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Chapter 10: Problem 13

Write Lewis structures for the following ionic compounds: (a) calcium chloride; (b) barium sulfide; (c) lithium oxide; (d) sodium fluoride.

Short Answer

Expert verified
The Lewis structures for the compounds are: Calcium Chloride - [Ca] :Cl- :Cl-, Barium Sulfide - [Ba] :S-:, Lithium Oxide - [Li] [Li] :O-:, Sodium Fluoride - [Na] :F-.

Step by step solution

01

Understand the components

Lewis structures depict individual atoms and their electrons. For an ionic compound, there should be a metal (from groups 1, 2, or 13) and a nonmetal. Metals lose electrons and become cations while nonmetals gain these electrons and become anions.
02

Lewis structure for calcium chloride (CaCl2)

Calcium (Ca) has two valence electrons which it can lose to become \(Ca^{2+}\). Chlorine (Cl) has seven valence electrons and can gain one to become \(Cl^{-}\). So, one calcium atom can pair with two chlorine atoms to form calcium chloride. In Lewis structure, calcium is represented as [Ca], showing it has lost two electrons, and each chlorine is shown as :Cl-, indicating the added electron.
03

Lewis structure for barium sulfide (BaS)

Barium (Ba) has two valence electrons, therefore it becomes \(Ba^{2+}\). Sulfur (S) has six valence electrons and can gain two, becoming \(S^{2-}\). So, one barium atom pairs with one sulfur atom to form barium sulfide. In Lewis structure, barium is: [Ba], and sulfur is: :S-:
04

Lewis structure for lithium oxide (Li2O)

Lithium (Li) has one valence electron to lose, becoming \(Li^{+}\). Oxygen (O) has six valence electrons and can gain two, becoming \(O^{2-}\). Therefore, two lithium atoms pair with one oxygen atom to form lithium oxide. In Lewis structure, each lithium is denoted as [Li] and oxygen as :O-:
05

Lewis structure for sodium fluoride (NaF)

Sodium (Na) has one valence electron to lose, therefore it turns into \(Na^{+}\). Fluorine (F) has seven valence electrons and can gain one, becoming \(F^-\). So, one sodium atom pairs with one fluorine atom to form sodium fluoride. In the Lewis structure, sodium is shown as [Na] and fluorine is :F-

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Most popular questions from this chapter

In your own words, define the following terms: (a) valence electrons; (b) electronegativity; (c) bonddissociation energy; (d) double covalent bond;(e) coordinate covalent bond.

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

Draw a plausible Lewis structure for the following series of molecules and ions: \((a) \operatorname{SiF}_{6}^{2-} ;\) (b) \(\mathrm{PF}_{5} ;\) (c) \(\mathrm{SF}_{4}\); (d) \(\mathrm{XeF}_{4}\). Describe the electron group geometry and molecular structure of these species.

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

Give several examples for which the following statement proves to be incorrect. "All atoms in a Lewis structure have an octet of electrons in their valence shells."
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