4.a) Draw two Lewis structures for HCP; one where C is central and one where P is central: b) Calculate formal charge for each a

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4.a) Draw two Lewis structures for HCP; one where C is central and one where P is central: b) Calculate formal charge for each a

tom in each structure: Which structure is favored? Explain your answer: 5. a) Draw all possible resonance structures for HCOSel (C is central) b) Calculate formal charge for each atom in each structure: Which structure is favored? Explain your answer:

Chemistry

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love history [14] · Answer 1 · 2024-07-31T12:00:35+03:00

One Hydrogen atom (H) and one Oxygen atom (O) surround the central Carbon atom (C) in the HCP Lewis structure (O). Carbon (C) and Phosphorus (P) have a triple bond, and Carbon (C) and Hydrogen (H) have a single bond.

<h3>How can you choose the ideal format for a formal charge?</h3>

The Lewis structure with the negative formal charges on the most electronegative atoms is the one to choose from when faced with a choice between numerous Lewis structures with similar formal charge distributions.

<h3>How do you determine the preferred resonance structure?</h3>

The resonance forms with the fewest non-zero formal charge atoms are selected. Resonance develops atoms that have a negative formal charge or are the most electronegative are preferred.

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