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So the one sulfur makes 6 valence electrons and the 2 fluorines have 12 valence electrons= 18 total..plus the one (1-) is 15... I'm confused about what the bonds are (double, single?) and where they are, and where and how many the electron (dots) are on each element

basically whats the lewis structure haha

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To my knowledge, there is no stable SF2^- ion.  For one thing, it would be a free radical, meaning that it has an odd number of electrons.  Free radicals tend to be quite reactive because of the single unpaired electron.

Fluorine has 7 valence electrons, not six.  You seem to have trouble counting electrons.  Assuming the anion exists, it would have 21 electrons, six for sulfur and seven each for the fluorine atoms, plus one more because of its "charge".  It would have no double bonds. There does exist a neutral sulfur difluoride molecule.  It has a bent geometry with single bonds to each fluorine and two lone pairs on the sulfur.

Your probably nonexistent SF2^- would have to have one more single electron on sulfur, giving it an expanded octet, and making the anion a free radical.  Not likely.

========= Follow up ==========

The dream is a little unclear about how to draw Lewis structures.  To accurately draw the Lewis structure you MUST count the valence electrons.

Hemiketal is having trouble counting electrons, too.  The question says, "SF2 1-" which I take to mean one sulfur, two fluorines, and a charge of -1.  Count the electrons: 6 + 2(7) + 1 = 21.

Electronegativity was first developed by Linus PAULING.  Pauli, as in Wolfgang Pauli, was a pioneer in quantum theory.
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Sulfur has six valence electrons, however, each fluorine actually has 7 valence electrons a piece (it is a group 7 atoms). This means your total electron count is 22.... 2(7)+6+2(for the negative charge)=??

So your structure will have sulfur as the central atom with no pi (double) bonds. Think about it, Fluorine is the most electronegative atom on the periodic table. This means it holds its electrons very tightly. the existence of a double bond would give fluorine a +1 formal charge. This is so not happening with the fact that fluorine has an electronegativity of 4 on the Pauli scale.

So, sulfur central atom, two sigmas (single) bonds to fluorine, each fluorine has 3 sets of lone pairs, that takes care of 16 of our electrons. the other 6 make three lone pairs on the sulfur (which can handle the exceeded valence octet because it is a huge atom).
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it is hard to think of the structure by counting the valence electrons. Instead, just look at the characteristics of each atom. You have one Sulfur and 2 fluorines. Sulfur is in column 6, and all column 6 atoms form 2 bonds as oxygen does. Fluorine makes one bond because it only needs one more electron to complete its orbit.

so you have one atom that makes 2 bonds, and two atoms that make one bond each.

the structure is F - S - F

there are two pairs of electrons on s, and three pairs on each of F.

but, you indicate that this molecule has an extra charge. As it is written, this is very not likely, since no atom could carry the extra electron, but S2F 1- could be what you mean.

if it is supposed to be S2F-, then the structure is S - S - F, with three pairs of electrons on the first sulfur atom.
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