Strength of reducing agent

[Samantha Jimenez 4k]

For one of the homework problems, it asks to rank metals of increasing strength of reducing agent. How would we go about answering these type of questions?

[Chase Yonamine 1J]

The smallest (more negative) Reduction potential is a stronger reducing agent

[Melody P 2B]

The smallest (more negative) Reduction potential is a stronger reducing agent

Why is that?

[Zenita Leang 2K]

If something is more negative, then it has more reducing power. To have more reducing power means it can gain more electrons. When E cell is more negative, this means that the reducing power is very high and and it can be easily oxidized.

[Hadji Yono-Cruz 2L]

The more negative the E cell, then the stronger the reducing agent.

[Katie_Duong_1D]

The more negative a reduction potential is, the stronger the reducing agent. The less negative/more positive a reduction potential is, the stronger the oxidizing agent.

[George Ghaly 2L]

The more positive a reduction potential is the easier it is for it to be reduced, and vice versa for an element to be oxidized. Therefore a lower reduction potential would make the best reducing agent.

[Sheridan Slaterbeck 1J]

The more negative the E, the more strong it is as a reducing agent (the thing being oxidized). Another way of saying it is a good donator.

[Chloe Likwong 2K]

Also, remember that the reducing agent is associated with the oxidation reaction.

[Jack Hewitt 2H]

The more negative the value of Ecell is the stronger the reducing agent is.

[Vicky Lu 1L]

Reducing agents are most spontaneous when in oxidation half reactions and therefore they want to lose e-. In order to rank, we can compare the E⁰. The most negative value should be the strongest reducing agent.