In this redox reaction, identify the reducing agent. 2Li + F2 2LiF

The oxidation number is the charge that an atom has; is an integer that represents the number of electrons an atom puts into play when it forms a given compound.

In other words, the oxidation number of an element is a value that indicates the number of electrons that element gains or loses when it combines with another.

Definition of redox reactions

Redox Reactions or Reduction-Oxidation Reactions are those in which electrons are transferred between the reactants, producing a change in the oxidation states with respect to the products.

In redox reactions there are two species:

Reducing Agent: transfers electrons to the medium increasing its oxidation state (it oxidizes).
Oxidizing Agent: captures electrons from the medium reducing its oxidation state (it is reduced).

Reducing agent in this case

In this case, you know the redox reaction:

2 Li + F₂ → 2 LiF

First of all, you should know that:

The state or oxidation number of an element in the ground state or uncombined is zero.
The sum of the oxidation states of a neutral molecule is 0.
Ions composed of a single atom have their oxidation number equal to their charge. For example: Li⁺.
Fluorine always has oxidation state -1 because it is the most electronegative element that exists (F⁻).

In this case, then you know that the oxidation number of each element is:

Li → oxidation number= 0

F₂ → oxidation number= 0

LiF → Li⁺ and F⁻ → oxidation number Li= +1 and oxidation number= -1

Finally, Li increases its oxidation number, so Li is the reducing agent.

Learn more about redox reactions:

https://brainly.com/question/2890416

https://brainly.com/question/15169665

https://brainly.com/question/14158723

#SPJ2