Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: hawkslax7 on November 06, 2007, 10:03:45 PM
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I'm having trouble drawing the lewis stucture of IF5. I was wondering if anyone could help.
Thanks.
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For 6 X- (with 7e- each) -->
7e-(6) = 42e- - 6e- (5 F with three sets of lone pairs each) =
12e- - 2e-(5 I-F bonds sharing electrons) =
2e- which accounts for lone pair on I
So
7(6) total electrons = 42
42-30 (non-bonding on F) = 12
12-10 (bonding I-F) = 2
2 (lone pair on I)
Now try drawing the Lewis structure if you understand this.
Understand that some halogens and other elements can have expanded octets and higher oxidation states.
http://en.wikipedia.org/wiki/Iodine_pentafluoride
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http://en.wikipedia.org/wiki/PF5
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http://en.wikipedia.org/wiki/PF5
This is not the same
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That's right, but we do not give here an exact solution, in this case for comparison with you good answer.
http://en.wikipedia.org/wiki/VSEPR
http://www.albion.edu/chemistry/LBL/S07%20Molecular%20Shape.ppt