Iodine trifluoride

<h2 id="reactions">Reactions</h2>
<p><a href="/facts/Fluorine/YUV0Fb8m">F2</a> reacts with <a href="/facts/Iodine/JlfMecMf">I2</a> to yield IF3 at −45 °C in <a href="/facts/Trichlorofluoromethane/bx7YxsjC">CCl3F</a>.  Alternatively, at low temperatures, the fluorination reaction I2 + 3<a href="/facts/Xenon_difluoride/vKS7zojD">XeF2</a> → 2IF3 + 3<a href="/facts/Xenon/9E3XR69R">Xe</a> can be used.  Not much is known about iodine trifluoride as it is so unstable.
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<h2 id="structure">Structure</h2>
<p>The iodine atom of iodine trifluoride has five electron pairs, of which two are lone-pairs, and the molecule is T-shaped  as predicted by <a href="/facts/VSEPR_Theory/WqsRgVRV">VSEPR Theory</a>.<a class="footnote-ref" id="fnref:1" href="#fn:1"><sup>1</sup></a>
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<h2 id="references">References</h2>

<ol>
<li id="fn:1"><p>Greenwood, Norman  N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li>
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Iodine trifluoride open-in-new

Iodine trifluoride