Strongly Reducing Metals

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Jesus Rodriguez 1J
Posts: 53
Joined: Sat Jul 22, 2017 3:00 am

Strongly Reducing Metals

Postby Jesus Rodriguez 1J » Sat Feb 24, 2018 8:37 am

How can we determine how strong of reducing agent metals are?

Esin Gumustekin 2J
Posts: 57
Joined: Thu Jul 27, 2017 3:01 am

Re: Strongly Reducing Metals

Postby Esin Gumustekin 2J » Sat Feb 24, 2018 9:55 am

The more negative the standard cell potential for that half reaction, the stronger the reducing agent.

Christy Zhao 1H
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

Re: Strongly Reducing Metals

Postby Christy Zhao 1H » Sat Feb 24, 2018 9:46 pm

The opposite goes for oxidizing agents; the more positive the standard cell potential, the stronger the oxidizing agent.

404995677
Posts: 82
Joined: Fri Sep 29, 2017 7:07 am

Re: Strongly Reducing Metals

Postby 404995677 » Sat Feb 24, 2018 11:28 pm

on page 580, it says "the most negative—the most strongly reducing— are usually found toward the left of the periodic table, and the most positive—the most strongly oxidizing—are found toward the upper right."

LMendoza 2I
Posts: 41
Joined: Sat Jul 22, 2017 3:00 am

Re: Strongly Reducing Metals

Postby LMendoza 2I » Sun Feb 25, 2018 11:59 am

When a metal is the reducing agent it generally means that this metal is being oxidized so the reduction potential of this metal would have to be more negative since the strongest oxidation elements have the lowest reduction potentials.

Angel Ni 2K
Posts: 50
Joined: Sat Jul 22, 2017 3:01 am

Re: Strongly Reducing Metals

Postby Angel Ni 2K » Sun Feb 25, 2018 4:40 pm

The lower the standard reduction potential, the more unlikely the metal will get reduced (since more negative E values result in more positive G values).


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