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Hi, this is Dr. B. Let's do the SF6 Lewis structure. On the periodic table, Sulfur:
6 valence electrons, plus Fluorine 7, but we have six of those. So 6 + 42 gives us 48
total valence electrons. Put the Sulfur at the center, and let's put some Fluorines around
it here, we have 6 of them...4, 5, 6. Draw chemical bonds between the atoms, 1, 2, 3,
and each of these represents two valence electrons. So I have six, I've used 12 valence electrons.
We'll go around the outside, 14, 16, 18, and 48. So you can check and see, each of the
Fluorines now has 8 valence electrons. And the Sulfur, it has more than 8, but because
it's in period 3, that's OK. It can hold more than 8. We've used all 48 valence electrons.
All the outer atoms have their octets. Sulfur's OK. You could check the formal charges if
you wanted to make sure that they worked out. They are all zero for this structure. That's
the SF6 Lewis structure. This is Dr. B., and thanks for watching.