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Chapter 10: Problem 22

Assign formal charges to the atoms in the following species, and then select the more likely skeletal structure. (a) \(\mathrm{H}_{2} \mathrm{NOH}\) or \(\mathrm{H}_{2} \mathrm{ONH}\) (b) SCS or CSS (c) NFO or FNO (d) \(\mathrm{SOCl}_{2}\) or \(\mathrm{OSCl}_{2}\) or \(\mathrm{OCl}_{2} \mathrm{S}\) (e) \(\mathrm{F}_{3} \mathrm{SN}\) and \(\mathrm{F}_{3} \mathrm{NS}\)

Short Answer

Expert verified
Assigning formal charges will help to determine the most likely skeletal structure for each listed compound.

Step by step solution

01

Understand Formal Charge

The formal charge on an atom is calculated by subtracting the sum of the number of lone pair electrons and half the number of bonding electrons from the total number of valence electrons. A neutral molecule would have total formal charges equal to 0.
02

Assigning Formal Charges for Compound (a)

For (a) \(\mathrm{H}_{2} \mathrm{NOH}\) and \(\mathrm{H}_{2} \mathrm{ONH}\). Calculate the formal charges for each nitrogen and oxygen in the two compounds. Based on the calculated values and the rule where the most electronegative atom usually carries the negative formal charge, choose the one that follows this rule the most.
03

Repeat for Other Compounds

Perform the same calculations and analysis for compounds (b) SCS or CSS, (c) NFO or FNO, (d) \(\mathrm{SOCl}_{2}\) or \(\mathrm{OSCl}_{2}\) or \(\mathrm{OCl}_{2} \mathrm{S}\), and (e) \(\mathrm{F}_{3} \mathrm{SN}\) and \(\mathrm{F}_{3} \mathrm{NS}\).
04

Draw Skeletal Structures

With the gained knowledge about most likely formal charges, proceed to draw the skeletal structures for each of the compounds. The structure that results in the least amount of charges is the more likely skeletal structure.

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Most popular questions from this chapter

Sketch the propene molecule, \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

The greatest bond length is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{Br}_{2} ;\) (d) BrCl.

The highest bond-dissociation energy is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2} ;\) (c) \(\mathrm{Cl}_{2} ;\) (d) \(\mathrm{I}_{2}\).

Write Lewis symbols for the following ions. (a) \(\mathrm{H}^{-}\) (b) \(\operatorname{Sn}^{2+} ;\) (c) \(\mathrm{K}^{+} ;\) (d) \(\mathrm{Br}^{-} ;\) (e) \(\mathrm{Se}^{2-} ;\) (f) \(\mathrm{Sc}^{3+}\).

If you have four electron pairs around a central atom, under what circumstances can you have a pyramidal molecule? Similarly, how can you have a bent molecule? What are the expected bond angles in each case?
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