Write "oxidation" before the reaction below which is anoxidation reaction; write "reduction" before the reaction belowwhich is a reduction reaction.

a.____________________ Na----> Na+ (small+) + e-
b.____________________ Cl + e- ----> Cl-
What does it mean when chemists say that a reactant isreduced?
What does it mean when chemists say that a reactant is areducing agent?
Is Francium (Fr) likely to be reduced in a chemical reaction?Would it be easy or difficult to separate Francium from ores? Explain your reasoning

losing an electron is oxidation

gaining an electron is reduction.

a reducing agent is oxidized.

Fr can easily lose an electron. Now separating it is another question, as there is only 2 ounces worldwide of this element at any one time. The longest life isotope of this element is 22 min. Never since discovery (1949, I think) has any weighable amount been produced. I rate this question unanswerable.

It would be difficult to separate Francium from ores. Francium is on the bottom left of the periodic table, therefore it loses electrons easily making it very difficult to give it the electrons necessary to separate it from ores

a. Oxidation: Na ----> Na+ (small+) + e-

b. Reduction: Cl + e- ----> Cl-

When chemists say that a reactant is reduced, it means that the reactant gains electrons, resulting in a decrease in oxidation state or an increase in the electron density around the atom or molecule.

When chemists say that a reactant is a reducing agent, it means that the reactant has a tendency to donate electrons to other species in a chemical reaction. In other words, it is capable of causing the reduction of another species by transferring electrons to it.

As for Francium (Fr), it is a highly reactive alkali metal and is likely to be reduced in a chemical reaction. It has a strong tendency to donate its single valence electron and achieve a stable electron configuration, so it is a very strong reducing agent. However, Francium is extremely rare and unstable, making it difficult to separate from ores. Because of its instability and short half-life, it is typically produced in laboratories and not found in nature in large quantities.