for the compound S2N2, it says that the Lewis structure is:
..
:S=N:
ll l
:N- S:
''
but then the upper left sulfur doesnt obey the octet rule. plus it has 24 instead of 22 valence electrons. it says that they have zero formal charge. what does that mean and how can this be correct?
i thought it was like this:
..
:S- N:
ll l
:N- S:
''
because now there are 22 valence electrons and they all obey the octet rule, but apparently the upper left sulfur would have a positive charge and the upper right nitrogen will have a negative charge. why?
please i really want to understand this