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Chapter 9: Problem 79

Draw four reasonable resonance structures for the \(\mathrm{PO}_{3} \mathrm{~F}^{2-}\) ion. The central \(\mathrm{P}\) atom is bonded to the three \(\mathrm{O}\) atoms and to the \(\mathrm{F}\) atom. Show formal charges.

Short Answer

Expert verified
Four possible resonance structures for the PO3F2- ion have been drawn considering P as the central atom bonded to three O atoms and one F atom, taking formal charges into account.

Step by step solution

01

Draw Central Atom and Surrounding Atoms

Firstly, a structure needs to be drawn with P atom as the central atom and three O atoms and one F atom surrounding it. Single bonds are drawn between the P and each of the other atoms initially.
02

Calculate and Assign Formal Charges

Formal charges are calculated by the formula: Formal charge = [# of valence electrons] - [(# of lone pair electrons) + 1/2(# bonding electrons)]. Assign these to all the atoms of the structure.
03

Draw First Resonance Structure

Form the first resonance structure by moving a pair of electrons from an oxygen atom next to the central phosphorus atom to create a double bond. Update the formal charges accordingly.
04

Draw Second Resonance Structure

Form the second resonance structure by moving a pair of electrons from the remaining single-bonded oxygen atom near the phosphorus atom to form a double bond. Update the formal charges again.
05

Draw Third and Fourth Resonance Structures

Draw the third and fourth resonance structures by considering movement of the lone pairs of electrons from the oxygen atoms of the double bonds to the phosphorous atom, and then the formation of a double bond between phosphorous and the fluorine atom. Each time, remember to update the formal charges.

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Most popular questions from this chapter

Explain the concept of formal charge. Do formal charges on a molecule represent actual separation of charges?

Explain why ions with charges greater than 3 are seldom found in ionic compounds.

Write the Lewis dot symbols of the reactants and products in the following reactions. (First balance the equations.) (a) \(\mathrm{Sr}+\mathrm{Se} \longrightarrow \mathrm{SrSe}\) (b) \(\mathrm{Ca}+\mathrm{H}_{2} \longrightarrow \mathrm{CaH}_{2}\) (c) \(\mathrm{Li}+\mathrm{N}_{2} \longrightarrow \mathrm{Li}_{3} \mathrm{~N}\) (d) \(\mathrm{Al}+\mathrm{S} \longrightarrow \mathrm{Al}_{2} \mathrm{~S}_{3}\)

Write Lewis structures for these ions: (a) \(\mathrm{O}_{2}^{2-}\), (b) \(\mathrm{C}_{2}^{2-},\) (c) \(\mathrm{NO}^{+}\), (d) \(\mathrm{NH}_{4}^{+}\). Show formal charges.

Draw three resonance structures for the chlorate ion, \(\mathrm{ClO}_{3}^{-}\). Show formal charges.
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