Chemistry
Net Ionic Equations
Net ionic equations are chemical equations that show only the soluble, strong electrolytes reacting and omit the spectator ions, which are not involved in the chemical change. This simplifies the equation and highlights the essential chemical reaction. Net ionic equations are commonly used in chemistry to focus on the key components of a reaction.
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eBook - PDFChemistry
Principles and Reactions
- William Masterton, Cecile Hurley(Authors)
- 2020(Publication Date)
- Cengage Learning EMEA(Publisher)
We will use Net Ionic Equations throughout this chapter and indeed the entire text to represent a wide variety of re-actions in water solution. Like all equations, Net Ionic Equations must show ■ ■ atom balance. There must be the same number of atoms of each element on both sides. In the preceding equation, the atoms present on both sides are one calcium atom, one carbon atom, and three oxygen atoms. ■ ■ charge balance. There must be the same total charge on both sides. In this equation, the total charge is zero on both sides. Ca 2 1 ( aq ) 1 CO 3 2 2 ( aq ) ¡ CaCO 3 ( s ) Spectator ions are in solution before, during, and after reaction. EXAMPLE Write a net ionic equation for any precipitation reaction that occurs when dilute solutions of the following ionic compounds are mixed. (a) NaOH and Cu(NO 3 ) 2 (b) Ba(OH) 2 and MgSO 4 (c) (NH 4 ) 3 PO 4 and K 2 CO 3 STRATEGY 1. Follow the plan: Figure 4.3: compound S ions S possible precipitates possible precipitates S (Figure 4.2) S insoluble compound S net ionic equation 2. In writing the net ionic equation, start with the insoluble compound on the right, then write the component ions on the left. Do not forget the physical states: ions ( aq ), product ( s ). SOLUTION (a) Ions in solution Possible precipitates Solubility Net ionic equation Na 1 and OH 2 from NaOH; Cu 2 1 and NO 3 2 from Cu(NO 3 ) 2 NaNO 3 and Cu(OH) 2 NaNO 3 is soluble; Cu(OH) 2 is insoluble. Cu 2 1 ( aq ) 1 2OH 2 ( aq ) S Cu(OH) 2 ( s ). (b) Ions in solution Possible precipitates Solubility Net ionic equation Ba 2 1 and OH 2 from Ba(OH) 2 ; Mg 2 1 and SO 4 2 2 from MgSO 4 Mg(OH) 2 and BaSO 4 Both BaSO 4 and Mg(OH) 2 are insoluble. Mg 2 1 ( aq ) 1 2OH 2 ( aq ) S Mg(OH) 2 ( s ) Ba 2 1 ( aq ) 1 SO 4 2 2 ( aq ) S BaSO 4 ( s ) (c) Ions in solution Possible precipitates Solubility Net ionic equation NH 4 1 and PO 4 3 2 from (NH 4 ) 3 PO 4 ; K 1 and CO 3 2 2 from K 2 CO 3 (NH 4 ) 2 CO 3 and K 3 PO 4 Both (NH 4 ) 2 CO 3 and K 3 PO 4 are soluble.
eBook - PDFChemistry
The Molecular Nature of Matter
- Neil D. Jespersen, Alison Hyslop(Authors)
- 2021(Publication Date)
- Wiley(Publisher)
In water, ionic compounds are completely dissociated into ions and are strong electrolytes. Write balanced molecular, ionic, and Net Ionic Equations. Reactions that occur in solution between ions are called ionic reac- tions. Equations for these reactions can be written in three different ways. In molecular equations, complete formulas for all reactants and products are used. In an ionic equation, soluble strong electro- lytes are written in dissociated (ionized) form; “molecular” formulas 210 CHAPTER 4 Molecular View of Reactions in Aqueous Solutions are used for solids, gases, and weak electrolytes. A net ionic equa- tion is obtained by eliminating spectator ions from the ionic equa- tion, and such an equation allows us to identify other combinations of reactants that give the same net reaction. An ionic or net ionic equa- tion is balanced only if both atoms and charges are balanced. Identify acids and bases based on their names and formulas and write balanced equations showing hydronium and hydroxide ions. An acid is a substance that produces hydronium ions, H 3 O + , when dissolved in water, and a base produces hydroxide ions, OH − , when dissolved in water. The oxides of nonmetals are generally acidic anhydrides and react with water to give acids. Metal oxides are usu- ally basic anhydrides because they tend to react with water to give metal hydroxides or bases. Strong acids and strong bases are also strong electrolytes. Weak acids and weak bases are weak electrolytes, which are incompletely ionized in water. In a solution of a weak electrolyte, there is a chemical equilibrium (dynamic equilibrium) between the non-ionized molecules of the solute and the ions formed by the reaction of the solute with water. Learn how to translate formulas to names and names to formulas for common acids and bases. Binary acids are named with the prefix hydro- and the suffix –ic added to the stem of the nonmetal name, followed by the word acid.
eBook - PDF- Morris Hein, Susan Arena, Cary Willard(Authors)
- 2016(Publication Date)
- Wiley(Publisher)
Charles D. Winters/Science Source Images I n the world today, we continually strive to express infor- mation in a concise, useful manner. From early child- hood, we are taught to translate our ideas and desires into sentences. In mathematics, we learn to describe numerical relationships and situations through mathemati- cal expressions and equations. Historians describe thou- sands of years of history in 500-page textbooks. Filmmakers translate entire events, such as the Olympics, into a few hours of entertainment. Chemists use chemical equations to describe reactions they observe in the laboratory or in nature. For example, as shown in the photo, flames and sparks result when aluminum foil is dropped into liquid bromine. Chemical equations provide us with the means to (1) summarize the reaction, (2) display the substances that are reacting, (3) show the products, and (4) indicate the amounts of all component substances in a reaction. C H A P T E R O U T L I N E 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Why Do Chemical Reactions Occur? 8.4 Types of Chemical Equations 8.5 Heat in Chemical Reactions 8.6 Climate Change The Greenhouse Effect Chemical Equations 8 148 CHAPTER 8 • Chemical Equations 8.1 The Chemical Equation Describe the information present in a chemical equation. Chemical reactions always involve change. Atoms, molecules, or ions rearrange to form different substances, sometimes in a spectacular manner. For example, the thermite reac- tion is a reaction between aluminum metal and iron(III) oxide, which produces molten iron and aluminum oxide. The substances entering the reaction are called the reactants, and the substances formed are called the products. In our example, reactants aluminum iron(III) oxide products iron aluminum oxide During reactions, chemical bonds are broken and new bonds are formed. The reactants and products may be present as solids, liquids, gases, or in solution.
eBook - PDF- John A. Olmsted, Gregory M. Williams, Robert C. Burk(Authors)
- 2020(Publication Date)
- Wiley(Publisher)
This is the law of conservation of charge. A balanced chemical equation describes a chemical reaction in which the amounts of all elements and of electrical charge are conserved. We refer to the species that take part in a chemical reaction as reagents. Reac- tants are reagents that are consumed in a reaction, whereas products are reagents that are produced in a reaction. In addition to providing a list of reactants and products of the reaction, a balanced chemical equation tells us the relative amounts of all the reagents. 1.7 Writing Chemical Equations 33 In this synthesis, the reactants are N 2 and H 2 , which react to produce NH 3 . Here is the balanced chemical equation: 1 N 2 molecule 3 H 2 molecules 2 NH 3 molecules 3 H 2 hydrogen N 2 Nitrogen + plus 2 NH 3 ammonia. Reactants Products 2 N atoms 6 H atoms 2 N atoms 6 H atoms yields All balanced chemical equations have the following features: 1. The reactants appear on the left and the products appear on the right. The arrow joining them indicates the direction of reaction. 2. An integer precedes the formula of each substance. These numbers are the stoichiometric coefficients. When no number appears (as for N 2 in this equation), the stoichiometric coefficient is 1. 3. The stoichiometric coefficients in a chemical equation are the smallest integers that give a balanced equation. 4. Charge is conserved. In this equation, all participants are neutral species, so charge is conserved regardless of the stoichiometric coefficients. Stoichiometric coefficients describe the relative numbers of molecules involved in the reaction. In any actual reaction, immense numbers of molecules are involved, but the rela- tive numbers are always related through the stoichiometric coefficients. Furthermore, these coefficients describe both the relative numbers of molecules and the relative numbers of moles involved in the reaction.
eBook - PDFIntroductory Chemistry
An Active Learning Approach
- Mark Cracolice, Edward Peters, Mark Cracolice(Authors)
- 2020(Publication Date)
- Cengage Learning EMEA(Publisher)
9.12 Other Double-Replacement Reactions Copyright 2021 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Due to electronic rights, some third party content may be suppressed from the eBook and/or eChapter(s). Editorial review has deemed that any suppressed content does not materially affect the overall learning experience. Cengage Learning reserves the right to remove additional content at any time if subsequent rights restrictions require it. 335 9.13 Summary of Net Ionic Equations 9.13 Summary of Net Ionic Equations Table 9.4 summarizes this chapter. The blue area is essentially the same as the last three rows of Table 8.3 in Section 8.11 (the table that summarized writing conven- tional equations). Na 1 (aq) 1 Cl 2 (aq) 1 K 1 (aq) 1 NO 3 2 (aq) S NR The total ionic equation is Na 1 (aq) 1 Cl 2 (aq) 1 K 1 (aq) 1 NO 3 2 (aq) S Na 1 (aq) 1 Cl 2 (aq) 1 K 1 (aq) 1 NO 3 2 (aq) You don’t necessarily have a reaction every time you mix solutions of ionic compounds! There is no net ionic equation for this combination because there is no reaction. Complete the Active Example. You improved your skill at writing Net Ionic Equations in gen- eral and understanding what happens when solutions are mixed and in which no reaction occurs in particular. What did you learn by working this Active Example? Practice Exercise 9.18 Write the net ionic equation that represents what happens when solutions of sodium nitrate and ammonium sulfate are mixed.
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