Chapter 2 Quiz #7: Expanded Octets

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Chapter 2 Quiz #7: Expanded Octets

Postby Amy_Shao_2D » Sat Nov 12, 2016 9:55 am

Draw the Lewis structure for XeO2F2. Explain why this structure would be allowed for Xe as a central atom but not for Ne as a central atom.

I don't really understand how to answer part 2 of the question. Is it because Ne is too small or something?

Ashley Van Belle 2B
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Re: Chapter 2 Quiz #7: Expanded Octets

Postby Ashley Van Belle 2B » Sat Nov 12, 2016 10:19 am

It is because Ne is too small. If you were to draw the Lewis Structure for XeO2F2, 6 shared electron bonds (One bond from each F, and two bonds from each O) and 2 unpaired electrons would be attached to the central atom in order for the formal charges to all be zero. This makes sense because oxygen has 6 valence electrons(x2), fluorine has 7 valence electrons(x2), and Xe has 8 valence electrons = 34 total electrons to be represented in the Lewis structure. Because Xe is larger and has more electrons, it can bond electrons in the d-orbital. Because it is a larger atom, it also doesn't hold onto its outer electrons as strongly as its inner electrons, making it easier to share those electrons with other atoms. The largest orbital that electrons occupy in Ne is the 2p orbital. It would not have the capability of bonding with two oxygens and 2 fluorines.

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