Activity Series

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.

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

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

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.hydrogen gas is bubbled through an aqueous solution of nickel (II) chloride

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

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 net ionic equation that describes this reaction?

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 volume of solution is needed to completely react with the magnesium?

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 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?

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:     

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? 

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

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:Sodium nitrate + copper(II) sulfate

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:Ammonium bromide + silver nitrate

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 carbonate + barium hydroxide

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:Aluminum nitrate + sodium phosphate

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

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.Ammonium sulfate + barium chloride

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:Sodium sulfide + nickel(II) sulfate

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:Lead(II) nitrate + potassium bromide

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.

Seven of the nine elements known since ancient times are metals. Referring to the activity series, are these metals mostly found at the bottom or top of the activity series?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)  →  Mn+(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-

Which region of the periodic table shown here contains the least readily oxidized elements?

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).

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?

The hypochlorite ion, ClO–, is the active ingredient in bleach. The perchlorate ion, ClO4−, is a main component of rocket propellants. In a redox reaction, which ion would you expect to be more easily reduced?

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

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) →

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