Problem: Two different compounds have the formula XeF2Cl2. Write Lewis structures for these two compounds, and describe how measurement of dipole moments might be used to distinguish between them.

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Xenon (EN = 2.60) is less electronegative than fluorine (EN = 3.98) and chlorine (EN = 3.16) so xenon is the central atom. We then need to count the total number of valence electrons for each element:

Fluorine and chlorine prefers to form 1 bond. There are two possible Lewis structures for this compound:

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Problem Details

Two different compounds have the formula XeF2Cl2. Write Lewis structures for these two compounds, and describe how measurement of dipole moments might be used to distinguish between them.

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Our tutors have indicated that to solve this problem you will need to apply the Dipole Moment concept. You can view video lessons to learn Dipole Moment. Or if you need more Dipole Moment practice, you can also practice Dipole Moment practice problems.

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Based on our data, we think this problem is relevant for Professor Hummel's class at UIUC.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.