Element's potentials

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Element's potentials

Postby EllaBerry » Thu Feb 28, 2019 6:12 pm

What makes an element be able to have a stranger reducing ability? A stronger oxidizing ability?

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Re: Element's potentials

Postby Chem_Mod » Thu Feb 28, 2019 6:43 pm

It varies depending on the elements, but one factor is the relative stability of the product that is formed after a redox reaction. As long as the reaction is overall spontaneous, it will be favorable to occur.

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Re: Element's potentials

Postby Matthew Mar 1J » Sat Mar 02, 2019 7:53 pm

From a numerical standpoint, you can look at the standard reduction potentials to determine relative reducing/oxidising strength. A lower, more negative potential means something is a stronger reducing agent and a more positive value means a stronger oxidising agent (stuff like this showed up on test 2).

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Re: Element's potentials

Postby Timothy_Yueh_4L » Sat Mar 02, 2019 9:00 pm

To break this down, an element that has a strong reducing ability is essentially the same as the reducing reagent, the element responsible for reducing another element in a redox reaction, and to determine between a group of elements in order of increasing reducing ability, we must determine which element has the strongest oxidizing potential. We can do this by comparing the elements' standard reduction potentials with the most negative value denoting the strongest element to be oxidized, hence the element with the strongest reducing ability. The same applies for the reverse when determining the strength of a group of oxidizing agent in which the higher reduction potential equates the stronger oxidizing agent.

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Re: Element's potentials

Postby IsabelLight2H » Sat Mar 02, 2019 11:12 pm

The more negative the E° the stronger the reducing agent!

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Re: Element's potentials

Postby 804994652 » Sun Mar 03, 2019 11:28 pm

Should we be using the periodic table reference in the text or the list of potentials in the textbook?

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