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Chapter 8: Problem 162

A polyatomic ion is composed of \(\mathrm{C}, \mathrm{N}\), and an unknown element \(X\). The skeletal Lewis structure of this polyatomic ion is \([\mathrm{X}-\mathrm{C}-\mathrm{N}]^{-} .\) The ion \(\mathrm{X}^{2-}\) has an electron configuration of \([\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{6} .\) What is element \(\mathrm{X} ?\) Knowing the identity of X, complete the Lewis structure of the polyatomic ion, including all important resonance structures.

Short Answer

Expert verified
Element X is Sulfur (S), and the polyatomic ion [X-C-N]鈦� is [S-C-N]鈦�. The completed Lewis structures are: 1. Resonance Structure 1: S(2 lone pairs) = C(1 lone pair) - N(2 lone pairs) 2. Resonance Structure 2: S(1 lone pair) - C(1 lone pair) = N(3 lone pairs) Both resonance structures follow the octet rule and utilize a total of 16 valence electrons.

Step by step solution

01

Identify Element X

First we need to find element X. We are given the electron configuration of X虏鈦� ion, which is [Ar]4s虏3d鹿鈦�4p鈦�. Since X has lost 2 electrons to give X虏鈦�, we need to add back the electrons. We now have the electron configuration: [Ar]4s虏3d鹿鈦�4p鈦� The electron configuration [Ar]4s虏3d鹿鈦�4p鈦� corresponds to the element Sulfur (S), which is in the 3rd Period and 16th Group of the periodic table.
02

Completing the Lewis Structure of the Polyatomic Ion

Now let's complete the Lewis structure of the polyatomic ion [S-C-N]鈦�. For this, we first count all the valence electrons in the ion: - Sulfur (S): 6 valence electrons (Group 16) - Carbon (C): 4 valence electrons (Group 14) - Nitrogen (N): 5 valence electrons (Group 15) - Additional electron due to negative charge: 1 electron The total number of valence electrons is 6 + 4 + 5 + 1 = 16 electrons. Now we draw the skeletal structure of the ion as [S-C-N]鈦�. We will complete the octet rule for each atom, starting with the central atom Sulfur. Sulfur: - Bonded to C = 1 bond, so we need to add three lone pairs (6 electrons) to complete the octet. Carbon: - Bonded to S and N = 2 bonds, so we need to add two lone pairs (4 electrons) to complete the octet. Nitrogen: - Bonded to C = 1 bond, so we need to add three lone pairs (6 electrons) to complete the octet. However, the total number of electrons used based on this structure would be 18 electrons (6 + 4 + 6 + 2 (due to the bonding)).
03

Drawing Resonance Structures

We will now adjust the bonds and lone pairs to draw resonance structures using only 16 electrons. - In the first resonance structure, we will move the lone pair of electrons from Nitrogen to form a double bond with Carbon, and Carbon will now have only one lone pair (2 electrons). - In the second resonance structure, we will move the lone pair of electrons from Sulfur to form a double bond with Carbon, and Carbon will now have only one lone pair (2 electrons). Now we have the following resonance structures: Resonance 1: S(2 lone pairs) = C(1 lone pair) - N(2 lone pairs) Resonance 2: S(1 lone pair) - C(1 lone pair) = N(3 lone pairs) Both resonance structures have 16 electrons in total, and each atom has a complete octet. In conclusion, element X is Sulfur, and the polyatomic ion [X-C-N]鈦� is [S-C-N]鈦�, with the two possible resonance structures as mentioned above.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electron Configuration
In understanding the atomic and molecular structures, recognizing the term electron configuration is pivotal. It details how electrons are distributed in an atom's orbitals, following a common notation representing energy levels, sublevels, and number of electrons. For instance, the electron configuration of the X2- ion is given as [Ar] 4s23d104p6.

Generally, electron configurations enable us to determine the number of valence electrons, which are crucial in bonding and chemical reactivity. For ions, electron configurations require adjustments to reflect gained or lost electrons during ion formation, allowing us to backtrack and identify the neutral atom - in this case, leading us to sulfur, with the neutral atom configuration [Ar]4s23d104p4.
Resonance Structures
When dealing with molecules and polyatomic ions, one must consider resonance structures. These are alternative Lewis structures for the same molecule that differ only in the positions of the electrons. Resonance structures illustrate that sometimes, a single Lewis structure does not fully capture the electron distribution within a molecule.

The creation of resonance structures is governed by specific rules, ensuring that electron pairs are only moved between atoms with proper bonding potential and electron capacity. In interactions where multiple resonance structures exist, such as in our [S-C-N]鈦� ion, the true electron distribution is a hybrid of these structures. This concept helps explain certain properties, like bond lengths and strengths, that cannot be explained by a single structure.
Octet Rule
Central to the formation of stable chemical compounds is the octet rule, which states that atoms tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electron configuration as a noble gas. In cased like our polyatomic ion, each atom strives to complete its octet, either by sharing electrons through covalent bonds or by having lone pairs of electrons.

However, exceptions to the octet rule exist, particularly with elements capable of having more or fewer than eight valence electrons. For example, sulfur can expand its octet, accommodating more than eight electrons, while elements like hydrogen are stable with just two.
Valence Electrons
Lastly, valence electrons are the electrons located in the outermost shell of an atom and are responsible for chemical bonding. By identifying valence electrons, one can predict the bonding patterns of an element, as seen in our [S-C-N]鈦� ion example.

Calculating the total number of valence electrons in a molecule or ion is the first step in crafting its Lewis structure. Elements from similar groups on the periodic table have the same number of valence electrons, which facilitates the prediction of their chemical behavior. In polyatomic ions, it's essential to adjust the valence electron count for the overall charge of the ion.

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Most popular questions from this chapter

Oxidation of the cyanide ion produces the stable cyanate ion, \(\mathrm{OCN}^{-}\). The fulminate ion, \(\mathrm{CNO}^{-}\), on the other hand, is very unstable. Fulminate salts explode when struck; \(\mathrm{Hg}(\mathrm{CNO})_{2}\) is used in blasting caps. Write the Lewis structures and assign formal charges for the cyanate and fulminate ions. Why is the fulminate ion so unstable? (C is the central atom in \(\mathrm{OCN}^{-}\) and \(\mathrm{N}\) is the central atom in \(\mathrm{CNO}^{-} .\) )

Which of the following ions have noble gas electron configurations? a. \(\mathrm{Fe}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Sc}^{3+}, \mathrm{Co}^{3+}\) b. \(\mathrm{Tl}^{+}, \mathrm{Te}^{2-}, \mathrm{Cr}^{3+}\) c. \(\mathrm{Pu}^{4+}, \mathrm{Ce}^{4+}, \mathrm{Ti}^{4+}\) d. \(\mathrm{Ba}^{2+}, \mathrm{Pt}^{2+}, \mathrm{Mn}^{2+}\)

Think of forming an ionic compound as three steps (this is a simplification, as with all models): (1) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three processes? d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is \(\mathrm{NaCl}\) stable but not \(\mathrm{Na}_{2} \mathrm{Cl} ? \mathrm{NaCl}_{2} ?\) What about \(\mathrm{MgO}\) compared to \(\mathrm{MgO}_{2}\) ? \(\mathrm{Mg}_{2} \mathrm{O} ?\)

Some plant fertilizer compounds are \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}, \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\), \(\mathrm{K}_{2} \mathrm{O}, \mathrm{P}_{2} \mathrm{O}_{5}\), and \(\mathrm{KCl}\). Which of these compounds contain both ionic and covalent bonds?

Borazine \(\left(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6}\right)\) has often been called "inorganic" benzene. Write Lewis structures for borazine. Borazine contains a sixmembered ring of alternating boron and nitrogen atoms with one hydrogen bonded to each boron and nitrogen.
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