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Chapter 22: Problem 92

(a) Which of the following compounds has the greatest ionic character: \(\mathrm{PCl}_{5}, \mathrm{SiCl}_{4}, \mathrm{CCl}_{4}, \mathrm{BCl}_{3} ?\) (b) Which of the following ions has the smallest ionic radius: \(\mathrm{F}^{-}, \mathrm{C}^{4-}, \mathrm{N}^{3-}, \mathrm{O}^{2-} ?(\mathrm{c})\) Which of the following atoms has the highest ionization energy: \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I} ?(\mathrm{~d})\) Which of the following oxides is most acidic: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{SiO}_{2}, \mathrm{CO}_{2} ?\)

Short Answer

Expert verified
(a) \(\mathrm{BCl}_{3}\) (b) \(\mathrm{F}^{-}\) (c) \(\mathrm{F}\) (d) \(\mathrm{SiO}_{2}\)

Step by step solution

01

Determine the compound with the greatest ionic character

Ionic character is influenced by the difference in electronegativity between ions in a molecule. In this case, \(\mathrm{BCl}_{3}\) has the highest ionic character, since Boron has the lowest electronegativity and therefore the biggest difference compared to Chlorine.
02

Identify the ion with the smallest ionic radius

Ionic radius tends to decrease across a period as effective nuclear charge increases. Also, it increases down a group due to the addition of energy levels. Among the given, \(\mathrm{F}^{-}\) has the smallest ionic radius.
03

Find the atom with the highest ionization energy

Ionization energy is the energy required to remove an electron from an atom. It tends to increase across a period and decrease down a group. Here, Fluorine (\(\mathrm{F}\)) has the highest ionization energy.
04

Determine the most acidic oxide

The acidity of an oxide depends on the electronegativity and oxidation states. In general, non-metal oxides are acidic, and among them, \(\mathrm{SiO}_{2}\) is more acidic compared to \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CO}_{2} \)

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Most popular questions from this chapter

Solid \(\mathrm{PCl}_{5}\) exists as \(\left[\mathrm{PCl}_{4}^{+}\right]\left[\mathrm{PCl}_{6}^{-}\right] .\) Draw Lewis structures for these ions. Describe the hybridization state of the \(\mathrm{P}\) atoms.

What are interstitial hydrides?

Unlike \(\mathrm{CaCO}_{3}, \mathrm{Na}_{2} \mathrm{CO}_{3}\) does not readily yield \(\mathrm{CO}_{2}\) when heated. On the other hand, \(\mathrm{NaHCO}_{3}\) undergoes thermal decomposition to produce \(\mathrm{CO}_{2}\) and \(\mathrm{Na}_{2} \mathrm{CO}_{3}\). (a) Write a balanced equation for the reaction. (b) How would you test for the \(\mathrm{CO}_{2}\) evolved? [Hint: Treat the gas with limewater, an aqueous solution of \(\left.\mathrm{Ca}(\mathrm{OH})_{2} .\right]\)

Give an example of a carbide and a cyanide.

Explain why two \(\mathrm{N}\) atoms can form a double bond or a triple bond, whereas two \(\mathrm{P}\) atoms normally can form only a single bond.
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