GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 1 of 12Chemical Reactions: Introduction to Reaction TypesIn this experiment, you will observe (on video and in lab) examples of the six basic types of chemicalreactions which are described below. You will write your observations of the reactions. Based onthose observations and the given word equations, you will write complete, balanced chemicalequations to effectively communicate the chemistry of the reactions.Introduction to Reaction Types1. Combination: A + B \u2192 ABIn a combination reaction, a new compound can be formed in one of three ways, by combining: a) 2elements, b) 1 element and 1 binary compound (consisting of 2 elements), or c) 2 binary compounds.The following are examples of combination reactions:The rusting of iron: 4Fe (s) + 3O2 (g) \u2192 2Fe2O3 (s)The formation of one kind of acid rain: SO3 (g) + H2O (l) \u2192 H2SO4 (aq)2. Decomposition: AB \u2192 A + BIn a decomposition reaction, a compound is broken down into two or more substances. In general,decomposition reactions occur when a solid compound is heated. This type of reaction almost alwaysproduces a gas. The following are examples of decomposition reactions:Heating mercury (II) oxide produces oxygen gas: 2HgO (s) \u2192 2Hg (l) + O2 (g).Leaving the cap off the carbonated soft drink bottle allows the carbonic acid to releasecarbon dioxide: H2CO3 (aq) \u2192 H2O (l) + CO2 (g).3. Single Replacement: A + BC \u2192 AC + BIn this type of reaction, a more \u201cactive metal\u201d displaces another element in solution. These reactionscan be further classified as a solid metal reacting with a) a metal ion solution, b) an acid solution, or c)water. An example of each is provided below:a) When a solid metal reacts with a metal solution, the solid metal\u2019s ions go into solutionwhile the metal ions originally in solution plate out onto the surface of solid metale.g., Zn (s) + CuSO4 (aq) \u2192 ZnSO4 (aq) + Cu (s).b) When a solid metal reacts with an acid, the metal replaces hydrogen in the acid to producehydrogen gas while the metal ion goes into solution with the anion from the acide.g., Mg (s) + 2HCl (aq) \u2192 H2 (g) + MgCl2 (aq).c) When a solid metal reacts with water, the metal replaces hydrogen in the water to producehydrogen gas while the metal ion goes into solution with hydroxide ione.g., Ca (s) + 2 H2O (aq) \u2192 H2 (g) + Ca(OH)2 (aq).To predict whether or not a single-replacement reaction will occur, we refer to the Activity Series forMetals (shown on the next page).GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 2 of 12Activity Series for MetalsLi > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe >Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > AuIf a solid metal is \u201cmore active\u201d \u2013 i.e., higher on the Activity Series \u2013 than the metal ion in solution orhydrogen for acids, the more active metal will displace the less active ion, so a reaction occurs. Themore active metal goes into solution while the less active ion either plates out for a metal ion orbubbles out as a gas for hydrogen ion. If the solid metal is less active than the metal ion or hydrogenin the compound, then no reaction occurs. Only six metals (Li, K, Ba, Sr, Ca, and Na) \u2013 called \u201cactivemetals\u201d \u2013 react directly with water to produce hydrogen gas and a metal hydroxide solution. Theseactive metals are the first six metals in the Activity Series.4. Double Replacement\/Precipitation: AB + CD \u2192 AD + CBThese reactions involve the mixing of two aqueous ionic compounds to produce a precipitate, aninsoluble ionic compound. The products of a double-replacement\/precipitation reaction can be predicted by switching the cations of the two compounds and using theSolubility Rules (see below) to determine if the compounds produced are soluble or insoluble.Solubility Rules for Ionic Compounds in WaterThe compound is SOLUBLE if it has:1. Li+, Na+, K+, or NH4+ ion (ALWAYS!)2. C2H3O2\u2013, NO3\u2013, ClO4\u20133. Cl\u2013, Br\u2013, or I\u2013, except compoundswith Ag+, Pb+2, Cu2+, and Hg2+2 areinsoluble4. SO42- except compounds withAg2SO4, CaSO4, SrSO4, BaSO4,PbSO4, and Hg2SO4 are insolubleThe compound is INSOLUBLE if it has:5. CO32\u2013, CrO42\u2013, PO43\u2013, except compoundswith Li+, Na+, K+, NH4+ are soluble6. S2\u2013, except compounds with Li+, Na+, K+,NH4+, Ca+2, Sr+2, Ba+2 are soluble7. Hydroxide ion, OH\u2013, except compoundswith Li+, Na+, K+, NH4+ are solubleSoluble ionic compounds will dissolve in water, so their physical states are indicated as aqueous, (aq),while insoluble ionic compounds will not dissolve in water, so their physical states are indicated assolid, (s). For a precipitation reaction to occur, at least one of the products must be insoluble; if bothproducts are soluble, then no reaction occurs. The presence of a precipitate is observed in the lab as acloudy mixture that results when two solutions are mixed. The following is an example of a doublereplacement\/precipitation reaction: Pb(NO3) 2 (aq) + K2CrO4 (aq) \u2192 2KNO3 (aq) + PbCrO4 (s)5. Acid-Base Neutralization: HX (aq) + YOH (aq) \u2192 H2O (l) + HX (aq)These reactions occur between an acid and a base. In general, acids are compounds that producehydrogen ions (H+), also called protons, when dissolved in water. The chemical formulas for acids aremost often given with the H\u2019s at the beginning, so acids are usually easy to recognize. A few commonacids are hydrochloric acid, HCl(aq), nitric acid, HNO3(aq), and sulfuric acid, H2SO4(aq). Bases arecompounds that produce hydroxide ions (OH\u2013) when dissolved in water. A few common bases aresodium hydroxide, NaOH, potassium hydroxide, KOH, calcium hydroxide, Ca(OH)2, and bariumhydroxide, Ba(OH)2. Other types of bases contain carbonate ion, CO3\u20132, and hydrogen carbonate (orbicarbonate) ion, HCO3\u2013.GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 3 of 12The two types of acid-base neutralization reactions involve a) an acid reacting with a base (containingthe hydroxide ion (OH\u2013)) to produce water and a salt (an ionic compound) or b) an acid reacting with abase containing carbonate (CO3\u20132) or hydrogen carbonate ion (HCO3\u2013) to produce water, carbondioxide gas, and a salt. An example of each is provided below:a) When an acid reacts with a base containing hydroxide ion (OH\u2013) to produce water and asalt, the hydrogens from the acid combine with the hydroxide from the base to form water whilethe salt is formed by combining the cation from the base with the anion from the acid. Thefollowing is an example of this type of reaction: HCl (aq) + NaOH (aq) \u2192 H2O (l) + NaCl(aq).b) When an acid reacts with a base containing carbonate (CO3\u20132) or hydrogen carbonateion (HCO3\u2013) to produce water, carbon dioxide gas, and a salt, the hydrogens from the acidcombine with the carbonate or hydrogen carbonate from the base to form water and carbondioxide gas while the salt is formed by combining the cation from the base combining with theanion from the acid\u2014e.g., HCl (aq) + NaHCO3 (aq) \u2192 H2O (l) + CO2 (g) + NaCl (aq).6. Combustion Reactions: Hydrocarbon (CxHy) + O2 (g) \u2192 CO2 (g) + H2O (g)In a combustion reaction, a hydrocarbon (composed of C and H) or a hydrocarbon derivative(composed of C, H, and O) is burned in oxygen to produce carbon dioxide gas and steam. Oneexample is the combustion of methane (natural gas): CH4 (g) + 2 O2 (g) \u2192 CO2 (g) + 2 H2O (g)**Lab Notebook**Record observations for all of the chemical reactions carried out during the lab in your lab book.These observations should include:\u2022 observations of the reactant(s) before the reaction\u2022 observations of the reaction mixture during the reaction\u2022 observations of the product(s) after the reaction.Your observations of a material should contain the color, clarity and state of matter, plus anyuseful descriptions of the material (for example, a sample of magnesium might be described as asmooth, shiny, silver, opaque solid).Your observations of the reaction in progress should include anything of potential interest, such as\u201cthe color changed from green to blue\u201d, \u201ca pungent odor is present now\u201d, \u201cthe test tube is gettingwarmer\u201d or \u201cbubbles are forming on the surface of the magnesium\u201d.Procedure:Safety and waste disposal directions are listed with each procedure.General Directions:1. Carry out the reactions using the approximate quantities of reagents indicated. Unless otherwisestated, use test tubes. To estimate 2 mL, measure 2 mL of water in a graduated cylinder and pour itinto a test tube. Save this test tube for comparison.GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 4 of 122. When combining solutions in a test tube, tap the tube a few times or use the Vortex mixer to ensurethat the solutions have mixed completely.3. To heat a solid in a test tube, position the test tube holder near the top of the test tube, and hold thetest tube in a slanted position so that the opening of the test tube is pointed away from people.Keep the bottom of the test tube in the hottest part of the burner, but continuously move it back andforth over the flame to avoid \u201chot spots\u201d (overheating one part of the test tube).4. There are different concentrations of the HCl and NaOH used in this laboratory session. Checklabels carefully for the proper chemical and concentration!A. Acids and Bases.CAUTION! NaOH and HCl can damage skin, eyes and clothing on contact. Rinse off any spillsimmediately with plenty of water for 10 minutes. In the event of a spill in the laboratory, notifyyour instructor immediately.Place one piece each of red litmus paper and blue litmus paper on a watch glass, leaving a 1-inchspace between them. Place a drop of 0.1M HCl(aq) on each piece of litmus paper using a stirring rodand record your observations. Then place a drop of 0.1M NaOH(aq) on each piece of litmus paper andrecord your observations. Place a drop of deionized water on each piece of litmus paper and recordyour observations.Red litmus paper Blue litmus paperBefore reactionReaction with 0.1M HClReaction with 0.1M NaOHReaction with H2OB. Combination Reactions1. Heat a piece of copper wire strongly in the Bunsen burner flame (using crucible tongs) until achange in appearance is noted. Record any changes in the appearance of the copper wire in yourlab report. Place the cooled wire in the regular trash.GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 5 of 12CAUTION: Do not look directly at the Mg ribbon as it burns, or you may damage your eyes.1. Hold a strip of magnesium ribbon in the burner flame (using crucible tongs).2. Scrape the ash away from any unreacted Mg metal and place only the ash in a watch glass. Add afew drops of distilled H2O. Carefully crush and stir the ash\/water mixture with a stirring rod.Place one drop of the solution on blue litmus paper and another drop on red litmus paper.3. Dispose of the wet ash and any unreacted Mg in the waste jar in the hood. Rinse off the pieces oflitmus paper with water, then dispose of them in the regular trash.Copper Metal Magnesium metalBefore heatingDuring heatingAfter heatingRed litmus Blue litmusMagnesium ash solutionMake sure you conclude whether the ash is acidic or basic.C. Decomposition Reactions1. Place approximately half a spatula full (roughly pea-sized) of copper(II) carbonate in a dry testtube. If you do not have a clean, dry test tube, ask your instructor for one. Do not try to drya test tube during the laboratory period. Observe the color of the sample. Using a test tubeclamp, heat the test tube over a Bunsen burner until you notice a color change (approximately 30seconds \u2013 1 minute). Be sure to constantly move the test tube to avoid overheating the glassware!Cool the test tube in an empty beaker. Record the color of the solid sample after heating. Whencool, dispose of the contents in the waste jar in the hood.Copper (II) carbonateBefore heatingDuring heatingAfter heatingGCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 6 of 12D. Single-Replacement ReactionsCAUTION: AgNO3 will stain skin and clothes!1. Place a piece of copper wire in a test tube with enough 1M AgNO3 to cover it. Allow the test tubeto stand for 5-10 minutes. Note changes in the appearance of both the wire and the solution.Dispose of the contents of the test tube in the waste jar in the hood.Copper Metal AgNO3 solutionBefore reactionDuring reactionAfter reactionCAUTION: 3 M HCl(aq) can damage skin and clothing on contact. Rinse any spills on skinimmediately with plenty of water for 10 minutes. Neutralize all spills on the lab bench with water orNaHCO3 solution, and rinse your hands thoroughly.2. Place a small piece of zinc metal in a test tube containing 2 mL of 3 M HCl, and record yourobservations. Dispose of the contents of the test tube in the waste jar in the hood.Zinc Metal HCl solutionBefore reactionDuring reactionAfter reactionE. Double Replacement\/Precipitation ReactionsCAUTION: AgNO3 will stain skin and clothing! Pb containing compounds are toxic and should notbe ingested. HCl, HNO3 and NaOH are corrosive and can cause chemical burns and damageclothing. Any hazardous chemical spilled on skin must be rinsed off with plenty of water for 10-15 minutes. If any spills occur in the laboratory, notify your instructor immediately.Use the 0.10 M solutions of each of these reagents (except Na2SO4 which is 1M, HNO3 which is 3Mand AgNO3 which is 1M). You will obtain solutions of AgNO3(aq), NaCl(aq), Ba(NO3)2(aq),HNO3(aq) and Pb(NO3)2(aq). To EACH of them you will add solutions of NaNO3(aq), NaCl(aq),Na2SO4(aq), NaOH(aq), KI(aq), and saturated Na2CO3(aq).First, record observations of each solution before the solutions are mixed.GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 7 of 12You will mix the pairs of chemicals and observe the reactions between them, watching in particular forthe appearance of a precipitate. All observations should be recorded in your data table in yournotebook. If no change occurs, write \u201cNR\u201d for \u201cNo reaction\u201d. If a precipitate appears or if thesolution changes in any other way, record your observations of the change.Here is an example data table for different reagents. Your data table will be much larger (considerusing the \u201clandscape\u201d orientation of the notebook, because this table will be wider than it is tall).KNO3(aq) KI(aq) KOH(aq)CuCl2(aq) NR A brown, opaque solidis present in a clear,dark purple solution.A translucent, blue gel-likeppt formed immediately.Pb(NO3)2(aq) NR An opaque yellow pptformed in the clearcolorless solution.The solution turned cloudywhite. Slowly a whiteopaque ppt settled in theclear, colorless solution.KCl(aq) NR NR NRProcedureNOTE: All waste for this part of the experiment should be poured into the labeled wastecontainers in the hood and the test tubes rinsed with a minimum amount of water, whichshould also be placed into the waste container. DO NOT dispose of any solutions or solidsdown the drain.1. Wash your well-plate thoroughly with soap and water, then rinse it completely with deionizedwater. A dirty well-plate can give incorrect results.2. Place 5 drops of each aqueous solution in the correct wells based on the table you constructed foryour observations.3. For each of the following combinations, mix 10 drops of each solution in a clean test tube, so anyreactions that take place can be observed on a larger scale:\u2022 0.10 M Ba(NO3)2(aq) and 0.10 M NaOH(aq)\u2022 3 M HNO3(aq) and 3 M NaOH(aq)\u2022 3 M HNO3(aq) and Saturated Na2CO3(aq)4. Have your lab instructor sign off on your Double Replacement\/Precipitation reaction observation table.5. In the discussion section of your laboratory notebook, write a balanced chemical equation and clearlyidentify the solid product for any precipitation reactions that you observe.GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 8 of 12F. Combustion Reaction1. Place about 10-15 drops of 2-propanol (isopropyl alcohol, C3H7OH) in a small evaporating dish.2. Ignite a wooden splint in the Bunsen burner and use the wooden splint to light the alcohol.2-propanolBefore ignitionDuring combustionAfter combustionGCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 9 of 12Chemical Reactions: Introduction to Reaction Types: Lab ReportName: ________________________Partner(s): _____________________Section Number: ________________Word Equations and Balanced Chemical EquationsTranslate each of the following word equations into a balanced chemical reactions by writing thecorrect chemical formulas (including physical states) for the reactants and products. Make sureto balance each equation.Example: Aluminum metal reacts with oxygen.aluminum metal + oxygen gas \u21924 Al (s) + 3 O2 (g) \u2192 2 Al2O3 (s)(Rewrite Entire Balanced Reaction)A. Combination Reactions1. Copper reacts with oxygen.copper metal + oxygen gas \u21922. Magnesium metal reacts with oxygen.magnesium metal + oxygen gas \u21923. Magnesium oxide (ash) reacts with water.magnesium oxide + water \u2192B. Decomposition Reactions1. Water decomposes.water \u21922. Copper(II) carbonate decomposes.copper(II) carbonate \u2192\u0394\u0394GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 10 of12C. Single-Replacement Reactions1. Copper reacts with silver nitrate to form silver metal and copper(II) nitrate.copper metal + silver nitrate \u21922. Zinc metal reacts with hydrochloric acid to produce zinc chloride and hydrogen.zinc metal + hydrochloric acid \u2192D. Double Replacement (precipitation) and Acid Base ReactionsRefer to your data table for the following selected sets of reactants and fill in the following blanks andbeaker drawings. If there is no net ionic reaction because all the ions are spectators still complete themolecular reaction, the ionic reaction, and the beaker drawings, then put NR only for the net ionicreaction. An example NOT from this experiment is presented first.Example: calcium acetate and ammonium sulfate Reaction type: ____precipitation________Molecular: Ca(CH3COO)2(aq) + (NH4)2SO4(aq) \u2192 CaSO4(s) + 2 NH4CH3COO(aq)________________________________Ionic: Ca2+(aq) + 2 CH3COO-(aq) + 2 NH4+(aq) + SO42-(aq) \u2192 CaSO4(s) + 2 CH3COO-(aq) + 2 NH4+(aq)____________Net Ionic: Ca2+(aq) + SO42-(aq) \u2192 CaSO4(s)______________________________________________________________+\u21921. lead (II) nitrate and potassium iodide Reaction type: _______________Molecular: ________________________________________________________________________Ionic: ____________________________________________________________________________Net Ionic: ________________________________________________________________________+\u2192GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 11 of122. nitric acid and sodium hydroxide Reaction type: _______________Molecular: ________________________________________________________________________Ionic: ____________________________________________________________________________Net Ionic: ________________________________________________________________________+\u21923. barium nitrate and sodium sulfate Reaction type: _______________Molecular: ________________________________________________________________________Ionic: ____________________________________________________________________________Net Ionic: ________________________________________________________________________+\u2192F. Combustion Reactions1. Isopropyl alcohol (C3H8O) undergoes combustion. Write the balanced chemical equation includingphysical states:GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 12 of12Balancing and Categorizing Chemical Equations:Balance each of the 12 chemical equations given below, and identify each as one of the six types listedbelow.Combination reaction (C)Decomposition reaction (D)Single-Replacement reaction (SR)Double-Replacement\/Precipitation reaction (DR)Acid-Base Neutralization reaction (N)Combustion reaction (B)TYPE_____ 1. _____ Al (s) + _____ NiCl2 (aq) \u2192 _____ Ni (s) + _____ AlCl3 (aq)_____ 2. _____ Ba(OH)2 (s) + ____ FeCl3 (aq) \u2192 ____ BaCl2 (aq) + ____ Fe(OH)3 (s)_____ 3. _____ C4H10 (l) + _____ O2 (g) \u2192 _____ CO2 (g) + _____ H2O (g)_____ 4. _____ KClO3 (l) \u2192 _____ KCl (l) + _____ O2 (g)_____ 5. _____ Al (s) + _____ I2 (s) \u2192 _____ AlI3 (s)_____ 6. _____ H2SO4 (aq) + _____ Mg(OH)2 (s) \u2192_____ H2O (l) + _____ MgSO4 (aq)_____ 7. _____ CH3OH (l) + _____ O2 (g) \u2192 _____ CO2 (g) + _____ H2O (g)_____ 8. _____ Ca (s) + _____ O2 (g) \u2192 _____ CaO (s)_____ 9. _____ Mg (s) + _____ CO2 (g) \u2192 _____ MgO (s) + _____ C (s)____ 10. _____ Na3PO4 (aq) + ____ MgCl2 (aq) \u2192 ____ Mg3(PO4)2 (s) + ___ NaCl (aq)____ 11. _____ HgO (s) \u2192 _____ Hg (l) + _____ O2 (g)____ 12. _____ H3PO4 (aq) + ____ NaOH (aq) \u2192 _____ H2O (l) + ____ Na3PO4 (aq)\u0394\u0394\u0394\u0394<\/p>\n","protected":false},"excerpt":{"rendered":"
GCC CHM 151LL: Chemical Reactions: Introduction to Reaction Types \u00a9 GCC, 2014 page 1 of 12Chemical Reactions: Introduction to Reaction TypesIn this experiment, you will…<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[],"tags":[],"class_list":["post-147689","post","type-post","status-publish","format-standard","hentry"],"_links":{"self":[{"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/posts\/147689","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/comments?post=147689"}],"version-history":[{"count":0,"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/posts\/147689\/revisions"}],"wp:attachment":[{"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/media?parent=147689"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/categories?post=147689"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/academicwritersbay.com\/answers\/wp-json\/wp\/v2\/tags?post=147689"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}