Complete the exercises below. Explain each of the following obser...

Question

Complete the exercises below. Explain each of the following observations: a. At room temperature, I₂ is a solid, Br₂ is a liquid, and Cl₂ and F₂ are both gases. b. F₂ cannot be prepared by electrolytic oxidation of aqueous F⁻ solutions. c. The halogens decrease in oxidizing power in the order F₂ > Cl₂ > Br₂ > I₂.

Accepted Answer

a. The physical states of halogens at room temperature are determined by the strength of intermolecular forces. Iodine (I₂) is a solid because it has the strongest London dispersion forces due to its larger number of electrons and greater polarizability. Bromine (Br₂) is a liquid as it has moderate London dispersion forces. Chlorine (Cl₂) and fluorine (F₂) are gases because they have weaker London dispersion forces due to their smaller size and fewer electrons.. b. Fluorine (F₂) cannot be prepared by electrolytic oxidation of aqueous F⁻ solutions because fluorine is a very strong oxidizing agent. In aqueous solutions, water is more easily oxidized than fluoride ions, leading to the production of oxygen gas instead of fluorine gas. This is due to the fact that the oxidation potential of water is lower than that of fluoride ions.. c. The oxidizing power of halogens decreases in the order F₂ \u003e Cl₂ \u003e Br₂ \u003e I₂ because of their electronegativity and bond dissociation energies. Fluorine is the most electronegative element, making it the strongest oxidizing agent as it readily gains electrons. As you move down the group, the electronegativity decreases and the bond dissociation energy increases, making the halogens less effective at gaining electrons and thus decreasing their oxidizing power.. To understand the trend in oxidizing power, consider the standard reduction potentials of the halogens. Fluorine has the highest reduction potential, indicating it is the most likely to gain electrons and act as an oxidizing agent. As you move down the group, the reduction potentials decrease, reflecting the decreasing oxidizing power.. The differences in physical states and chemical reactivity among the halogens can be attributed to their molecular size, electron configuration, and the resulting intermolecular forces and electronegativity. These factors collectively influence their physical properties and chemical behavior.

주요 개념

States of Matter and Molecular Interactions

Electrolysis and Ion Stability

Oxidizing Power of Halogens