Net Ionic Equations and Reactions

The video tutorial explains how to write and balance net ionic equations using the example of sodium chloride and zinc nitrate. It begins by balancing the molecular equation, then discusses the solubility of compounds and their states. The tutorial demonstrates that all ions remain unchanged, indicating no reaction occurs. The complete ionic equation is analyzed, showing identical reactants and products, leading to the conclusion that no net ionic equation is necessary.

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

• Determine the solubility of compounds

• Write the complete ionic equation

• Balance the molecular equation

• Identify the spectator ions

How do you balance the chlorines in the reaction between NaCl and Zn(NO3)2?

• Add a coefficient of 2 in front of NaCl

• Add a coefficient of 3 in front of Zn(NO3)2

• Add a coefficient of 2 in front of Zn(NO3)2

• Add a coefficient of 3 in front of NaCl

What is the state of sodium chloride in the reaction?

• Gas

• Liquid

• Solid

• Aqueous

What is the role of solubility in determining the state of compounds?

• It determines if a compound is gaseous

• It determines if a compound is liquid

• It determines if a compound is solid

• It determines if a compound is aqueous

Why is there no reaction in the complete ionic equation for NaCl and Zn(NO3)2?

• All ions are different in reactants and products

• A new compound is formed

• All ions are the same in reactants and products

• There is a change in the state of ions

What is observed in the complete ionic equation for NaCl and Zn(NO3)2?

• Formation of a precipitate

• No change in ions

• Gas evolution

• Color change

What happens to the nitrate ions in the reaction?

• They form a new compound

• They remain unchanged

• They precipitate out

• They react with sodium ions

Which ions are considered spectator ions in this reaction?

• Zinc and nitrate ions

• Chloride and zinc ions

• Sodium and nitrate ions

• Sodium and chloride ions

What is the conclusion about the net ionic equation for the reaction?

• The reaction forms a precipitate

• The reaction is exothermic

• A net ionic equation can be written

• No net ionic equation can be written