CHEMISTRY-TEXT
8th Edition
ISBN: 9780134856230
Author: Robinson
Publisher: PEARSON
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Chapter 7, Problem 7.103SP
Interpretation Introduction
Interpretation:
The resonance form of the given structure needs to be determined. The formal charges need to be assigned. The two resonance structures need to be compared on the basis of the contributor to the resonance hybrid.
Concept introduction:
Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that existing on each bonded atom.
Lewis dot structure is also known as Lewis dot formula or electron dot structure. The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.
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Write the resonance structure for each of the following compounds. Which resonance structure contributes most to the hybrid? Explain your choice. Be sure write the formal charges where appropriate
Write resonance structure for each of the following compounds and formal charges where appropriate. Which one most to hybrid? Explain.
In the fictitious molecule, highlight the atoms that have nonzero formal charges. Assume all lone pairs are shown.
Chapter 7 Solutions
CHEMISTRY-TEXT
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