Question

Some of the conditions that play a role in the degree of reduction of a reaction include the strength of the reducing agent as well as the pH of the solution. In part III, you will observe the reduction of the permanganate ion in the presence of an acid as well as in the presence of a base. You will use visual observations to identify which product is formed. Possible products of the reduction of the permanganate ion include the green MnO2 (manganate ion), the brown-black solid MnO and the pale pink Mnº? This pale pink color is often so pale that it is not detected and looks colorless instead. The Fe*'most often produces a pale green Fe*2 that is also often too pale to detect. When the product is too pale to detect confirmation that the reaction occurred depends on the color observations of the other reactants present. As you mix combinations of these oxidizing agents with the halogens you may or may not see a chemical reaction. No reaction indicates that the oxidizing agent was not strong enough to cause a reaction.

im having a hard time finding whether the following chemicals made reactions are not based off of their colors, and the above questions 2,3,and 4.

Answer 1

Question 2.

The reducing power of the given halides: Cl^- < Br^- < I^-

Explanation: Higher the size of a halide ion, the lower is its electronegativity and hence the higher will be its reducing power.

Question 3.

F2 is predicted to be a stronger oxidizing agent than Cl2.

Explanation: Fluorine is more electronegative than chlorine, hence F2 is a stronger oxidizing agent than Cl2.

Question 4.

Oxidizing strength of halogens: F2 > Cl2 > Br2 > I2

Reducing strength of halogens: F2 < Cl2 < Br2 < I2

Oxidizing strength of halide ions: F^- > Cl^- > Br^- > I^-

Reducing strength of halide ions: F^- < Cl^- < Br^- < I^-