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Chapter 10: Problem 55

Which of the following species would you expect to be diamagnetic and which paramagnetic: (a) \(\mathrm{OH}^{-} ;\) (b) \(\mathrm{OH} ;(\mathrm{c}) \mathrm{NO}_{3} ;(\mathrm{d}) \mathrm{SO}_{3} ;(\mathrm{e}) \mathrm{SO}_{3}^{2-} ;(\mathrm{f}) \mathrm{HO}_{2} ?\)

Short Answer

Expert verified
(a) \(\mathrm{OH}^{-}\) is paramagnetic, (b) \(\mathrm{OH}\) is diamagnetic, (c) \(\mathrm{NO}_{3}\) is diamagnetic, (d) \(\mathrm{SO}_{3}\) is diamagnetic, (e) \(\mathrm{SO}_{3}^{2-}\) is paramagnetic, (f) \(\mathrm{HO}_{2}\) is paramagnetic.

Step by step solution

01

Determine the electron configuration of each species

Use the periodic table to determine the electron configuration of each atom in the given species. Then combine these configurations to find the overall electron configuration of the entire species. Remember to add or subtract an electron if the species is an anion (negative charge) or a cation (positive charge).
02

Check if there are any unpaired electrons

Examine the electron configuration of each species. If all the electrons are paired, then the species is diamagnetic. If there is at least one unpaired electron, then the species is paramagnetic.
03

Assign each species as diamagnetic or paramagnetic

Based on step 2, assign each species as diamagnetic or paramagnetic.

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Most popular questions from this chapter

One of the following ions has a trigonal-planar shape: $\mathrm{SO}_{3}^{2-} ; \mathrm{PO}_{4}^{3-} ; \mathrm{PF}_{6}^{-} ; \mathrm{CO}_{3}^{2-} .$ Which ion is it? Explain.

In your own words, define the following terms: (a) valence electrons; (b) electronegativity; (c) bonddissociation energy; (d) double covalent bond;(e) coordinate covalent bond.

Hydrogen azide, \(\mathrm{HN}_{3}\), is a liquid that explodes violently when subjected to physical shock. In the \(\mathrm{HN}_{3}\) molecule, one nitrogen- to-nitrogen bond length is \(113 \mathrm{pm},\) and the other is \(124 \mathrm{pm} .\) The \(\mathrm{H}-\mathrm{N}-\mathrm{N}\) bond angle is \(112^{\circ} .\) Draw Lewis structures and a sketch of the molecule consistent with these facts.

Write Lewis structures for the following ionic compounds: (a) calcium chloride; (b) barium sulfide; (c) lithium oxide; (d) sodium fluoride.

A pair of isoelectronic species for \(C\) and \(N\) exist with the formula \(\mathrm{X}_{2} \mathrm{O}_{4}\) in which there is an \(\mathrm{X}-\mathrm{X}\) bond. \(\mathrm{A}\) corresponding fluoride of boron also exists. Draw Lewis structures for these species and describe their shapes.
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