Xenon tetrafluoride Lewis structure

In many expanded-octet molecules, one or more of the electron pairs around the central atom are unshared. Recall, for example, the Lewis structure of xenon tetrafluoride, XeF4 (Example 7.4). 

I Self-Test 2.10B Write the lewis structure for the l ion and give the number of 25 Xenon tetrafluoride, XeF4 I electrons in the expanded valence shell. 

Let s work two examples illustrating the steps necessary to produce a good Lewis structure. We will take HN02 and XeF4 for these examples. The first molecule is nitrous acid. It is an example of an oxyacid. (Oxyacids are compounds containing hydrogen, oxygen, and one other element.) The other compound is xenon tetrafluoride. 

Self-Test 2.10A Write the Lewis structure for xenon tetrafluoride, XeF4, and give the number of electrons in the expanded octet. 

Xenon is a noble gas that will form a few compounds with nonmetals that strongly attract electrons. Draw the correct Lewis structure for xenon tetrafluoride (Xep4). 

Draw a Lewis structure of the noble gas compound xenon tetrafluoride (Xep4) in which all F atoms are bonded to the central Xe atom. 

Draw the Lewis structure of xenon tetrafluoride (XeF4). 

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