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Chapter 44: Problem 1

The H-X bond strength decreases in the series HF, HCl, HBr, HI. Explain this trend in terms of the molecular structure of the molecules.

Short Answer

Expert verified
The H-X bond strength decreases in the series HF, HCl, HBr, HI due to increasing atomic size, decreasing atomic orbital overlap, and increasing electron shielding.

Step by step solution

01

Understanding the Relation of Atomic Size with Bond Strength

Typically, as the size of an atom increases, the bond strength decreases. This is because the positively charged nucleus of a larger atom is less able to attract the bonded electrons than in the case of a smaller atom's nucleus. So, in this case, as the halogens in the series – F, Cl, Br, I – increase in size, the bond strength should decrease.
02

Overview of Atomic Orbital Overlap

The strength of a bond can also be related to the extent of overlap of atomic orbitals. Greater the overlap, stronger is the bond. Since the size of atomic orbitals also increases with atomic size, smaller atoms like fluorine can have better orbital overlap leading to stronger bonds.
03

Concept of Electron Shielding

Electron shielding refers to the repulsion between the electrons in the bond. As we move down the group, additional electron shells are added which leads to increased shielding. This increased shielding weakens the bond as it causes the bond electrons to be less attracted to the nuclei.
04

Combining all information into an explanation

The decrease in H-X bond strength in the series HF, HCl, HBr, HI can be explained by a combination of the above factors: increasing atomic size, decreasing orbital overlap, and increasing electron shielding. As we go from HF to HI, these factors contribute to a decrease in bond strength.

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Most popular questions from this chapter

Which hydrogen atom is the most acidic hydrogen atom in HCOOH?

What structural feature or atomic property accounts for the decrease in the partial charge on the acidic hydrogen in the series HOCl, HOBr, HOI?

What structural features or atomic property causes the partial charge on the acidic hydrogen to increase in the series \(\mathrm{CH}_{3} \mathrm{COOH}, \quad \mathrm{CH}_{2} \mathrm{ClCOOH}\), \(\mathrm{CHCl}_{2} \mathrm{COOH}, \mathrm{CCl}_{3} \mathrm{COOH} ?\)

Which hydrogen atom is the most acidic hydrogen atom in \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) ?
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