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Chapter 20: Problem 71

How does the oxyacid strength of the halogens vary as the number of oxygens in the formula increases?

Short Answer

Expert verified
The oxyacid strength of halogens increases as the number of oxygens in the formula increases. This is due to the increased electron-withdrawing effect caused by the presence of multiple oxygen atoms, which weakens the bond between the hydrogen atom and the oxygen atom, making it easier to release the hydrogen ion as a proton and enhancing the acidity of the molecule.

Step by step solution

01

Understanding Oxyacids of Halogens

Oxyacids are a class of compounds that contain an acidic hydrogen atom bonded to an oxygen atom. Oxyacids of halogens are compounds in which the halogen atoms (such as fluorine, chlorine, bromine, and iodine) are attached to these oxygen atoms. These compounds have the general formula HOXO_n, where X represents the halogen and n represents the number of oxygen atoms. Examples include hypochlorous acid (HOCl), chlorous acid (HClO_2), chloric acid (HClO_3), and perchloric acid (HClO_4).
02

Comparing Oxyacid Strengths

To understand the variation in oxyacid strength as the number of oxygens in the formula increases, we will analyze the relationship between the presence of oxygens and the strength of the bond between the hydrogen atom and the oxygen atom. An oxyacid is considered stronger when this bond is weaker, and easier to break, thus allowing the hydrogen ion to be released as a proton (H^+).
03

The Effect of Increasing the Number of Oxygens

As the number of oxygen atoms in the oxyacid molecule increases, there is an increase in the electron-withdrawing effect. The oxygen atoms are more electronegative, which means they have a higher affinity for electrons and will draw the bonding electrons away from the hydrogen atom. This causes a decrease in the bond strength between the hydrogen and the oxygen atoms, making the compound more acidic.
04

Understanding the Relationship

As a result, we can establish a relationship between the number of oxygens in the oxyacid formula and the acidity of the compound: the more oxygens, the greater the acidity. This is because the presence of multiple oxygen atoms enhances the electron-withdrawing effect. In summary, oxyacid strength of halogens increases as the number of oxygens in the formula increases, due to the increased electron-withdrawing effect. This effect weakens the bond between the hydrogen atom and the oxygen atom, making it easier to release the hydrogen ion as a proton and enhancing the acidity of the molecule.

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Most popular questions from this chapter

An unknown element is a nonmetal and has a valence electron configuration of \(n s^{2} n p^{4}\). a. How many valence electrons does this element have? b. What are some possible identities for this element? c. What is the formula of the compound(s) this element would form with lithium? hydrogen? magnesium? aluminum? fluorine?

The electrolysis of aqueous sodium chloride (brine) is an important industrial process for the production of chlorine and sodium hydroxide. In fact, this process is the second largest consumer of electricity in the United States, after the production of aluminum. Write a balanced equation for the electrolysis of aqueous sodium chloride (hydrogen gas is also produced).

Phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) is a triprotic acid, phosphorous acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{3}\right)\) is a diprotic acid, and hypophosphorous acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{2}\right)\) is a monoprotic acid. Explain this phenomenon.

Use the symbols of the elements described in the following clues to fill in the blanks that spell out the name of a famous American scientist. Although this scientist was better known as a physicist than as a chemist, the Philadelphia institute that bears his name does include a biochemistry research facility. (1) The oxide of this alkaline earth metal is amphoteric. (2) The element that makes up approximately \(3.0 \%\) by mass of the human body. (3) The element having a \(7 s^{1}\) valence electron configuration. (4) This element is the alkali metal with the least negative standard reduction potential. Write its symbol in reverse order. (5) The alkali metal whose ion is more concentrated in intracellular fluids as compared with blood plasma. (6) This is the only alkali metal that reacts directly with nitrogen to make a binary compound with formula \(\mathrm{M}_{3} \mathrm{~N}\). (7) This element is the first in Group \(3 \mathrm{~A}\) for which the \(+1\) oxidation state is exhibited in stable compounds. Use only the second letter of its symbol.

Lead forms compounds in the \(+2\) and \(+4\) oxidation states. All lead(II) halides are known (and are known to be ionic). Only \(\mathrm{PbF}_{4}\) and \(\mathrm{PbCl}_{4}\) are known among the possible lead(IV) halides. Presumably lead(IV) oxidizes bromide and iodide ions, producing the lead(II) halide and the free halogen: Suppose \(25.00 \mathrm{~g}\) of a lead(IV) halide reacts to form \(16.12 \mathrm{~g}\) of a lead(II) halide and the free halogen. Identify the halogen.
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