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In the BEST Lewis structure for hydrogen cyanide, HCN, the formal charge charge on H is __________, the formal charge on C is___________ , and the formal charge on N is _________. Indicate formal charge with a sign followed by a numerical charge (e.g. -2, +1) unless the charge is 0, then enter 0.

The formal charge is the "charge" an element would have in a molecule or ion if all of the bonding electrons were shared equally between atoms. Use the References to access important values if needed for this question. We can draw three inequivalent Lewis structures for dinitrogen monoxide, N₂O . The concepts of formal charge and electronegativity can help us choose the structure that is the most significant representation. 1. Assign formal charges to the elements in each of the structures below. Formal Charge N₁ N₂ :N,=N,-O: || A N=N,=Ô N-N,=O: C 2. The structure that contributes most significantly to the overall electronic structure of N₂O is ↑ Formal Charge

Consider the SO 3 molecule. How many valence electrons does the molecule have?   How many lone pairs of electrons are on the central atom?   How many lone pairs of electrons in total are on the substituent atoms?   How many resonance structures can be drawn for the molecule?  If the ion doesn't exhibit resonance, indicate "1" as only one structure can be drawn for the molecule.