Chemical Reactions and Ionic Equations

The video tutorial explains how to write a net ionic equation for the reaction between magnesium and hydrochloric acid. It begins with balancing the molecular equation, identifying the states of each substance, and splitting soluble compounds into ions. The complete ionic equation is then written, and spectator ions are removed to derive the net ionic equation.

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

• Balance the molecular equation

• Split compounds into ions

• Identify spectator ions

• Determine the states of substances

What state is magnesium in during the reaction with hydrochloric acid?

• Aqueous

• Gas

• Solid

• Liquid

Which of the following is typically aqueous in a reaction involving hydrochloric acid?

• Chlorine gas

• Magnesium

• Magnesium chloride

• Hydrogen gas

What charge does a hydrogen ion have in the context of this reaction?

• 2+

• 1+

• 1-

• 2-

In which group of the periodic table is chlorine found, and what is its ionic charge?

• Group 16, 2-

• Group 2, 2+

• Group 17, 1-

• Group 1, 1+

What is the purpose of balancing the equation before writing the complete ionic equation?

• To simplify the reaction

• To identify spectator ions

• To ensure the correct number of ions

• To determine the states of substances

How many chloride ions are present when magnesium chloride dissociates?

• Two

• One

• Three

• Four

What are spectator ions in a chemical reaction?

• Ions that are gases

• Ions that do not change during the reaction

• Ions that participate in the reaction

• Ions that are solids

Which ions are crossed out to derive the net ionic equation?

• Ions that are solids

• Ions that are different on both sides

• Ions that are gases

• Ions that are the same on both sides

What is the final product of the net ionic equation for the reaction between magnesium and hydrochloric acid?

• Hydrogen gas

• Magnesium chloride

• Chlorine gas

• Magnesium oxide