Activity Series

Assume you have a highly magnified view of a solution of HCl that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear and hydrogen gas would be released. Represent this change using symbols for the elements, and write out the balanced equation.

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Iron metal is added to a solution of copper(II) nitrate

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (c) hydrobromic acid is added to tin metal

Which of the following reactions could be used to produce hydrogen gas?a. Ag(s) + HCl(aq) →b. Ni(s) + H2O(l) →c. Al(s) + H2O(l) →d. Zn(s) + HCl(aq) →

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (e) aluminum metal is added to a solution  of cobalt(II) sulfate.

Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions?(a) Mn(s) + NiCl2(aq) →

Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions?(b) Cu(s) + Cr(CH3COO)3(aq) → 

Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions? (d) Pt(s) + HBr(aq) →

Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions?(e) H2(g) + CuCl2(aq) →

(a) Use the following reactions to prepare an activity series for the halogens:Br2 (aq) + 2 NaI (aq) → 2 NaBr (aq) + I 2 (aq)Cl2 (aq) + 2 NaBr (aq) → 2 NaCl (aq) + Br 2 (aq) 

Determine whether HI can dissolve 2.30g Al.a. Yesb. No

Using the activity series provided below write a balanced reaction (if any) for the following choices. a) Magnesium is added to a solution of Cobalt (II) bromide.   b) Hydrobromic acid is added to Silver metal.    

Write a balanced chemical reaction showing how the metal Al dissolves in HI.a. Al(s) + 6H+(aq) → Al 3+(aq) + 3H 2(g)b. 2Al(s) + 3H+(aq) → 2Al 3+(aq) + 3H 2(g)c. 2Al(s) + 6H+(aq) → 2Al 3+(aq) + 3H 2(g)d. Al(s) + 3H+(aq) → Al 3+(aq) + 3H 2(g)

Using the activity series provided below write a balanced reaction (if any) for the following choices. a) Hydrogen gas passing through a solution of Mercury (II) acetate.   b) Chlorine gas evolved through a solution of Sodium bromide.   

Write the balanced molecular equation (ME) and net ionic equation (NIE) for the following reaction. Be sure to include the correct states in the final equation and charges for ions in the NIE. CuCl2(aq) + Pb(s) → ME:   NIE:     

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations.Potassium chloride + iron(III) nitrate

If you don't think cobalt would work as the redox-active partner ion in the sodium version of the electrode, suggest an alternative metal ion.

Using the activity series (Table 4.5 in the textbook), write balanced chemical equations for the following reactions.hydrogen gas is bubbled through an aqueous solution of nickel (II) chloride

Identify which redox reactions occur spontaneously in the forward direction.a. 2 Al (s) + 3 Pb2+ (aq) → 2 Al3+ (aq) + 3 Pb (s)b. 2 Ag+ (aq) + Ni (s) → 2 Ag (s) + Ni2+ (aq)c. Mg2+ (aq) + Zn (s) → Mg (s) + Zn2+ (aq)d. Sn (s) + Mn2+ (aq) → Sn2+ (aq) + Mn (s)

Determine which redox reaction occurs spontaneously in the forward direction.a. Ni (s) + Pb2+ (aq) → Ni2+ (aq) + Pb (s)b. Al (s) + 3 Ag+ (aq) → Al3+ (aq) + 3 Ag (s)c. Pb (s) + Mn2+ (aq) → Pb2+ (aq) + Mn (s)d. Ni (s) + Zn2+ (aq) → Ni2+ (aq) + Zn (s)

Using the activity series (refer to the following table), write balanced chemical equations for the following reactions. If no reaction occurs, simply write no reaction.Activity Series of Metals in Aqueous SolutionMetalOxidation ReactionLithiumLi( s )  →  Li+ ( aq ) + e-PotassiumK( s )  →  K +  ( aq ) + e-BariumBa( s )  →  Ba2 +  ( aq ) + 2e-CalciumCa( s )  →  Ca2 +  ( aq ) + 2e-SodiumNa( s )  →  Na +  ( aq ) + e-MagnesiumMg( s )  →  Mg2 +  ( aq ) + 2e-AluminumAl( s )  →  Al3 +  ( aq ) + 3e-ManganeseMn( s )  →  Mn2 +  ( aq ) + 2e-ZincZn( s )  →  Zn2 +  ( aq ) + 2e-ChromiumCr( s )  →  Cr3 +  ( aq ) + 3e-IronFe( s )  →  Fe2 +  ( aq ) + 2e-CobaltCo( s )  →  Co2 +  ( aq ) + 2e-NickelNi( s )  →  Ni2 +  ( aq ) + 2e-TinSn( s )  →  Sn2 +  ( aq ) + 2e-LeadPb( s )  →  Pb2 +  ( aq ) + 2e-HydrogenH2 ( g )  →  2H +  ( aq ) + 2e-CopperCu( s )  →  Cu2 +  ( aq ) + 2e-SilverAg( s )  →  Ag +  ( aq ) + e-MercuryHg( l )  →  Hg2 +  ( aq ) + 2e-PlatinumPt( s )  →  Pt2 +  ( aq ) + 2e-GoldAu( s )  →  Au3 +  ( aq ) + 3e-Hydrochloric acid is added to gold metal.

Predict the products for the following combination of reactants: Al3+(aq) + Pb(s)A. Al(s) and Pb(s)B. Al(s) and Pb2+(s)C. Al3+(aq) and Pb4+(aq)D. Al3+(aq) and Pb2+(aq)E. no reaction occurs

What will happen if Ag(s) and K+(aq) come into contact? K is above Ag on the activity series. A) No reaction will occur because K(s) is more easily oxidized than Ag(s). B) Silver will be oxidized, and potassium will be reduced. C) The compound AgK will form. D) The ion AgK+ will form. E) Silver will be reduced, and potassium will be oxidized.

Suppose you have 5.05 g of powdered magnesium metal, 1.05 L of 2.00 M  potassium nitrate solution, and 1.05 L of 2.00 M  silver nitrate solution.What is the net ionic equation that describes this reaction?

Given the following sets of reactions, which (if any) will not undergo a reaction?I.    Pt(s) + KNO3(aq) →II.   Ag(s) + Ni(NO3)2(aq) →III.  Ca(s) + Zn(NO3)2(aq) →IV. Fe(s) + Sn2+(aq) → V.  Ba2+(aq) + Cu2+(aq) →A. I and II onlyB. II, III, and IV onlyC. III and IV onlyD. II and V E. I, II, and V only

Copper, silver, and gold have all been know since ancient times, whereas most of the other metals have not. Can you suggest an explanation?Figure Discovering the elements.

The labels have fallen off three bottles containing powdered samples of metals; one contains zinc, one lead, and the other platinum. You have three solutions at your disposal: 1 M sodium nitrate, 1 M nitric acid, and 1 M nickel nitrate.How could you use these solutions to determine the identities of each metal powder? 

The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl2(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO3)2(aq), nickel metal is deposited on the strip.Which elements more closely define the position of cadmium in the activity series?

If we want to precipitate copper metal from an aqueous solution of CuSO 4, which of the following reactants should we add to our solution?Choose 1 answer:a. I2(s)b. Ag(s)c. Zn(s)d. AgNO3(aq)

Determine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. A. 2.15 g AlB. 4.85 g Cu C. 2.42 g Ag

Consider the following unbalanced oxidation-reduction reactions in aqueous solution:Ag+(aq) + Li(s) → Ag(s) + Li+ (aq)Fe(s) + Na+ (aq) → Fe2+(aq) + Na(s)K(s) + H2O(l) → KOH(aq) + H2(g)Use the activity series to predict which of these reactions should occur (Section 4.4 in the textbook).

Based on the activity series, which one of the reactions below will occur? A) Pb(s) + Nil2(aq) → Pbl2 (aq) + Ni(s) B) SnBr2(aq) + Cu(s) → CuBQ(aq) + Sn(s) C) Fe(s) + ZnCl2(aq)→ FeCl2(aq) + Zn(s) D) Mn(s) + NiCl2(aq) → MnCl2(aq) + Ni(s) E) None of the reactions will occur

Which of these metals will be oxidized by the ions of aluminum?A) magnesiumB) ironC) chromiumD) nickelE) zinc

Which metal in the activity series reduces Al3+ ions but not Na+ ions?a. Mgb. Cuc. Fed. Cr

Suppose you wanted to cause Ni2+ ions to come out of solution as solid Ni.Which metal could you use to accomplish this?a. Feb. Pbc. Mnd. Mge. Cu

Which metal can be used as a sacrificial electrode to prevent the rusting of an iron pipe?a) Aub) Agc) Cud) Mn

Which of the following metals is the best reducing agent?A) NiB) MgC) FeD) Co

Which of the following metal cations is the best oxidizing agent?A) Co2+B) Zn2+C) Cd2+D) Cu2+

Which of the following reagents would oxidize Zn to Zn2+, but not Sn to Sn2+?Br2Br-Ca^2+Co^2+CaCoWhich of the following reagents would oxidize I- to I2, but not F- to F2?Br2CoCaCa^2+Br-Co^2+

Bronze is a solid solution of Cu(s) and Sn(s); solutions of metals like this that are solids are called alloys. There is a range of compositions over which the solution is considered a bronze. Bronzes are stronger and harder than either copper or tin alone.The reaction below is an example of a reaction you could do to remove all the tin from this bronze to leave a pure copper sample. Complete the explanation.Sn(s) + 2HCl(aq)     SnCl2(aq) + H2(g)According to the Activity Series of Metals Sn is ______ H and Cu is ______ it. That is, Sn can be _______ to _____ by HCl(aq), but Cu(s) cannot. We can treat bronze with HCl(aq) to remove Sn as _______ and leave a pure Cu sample.Options:    below      Sn2+(aq)      above       oxidized      Sn2+(aq) 

Using the activity series (Table 4.5 in the textbook), write balanced chemical equations for the following reactions.aluminum metal is added to a solution of cobalt (II) sulfate

Using the activity series (refer to the following table), write balanced chemical equations for the following reactions. If no reaction occurs, simply write no reaction.Activity Series of Metals in Aqueous SolutionMetalOxidation ReactionLithiumLi( s )  →  Li+ ( aq ) + e-PotassiumK( s )  →  K +  ( aq ) + e-BariumBa( s )  →  Ba2 +  ( aq ) + 2e-CalciumCa( s )  →  Ca2 +  ( aq ) + 2e-SodiumNa( s )  →  Na +  ( aq ) + e-MagnesiumMg( s )  →  Mg2 +  ( aq ) + 2e-AluminumAl( s )  →  Al3 +  ( aq ) + 3e-ManganeseMn( s )  →  Mn2 +  ( aq ) + 2e-ZincZn( s )  →  Zn2 +  ( aq ) + 2e-ChromiumCr( s )  →  Cr3 +  ( aq ) + 3e-IronFe( s )  →  Fe2 +  ( aq ) + 2e-CobaltCo( s )  →  Co2 +  ( aq ) + 2e-NickelNi( s )  →  Ni2 +  ( aq ) + 2e-TinSn( s )  →  Sn2 +  ( aq ) + 2e-LeadPb( s )  →  Pb2 +  ( aq ) + 2e-HydrogenH2 ( g )  →  2H +  ( aq ) + 2e-CopperCu( s )  →  Cu2 +  ( aq ) + 2e-SilverAg( s )  →  Ag +  ( aq ) + e-MercuryHg( l )  →  Hg2 +  ( aq ) + 2e-PlatinumPt( s )  →  Pt2 +  ( aq ) + 2e-GoldAu( s )  →  Au3 +  ( aq ) + 3e-Hydrogen gas is bubbled through a solution of silver nitrate.

Which metal can be oxidized with an Sn 2+ solution but not with an Fe 2+ solution?

Which of the following reagents would oxidize Cr to Cr2, but not Ag to Ag?A) Co2+B) Ca2+C) Br-D) CoE) CaF) Br2

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (b) zinc metal is added to a solution of magnesium sulfate

Based on the activity series (Table 4.5), what is the outcome (if any) of each of the following reactions? (c) Cr(s) + NiSO4(aq) →

Suppose you have 5.05 g of powdered magnesium metal, 1.05 L of 2.00 M  potassium nitrate solution, and 1.05 L of 2.00 M  silver nitrate solution.Which one of the solutions will react with the magnesium powder?

Suppose you have 5.05 g of powdered magnesium metal, 1.05 L of 2.00 M  potassium nitrate solution, and 1.05 L of 2.00 M  silver nitrate solution.What is the molarity of the Mg2+ ions in the resulting solution?

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:Br2(aq) + 2 NaI(aq) → 2 NaBr(aq) + I2(aq)Cl2(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br2(aq)Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed.

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:Br2(aq) + 2NaI(aq)  →  2NaBr(aq) + I2(aq)Cl2(aq) + 2NaBr(aq)  →  2NaCl(aq) + Br2(aq)Which elemental halogen would you predict is the most stable, upon mixing with other halides?

Chlorine dioxide gas (ClO2) is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced.Why do you think that ClO2 is reduced so readily?

Using the activity series (Table 4.5 in the textbook), write balanced chemical equations for the following reactions.iron metal is added to a solution of copper (II) nitrate

Suppose you wanted to cause Pb2+ ions to come out of solution as solid Pb(s). Which metal(s) could you use to accomplish this?Check all that apply.(a) Zn(b) Mn(c) Ca(d) Au(e) sn(f) Al(g) Cu(h) Fe

Lanthanum metal forms cations with a charge of 3+. Consider the following observations about the chemistry of lanthanum: When lanthanum metal is exposed to air, a white solid (compound A) is formed that contains lanthanum and one other element. When lanthanum metal is added to water, gas bubbles are observed and a different white solid (compound B) is formed. Both A and B dissolve in hydrochloric acid to give a clear solution. When either of these solutions is evaporated, a soluble white solid (compound C) remains. If compound C is dissolved in water and sulfuric acid is added, a white precipitate (compound D) forms.Based on the preceding observations, what can be said about the position of lanthanum in the activity series (Table 4.5 in the textbook)?

You may want to reference (Pages 137 - 144)Section 4.4 while completing this problem.Which of these metals is the easiest to oxidize?(a) gold (b) lithium (c) iron (d) sodium (e) aluminum

Which metal is most easily oxidized?(a) Sr(b) Fe(c) Pt

Using the activity series (refer to the following table), write balanced chemical equations for the following reactions. If no reaction occurs, simply write no reaction.Activity Series of Metals in Aqueous SolutionMetalOxidation ReactionLithiumLi( s )  →  Li+ ( aq ) + e-PotassiumK( s )  →  K +  ( aq ) + e-BariumBa( s )  →  Ba2 +  ( aq ) + 2e-CalciumCa( s )  →  Ca2 +  ( aq ) + 2e-SodiumNa( s )  →  Na +  ( aq ) + e-MagnesiumMg( s )  →  Mg2 +  ( aq ) + 2e-AluminumAl( s )  →  Al3 +  ( aq ) + 3e-ManganeseMn( s )  →  Mn2 +  ( aq ) + 2e-ZincZn( s )  →  Zn2 +  ( aq ) + 2e-ChromiumCr( s )  →  Cr3 +  ( aq ) + 3e-IronFe( s )  →  Fe2 +  ( aq ) + 2e-CobaltCo( s )  →  Co2 +  ( aq ) + 2e-NickelNi( s )  →  Ni2 +  ( aq ) + 2e-TinSn( s )  →  Sn2 +  ( aq ) + 2e-LeadPb( s )  →  Pb2 +  ( aq ) + 2e-HydrogenH2 ( g )  →  2H +  ( aq ) + 2e-CopperCu( s )  →  Cu2 +  ( aq ) + 2e-SilverAg( s )  →  Ag +  ( aq ) + e-MercuryHg( l )  →  Hg2 +  ( aq ) + 2e-PlatinumPt( s )  →  Pt2 +  ( aq ) + 2e-GoldAu( s )  →  Au3 +  ( aq ) + 3e-Nickel metal is added to a solution of copper(II) nitrate.

Complete and balance the equation for this single-displacement reaction. Phases are optional. AgNO3 + Al → 

MetalNotesLithium (Li+)Can displace Hydrogen from liquid water, steam, and acids.Potassium (K+)Barium (Ba2+)Strontium (Sr2+)Calcium (Ca2+)Sodium (Na+)Magnesium (Mg2+)Can displace Hydrogen from steam and acids.Aluminum (Al3+)Zinc (Zn2+)Chromium (Cr2+, Cr3+)Iron (Fe2+, Fe3+)Cadmium (Cd2+)Can displace Hydrogen from acids.Cobalt (Co2+)Nickel (Ni2+)Tin (Sn2+)Lead (Pb2+)HydrogenAntimony (Sb3+)Arsenic (As3+, As5+)Bismuth (Bi3+)Copper (Cu+, Cu2+)Mercury (Hg22+, Hg2+)Silver (Ag+)Palladium (Pd3+)Platinum (Pt2+, Pt3+)Gold (Au+, Au3+)A metal that is high on the series proceeds in the ________directon and _______ electrons, forming ____________.A metal that is low on the series proceeds in the ________ direction and _______ electrons, forming ________.Therefore, a metal that is high on the series is _______ to oxidize, whereas a metal that is low on the series is _______ to oxidize. 

Determine whether each redox reaction is spontaneous. Drag the appropriate equations to their respective bins.

Which region of the periodic table shown here contains elements that are easiest to oxidize?

Which of these ions will spontaneously react with (Ni)(s) in solution?a. Sn2+b. Cr3+c. Na+d. Ca2+

The metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl2(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO3)2(aq), nickel metal is deposited on the strip.What experiments would you need to perform to locate more precisely the position of cadmium in the activity series?

Reaction of copper metal with silver ion. When copper metal is placed in a solution of silver nitrate, a redox reaction forms silver metal and a blue solution of copper(II) nitrate.Why does this solution turn blue?

Using the activity series (Table 4.5 in the textbook), write balanced chemical equations for the following reactions.hydrobromic acid is added to tin metal

Using the activity series (Table 4.5 in the textbook), write balanced chemical equations for the following reactions.zinc metal is added to a solution of magnesium sulfate

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:Br2(aq) + 2 NaI(aq) → 2 NaBr(aq) + I2(aq)Cl2(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br2(aq)Predict whether a reaction will occur when elemental bromine and lithium chloride are mixed.

Using the activity series (refer to the following table), write balanced chemical equations for the following reactions. If no reaction occurs, simply write no reaction.Activity Series of Metals in Aqueous SolutionMetalOxidation ReactionLithiumLi( s )  →  Li+ ( aq ) + e-PotassiumK( s )  →  K +  ( aq ) + e-BariumBa( s )  →  Ba2 +  ( aq ) + 2e-CalciumCa( s )  →  Ca2 +  ( aq ) + 2e-SodiumNa( s )  →  Na +  ( aq ) + e-MagnesiumMg( s )  →  Mg2 +  ( aq ) + 2e-AluminumAl( s )  →  Al3 +  ( aq ) + 3e-ManganeseMn( s )  →  Mn2 +  ( aq ) + 2e-ZincZn( s )  →  Zn2 +  ( aq ) + 2e-ChromiumCr( s )  →  Cr3 +  ( aq ) + 3e-IronFe( s )  →  Fe2 +  ( aq ) + 2e-CobaltCo( s )  →  Co2 +  ( aq ) + 2e-NickelNi( s )  →  Ni2 +  ( aq ) + 2e-TinSn( s )  →  Sn2 +  ( aq ) + 2e-LeadPb( s )  →  Pb2 +  ( aq ) + 2e-HydrogenH2 ( g )  →  2H +  ( aq ) + 2e-CopperCu( s )  →  Cu2 +  ( aq ) + 2e-SilverAg( s )  →  Ag +  ( aq ) + e-MercuryHg( l )  →  Hg2 +  ( aq ) + 2e-PlatinumPt( s )  →  Pt2 +  ( aq ) + 2e-GoldAu( s )  →  Au3 +  ( aq ) + 3e-Chromium metal is immersed in an aqueous solution of cobalt(II) chloride.

Using the activity series (refer to the following table), write balanced chemical equations for the following reactions. If no reaction occurs, simply write no reaction.Activity Series of Metals in Aqueous SolutionMetalOxidation ReactionLithiumLi( s )  →  Li+ ( aq ) + e-PotassiumK( s )  →  K +  ( aq ) + e-BariumBa( s )  →  Ba2 +  ( aq ) + 2e-CalciumCa( s )  →  Ca2 +  ( aq ) + 2e-SodiumNa( s )  →  Na +  ( aq ) + e-MagnesiumMg( s )  →  Mg2 +  ( aq ) + 2e-AluminumAl( s )  →  Al3 +  ( aq ) + 3e-ManganeseMn( s )  →  Mn2 +  ( aq ) + 2e-ZincZn( s )  →  Zn2 +  ( aq ) + 2e-ChromiumCr( s )  →  Cr3 +  ( aq ) + 3e-IronFe( s )  →  Fe2 +  ( aq ) + 2e-CobaltCo( s )  →  Co2 +  ( aq ) + 2e-NickelNi( s )  →  Ni2 +  ( aq ) + 2e-TinSn( s )  →  Sn2 +  ( aq ) + 2e-LeadPb( s )  →  Pb2 +  ( aq ) + 2e-HydrogenH2 ( g )  →  2H +  ( aq ) + 2e-CopperCu( s )  →  Cu2 +  ( aq ) + 2e-SilverAg( s )  →  Ag +  ( aq ) + e-MercuryHg( l )  →  Hg2 +  ( aq ) + 2e-PlatinumPt( s )  →  Pt2 +  ( aq ) + 2e-GoldAu( s )  →  Au3 +  ( aq ) + 3e-A solution of zinc nitrate is added to a solution of magnesium sulfate.

Which of the following reagents would oxidize Zn to Zn2+, but not Sn to Sn2+?A. Br2B. Br-C. Ca2+D. Co2+E. CaF. Co

Which of the following reagents would oxidize Cr to Cr3+, but not Pb to Pb2+?a) Cob) Br2c) Ca2+d) Co2+e) Br-f) Ca

Which of the following reagents would oxidize Ag to Ag+, but not Au to Au3+?a) Cob) Co2+c) Cad) Ca2+e) Br2f) Br-