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Chapter 9: Problem 48

How would you expect the extent of overlap of the bonding atomic orbitals to vary in the series IF, ICl, IBr, and \(I_{2}\) ? Explain your answer.

Short Answer

Expert verified
The extent of overlap of the bonding atomic orbitals in the series IF, ICl, IBr, and I2 varies due to the size and electronegativity differences between the iodine and halogen atoms. The overlap is the least for IF and the greatest for I2, with ICl and IBr exhibiting intermediate overlap extents, as the size difference and electronegativity difference decrease in the order IF > ICl > IBr > I2.

Step by step solution

01

Analyze atomic size

In order to discuss the extent of the overlap of the bonding atomic orbitals in these compounds, we need to consider the size of the atoms involved. The size of the atoms generally increases going down a group in the periodic table. Therefore, among the halogens (F, Cl, Br, and I), fluorine is the smallest and iodine is the largest.
02

Review electronegativity differences

Electronegativity is the ability of an atom in a molecule to attract electrons to itself. In general, electronegativity decreases as we go down a group in the periodic table, so the electronegativity difference between iodine and the other halogens also plays a role in the extent of orbital overlap.
03

Consider atomic size and electronegativity differences for IF

In IF, the iodine atom is much larger than the fluorine atom, but the electronegativity difference is also significant. Due to the size difference, the extent of the overlap of the bonding atomic orbitals would be lesser compared to other molecules in the series.
04

Consider atomic size and electronegativity differences for ICl

In the ICl molecule, the size difference between iodine and chlorine atoms is smaller compared to IF, and the electronegativity difference is also smaller. As a result, the extent of the overlap of the bonding atomic orbitals in ICl would be greater than in IF but might still be lesser compared to IBr and I2.
05

Consider atomic size and electronegativity differences for IBr

In IBr, the size difference between iodine and bromine atoms is even smaller. The electronegativity difference is also smaller. Therefore, the extent of the overlap of the bonding atomic orbitals in IBr would be greater than in both IF and ICl.
06

Consider atomic size and electronegativity differences for I2

In the I2 molecule, both atoms are iodine, so there is no size difference and no electronegativity difference. As a result, the extent of the overlap of the bonding atomic orbitals would be the greatest among the molecules in this series.
07

Conclusion

The extent of overlap of the bonding atomic orbitals in the series IF, ICl, IBr, and I2 varies with the size and electronegativity differences between the atoms involved. The overlap would be the least for IF and the greatest for I2, with ICl and IBr exhibiting intermediate overlap extents in the series, as the size difference and electronegativity difference decrease in the order IF > ICl > IBr > I2.

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