Equations total ionic equation

Describe reactions in aqueous solutions by writing formula unit equations, total ionic equations, and net ionic equations... 

In this chapter we examine some types of chemical reactions. Millions of reactions are known, so it is useful to group them into classes, or types, so that we can deal systematically with these massive amounts of information. We will describe how some compounds behave in aqueous solution, including how well their solutions conduct electricity and whether or not the compounds dissolve in water. We introduce several ways to represent chemical reactions in aqueous solution—formula unit equations, total ionic equations, and net ionic equations—and the advantages and disadvantages of these methods. 

Key Terms Formula equation Total ionic equation Net ionic equation... 

When nickel nitrate and sodium carbonate solutions are combined, solid nickel carbonate precipitates, leaving a solution of sodium nitrate. Write the conventional equation, total ionic equation, and net ionic equation for this reaction. 

Conventional equation, total ionic equation, net ionic equation, spectator ion... 

In Formula Unit Equation In Total Ionic Equation... 

We can now write the complete or total ionic equation for each of the reactions. All we need to do for this step is to write the separated ions and non-ionized species on one line ... 

We can now follow the steps used previously to convert each of these to a total ionic equation ... 

This equation can be written as a total ionic equation. 

This equation does not show the change that occurs, however. It shows the reactants and products as intact compounds. In reality, soluble ionic compounds dissociate into their respective ions in solution. So chemists often use a total ionic equation to show the dissociated ions of the soluble ionic compounds. 

Notice that the precipitate, AgCl, is still written as an ionic formula. This makes sense because precipitates are insoluble, so they do not dissociate into ions. Also notice that the spectator ions appear on both sides of the equation. Here is the total ionic equation again, with slashes through the spectator ions. 

Step 4 This will give you the total ionic equation. Next you can... 

Step 5 Finally, by rewriting the total ionic equation without the spectator ions, you will have the net ionic equation. 

O Briefly compare the relationships among a chemical formula, a total ionic equation, and a net ionic equation. Use sentences or a graphic organizer. 

Write total ionic equations for reactions in aqueous solutions. 

However, it is more correct to describe the reaction by using a total ionic equation as shown below. When you write a total ionic equation, make sure that both the mass and the electric charge are conserved. 

When two solutions are mixed, all of the ions are present in the combined solution. In many cases, some of the ions will react with each other. However, some ions do not react. These spectator ions remain unchanged in the solution as aqueous ions. In the equation above, the K" and NO3 ions appear as aqueous ions both on the reactants side and on the products side. Because K" and NO3 ions are spectator ions in the above reaction, they can be removed from the total ionic equation. What remains are the substances that do change during the reaction. 

Write a total ionic equation for each of the following unbalanced formula equations ... 

Predict the products for each of the following reactions. If no reaction happens, write no reaction. Write a total ionic equation for each reaction that does happen. 

A total ionic equation shows all aqueous ions for a reaction. 

Spectator ions do not change during a reaction and can be removed from the total ionic equation. 

Which ions in a total ionic equation are called spectator ions Why ... 

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