Concept explainers
(a)
Interpretation:
The most important Lewis structures of ring molecule below have to be drawn and non- zero formal charges and lone pairs have to be shown along with any possible resonance structures.
Concept Introduction:
Lewis structures represent covalent bonds and describe valence electrons configuration of atoms. The covalent bonds are depicted by lines and unshared electron pairs by pairs of dots. The sequence to write Lewis structure of some molecule is given as follows:
- The central atom is identified and various other atoms are arranged around it. This central atom so chosen is often the least electronegative.
- Total valence electrons are estimated for each atom.
- single bond is first placed between each atom pair.
- The electrons left can be allocated as unshared electron pairs or as multiple bonds around the
symbol of the element to satisfy the octet (or duplet) for each atom. - Add charge on the overall structure in case of polyatomic cation or anion.
The formal charge on each atom in the Lewis structure can be calculated from the equation written as follows:
Here,
(b)
Interpretation:
The most important Lewis structures of below ring molecule have to be drawn and non- zero formal charges and lone pairs have to be shown along with any possible resonance structures.
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The most important Lewis structures of below ring molecule has to be drawn and non- zero formal charges and lone pairs have to be shown along with any possible resonance structures.
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The most important Lewis structures of ring molecules have to be drawn and non- zero formal charges and lone pairs have to be shown along with any possible resonance structures.
Concept Introduction:
Refer to part (a).
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Chemical Principles: The Quest for Insight
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- Compute and add on the formal charges in these Lewis structures. Trimethylamine oxidearrow_forwardDraw resonance structures for each of these ions: NSO− and SNO−. (The atoms are bonded in the order given in each case, that is, S is the central atom in NSO−.) Use formal charges to determine which ion is likely to be more stable. Explain why the two ions cannot be considered resonance structures of each other.arrow_forward
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