The reactants must be soluble and both nitrates and sodium salts are alwaysī. Appropriate spectator ions mightīe nitrate as anion and sodium as cation. Is with S 2- in the reactants do not take part in Whatever anion is with Cu 2+ and whatever cation the net ionic equation for theįormation of Cus would show only these two ions. The formula of copper (II) sulfide is CuS. Write the net ionic equation for the formation of a precipitate ofįor each reaction name the appropriate spectator ions.Ī. Write the net ionic equation for the formation of the insoluble compoundī. Now we must also be certain that equations are balanced by charge that is, the total charge on the reactants must equal the total charge on the products.Ī. Previously we have been concerned only with balancing equations by numbers and kinds of atoms. Like all equations, net ionic equations must be balanced. It is present as a spectator ion and need not be shown in the equation. This statement gives us enough information to write the equationĪgain, the identity of the anion of the acid is not important. When magnesium is added to an acid, hydrogen gas and magnesium ions are formed. Net ionic equations are also useful in showing displacement reactions. The chloride and potassium ions are nonparticipating spectator ions. (b) When hydrochloric acid is added to a solution of potassium nitrate, the hydrogen ions of the acid combine with the hydroxide ions of the potassium hydroxide to form molecules of water. The sodium and the nitrate ions are nonparticipating spectator ions. They would not appearįIGURE 11.5 (a) When a solution of silver nitrate is added to a solution of sodium chloride, the silver ions combine with the chloride ions to form a precipitate of silver chloride. This equation shows clearly that the hydrogen and the hydroxide ions reactĪnd that the sodium and chloride ions are spectator ions. Rewriting this equation to show the acid, the hydroxide, and the salt as ions - which is the way these compounds exist in solution - would give the equation For example, the equation for the reaction of hydrochloric acid with sodium hydroxide would be Previously we would have written this neutralization reaction using complete formulas. Hydrogen ions and hydroxide ions react to form water, a covalent All acids release hydrogen ions in solution. When an acid reacts with a hydroxide, water andĪ salt are formed. The net ionic equation for the reaction of silver ion with chloride isĬonsider another situation. The best equation for a reaction is one that shows only the participating ions such an equation is called the ![]() Meaning that they do not participate in the reaction - just as people in the stands at a football game are spectators, meaning that they do not participate in the game. This last equation shows clearly that only the silver and the chloride ions take part in the reaction the sodium and nitrate ions do nothing. Assuming that nitrate was the anion with silver and sodium the cation with chloride, the equation would have beenĪnother way to write the equation shows the ionic compounds in solution as separate ions: (the supernatant liquid), but they do not participate in the reaction (see FigureĮarlier we would have written the equation differently. The other ions are still present in the solution surrounding the precipitate We can write an equation for the reaction: When the two solutions are combined, a white precipitate of silver chloride forms. The second contains chloride ions and a cation whose chloride is soluble. One contains silver ions and an anion whose silver salt is soluble. In solution, the sodium ions and the chloride ions behave independently of each other.Ĭonsider a particular example of this independent behavior. ![]() In the solid state, these ions are arranged in a three-dimensional lattice, one kind of ion alternating with the other. It exists not as sodium chloride units but as sodium ions and chloride ions. Sodium chloride is a typical ionic compound. ![]() One kind (cations) carry a positive charge, and the second kind (anions) carry a negative charge. The former are a combination of two different kinds of particles. The latter exist as molecules whether in the pure state (crystals, liquids) or in solution. Ionic compounds are different from those containing only covalent bonds.
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