Read the following chemical equation.

Cl2 (g) + K + Br - → K + Cl - + Br2 (g)

What most likely happens during this reaction?

Potassium loses an electron.

Potassium gains an electron.

Bromine loses an electron.

Bromine gains an electron.

Bromine loses an electron.

Explanation:

Oxide-reduction reactions, also called redox, involve the transfer or transfer of electrons between two or more chemical species. In these reactions two substances interact: the reducing agent and the oxidizing agent.

An oxidizing element or oxidizing agent is one that reaches a stable energy state as a result of which the oxidant is reduced and gains electrons. The oxidizing agent causes oxidation of the reducing agent generating the loss of electrons of the substance and, therefore, oxidizes in the process.

In other words, the oxidizing agent is that chemical species that in a redox process accepts electrons released by the reducing agent and, therefore, is reduced in said process. The oxidizing agent is reduced because, upon receiving electrons from the reducing agent, a decrease in the value of the charge or oxidation number of one of the atoms of the oxidizing agent is induced.

The oxide reduction reaction involves B elements with positive (B + ) or negative (B-) charge. The positive sign on any element B + indicates that element B has lost an electron. Since electrons have a negative charge, it means that the loss of that electron causes a negative charge to be lost and the element to be positively charged. The opposite case is when the element receives an electron, as in the case of B-. Upon receiving an electron, a negative charge is received, the element is negatively charged.

An element that does not indicate its positive or negative charge indicates that it is electrically neutral, that is to say that its charge is zero.

Taking into account all of the above, observe that in the reaction given as data the chlorine changes its oxidation number from the value 0 (Cl₂) to - 1 (Cl-), thus gaining an electron. And bromine changes its oxidation state from - 1 (Br-) to 0 (Br₂), thus losing an electron.

So, most likely during this reaction, bromine loses an electron.

Bromine gains an electron

Explanation:

According to oxidation and reduction