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Chapter 8: Problem 14

What is the Lewis symbol for each of the following atoms or ions? (a) \(\mathrm{K},\) (b) As, (c) \(\mathrm{Sn}^{2+},(\mathbf{d}) \mathrm{N}^{3-}\) .

Short Answer

Expert verified
The Lewis symbols for the given atoms and ions are: (a) \(\text{K}\bullet\) , (b) \[\begin{array}{c}\cdot \text{As} \cdot \\ | \end{array}\], (c) \(\bullet \text{Sn}^{2+} \bullet\), and (d) \[\begin{array}{c}\cdot \text{N}^{3-} \cdot \\ | \end{array}\].

Step by step solution

01

Determine valence electrons for each atom/ion

(a) Potassium (K) - As it belongs to the first group in the periodic table, it has only 1 valence electron. (b) Arsenic (As) - Being a member of Group 15 in the periodic table, it has 5 valence electrons. (c) Tin(II) ion (Sn²⁺) - Tin, as a Group 14 element, has 4 valence electrons. However, due to the 2+ charge, which means it loses 2 electrons, that leaves it with 2 valence electrons. (d) Nitride ion (N³⁻) - Nitrogen, as a Group 15 element, has 5 valence electrons. Since the ion has a 3- charge, it gains 3 electrons, thus giving it a total of 8 valence electrons.
02

Represent elements and ions with their symbols and valence electrons

(a) Potassium (K) - \[\text{K}\bullet\] (b) Arsenic (As) - \[\begin{array}{c}\cdot \text{As} \cdot \\ | \end{array}\] (c) Tin(II) ion (Sn²⁺) - \[\bullet \text{Sn}^{2+} \bullet\] (d) Nitride ion (N³⁻) - \[\begin{array}{c}\cdot \text{N}^{3-} \cdot \\ | \end{array}\] The Lewis symbols for the given atoms and ions are: (a) K• , (b) ∙As∙| , (c) •Sn²⁺• , and (d) ∙N³⁻∙| .

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Most popular questions from this chapter

Ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl},\) is a very soluble salt in water. (a) Draw the Lewis structures of the ammonium and chloride ions. (b) Is there an \(\mathrm{N}-\) Cl bond in solid ammonium chloride? (c) If you dissolve 14 gof ammonium chloride in 500.0 \(\mathrm{mL}\) of water, what is the molar concentration of the solution? (d) How many grams of silver nitrate do you need to add to the solution in part (c) to precipitate all of the chloride as silver chloride?

By referring only to the periodic table, select (a) the most electronegative element in group \(6 \mathrm{A} ;(\mathbf{b})\) the least electronegative element in the group Al, Si, P; (c) the most electronegative element in the group \(\mathrm{Ga}, \mathrm{P}, \mathrm{Cl}, \mathrm{Na} ;(\mathbf{d})\) the element in the group \(\mathrm{K}\) \(\mathrm{C}, \mathrm{Zn}, \mathrm{F}\) that is most likely to form an ionic compound with Ba.

Fill in the blank with the appropriate numbers for both electrons and bonds (considering that single bonds are counted as one, double bonds as two, and triple bonds as three). (a) Fluorine has _____ valence electrons and makes______ bond(s) in compounds. (b) Oxygen has _____ valence electrons and makes ______ bond(s) in compounds. (c) Nitrogen has _____ valence electrons and makes ______ bond(s) in compounds. (d) Carbon has _____ valence electrons and makes ______ bond(s) in compounds.

Which of these elements are unlikely to form covalent bonds? S, H, K, Ar, Si.

Based on Lewis structures, predict the ordering, from shortest to longest, of \(N-O\) bond lengths in \(N O^{+}, N O_{2}^{-},\) and \(N O_{3}^{-} .\)
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