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Chapter 10: Problem 54

Write plausible Lewis structures for the following free radicals: (a) \(\cdot \mathrm{C}_{2} \mathrm{H}_{5} ;\) (b) \(\mathrm{HO}_{2}\) "; (c) ClO?.

Short Answer

Expert verified
The Lewis structures are as follows: (a) For \(\cdot C_{2}H_{5}\) : \(C - C - H\) with single bonds between the atoms and an unpaired electron on the Carbon atom. There are three hydrogens bonded to one Carbon atom and two hydrogens bonded to the other. (b) For \(HO_{2}\) : \(O - O - H\) with single bonds between the atoms and an unpaired electron on the Oxygen atom. (c) For \(ClO\) : \(Cl - O\) with a single bond between the atoms and an unpaired electron on the Cl atom.

Step by step solution

01

Identification of central atom

Identify the central atom for each of the molecules. The central atom is usually the one that has the most bonding capacity which is \(\mathrm{C}\) for \(\cdot\mathrm{C}_{2}\mathrm{H}_{5}\), \(\mathrm{O}\) for \(\mathrm{HO}_{2}\), and \(\mathrm{Cl}\) for \(\mathrm{ClO}\).
02

Determination of total valence electrons

Determine the total number of valence electrons for each molecule. \(C_{2}H_{5}\) has 14 valence electron, \(HO_{2}\) has 13 valence electrons, and \(ClO\) has 13 valence electron.
03

Draw skeletal structure and placing electrons

Draw the skeleton of the molecule and place the electrons. Here, hydrogen atoms are always terminal. Also remember that each bond uses 2 electrons.
04

Place remaining electrons

After placing bonding electrons, place the remaining electrons as lone pairs on each atom, starting with the outer atoms first. Remember atoms follow the octet rule (except Hydrogen follows a duet), which means they should have 8 electrons in their outer shell. Atomic hydrogen has one electron in its 1s orbital, it will always share its one electron to achieve stable configuration of Helium.
05

Placement of unpaired electron

Place the unpaired electron on the central atom to form the free radical. In these structures, an unpaired electron must be present because radicals have an odd number of valence electrons.

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Most popular questions from this chapter

Without referring to tables in the text, indicate which of the following bonds you would expect to have the greatest bond length, and give your reasons. (a) \(\mathrm{O}_{2}\); (b) \(\mathrm{N}_{2} ;\) (c) \(\mathrm{Br}_{2} ;\) (d) \(\mathrm{BrCl}\).

One of the allotropes of sulfur is a ring of eight sulfur atoms. Draw the Lewis structure for the \(S_{8}\) ring. Is the ring likely to be planar? The \(S_{8}\) ring can be oxidized to produce \(S_{8}\) O. In \(S_{8} O,\) the oxygen atom is bonded to one of the S atoms and the Sg ring is still intact. Draw the Lewis structure for \(\mathrm{S}_{8} \mathrm{O}\).

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

Each of the following molecules contains one or more multiple covalent bonds. Draw plausible Lewis structures to represent this fact, and predict the shape of each molecule. (a) \(\mathrm{CO}_{2} ;\) (b) \(\mathrm{Cl}_{2} \mathrm{CO} ;\) (c) CINO \(_{2}\).

Write acceptable Lewis structures for the following molecules: (a) \(\mathrm{H}_{2} \mathrm{NNH}_{2}\); (b) HOClO; (c) (HO) \(_{2}\) SO; (d) HOOH (e) SO \(_{4}^{2-}\).
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