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Chapter 10: Problem 25

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 \(_{4}^{2-}\).

Short Answer

Expert verified
The Lewis structure will involve proper distribution of total electrons in the molecule amongst the atoms, according to their valence electrons and requirements of octet rule.

Step by step solution

01

Lewis structure for \( \mathrm{H}_{2} \mathrm{NNH}_{2} \)

The molecule has three Nitrogen atoms, each with 5 valence electrons and two Hydrogen atoms each with 1 valence electron. This totals 16 electrons. Start with a trial structure by connecting atoms with single bonds. This uses 8 electrons, leaving 8 electrons. These 8 electrons are distributed evenly on the Nitrogen atoms.
02

Lewis structure for HOClO

This molecule is composed of Hydrogen with 1 valence electron, Chlorine with 7 valence electrons, and two Oxygen atoms with 6 valence electrons each. This totals 20 electrons. Start with a trial structure with Hydrogen attached to Oxygen, and another Oxygen attached to Chlorine. This uses 8 electrons, leaving 12 electrons. These 12 electrons are distributed between the Oxygens and the Chlorine.
03

Lewis structure for \( (HO) \(_{2}\) SO \)

This molecule is made up of Sulfur with 6 valence electrons, Oxygen with 6 valence electrons and two Hydrogen atoms with 1 valence electron each. This totals 14 electrons. The trial structure should first form single bonds. This uses 8 electrons, leaving 6 electrons that should be equally distributed on the Oxygen atoms.
04

Lewis structure for HOOH

This molecule has two Hydrogen atoms each with 1 valence electron and two Oxygen atoms each with 6 valence electrons, totaling 14 electrons. The Hydrogen atoms will be attached to the Oxygen atoms through single bonds, using up 4 electrons, and the remaining 10 electrons are to be distributed equally amongst the Oxygen atoms.
05

Lewis structure for \( SO \(_{4}^{2-}\) \)

This molecule constitutes Sulfur with 6 valence electrons, 4 Oxygen atoms with 6 valence electrons each and 2 extra electrons from the charge of the molecule. This gives 32 electrons. The trial structure comes from connecting all Oxygen atoms to Sulfur through single bonds using up 8 electrons, leaving 24 electrons. Remaining 24 electrons should be equally distributed over the oxygen atoms.

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Most popular questions from this chapter

A few years ago the synthesis of a salt containing the \(\mathrm{N}_{5}^{+}\) ion was reported. What is the likely shape of this ion-linear, bent, zigzag, tetrahedral, seesaw, or square-planar? Explain your choice.

Of the following species, the one with a triple covalent bond is (a) \(\mathrm{NO}_{3}^{-} ;\) (b) \(\mathrm{CN}^{-} ;\) (c) \(\mathrm{CO}_{2} ;\) (d) \(\mathrm{AlCl}_{3}\).

Which of the following molecules would you expect to be polar: (a) \(\mathrm{HCN} ;\) (b) \(\mathrm{SO}_{3} ;\) (c) \(\mathrm{CS}_{2} ;\) (d) OCS; (e) \(\operatorname{SOCl}_{2} ;\) (f) \(\operatorname{SiF}_{4} ;\) (g) \(\operatorname{POF}_{3}\) ? Give reasons for your conclusions.

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable: (a) \(\mathrm{HCO}_{2}=\) (b) \(\mathrm{HCO}_{3}^{-}\) (c) \(\mathrm{FSO}_{3}^{-}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}^{2-}\) (the nitrogen atoms are joined centrally with one oxygen atom on one \(\mathrm{N}\) and two on the other)

By means of Lewis structures, represent bonding between the following pairs of elements: (a) Cs and \(\mathrm{Br} ;\) (b) \(\mathrm{H}\) and \(\mathrm{Sb} ;\) (c) \(\mathrm{B}\) and \(\mathrm{Cl} ;\) (d) \(\mathrm{Cs}\) and \(\mathrm{Cl}\); (e) Li and O; (f) Cl and L. Your structures should show whether the bonding is essentially ionic or covalent.
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