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Chapter 10: Problem 15

Derive the correct formulas for the following ionic compounds by writing Lewis structures. (a) lithium sulfide; (b) sodium fluoride; (c) calcium iodide; (d) scandium chloride.

Short Answer

Expert verified
The correct formula for (a) lithium sulfide is \( Li_2S \), (b) sodium fluoride is \( NaF \), (c) calcium iodide is \( CaI_2 \), and (d) scandium chloride is \( ScCl_3 \).

Step by step solution

01

Define the Lewis structure and Valence Electrons

For any compound, a Lewis structure can be created to illustrate how atoms are bonded and any lone pairs of electrons. To begin with, determine the number of valence electrons for each of the atoms. Lithium (Li) has 1 valence electron, Sulfur (S) has 6, Sodium (Na) has 1, Fluorine (F) has 7, Calcium (Ca) has 2, Iodine (I) has 7, Scandium (Sc) has 3 and Chlorine (Cl) has 7.
02

Lithium Sulfide - Li2S

Since Sulfur needs two more electrons to complete its octet, and Lithium has only one electron to give (it loses this electron to achieve stability), two Lithium atoms will be required to bond with one Sulfur atom to form lithium sulfide, creating a formula of \( Li_2S \). The Lewis structure would represent this.
03

Sodium Fluoride - NaF

Fluorine needs one more electron to complete its octet, and Sodium has that one electron to give, so one atom of each will bond together to form sodium fluoride, creating a formula of \( NaF \). The Lewis structure would represent this.
04

Calcium Iodide - CaI2

Iodine needs one more electron to complete its octet, but Calcium has two electrons to give (it loses its electrons to achieve stability), two Iodine atoms will be required to bond with one Calcium atom to make calcium iodide, with a formula of \( CaI_2 \). The Lewis structure would represent this.
05

Scandium Chloride - ScCl3

Chlorine needs one more electron to complete its octet, and since Scandium has three electrons to give (it loses its electrons to achieve stability), three Chlorine atoms will be necessary to bond with one Scandium atom to make scandium chloride, with a formula of \( ScCl_3 \). The Lewis structure would represent this.

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Most popular questions from this chapter

Predict the shapes of the following sulfur-containing species. (a) \(\mathrm{SO}_{2} ;\) (b) \(\mathrm{SO}_{3}^{2-} ;\) (c) \(\mathrm{SO}_{4}^{2-}\).

The molecular shape of \(\mathrm{BF}_{3}\) is planar (see Table 10.1 ). If a fluoride ion is attached to the \(B\) atom of \(B F_{3}\) through a coordinate covalent bond, the ion \(\mathrm{BF}_{4}^{-}\) results. What is the shape of this ion?

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.

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) \(\mathrm{N}_{2}\); (b) HCN; (c) \(\mathrm{NH}_{4}^{+} ;\) (d) \(\mathrm{NO}_{3}^{-} ;\) (e) NSF.

Write plausible Lewis structures for the following odd-electron species: (a) \(\mathrm{CH}_{3} ;\) (b) \(\mathrm{ClO}_{2} ;\) (c) \(\mathrm{NO}_{3}\).
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