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Chapter 7: Problem 59

Predict whether each of the following oxides is ionic or molecular: $\mathrm{ZnO}, \mathrm{K}_{2} \mathrm{O}, \mathrm{SO}_{2}, \mathrm{OF}_{2}, \mathrm{TiO}_{2}$

Short Answer

Expert verified
The given oxides can be classified as follows: \(ZnO\): Ionic \(K_2O\): Ionic \(SO_2\): Molecular \(OF_2\): Molecular \(TiO_2\): Ionic

Step by step solution

01

Identify the component elements and their electronegativities

Check the periodic table for the electronegativity values of the elements in each oxide: Zn: 1.65 (metal) O: 3.44 (nonmetal) K: 0.82 (metal) S: 2.58 (nonmetal) F: 3.98 (nonmetal) Ti: 1.54 (metal)
02

Determine the electronegativity differences for each oxide

Calculate the difference in electronegativity values for each oxide: ZnO: 3.44 - 1.65 = 1.79 K2O: 3.44 - 0.82 = 2.62 SO2: 3.44 - 2.58 = 0.86 OF2: 3.98 - 3.44 = 0.54 TiO2: 3.44 - 1.54 = 1.90
03

Categorize the oxides as ionic or molecular based on electronegativity differences

Determine if each oxide is ionic or molecular based on their electronegativity differences. If the difference is greater than 1.7, it is generally considered ionic. Otherwise, it is molecular: ZnO: 1.79 > 1.7 => ionic K2O: 2.62 > 1.7 => ionic SO2: 0.86 < 1.7 => molecular OF2: 0.54 < 1.7 => molecular TiO2: 1.90 > 1.7 => ionic So, the given oxides can be classified as follows: ZnO: Ionic K2O: Ionic SO2: Molecular OF2: Molecular TiO2: Ionic

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Most popular questions from this chapter

(a) Does metallic character increase, decrease, or remain unchanged as one goes from left to right across a row of the periodic table? (b) Does metallic character increase, decrease, or remain unchanged as one goes down a column of the periodic table? (c) Are the periodic trends in (a) and (b) the same as or different from those for first ionization energy?

Give examples of transition metal ions with +3 charge that have an electron configuration of \(n d^{5}(n=3,4,5 \ldots)\).

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