Rank these species by their ability to act as an oxidizing agent from best oxidizing agent to best reducing agent. ag+ cr3+ sn2+ na+

From best oxidizing agent to best reducing agent : Ag⁺, Sn²⁺, Cr³⁺, Na⁺

The oxidation-reduction reaction or abbreviated as Redox is a chemical reaction in which there is a change in oxidation number

3 basic theories explain this Redox concept:

The oxidation reaction is the binding of a substance with oxygen. (O₂)

For example:

2SO₂ + O₂ > 2SO₃

The reduction reaction is the release of oxygen from a substance.

For example:

2CuO → 2Cu + O₂

Oxidation is an electron release event

Example:

2F ---> 2Fe³⁺ + 6e⁻

The reduction is an electron capture event

Example:

3O₂ + 6e⁻ ---> 3O²⁻

Oxidation is an increase  in oxidation number, while reduction is a decrease in oxidation number.

In the redox reaction, it is also known

Reducing agents are substances that experience oxidation

Oxidizing agents are substances that experience reduction

The metal activity series is expressed in voltaic series

Li-K-Ba-Ca-Na-Mg-Al-Mn- (H2O) -Zn-Cr-Fe-Cd-Co-Ni-Sn-Pb- (H) -Cu-Hg-Ag-Pt-Au

The more to the left, the metal is more reactive (easily release electrons) and the stronger reducing agent

The more to the right, the metal is less reactive (harder to release electrons) and the stronger oxidizing  agent

So that the metal located on the left can push the metal on the right in the redox reaction

From the ion ion below:

 Ag⁺ ;Cr³⁺ ;Sn²⁺; Na⁺

If we sort according to the voltaic series: (from left to right)

Na, Cr, Sn, Ag

Then:

Na, the most reactive, strong reducing agent

Ag, less reactive, strong oxidizing agents

So that the order from best oxidizing agent to best reducing agent.

Ag⁺, Sn²⁺, Cr³⁺, Na⁺

an oxidation-reduction reaction

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a reducing agent during a redox reaction

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loses electrons in a chemical reaction

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Keywords: reduction, oxidation

2b2t

explanation:

2b2t