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Chapter 10: Problem 28

Represent the following ionic compounds by Lewis structures: (a) barium hydroxide; (b) sodium nitrite; (c) magnesium iodate; (d) aluminum sulfate.

Short Answer

Expert verified
Lewis structures for ionic compounds represent the transfer of electrons from one atom to the other resulting in ions. In the case of the four compounds listed, the metal atoms each lose electrons to become positive cations, while the nonmetal groups each gain electrons to become negative anions. Draw the structures with the metal atoms having no electrons and the nonmetal groups surrounded by 8 electrons.

Step by step solution

01

Drawing Lewis Structure for Barium Hydroxide

To start, remember Barium has 2 valence electrons and Hydroxide has 7. In the structure, Barium must lose 2 electrons (forming a 2+ cation) and each Hydroxide must gain one electron (forming a 1- anion). Draw Barium with no electrons around it and two Hydroxides each surrounded by 8 electrons.
02

Drawing Lewis Structure for Sodium Nitrite

Sodium has 1 valence electron and Nitrite (NO2) has 5 electrons from Nitrogen and 6 from each Oxygen. In the structure, Sodium must lose 1 electron (forming a 1+ cation) and Nitrite must gain one electron (forming a 1- anion). Draw Sodium with no electrons around it and Nitrite surrounded by 8 electrons in each atom.
03

Drawing Lewis Structure for Magnesium Iodate

Magnesium has 2 valence electrons and Iodate (IO3) has 7 electrons from Iodine and 6 from each Oxygen. In the structure, Magnesium must lose 2 electrons (forming a 2+ cation) and each Iodate must gain one electron (forming a 1- anion). Draw Magnesium with no electrons around it and three Iodates each surrounded by 8 electrons.
04

Drawing Lewis Structure for Aluminum Sulfate

Aluminum has 3 valence electrons and Sulfate (SO4) has 6 electrons from Sulfur and 6 from each Oxygen. In the structure, each Aluminum must lose 3 electrons (forming a 3+ cation) and each Sulfate must gain two electrons (forming a 2- anion). Draw two Aluminums each with no electrons around them and three Sulfates each surrounded by 8 electrons.

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Most popular questions from this chapter

Write a plausible Lewis structure for \(\mathrm{C}_{3} \mathrm{O}_{2},\) a substance known as carbon suboxide.

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.

Suggest reasons why the following do not exist as stable molecules: (a) \(\mathrm{H}_{3} ;\) (b) \(\mathrm{HHe} ;\) (c) \(\mathrm{He}_{2}\); (d) \(\mathrm{H}_{3} \mathrm{O}\).

Draw plausible Lewis structures for the following species; use expanded valence shells where necessary. (a) \(\mathrm{Cl}_{2} \mathrm{O} ;\) (b) \(\mathrm{PF}_{3} ;\) (c) \(\mathrm{CO}_{3}^{2-} ;\) (d) \(\mathrm{BrF}_{5}\).

Sketch the probable geometric shape of a molecule of (a) \(\mathrm{N}_{2} \mathrm{O}_{4}\left(\mathrm{O}_{2} \mathrm{NNO}_{2}\right) ;\) (b) \(\mathrm{C}_{2} \mathrm{N}_{2}(\mathrm{NCCN}) ;\) (c) \(\mathrm{C}_{2} \mathrm{H}_{6}\) \(\left(\mathrm{H}_{3} \mathrm{CCH}_{3}\right) ;(\mathrm{d}) \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\left(\mathrm{H}_{3} \mathrm{COCH}_{3}\right)\).
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