They react with nickel ions

How do you identify spectator ions in a reaction?

• They change color

• They are present in both reactants and products

• They form a precipitate

• They are gases

What is the net ionic equation for the reaction?

• Ni^2+ + 2NH4^+ -> Ni(NH4)2

• Ni^2+ + S^2- -> NiS

• 2NH4^+ + 2Cl^- -> 2NH4Cl

• Ni^2+ + 2Cl^- -> NiCl2

What is the state of nickel sulfide in the reaction?

• Aqueous

• Gas

• Liquid

• Solid