<p>SO2.</p>
<p>whenever i see the structure of this, it appears as if the sulfur has 10 valence electrons after sharing (which is impossible)..</p>
<p>the sulfur has one lone pair of electrons..and then it has a double bond with each oxygen. (4x2)+2=10</p>
<p>can someone help me out</p>
<p>It doesn't have a double bond with both oxygen atoms. The structure is O=S-O, and sulfur has a lone pair while each oxygen atom has the appropriate lone pairs to complete the octet.</p>
<p>Also, don't call 10 valence electrons impossible. Xenon has 12 in XeF4.</p>
<p>Sorry, must have been a misprint in the PR book!</p>
<p>"Also, don't call 10 valence electrons impossible. Xenon has 12 in XeF4."</p>
<p>i havent seen anything like that ever come up.</p>
<p>EDIT: I doubt those would ever show up on the sat II chem im sayin</p>
<p>Xenon tetrafluoride is the classic example of the square planar geometry. Xenon bonds to a fluoride with 90 degree bond angles on a single plane, and has 1 lone pair on either side of it (above/below). There are a lot of compounds like this. Another example is phosphorus pentachloride (5 single bonds, no lone pairs on phosphorus).</p>