Arrange these species by their ability to act as an oxidizing agent.

Question

Mg²⁺

Fe²⁺

Pb²⁺

Au³⁺

Answer 1

An easy way to determine the rank order of oxidizing strength is to look at the standard reduction potentials for the various ions. Find a table and look up the values. I found the following:

Au³⁺ = +1.5 V

Pb²⁺ = -0.13 V

Fe²⁺ = -0.45 V

Mg²⁺ = -2.3 V

These values indicate that Au³⁺ is the most easily reduced and Mg²⁺ is the hardest to reduce. Thus, Au³⁺ is the strongest oxidizing agent, followed by Pb²⁺, Fe²⁺ and Mg²⁺ is the weakest oxidizing agent.

Answer 2

Great Day Cheyenne!

Oxidizing agent is a substance that will be reduced.

Meaning the substance will gain electrons. Leo and Ger

The more attraction the substance or element in this case exhibits in attracting electrons the stronger the oxidizing agent.

To analyze the elements you must look at the electronegativity of the metal.

Low electronegativity means strong reducing agent element and weak oxidizing agent element.

High electronegativity means weak reducing agent element and strong oxidizing agent element.

Rank the neutral elements in terms of electronegativity strength from strong to weak.

Pb, Au, Fe, Mg

You would predict this is the order of strength as oxidizing agents as ions, but Au has a charge of +3, which would make Au +3 a stronger oxidizing agent than Pb+2

Correct order of oxidizing agent strength is as follows: Au+3 , Pb+2, Fe+2 , Mg +2

Strong and weak are used as relative terms. Metals inherently want to lose electrons and tend always to be weaker oxidizing agents than all non metals.

Hope this Helps!

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Yours in Chemistry success!

Dale