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Answer: A rule for drawing plausible Lewis structures is
Chapter 9, Problem 87P(choose chapter or problem)
A rule for drawing plausible Lewis structures is that the central atom is invariably less electronegative than the surrounding atoms. Explain why this is so. Why does this rule not apply to compounds like \(\mathrm {H_2O}\) and \(\mathrm {NH_3}\)?
Questions & Answers
QUESTION:
A rule for drawing plausible Lewis structures is that the central atom is invariably less electronegative than the surrounding atoms. Explain why this is so. Why does this rule not apply to compounds like \(\mathrm {H_2O}\) and \(\mathrm {NH_3}\)?
ANSWER:Step 1 of 2
Here, we are going to explain the why the rules for Lewis structure is not applicable for the \(H_2O\) and \(NH_3\).
Lewis structure of the compound or molecule, least electronegative atom occupies the center position .Generally hydrogen and fluorine atom occupies a terminal position in the Lewis structure.This is because most electronegative atom present in the center position of the molecule electron density is pulled towards that position .Hence, most of electron density is present in the center position of the compound or molecule .
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