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Chapter 8: Problem 27

Without using Fig. \(8.3\), predict the order of increasing electronegativity in each of the following groups of elements. a. \(\mathrm{C}, \mathrm{N}, \mathrm{O}\) c. \(\mathrm{Si}, \mathrm{Ge}, \mathrm{Sn}\) b. \(\mathrm{S}, \mathrm{Se}, \mathrm{Cl}\) d. Tl, S, Ge

Short Answer

Expert verified
The order of increasing electronegativity for each group of elements is as follows: a. C < N < O b. S < Se < Cl c. Sn < Ge < Si d. Tl < Ge < S

Step by step solution

01

a. C, N, O

In this group, the elements are found in the same period (Period 2), and we know electronegativity increases from left to right across a period. So, the order of increasing electronegativity in this group is: C < N < O.
02

b. S, Se, Cl

In this group, the elements are found in the same period (Period 3). Following the trend of electronegativity increasing across a period from left to right, the order of increasing electronegativity is: S < Se < Cl.
03

c. Si, Ge, Sn

In this group, the elements are found in the same group, Group 14, but in different periods (Si in Period 3, Ge in Period 4, and Sn in Period 5). Electronegativity decreases as we move down a group, so the order of increasing electronegativity is: Sn < Ge < Si.
04

d. Tl, S, Ge

In this group, the elements are found in different groups and periods. To determine the order of electronegativity, we will compare their positions in the periodic table. Tl (Period 6, Group 13) is below Ge (Period 4, Group 14), so its electronegativity should be lower. S (Period 3, Group 16) is above and to the right of Ge, so it should have a higher electronegativity. Therefore, the order of increasing electronegativity is: Tl < Ge < S.

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Most popular questions from this chapter

Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers. a. \(\mathrm{NaCl}, \mathrm{KCl}\) b. \(\mathrm{LiF}, \mathrm{LiCl}\) c. \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgO}\) d. \(\mathrm{Fe}(\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}\) e. \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{O}\) f. \(\mathrm{MgO}, \mathrm{BaS}\)

Two different compounds have the formula \(\mathrm{XeF}_{2} \mathrm{Cl}_{2} .\) Write Lewis structures for these two compounds, and describe how measurement of dipole moments might be used to distinguish between them.

Write Lewis structures that obey the octet rule for each of the following molecules. a. \(\mathrm{CCl}_{4}\) c. \(\mathrm{SeCl}_{2}\) b. \(\mathrm{NCl}_{3}\) d. \(\mathrm{ICl}\) In each case, the atom listed first is the central atom.

Identify the five compounds of \(\mathrm{H}, \mathrm{N}\), and \(\mathrm{O}\) described below. For each compound, write a Lewis structure that is consistent with the information given. a. All the compounds are electrolytes, although not all of them are strong electrolytes. Compounds \(\mathrm{C}\) and \(\mathrm{D}\) are ionic and compound \(\mathrm{B}\) is covalent. b. Nitrogen occurs in its highest possible oxidation state in compounds \(\mathrm{A}\) and \(\mathrm{C}\); nitrogen occurs in its lowest possible oxidation state in compounds \(\mathrm{C}, \mathrm{D}\), and \(\mathrm{E}\). The formal charge on both nitrogens in compound \(\mathrm{C}\) is \(+1\); the formal charge on the only nitrogen in compound \(\mathrm{B}\) is \(0 .\) c. Compounds A and E exist in solution. Both solutions give off gases. Commercially available concentrated solutions of compound \(\mathrm{A}\) are normally \(16 M .\) The commercial, concentrated solution of compound \(\mathrm{E}\) is \(15 M\). d. Commercial solutions of compound \(\mathrm{E}\) are labeled with a misnomer that implies that a binary, gaseous compound of nitrogen and hydrogen has reacted with water to produce ammonium ions and hydroxide ions. Actually, this reaction occurs to only a slight extent. e. Compound \(\mathrm{D}\) is \(43.7 \% \mathrm{~N}\) and \(50.0 \% \mathrm{O}\) by mass. If compound D were a gas at STP, it would have a density of \(2.86 \mathrm{~g} / \mathrm{L}\). f. A formula unit of compound \(\mathrm{C}\) has one more oxygen than a formula unit of compound D. Compounds \(\mathrm{C}\) and \(\mathrm{A}\) have one ion in common when compound \(\mathrm{A}\) is acting as a strong electrolyte. g. Solutions of compound \(\mathrm{C}\) are weakly acidic; solutions of compound \(\mathrm{A}\) are strongly acidic; solutions of compounds \(\mathrm{B}\) and \(\mathrm{E}\) are basic. The titration of \(0.726 \mathrm{~g}\) compound \(\mathrm{B}\) requires \(21.98 \mathrm{~mL}\) of \(1.000 M \mathrm{HCl}\) for complete neutralization.

Give one example of a compound having a linear molecular structure that has an overall dipole moment (is polar) and one example that does not have an overall dipole moment (is nonpolar). Do the same for molecules that have trigonal planar and tetrahedral molecular structures.
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