\[\ce{SO_3} \left( g \right) + \ce{H_2O} \left( l \right) \rightarrow \ce{H_2SO_4} \left( aq \right)\]. Fluorine is the most reactive halogen, while iodine is the least. A double-replacement reaction is a reaction in which the positive and negative ions of two ionic compounds exchange places to form two new compounds. A double-replacement reaction occurs between sodium sulfide and hydrogen chloride. \[2 \ce{S} \left( s \right) + 3 \ce{O_2} \left( g \right) \rightarrow 2 \ce{SO_3} \left( g \right) \nonumber \]. Double Displacement Reactions. Become familiar with some of the observable signs of these reactions. Here are some examples of each kind of double replacement reaction . When aqueous hydrochloric acid is reacted with aqueous sodium hydroxide, the products are aqueous sodium chloride and water. Ammonium ion and nitrate ion are \(1+\) and \(1-\) respectively, while barium and sulfate are \(2+\) and \(2-\). Double replacement reactions are also called double displacement reactions or metathesis reactions. A precipitate forms in a double-replacement reaction when the cations from one of the reactants combine with the anions from the other reactant to form an insoluble ionic compound. Example \(\PageIndex{1}\): Combustion of Solid Potassium. Sulfur trioxide gas reacts with water to form sulfuric acid. -- predict the reaction type (precipitation, neutralization or gaseous) -- record your observations Formulas are correct and the resulting combination reaction is balanced. Write the balanced chemical equation for the combination reaction of potassium with oxygen. 1. Example 1: When solutions of sodium sulfate and silver nitrate are mixed, there is an immediate formation of a precipitate. Also be aware that skin discoloration will result from contact with AgNO3. Both are double replacement reactions. A precipitation reaction, therefore, is predicted to occur, as described by the following equations: \[\ce{NaF}(aq)+\ce{AgNO3}(aq)\rightarrow \ce{AgF}(s)+\ce{NaNO3}(aq)\hspace{20px}\ce{(molecular)}\], Example \(\PageIndex{1}\): Predicting Precipitation Reactions. There are very strong attractive forces that occur between \(\ce{Pb^{2+}}\) and \(\ce{I^-}\) ions and the result is a brilliant yellow precipitate (see figure below). When solutions of sodium sulfide and hydrochloric acid are mixed, the products of the reaction are aqueous sodium chloride and hydrogen sulfide gas. In adouble replacement reactions,typically one of the products is a precipitate, a gas, or a molecular compound. breaks into its ions in solution. If you determine that a reaction will occur, write the correct formula(s) of the products after the arrow. -- write the balanced equation, including all physical states. Precipitation reactions and neutralization reactions are two common types of double replacement reactions. AgNO (aq) + NaCl (aq) AgCl (s) + NaNO (aq) Most phosphates, carbonates, chromates and sulfides are insoluble (except those of the alkali metals and ammonium). A precipitate forms in a double-replacement reaction when the cations from one of the reactants combine with the anions from the other reactant to form an insoluble ionic compound. Neutralization reactions are exothermic, and are generally accompanied by a noticeable release of heat. Sulfur can also combine with oxygen to form sulfur trioxide. Aqueous sodium chloride + aqueous silver nitrate, Aqueous sodium phosphate + aqueous copper (II) sulfate, Hydrochloric acid + solid sodium bicarbonate (just a small scoop), Aqueous nickel (II) nitrate + aqueous sodium hydroxide, Hydrochloric acid + aqueous sodium hydroxide, Aqueous sodium carbonate + aqueous cobalt (II) nitrate, Aqueous sodium chloride + aqueous potassium nitrate, Aqueous iron (III) chloride + aqueous ammonium hydroxide. -- predict the names and states of the products formed Double replacement reactions can be of two major types: (1) precipitation reactions wherein, at least one of the products forms a solid precipitate during the reaction, and (2) acid-base neutralization reactions, wherein an acid is neutralized by a base to form a salt and water. Compounds swap parts and you have new materials. Magnesium reacts rapidly and dramatically when ignited, combining with oxygen from the air to produce a fine powder of magnesium oxide. For example, mixing solutions of silver nitrate and sodium fluoride will yield a solution containing Ag+, \(\ce{NO3-}\), Na+, and F ions. Write the rest of the chemical equation and balance it. The equation is then easily balanced with coefficients. In A, the production of a gas drives the reaction. Ammonium ion and nitrate ion are \(1+\) and \(1-\) respectively, while barium and sulfate are \(2+\) and \(2-\). Double-replacement reactions generally occur between substances in aqueous solution. Take this reaction into consideration NaOH (s) +HCl (l) HX2O (l) +NaCl (aq) N a O H ( s) + H C l ( l) H X 2 O ( l) + N a C l ( a q) none of the products are insoluble. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. When finished, complete the data sheet by writing the balanced equation for each reaction. The solubility guidelines indicate PbCO3 is insoluble, and so a precipitation reaction is expected. Video \(\PageIndex{2}\): Mercury (II) oxide is a red solid. NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l) Neutralization reactions are feasible as double displacement reaction thanks to the production of water H2O, a weak electrolyte that barely disassociate on its own. Precipitation reactions involve the formation of one or more insoluble products. Write a complete and balanced chemical equation for the following double-replacement reactions. A combination reaction is a reaction in which two or more substances combine to form a single new substance. The only discernable difference between these patterns is the order in whichthe products, "QD" and "AZ," are written. The general form of a decomposition reaction is: Most decomposition reactions require an input of energy in the form of heat, light, or electricity. The double-replacement reaction generally takes the form of AB + CD AD + CB where A and C are positively-charged cations, while B and D are negatively-charged anions. A double replacement reaction occurs when two reactants swap bonds. Predict the products of simple reactions. Many reactions of this type involve the exchange of ions between ionic compounds in aqueous solution and are sometimes referred to as double displacement, double replacement, or metathesis reactions. Precipitation reactions are an example of a double-displacement reaction. Accessibility StatementFor more information contact us atinfo@libretexts.org. The cations of both reactants are \(+1\) charged ions, while the anions are \(-1\) charged ions. Example 6: Name the ionic compound Al(NO3)3. Many examples in this category are reactions that produce water. \[\ce{Al} + \ce{Fe_2O_3} \rightarrow \ce{Al_2O_3} + \ce{Fe} \nonumber\], \[2 \ce{Al} + \ce{Fe_2O_3} \rightarrow \ce{Al_2O_3} + 2 \ce{Fe} \nonumber\]. The first four types of reactions will be discussed in this section. where \(\ce{Y}\) is a nonmetal and replaces the nonmetal \(\ce{Z}\) in the compound with \(\ce{X}\). In double-replacement reaction,one ofthree possible types of products usually form. Aqueous sodium chloride + aqueous potassium nitrate, 9. Indeed, such double precipitations are very much possible, though rare. Combination reactions can also be called synthesis reactions or condensation or addition reactions. Summary. (a) The two possible products for this combination are KNO3 and BaSO4. Inform your instructor of any chemical contact as soon as possible. Meaning that as the reaction proceeds, the formation of water would act like a H+ / OH . Predict the result of mixing reasonably concentrated solutions of the following ionic compounds. A double replacement reaction will occur if a formation of a precipitate , gas or water takes place. \[\ce{Mg} \left( s \right) + \ce{Cu(NO_3)_2} \left( aq \right) \rightarrow \ce{Mg(NO_3)_2} \left( aq \right) + \ce{Cu} \left( s \right)\]. \[\ce{(NH_4)_2SO_4} \left( aq \right) + \ce{Ba(NO_3)_2} \left( aq \right) \rightarrow 2 \ce{NH_4NO_3} \left( aq \right) + \ce{BaSO_4} \left( s \right)\nonumber \]. The general form of a double-replacement (also called double-displacement) reaction is: \[\ce{AB} + \ce{CD} \rightarrow \ce{AD} + \ce{BC}\]. When solutions of sodium sulfide and hydrochloric acid are mixed, the products of the reaction are aqueous sodium chloride and hydrogen sulfide gas. Legal. This must be taken into account when exchanging partners and writing the new formulas. An example of a precipitation reaction is given below: (1) C d S O 4 ( a q) + K 2 S ( a q) C d S ( s) + K 2 S O 4 ( a q) To predict the products, we need to know that aluminum will replace iron and form aluminum oxide (the metal will replace the metal ion in the compound). The products of the reaction are aqueous magnesium nitrate and solid copper metal. In order for a reaction to occur, one of the products is usually a solid precipitate, a gas, or a molecular compound such as water. Accessibility StatementFor more information contact us atinfo@libretexts.org. One merely needs to identify all the ions present in the solution and then consider if possible cation/anion pairing could result in an insoluble compound. One product is indicated as a guide. 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Then, the equation is balanced. We can write that as follows: hydrogen reacts with oxygen to make water We can represent this chemical change more succinctly as hydrogen + oxygen water The cations of both reactants are \(+1\) charged ions, while the anions are \(-1\) charged ions. For purposes of predicting the identities of solids formed by precipitation reactions, one may simply refer to patterns of solubility that have been observed for many ionic compounds (Table \(\PageIndex{1}\)). Two compounds may also react to form a more complex compound. After exchanging partners, the balanced equation is: \[\ce{NaCN} \left( aq \right) + \ce{HBr} \left( aq \right) \rightarrow \ce{NaBr} \left( aq \right) + \ce{HCN} \left( g \right)\]. (You cannot swap both; you would end up with the same substances you started with.) In adouble replacement reactions,typically one of the products is a precipitate, a gas, or a molecular compound. This reaction is generally a double replacement reaction in the form: AB (aq) + CD (aq) AD + CB The question remains, will AD or CB remain in solution or form a solid precipitate? Note the abbreviation "\(\text{elec}\)" above the arrow to indicate the passage of an electric current to initiate the reaction. Example 5: Write the formula for magnesium phosphate. A single-replacement reaction is a chemical reaction in which one element is substituted for another element in a compound, generating a new element and a new compound as products. A double-replacement reaction occurs when parts of two ionic compounds are exchanged, making two new compounds. other via strong electrostatic forces. It is. \[\ce{S} \left( s \right) + \ce{O_2} \left( g \right) \rightarrow \ce{SO_2} \left( g \right) \nonumber \]. All formulas are correct and the equation is balanced. Both carbonic acid and sulfurous acid are unstable and will decompose to form carbon dioxide and sulfur dioxide gases, respectively: sulfuric acid + aqueous lithium hydroxide. The general forms of these sixkinds of reactions are summarized in Table \(\PageIndex{1}\), along with examples of each. 2. Click here to view We have moved all content for this concept to for better organization. Then, the equation is balanced. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is. Mercury (II) oxide, a red solid, decomposes when heated to produce mercury and oxygen gas. Combination reactions can also take place when an element reacts with a compound to form a new compound composed of a larger number of atoms. A vivid example of precipitation is observed when solutions of potassium iodide and lead nitrate are mixed, resulting in the formation of solid lead iodide: \[\ce{2KI}(aq)+\ce{Pb(NO3)2}(aq)\rightarrow \ce{PbI2}(s)+\ce{2KNO3}(aq)\]. A good estimate is to use three full dropper squirts of each chemical. Potassium is a very reactive alkali metal that must be stored under oil in order to prevent it from reacting with air. A metal carbonate decomposes into a metal oxide and carbon dioxide gas. A precipitation reaction is a double-replacement reaction in which one product is a solid precipitate. More information on these important concepts is provided in the text chapter on solutions. A double replacement reaction is a type of chemical reaction that occurs when two reactants exchange cations or anions to yield two new products. A precipitation reaction is one in which dissolved substances react to form one (or more) solid products. For ionic compounds, it means that the compound. Either perspective should allow you to predict the proper products, as long as you pair a cation with an anion and not a cation with a cation or an anion with an anion. Aqueous nickel(II) nitrate + aqueous sodium hydroxide. The reaction of a sodium carbonate solution with hydrochloric acid produces aqueous sodium chloride, carbon dioxide gas, and water. \[\ce{Na_2CO_3} \left( aq \right) + 2 \ce{HCl} \left( aq \right) \rightarrow 2 \ce{NaCl} \left( aq \right) + \ce{CO_2} \left( g \right) + \ce{H_2O} \left( l \right)\nonumber \]. In a double replacement, the ions . This page titled 11.9: Double Replacement Reactions is shared under a CK-12 license and was authored, remixed, and/or curated by CK-12 Foundation via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request. All formulas are correct and the equations are balanced. When nonmetals react with one another, the product is a molecular compound. The net ionic equation for this reaction, derived in the manner detailed in the previous module, is, (c) The two possible products for this combination are PbCO3 and NH4NO3. \[2 \ce{HgO} \left( s \right) \rightarrow 2 \ce{Hg} \left( l \right) + \ce{O_2} \left( g \right)\]. Aqueous iron (III) chloride + aqueous ammonium hydroxide, 5. To determine whether a product ionic compound will be soluble or insoluble, consult the Solubility Rules provided at the end of the Background section. cation = iron (III) = Fe+3 anion = chloride = Cl-1 \[2 \ce{Na} \left( s \right) + \ce{Cl_2} \left( g \right) \rightarrow 2 \ce{NaCl} \left( s \right) \nonumber \]. Formation of a Precipitate. A reaction is also considered to be a decomposition reaction even when one or more of the products are still compounds. Write a balanced equation for the decomposition of water. Precipitation: The water-soluble ionic compounds undergo a reaction to form a water-insoluble product then it is termed as a precipitation reaction. For example, calcium carbonate decomposes into calcium oxide and carbon dioxide. One product is indicated as a guide. Many reactions of this type involve the exchange of ions between ionic compounds in aqueous solution and are sometimes referred to as double displacement, double replacement, or metathesis reactions. A characteristic of a double-replacement equation is that there are two compounds as reactants and two different compounds as products. Combine the ions in a ratio that results in the formation of a neutral ionic compound. How is that a problem? 4.7: Double Replacement Reactions is shared under a CC BY-NC license and was authored, remixed, and/or curated by LibreTexts. The general form of a double-replacement (also called double-displacement) reaction is: \[\ce{AB} + \ce{CD} \rightarrow \ce{AD} + \ce{CB}\nonumber \]. The general form of a double-replacement (also called double-displacement) reaction is: \[\ce{AB} + \ce{CD} \rightarrow \ce{AD} + \ce{CB}\nonumber \]. If results are not obtained immediately, give the reaction some time. (*Note: zinc forms ions with a \(+2\) charge), Predict the products for the following reaction: \(\ce{Fe} + \ce{CuSO_4}\) (in this reaction, assume iron forms ions with a \(+2\) charge). Credit: MrLundScience. One of the products could also be carbonic acid (H2CO3) or sulfurous acid (H2SO3). are soluble except for those containing Ag, Most sulfates are soluble, except for BaSO. The products are elements and the equation is balanced. 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\|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Example \(\PageIndex{1}\): Double-Replacement Reactions, http://commons.wikimedia.org/wiki/File:Barter-Chickens_for_Subscription.jpg(opens in new window), https://www.flickr.com/photos/44200742@N07/5533819494(opens in new window), source@https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/, \(\ce{NaCN} \left( aq \right) + \ce{HBr} \left( aq \right) \rightarrow\) (hydrogen cyanide gas is formed), \(\ce{(NH_4)_2SO_4} \left( aq \right) + \ce{Ba(NO_3)_2} \left( aq \right) \rightarrow\) (a precipitate of barium sulfate forms), The double-replacement reaction generally takes the form of. Aqueous sodium chloride + aqueous silver nitrate. A double-replacement reaction is a reaction in which the positive and negative ions of two ionic compounds exchange places to form two new compounds. cation = magnesium = Mg+2 anion = phosphate = PO4 -3 Write a complete and balanced chemical equation for the double-replacement reaction \(\ce{(NH_4)_2SO_4} \left( aq \right) + \ce{Ba(NO_3)_2} \left( aq \right) \rightarrow\) (a precipitate of barium sulfate forms). All halides (chlorides etc.) A precipitate forms in a double-replacement reaction when the cations from one of the reactants combine with the anions from the other reactant to form an insoluble ionic compound. The products of such a reaction are the metal hydroxide and hydrogen gas. Usually, a double displacement reaction results in precipitate formation. Most chemical reactions can be classified into one or more of sixbasic types: combinationreactions, decomposition reactions, the two exchange reactions, acidbase reactions, combustion reactions, and oxidationreduction reactions. A very common example is the reactions of oxides with water. \[\ce{Na_2S} \left( aq \right) + 2 \ce{HCl} \left( aq \right) \rightarrow 2 \ce{NaCl} \left( aq \right) + \ce{H_2S} \left( g \right)\nonumber \]. Somechemicalreactionsare like that. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. A precipitate will form if the resulting compound is insoluble in water. There are very strong attractive forces that occur between \(\ce{Pb^{2+}}\) and \(\ce{I^-}\) ions and the result is a brilliant yellow precipitate (Figure \(\PageIndex{3}\)). If you determine that a reaction will not occur, write no reaction after the arrow. 5.4: Classifying Chemical Reactions is shared under a not declared license and was authored, remixed, and/or curated by Deboleena Roy (American River College). However carbonic acid decomposes to carbon dioxide and water: \[\ce{2 HNO3 (aq) + NaHCO3 (aq) 2 NaNO3 (aq) + H2CO3 (aq)}\] decomposes, \[\ce{2 HNO3 (aq) + NaHCO3 (aq) 2 NaNO3 (aq) + H2O (l) + CO2 (g)}\]. A precipitation reaction is a double-replacement reaction in which one product is a solid precipitate. The solubility guidelines indicate all nitrate salts are soluble but that AgF is one of the exceptions to the general solubility of fluoride salts. Solubility rules are used to predict whether some double-replacement reactions will occur. { "6.3.01:_Practice_Problems-_Precipitation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "6.01:_Solutions_and_Solution_Concentration" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.02:_Solutions_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.03:_Precipitation_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.04:_Classifying_Chemical_Reactions_(Acids_and_Bases)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6.05:_Classifying_Chemical_Reactions_(Redox)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Matter_and_Measurement" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms_and_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Nuclei_Ions_and_the_Periodic_Table" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Molecules_Compounds_and_Quantifying_Chemicals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Transformations_of_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Aqueous_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Ideal_Gas_Behavior" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Thermochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "showtoc:no", "source[1]-chem-98782", "source[2]-chem-98782" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FOregon_Tech_PortlandMetro_Campus%2FOT_-_PDX_-_Metro%253A_General_Chemistry_I%2F06%253A_Aqueous_Reactions%2F6.03%253A_Precipitation_Reactions, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), \[\ce{Ag+}(aq)+\ce{F-}(aq)\rightarrow \ce{AgF}(s)\hspace{20px}\ce{(net\: ionic)}\], \[\ce{Ag+}(aq)+\ce{Cl-}(aq)\rightarrow \ce{AgCl}(s) \nonumber\], \[\ce{Pb^2+}(aq)+\ce{CO3^2-}(aq)\rightarrow \ce{PbCO3}(s) \nonumber\], Precipitation Reactions and Solubility Rules, 6.2.1: Practice Problems- Solutions Chemistry, http://cnx.org/contents/85abf193-2bda7ac8df6@9.110, Types of Chemical Reactions Rachael Harper Delupio, Lost Angles Trade Technical College, Classifying Chemical Reactions,Nicola Burrmann, Heartland Community College, Classify chemical reactions as one of these three types given appropriate descriptions or chemical equations. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Somechemicalreactionsare like that. How do chemists cope with this overwhelming diversity? One type of combination reaction that occurs frequently is the reaction of an element with oxygen to form an oxide. Perform the following reactions, and record your observations for each on the data sheet. Use IUPAC nomenclature rules to write the chemical formula or the chemical name. Write the rest of the chemical equation and balance it. In order for a reaction to occur, one of the products is usually a solid precipitate, a gas, or a molecular compound such as water. A double-replacement reaction occurs between sodium sulfide and hydrogen chloride. The general form of a combination reaction is: One combination reaction is two elements combining to form a compound. All formulas are correct and the equations are balanced. The other product of the reaction, potassium nitrate, remains soluble. All double replacement reactions have the general form: Reactions that can be classified as double replacements include precipitation reactions, neutralization reactions and gas forming reactions. Solutions: 6 M sodium hydroxide, 3 M sulfuric acid, 6 M hydrochloric acid; all other solutions are 0.1 M and include silver nitrate, sodium chloride, iron (III) chloride, ammonium hydroxide, sodium carbonate, cobalt (II) nitrate, sodium phosphate, copper (II) sulfate, potassium nitrate, nickel (II) nitrate, barium chloride. Some unstable acids decompose to produce nonmetal oxides and water. \[\ce{Pb(NO3)2 (aq) + 2 NaCl (aq) 2 NaNO3 (aq) + PbCl2 (s)}\]. What is the formula for the expected precipitate? Compounds swap parts and you have new materials. Notice that in order to write and balance the equation correctly, it is important to remember the seven elements that exist in nature as diatomic molecules (\(\ce{H_2}\), \(\ce{N_2}\), \(\ce{O_2}\), \(\ce{F_2}\), \(\ce{Cl_2}\), \(\ce{Br_2}\), and \(\ce{I_2}\)). First identify the cation and anion in this compound. Accessibility StatementFor more information contact us atinfo@libretexts.org. Balance the equation (to ensure mass conservation). The reaction of a sodium carbonate solution with hydrochloric acid produces aqueous sodium chloride, carbon dioxide gas, and water. compounds of these anions with group 1 metal cations and ammonium ion, hydroxides of group 1 metal cations and Ba, Adelaide Clark, Oregon Institute of Technology, Crash Course Chemistry: Crash Course is a division of. This video is a response to a comment that reads as follows:"What should I do if the problem only gives me the left side of the equation? Calcium oxide reacts readily with water to produce an aqueous solution of calcium hydroxide. This must be taken into account when exchanging partners and writing the new formulas. For example: 2HCl (aq) + Zn (s) ZnCl 2 (aq) + H 2 (g) is an example of a single-replacement reaction. The predicted products are lead (II) chloride (insoluble) and sodium nitrate (soluble). Write chemical formulas for each reactant and place a yield arrow ( ) after the last reactant. The extent to which a substance may be dissolved in water, or any solvent, is quantitatively expressed as its solubility, defined as the maximum concentration of a substance that can be achieved under specified conditions. A and B are cations and X and Y are anions. The element chlorine reacts with an aqueous solution of sodium bromide to produce aqueous sodium chloride and elemental bromine. Faced with a wide range of varied interactions between chemical substances, scientists have found it convenient (or even necessary) to classify chemical interactions by identifying common patterns of reactivity. Legal. The acid formed in the reaction falls to the ground as acid rain. The following threemodules will provide an introduction to three of the most prevalent types of chemical reactions: precipitation, acid-base, and oxidation-reduction. There is no commandment that says "Thou shalt not have two precipitates in one reaction". You have something I want, and I have something you want. If we start with solid sodium chloride and solid silver nitrate crystals there is no. Download for free at http://cnx.org/contents/85abf193-2bda7ac8df6@9.110). Both the cation and anion must be named. The most famous example is probably the formation of lithopone. Metal hydroxides decompose on heating to yield metal oxides and water. When the element that is doing the replacing is a nonmetal, it must replace another nonmetal in a compound, and the general equation becomes: \[\ce{Y} + \ce{XZ} \rightarrow \ce{XY} + \ce{Z}\]. The generic balanced chemical equation is AX + BY AY+ BX. For a double replacement to occur, you must start with two ionic compounds in aqueous solution (dissolved in water). In B, the production of a precipitate drives the reaction. In order for a reaction to occur, one of the products is usually a solid precipitate, a gas, or a molecular compound such as water. In a double-replacement reaction, what type of compounds are usually the reactants? Balance the equation. Zinc reacts with hydrochloric acid to produce aqueous zinc chloride and hydrogen (figure below). Double-replacement reactions generally occur between substances in aqueous solution. Accessibility StatementFor more information contact us atinfo@libretexts.org. If precipitation is expected, write a balanced net ionic equation for the reaction. Predict the products for the following reaction: \(\ce{CO_2} \left( g \right) + \ce{H_2O} \left( l \right)\), Write the chemical equation for the single replacement reaction between zinc solid and lead (II) nitrate solution to produce zinc nitrate solution and solid lead. The practice of barter (trading one thing for another) has been in existencefor a very longtime. Aqueous barium chloride + sulfuric acid, 6. This subcategory of single-replacement reactions is called a metal replacement reaction because it is a metal that is being replaced (copper). Precipitation reactions also play a central role in many chemical analysis techniques, including spot tests used to identify metal ions and gravimetric methods for determining the composition of matter (see the last module of this chapter). Write a complete and balanced chemical equation for the following double-replacement reactions. Perform and observe the results of a variety of double replacement reactions. In this reaction, \(\ce{A}\) and \(\ce{C}\) are positively-charged cations, while \(\ce{B}\) and \(\ce{D}\) are negatively-charged anions. Some metals are so reactive that they are capable of replacing the hydrogen in water. Occasionally, a reaction will produce both a gas and a molecular compound. Be especially cautious when using the 6M HCl, 3M H2SO4 and 6M NaOH as they can burn your skin. A double displacement precipitation is a reaction in which two soluble ionic compounds react to form an insoluble precipitate. It is important to note, however, that many reactions can be assigned to more than one classification, as you will see in our discussion. Write the chemical equation for the synthesis of silver bromide, \(\ce{AgBr}\). Many examples in this category are reactions that produce water. In both cases, use the ionic charges of both reactants to construct the correct formulas of the products. The double-replacement reaction generally takes the form of AB + CD AD + CB where A and C are positively-charged cations, while B and D are negatively-charged anions. For a neutral compound, three Mg+2 are needed for every 2 PO4 -3 The formula of the compound is Mg3(PO4)2. 7.1 LectureDouble Replacement ReactionsPrecipitation Reaction (insoluble product)Gas Forming Reaction (bubbles)Neutralization Reaction (water formed)No React. \[\ce{CaO} \left( s \right) + \ce{H_2O} \left( l \right) \rightarrow \ce{Ca(OH)_2} \left( aq \right)\]. How do they predict which compounds will react with one another and what products will be formed? A double-replacement reaction is a reaction in which the positive and negative ions of two ionic compounds exchange places to form two new compounds. In a hydrogen replacement reaction, the hydrogen in the acid is replaced by an active metal. The result is two new compounds. \[\ce{H2SO4 (aq) + 2 LiOH (aq) Li2SO4 (aq) + 2 H2O (l)}\]. Many examples in this category are reactions that produce water. In double-replacement reaction,one ofthree possible types of products usually form. Describe each of the following compounds as ionic, covalent, or acid. Sodium hydroxide decomposes to produce sodium oxide and water. Write balanced chemical equations for each double replacement reaction studied. For a neutral compound, one Fe+3 is needed for every 3 Cl-1 The formula of the compound is FeCl3. Lead iodide is a bright yellow solid that was formerly used as an artists pigment known as iodine yellow (Figure \(\PageIndex{1}\)). \[\ce{K} \left( s \right) + \ce{O_2} \left( g \right) \rightarrow \ce{K_2O} \left( s \right) \nonumber\]. Personal Protective Equipment (PPE) required: safety goggles, lab coat, closed-toe shoes. Precipitation Reaction Reactions of Acids Reactivity Series Redox Reactions Redox Titration Representing Chemical Reactions Single and Double Replacement Reactions Skeleton Equation Stoichiometric Calculations For the reaction: NaCl + AgNO 3 NaNO 3 + AgCl. In a precipitation reaction (one type of double-replacement reaction), two soluble ionic compounds in aqueous solution are mixed and result in an insoluble solid compound called a precipitate. In this general reaction, element \(\ce{A}\) is a metal and replaces element \(\ce{B}\), also a metal, in the compound BC. { "01:_Measurements_in_the_Laboratory_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Paper_Chromatography_of_Gel_Ink_Pens_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_The_Properties_of_Oxygen_Gas_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Detection_and_Absorption_of_Ultraviolet_Light_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Flame_Tests_and_Atomic_Spectra_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Lewis_Structures_and_Molecular_Shapes_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Electrical_Conductivity_of_Aqueous_Solutions_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Acid_Bases_and_pH_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Single_Replacement_Reactions_and_Batteries_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Double_Replacement_Reactions_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Synthetic_Polymers_and_Plastics_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Making_Soap_-_Saponification_(Experiment)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Chem_10_Experiments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chem_11_Experiments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chem_12_Experiments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chem_9_Experiments : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, 10: Double Replacement Reactions (Experiment), [ "article:topic", "double-displacement reactions", "authorname:smu", "showtoc:no", "license:ccbync" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FAncillary_Materials%2FLaboratory_Experiments%2FWet_Lab_Experiments%2FGeneral_Chemistry_Labs%2FOnline_Chemistry_Lab_Manual%2FChem_9_Experiments%2F10%253A_Double_Replacement_Reactions_(Experiment), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), 9: Single Replacement Reactions and Batteries (Experiment), 11: Synthetic Polymers and Plastics (Experiment). After exchanging partners, the balanced equation is: \[\ce{NaCN} \left( aq \right) + \ce{HBr} \left( aq \right) \rightarrow \ce{NaBr} \left( aq \right) + \ce{HCN} \left( g \right)\nonumber \]. There are two equivalent ways of considering a double-replacement equation: either the cations are swapped, or the anions are swapped. A double replacement reaction can occur between two ionic compounds or two covalent compounds. Neutralization, precipitation, and gas formation are types of double replacement reactions. Video \(\PageIndex{2}\): A review of precipitation reactions. Legal. Double replacement reactions take the general form: AB + CD AD + CB. For example: K2S(aq. Equipment: 9 small test tubes, plastic test tube rack. Legal. The solubility guidelines in Table \(\PageIndex{1}\) may be used to predict whether a precipitation reaction will occur when solutions of soluble ionic compounds are mixed together. The cations and anions trade partners resulting in two new ionic compounds (or possibly an acid).

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