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Chapter 9: Problem 4

Write Lewis dot symbols for the following ions: (a) \(\mathrm{Li}^{+},(\mathrm{b}) \mathrm{Cl}^{-},(\mathrm{c}) \mathrm{S}^{2-},(\mathrm{d}) \mathrm{Sr}^{2+},(\mathrm{e}) \mathrm{N}^{3-}\)

Short Answer

Expert verified
The Lewis dot symbols are given as follows: (a) \(Li^{+} : Li\), (b) \(Cl^{-} : Cl \) surrounded by 8 dots, (c) \(S^{2-} : S\) surrounded by 8 dots, (d) \(Sr^{2+} : Sr\), (e) \(N^{3-} : N\) surrounded by 8 dots.

Step by step solution

01

Lewis dot symbol for \(Li^{+}\)

The symbol for Lithium (Li) is usually accompanied by one dot representing its single valence electron. However, in the case of a \(Li^{+}\) ion, the electron has been lost, leaving it without any valence electron. Thus, the Lewis Dot symbol for \(Li^{+}\) is just `Li`.
02

Lewis dot symbol for \(Cl^{-}\)

The symbol for Chlorine (Cl) is usually accompanied by seven dots representing its seven valence electrons. However, in the case of a \(Cl^{-}\) ion, it has gained an additional electron, which makes it a complete octet. Thus, the Lewis Dot symbol for \(Cl^{-}\) is `Cl` surrounded by eight dots.
03

Lewis dot symbol for \(S^{2-}\)

The symbol for Sulfur (S) is usually accompanied by six dots representing its six valence electrons. However, in the case of a \(S^{2-}\) ion, it has gained two additional electrons, making it a complete octet. Thus, the Lewis Dot symbol for \(S^{2-}\) is `S` surrounded by eight dots.
04

Lewis dot symbol for \(Sr^{2+}\)

The symbol for Strontium (Sr) is usually without dots, as it belongs to the alkali earth metals and its valence electrons are lost when it forms an ion. Thus, the Lewis Dot symbol for \(Sr^{2+}\) is just `Sr`.
05

Lewis dot symbol for \(N^{3-}\)

The symbol for Nitrogen (N) is usually accompanied by five dots representing its five valence electrons. However, in the case of a \(N^{3-}\) ion, it has gained three additional electrons, making it a complete octet. Thus, the Lewis Dot symbol for \(N^{3-}\) is `N` surrounded by eight dots.

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Most popular questions from this chapter

Write Lewis structures for the following species, including all resonance forms, and show formal charges: (a) \(\mathrm{HCO}_{2}^{-},\) (b) \(\mathrm{CH}_{2} \mathrm{NO}_{2}^{-}\). Relative positions of the atoms are as follows:

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