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Chapter 12: Problem 2
Draw the Lewis representation for each of the following atoms. a) iodine b) sulfur c) phosphorus
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Indicate the total number of electrons in the Lewis structure in Model 3 for each molecule below. a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)
Use your checklist to determine whether or not the following is a valid structure for \(\mathrm{CO}_{2}:\) $$\ddot{\mathrm{O}}=\mathrm{C}=\ddot{\mathrm{O}}$$ For each item in your checklist, describe how you determined whether or not it was met. Then indicate whether or not the above structure is valid.
Calculate the total number of valence electrons in each of these molecules by summing up the number of valence electrons present in each constituent atom. In each case, explicitly show how you reached your final answer. a) \(\mathrm{H}_{2} \mathrm{CO}\) b) \(\mathrm{N}_{2}\) c) \(\mathrm{Cl}_{2}\)
Create a checklist that can be used to determine if a Lewis structure for a molecule is correct. Two items from the Information section are included below as a start. H must be surrounded by two electrons - a single bond. C, \(\mathrm{N}, \mathrm{O}\), and \(\mathrm{F}\) must be surrounded by eight electrons (the octet rule).
Given the shell model of the atom, suggest a possible reason that Lewis proposed a maximum of two electrons for hydrogen and a maximum of eight for carbon, nitrogen, oxygen, and fluorine atoms.
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