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Chapter 10: Problem 16

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures. (a) \(\mathrm{Al}(\mathrm{OH})_{3}\); (c) \(\mathrm{NH}_{4} \mathrm{F}\); (d) \(\mathrm{KClO}_{3}\); (b) \(\mathrm{Ca}(\mathrm{CN})_{2}\); (e) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\).

Short Answer

Expert verified
Each of the ionic compounds has been represented using Lewis structures representing the ionic bonds and lone pairs of electrons as needed.

Step by step solution

01

Draw the Lewis structure for \(\mathrm{Al}(\mathrm{OH})_{3}\)

On the left will be the Aluminium (Al) atom having 3 electrons in its valence shell. On the right side, we will have Hydroxide (OH)- ions. Magnesium Al has a +3 charge which it achieves by losing its three electrons. Hydroxide ion (OH)- has a -1 charge which it achieves by gaining one electron. However, to balance the +3 charge of Al, we need three OH- ions. Hence, the Lewis structure will include Al in the center bonded to three OH- ions each of which consist of one Oxygen atom double-bonded to a hydrogen atom and having two extra electron pairs.
02

Draw the Lewis structure for \(\mathrm{NH}_4\mathrm{F}\)

The Ammonium ion (NH4)+ has a +1 charge which it achieves by losing one electron. It consists of a Nitrogen atom in the center with single bonds to four Hydrogen atoms. Fluorine (F) has a -1 charge which it accomplishes by gaining an electron. Hence, the lewis structure will include one NH4+ ion bonded to a F- ion.
03

Draw the Lewis structure for \(\mathrm{KClO}_3\)

The potassium ion (K)+ has a +1 charge which it achieves by losing one electron. Chlorate (ClO3)- has a -1 charge which it accomplishes by gaining an electron. It consists of a Chlorine atom in the center single-bonded to three Oxygen atoms. Hence, the lewis structure will include one K+ ion bonded to one ClO3- ion.
04

Draw the Lewis structure for \(\mathrm{Ca}(\mathrm{CN})_{2}\)

The Calcium ion (Ca)2+ has a +2 charge which it achieves by losing two electrons. Cyanide (CN)-1 has a -1 charge which it accomplishes by gaining an electron. It consists of a Carbon atom triple-bonded to a Nitrogen atom with an extra electron pair on the nitrogen atom. To balance the +2 charge of Ca, we need two CN- ions. Hence, the Lewis structure will include one Ca2+ ion bonded to two CN- ions.
05

Draw the Lewis structure for \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

The Barium ion (Ba)2+ has a +2 charge which it achieves by losing two electrons. Phosphate (PO4)3- has a -3 charge which it accomplishes by gaining three electrons. It consists of one Phosphorus atom in the center, double-bonded to an Oxygen atom and single-bonded to three Oxygen atoms each of which has an additional electron pair. To balance the -6 total charge of two PO4 3- ions, we need three Ba2+ ions. Hence, the Lewis structure will include three Ba2+ ions bonded to two PO4 3- ions.

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Most popular questions from this chapter

Which of the following molecules would you expect to have a resultant dipole moment \((\mu) ;\) (a) \(\mathrm{F}_{2}\), (b) \(\mathrm{NO}_{2}\) (c) \(\mathrm{BF}_{3},\) (d) \(\mathrm{HBr},\) (e) \(\mathrm{H}_{2} \mathrm{CCl}_{2}\), (f) \(\mathrm{SiF}_{4},\) (g) OCS? Explain.

Write a plausible Lewis structure for \(\mathrm{NO}_{2}\), and indicate whether the molecule is diamagnetic or paramagnetic. Two \(\mathrm{NO}_{2}\) molecules can join together (dimerize) to form \(\mathrm{N}_{2} \mathrm{O}_{4}\). Write a plausible Lewis structure for \(\mathrm{N}_{2} \mathrm{O}_{4},\) and comment on the magnetic properties of the molecule.

The highest bond-dissociation energy is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2} ;\) (c) \(\mathrm{Cl}_{2} ;\) (d) \(\mathrm{I}_{2}\).

What is the VSEPR theory? On what physical basis is the VSEPR theory founded?

Describe the carbon-to-sulfur bond in \(\mathrm{H}_{2} \mathrm{CSF}_{4}\). That is, is it most likely a single, double, or triple bond?
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