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Chapter 9: Problem 42

How would you expect the extent of overlap of atomic orbitals to vary in the series IF, ICl, \(\mathrm{IBr}\), and \(\mathrm{I}_{2}\) ?

Short Answer

Expert verified
The extent of overlap in atomic orbitals is expected to decrease as the atomic size of the halogens increases across the given series, IF, ICl, \(\mathrm{IBr}\), and \(\mathrm{I}_{2}\). This is because larger orbitals have less significant overlap, resulting in weaker bonds. Therefore, the overlap will vary in the order: IF > ICl > \(\mathrm{IBr}\) > \(\mathrm{I}_{2}\).

Step by step solution

01

Understanding atomic orbital overlap

Atomic orbital overlap refers to the degree to which two atoms share their electron clouds when forming a bond. This overlap is the foundation of covalent bonding, where electrons are shared between two atoms. Generally, greater overlap between atomic orbitals results in a stronger and shorter bond.
02

Understanding the trend in atomic size

As we move down a group in the periodic table, the atomic size increases. This is because electrons are added to higher energy levels, which are further from the nucleus. Consequently, the size of the orbitals also increases. In the given series, the atoms bonded to iodine belong to Group 17 (halogens). Going down the group, we have fluorine (F), chlorine (Cl), and bromine (Br).
03

Analyzing the effect of atomic size on overlap

As the size of an atomic orbital increases, the area where an effective overlap can occur decreases. When an atom has a larger orbital, it is more difficult for another atom's orbital to have a significant overlap with it. Therefore, the larger the orbitals, the less likely they are to overlap significantly, resulting in a weaker bond.
04

Applying the trends to the given series

As we go through the series IF, ICl, \(\mathrm{IBr}\), and \(\mathrm{I}_{2}\), the atomic size of the halogens increases. This means that the size of their orbitals also increases. Since larger orbitals have less significant overlap with each other, we can expect the extent of overlap to decrease as we go through the series. So, the extent of overlap in atomic orbitals is expected to be greatest for IF and least for \(\mathrm{I}_{2}\). It will vary in the order: IF > ICl > \(\mathrm{IBr}\) > \(\mathrm{I}_{2}\).

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Most popular questions from this chapter

How many nonbonding electron pairs are there in each of the following molecules: (a) \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~S} ;\) (b) \(\mathrm{HCN}\); (c) \(\mathrm{H}_{2} \mathrm{C}_{2}\) (d) \(\mathrm{CH}_{3} \mathrm{~F}\) ?

(a) Draw a picture showing how two \(p\) orbitals on two different atoms can be combined to make a sigma bond. (b) Sketch a \(\pi\) bond that is constructed from \(p\) orbitals. (c) Which is generally stronger, a \(\sigma\) bond or a \(\pi\) bond? Explain. (d) Can two s orbitals make a \(\pi\) bond? Explain.

The reaction of three molecules of fluorine gas with a Xe atom produces the substance xenon hexafluoride, \(\mathrm{XeF}_{6}\) : $$ \mathrm{Xe}(g)+3 \mathrm{~F}_{2}(g) \longrightarrow \mathrm{XeF}_{6}(s) $$ (a) Draw a Lewis structure for \(\mathrm{XeF}_{6}\). (b) If you try to use the VSEPR model to predict the molecular geometry of \(\mathrm{XeF}_{6 r}\) you run into a problem. What is it? (c) What could you do to resolve the difficulty in part (b)? (d) Suggest a hybridization scheme for the Xe atom in \(\mathrm{XeF}_{6}\). (e) The molecule \(\mathrm{IF}_{7}\) has a pentagonal- bipyramidal structure (five equatorial fluorine atoms at the vertices of a regular pentagon and two axial fluorine atoms). Based on the structure of \(\mathrm{IF}_{7}\), suggest a structure for \(\mathrm{XeF}_{6}\)

The lactic acid molecule, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}\), gives sour milk its unpleasant, sour taste. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many \(\pi\) and how many \(\sigma\) bonds are in the molecule? (c) Which \(\mathrm{CO}\) bond is shortest in the molecule? (d) What is the hybridization of atomic orbitals around each carbon atom associated with that short bond? (e) What are the approximate bond angles around each carbon atom in the molecule?

The molecule shown here is difluaromethane \(\left(\mathrm{CH}_{2} \mathrm{~F}_{2}\right)\) which is used as a refrigerant called R-32. (a) Based on the structure, how many electron domains surround the \(C\) atom in this molecule? (b) Would the molecule have a nonzero dipole moment? (c) If the molecule is polar, in what direction will the overall dipole moment vector point in the molecule? [Sections \(9.2\) and 9.3]
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