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Chapter 9: Problem 33

List these bonds in order of increasing ionic character: the lithium-to- fluorine bond in \(\mathrm{LiF},\) the potassium-to-oxygen bond in \(\mathrm{K}_{2} \mathrm{O},\) the nitrogen-tonitrogen bond in \(\mathrm{N}_{2}\), the sulfur-to-oxygen bond in \(\mathrm{SO}_{2}\), the chlorine-to-fluorine bond in \(\mathrm{ClF}_{3}\).

Short Answer

Expert verified
The bonds, when listed in order of increasing ionic character, are as follows: N2 < SO2 = ClF3 < K2O < LiF.

Step by step solution

01

Determine the Electronegativity of Each Atom in the Bond

Using an electronegativity table, determine the electronegativity of each of the atoms involved in the bonds. - Lithium (Li): 1.0 - Fluorine (F): 4.0 - Potassium (K): 0.8 - Oxygen (O): 3.5 - Nitrogen (N): 3.0 - Sulfur (S): 2.5 - Chlorine (Cl): 3.0
02

Calculate the Difference in Electronegativity for Each Bond

Compute the absolute difference in electronegativity for each bond: - LiF: \(|4.0 - 1.0| = 3.0\) - K2O: \(|3.5 - 0.8| = 2.7\) - N2: \(|3.0 - 3.0| = 0\) - SO2: \(|3.5 - 2.5| = 1.0\) - ClF3: \(|4.0 - 3.0| = 1.0\) The larger the difference in electronegativity, the more ionic the bond is.
03

Rank the Bonds in Increasing Ionic Character

Arrange the bonds in order of increasing ionic character, from least ionic to most ionic, using the calculated electronegativity differences. - N2 (0) - SO2 = ClF3 (1.0) - K2O (2.7) - LiF (3.0) So, the order of increasing ionic character is: N2 < SO2 = ClF3 < K2O < LiF

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Most popular questions from this chapter

Give the empirical formulas and names of the compounds formed from the following pairs of ions: (a) \(\mathrm{Rb}^{+}\) and \(\mathrm{I}^{-},\) (b) \(\mathrm{Cs}^{+}\) and \(\mathrm{SO}_{4}^{2-}\) (c) \(\mathrm{Sr}^{2+}\) and \(\mathrm{N}^{3-},(\mathrm{d}) \mathrm{Al}^{3+}\) and \(\mathrm{S}^{2-}\).

The species \(\mathrm{H}_{3}^{+}\) is the simplest polyatomic ion. The geometry of the ion is that of an equilateral triangle. (a) Draw three resonance structures to represent the ion. (b) Given the following information and $$ \begin{aligned} 2 \mathrm{H}+\mathrm{H}^{+} \longrightarrow \mathrm{H}_{3}^{+} & \Delta H^{\circ}=-849 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{H}_{2} \longrightarrow 2 \mathrm{H} & \Delta H^{\circ}=436.4 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ calculate \(\Delta H^{\circ}\) for the reaction $$ \mathrm{H}^{+}+\mathrm{H}_{2} \longrightarrow \mathrm{H}_{3}^{+} $$

Draw Lewis structures for these organic molecules, in each of which there is one \(\mathrm{C}=\mathrm{C}\) bond and the rest of the carbon atoms are joined by \(\mathrm{C}-\mathrm{C}\) bonds: \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{~F}, \mathrm{C}_{3} \mathrm{H}_{6}, \mathrm{C}_{4} \mathrm{H}_{8}\).

Comment on the correctness of this statement: All compounds containing a noble gas atom violate the octet rule.

For each of the following pairs of elements, state whether the binary compound they form is likely to be ionic or covalent. Write the empirical formula and name of the compound: (a) \(\mathrm{B}\) and \(\mathrm{F}\), (b) \(\mathrm{K}\) and \(\mathrm{Br}\).
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