Question

The oxidizing power of \(\mathrm{HXO}_{4}\) type compounds of halogens is in the order (a) \(\mathrm{HIO}_{4}>\mathrm{HBrO}_{4}>\mathrm{HClO}_{4}\) (b) \(\mathrm{HIO}_{4}>\mathrm{HClO}_{4}>\mathrm{HBrO}_{4}\) (c) \(\mathrm{HBrO}_{4}>\mathrm{HIO}_{4}>\mathrm{HClO}_{4}\) (d) \(\mathrm{HClO}_{4}>\mathrm{HBrO}_{4}>\mathrm{HIO}_{4}\)

Short answer

The order of oxidizing power is \(\mathrm{HClO_4 > HBrO_4 > HIO_4}\), so option (d) is correct.

Step-by-step solution

Understanding Oxidizing Power

Oxidizing power is the ability of a compound to gain electrons. In halogen oxoacids, this depends on the ability of the central atom (halogen) to accept electrons. Higher oxidizing power is associated with higher ability to accept electrons.

Identifying Halogen Atoms

In the given acids, the halogens involved are Iodine (I), Bromine (Br), and Chlorine (Cl). The central atom in each compound ("HXO_4" type) is the halogen, which will affect the oxidizing power.

Considering Electronegativity and Oxidation States

Chlorine has the highest electronegativity among Iodine, Bromine, and Chlorine. The oxidation state for each halogen in "HXO_4" type is +7. The oxidizing ability of these compounds is generally influenced by both the electronegativity and the oxidation state of the halogen.

Determining the Oxidizing Power Order

In halogen oxoacids, higher electronegativity corresponds to higher oxidizing power because the halogen can accept more electrons. Therefore, the order of electronegativity is Cl > Br > I, resulting in the order of oxidizing power as: \[\mathrm{HClO_4 > HBrO_4 > HIO_4}\] Thus, \mathrm{HClO_4} has the highest oxidizing power among the given options.

Conclusion

After understanding the concepts and comparing the electronegativity, we determine that the correct order of oxidizing power for the given halogen oxoacids is \(\mathrm{HClO_4 > HBrO_4 > HIO_4}\). The correct answer is option (d).

Key concepts

Oxidizing Power

Oxidizing power refers to how effectively a compound can gain electrons through a chemical reaction. It is an essential concept when studying halogen oxoacids. These acids include halogens combined with oxygen and typically appear in a form such as \(HXO_4\). The halogen is the central atom in these compounds and determines their oxidizing ability.
In simple terms, higher oxidizing power means the halogen oxoacid can more easily snap up electrons from other substances, causing them to oxidize. This ability to accept electrons is crucial in many chemical reactions, impacting how substances interact or transform. Understanding which halogen oxoacid has the greatest oxidizing power can help predict reaction behaviors and characteristics.

Electronegativity

Electronegativity is pivotal in explaining the differences in oxidizing power among halogen oxoacids. It measures an atom's ability to attract electrons within a chemical bond. Among the halogens, chlorine (Cl) is the most electronegative, followed by bromine (Br) and iodine (I). This order influences the behavior of halogen oxoacids like \(ailofthisdocn{HClO_4}\), \(HBrO_4\), and \(HIO_4\).
Highly electronegative atoms can attract electrons more strongly. In halogen oxoacids, a higher electronegativity leads to greater oxidizing potential. Therefore, \(HClO_4\), with its highly electronegative chlorine atom, has a stronger oxidizing power compared to \(HBrO_4\) and \(HIO_4\). It is crucial to comprehend this concept, as it affects the capabilities of various chemical compounds in redox reactions.

Halogen Atoms

Halogen atoms are elements from Group 17 of the periodic table. These include chlorine (Cl), bromine (Br), and iodine (I). Each of these atoms has its unique properties and behaviors.
In the context of the halogen oxoacids, the particular halogen atom plays a crucial role in determining the chemical properties like oxidizing power. The intrinsic properties of each halogen, such as size and electron affinity, impact how they function in oxoacids. Despite having the same formal oxidation state in the \(HXO_4\) type compounds (+7), the differences in electronegativity and atomic structure lead to disparities in their oxidizing capabilities. Understanding these foundational attributes of halogen atoms can assist in predicting and rationalizing the outcomes of chemical reactions involving these oxoacids.

Oxidation States

Oxidation states, often called oxidation numbers, are vital when evaluating halogen oxoacids' properties. They indicate the degree of oxidation of an atom within a compound. In \(HXO_4\) type compounds, the halogen typically displays its highest oxidation state at +7.
The oxidation state is significant because it correlates with an element's capability to influence the oxidizing power. Higher oxidation states frequently mean higher oxidizing abilities because the electron-deficient state is more receptive to gaining electrons through a chemical reaction. In the case of \(HClO_4\), \(HBrO_4\), and \(HIO_4\), each has the +7 oxidation state. Here, the combination of high oxidation states and electronegativity differences among the halogens leads to the varying oxidizing powers of these acids. Understanding oxidation states enables one to predict the oxidizing strength effectively and anticipate reaction outcomes.