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? 

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.

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?

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 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)

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+

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?

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

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