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Chapter 10: Problem 135

The formal charges on the \(\mathrm{O}\) atoms in the ion \([\mathrm{ONO}]^{+}\) is \((\mathrm{a})-2 ;(\mathrm{b})-1 ;(\mathrm{c}) 0 ;(\mathrm{d})+1\).

Short Answer

Expert verified
The formal charge on each Oxygen atom in the [ONO]+ ion is 0.

Step by step solution

01

Determine the number of Valence Electrons

Start by determining the number of valence electrons for the Oxygen atom. Oxygen, being in Group 6 or 16 of the periodic table, has 6 valence electrons.
02

Build Lewis Structure

Try to build Lewis Structure for the [ONO]+ ion. \(\mathrm{O}\) atom at each end is connected to \(\mathrm{N}\) atom in the middle by a double bond, leaving 2 lone pairs on each Oxygen. The Nitrogen atom is bonded once to a single free electron which results in the ion's positive charge. Therefore, the structure for [ONO]+ ion is:: O=NO+
03

Calculate the Formal Charge

The formula for calculating formal charge is: Formal charge = Valence electrons - (Number of lone pair electrons + 1/2 * number of bonding electrons). For the Oxygen atoms in [ONO]+, both with a lone pair and double bonds respectively, this amounts to: Formal charge of O = 6 valence electrons - (4 lone pair electrons + 1/2 * 4 bonding electrons) = 6 - (4 + 2) = 0. Therefore the formal charge on the Oxygen atoms is (c) 0.

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Most popular questions from this chapter

One reaction involved in the sequence of reactions leading to the destruction of ozone is $$\mathrm{NO}_{2}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \longrightarrow \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})$$ Calculate \(\Delta H^{\circ}\) for this reaction by using the thermodynamic data in Appendix D. Use your \(\Delta H^{\circ}\) value, plus data from Table \(10.3,\) to estimate the nitrogenoxygen bond energy in \(\mathrm{NO}_{2}\). [Hint: The structure of nitrogen dioxide, \(\mathrm{NO}_{2}\), is best represented as a resonance hybrid of two equivalent Lewis structures.]

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 \(\mathrm{F}_{3} \mathrm{NS}\)

One possibility for the electron-group geometry for seven electron groups is pentagonal-bipyramidal, as found in the IF \(_{7}\) molecule. Write the VSEPR notation for this molecule. Sketch the structure of the molecule, labeling all the bond angles.

Although the notion that a Lewis structure in which formal charges are zero or held to a minimum seems to apply in most instances, describe several significant situations in which this appears not to be the case.

Carbon suboxide has the formula \(\mathrm{C}_{3} \mathrm{O}_{2} .\) The carbon- to-carbon bond lengths are \(130 \mathrm{pm}\) and carbon-to-oxygen, \(120 \mathrm{pm} .\) Propose a plausible Lewis structure to account for these bond lengths, and predict the shape of the molecule.
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