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Chapter 7: Problem 64

Arrange the following oxides in order of increasing acidity: \(\mathrm{CO}_{2}, \mathrm{CaO}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{SO}_{3}, \mathrm{SiO}_{2},\) and \(\mathrm{P}_{2} \mathrm{O}_{5}\)

Short Answer

Expert verified
The oxides arranged in order of increasing acidity are: \(\mathrm{CaO} < \mathrm{Al}_{2} \mathrm{O}_{3} < \mathrm{SiO}_2 < \mathrm{CO}_2 < \mathrm{P}_{4} \mathrm{O}_{10} < \mathrm{SO}_3\) (Calcium oxide) \(\mathrm{CaO} < \mathrm{Al}_{2} \mathrm{O}_{3}\) (Aluminum oxide) \(< \mathrm{SiO}_2\) (Silicon dioxide) \(< \mathrm{CO}_2\) (Carbon dioxide) \(< \mathrm{P}_{4} \mathrm{O}_{10}\) (Phosphorus pentoxide) \(< \mathrm{SO}_3\) (Sulfur trioxide).

Step by step solution

01

Classify the Oxides based on Metals and Non-Metals

In the given set of oxides, we need to first identify the metal and non-metal based oxides. Metal oxides are typically basic in nature, whereas non-metal oxides are acidic. \(\mathrm{CO}_{2}\) - Non-metal oxide (Carbon dioxide) \(\mathrm{CaO}\) - Metal oxide (Calcium oxide) \(\mathrm{Al}_{2} \mathrm{O}_{3}\) - Metal oxide (Aluminum oxide) \(\mathrm{SO}_{3}\) - Non-metal oxide (Sulfur trioxide) \(\mathrm{SiO}_{2}\) - Non-metal oxide (Silicon dioxide) \(\mathrm{P}_{4} \mathrm{O}_{10}\) - Non-metal oxide (Phosphorus pentoxide)
02

Determine the Acidic Character of Non-metal Oxides

Non-metal oxides are acidic in nature, and their acidity increases with increasing electronegativity of the non-metal. Hence, we can compare the electronegativity values of non-metals to determine their acidic nature. Here are the electronegativity values of the non-metals in the given oxides: Carbon: 2.55 Sulfur: 2.58 Silicon: 1.90 Phosphorus: 2.19 Based on these electronegativity values, we can deduce the order of increasing acidity for non-metal oxides as: \(\mathrm{SiO}_2 < \mathrm{CO}_2 < \mathrm{P}_{4} \mathrm{O}_{10} < \mathrm{SO}_3\)
03

Determine the Acidic Character of Metal Oxides

Metal oxides are basic in nature, and their basicity decreases with increasing electronegativity of the metal. Some metal oxides, like aluminum oxide, exhibit amphoteric behavior, which means that they can act as both an acid and a base. In this step, we can compare the electronegativity values of the metals to determine their acidic nature. Here are the electronegativity values of the metals in the given oxides: Calcium: 1.00 Aluminum: 1.61 Based on these electronegativity values, we can deduce the order of increasing acidity for metal oxides as: \(\mathrm{CaO} < \mathrm{Al}_{2} \mathrm{O}_{3}\)
04

Combine the order of Acidic Character for Non-metal Oxides and Metal Oxides

With the order of increasing acidity determined in Steps 2 and 3, we can now combine the two orders to form a comprehensive order of increasing acidity for all the given oxides: \(\mathrm{CaO} < \mathrm{Al}_{2} \mathrm{O}_{3} < \mathrm{SiO}_2 < \mathrm{CO}_2 < \mathrm{P}_{4} \mathrm{O}_{10} < \mathrm{SO}_3\) Thus, the oxides arranged in order of increasing acidity are: (Calcium oxide) \(\mathrm{CaO} < \mathrm{Al}_{2} \mathrm{O}_{3}\) (Aluminum oxide) \(< \mathrm{SiO}_2\) (Silicon dioxide) \(< \mathrm{CO}_2\) (Carbon dioxide) \(< \mathrm{P}_{4} \mathrm{O}_{10}\) (Phosphorus pentoxide) \(< \mathrm{SO}_3\) (Sulfur trioxide).

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Most popular questions from this chapter

Write electron configurations for the following ions, and determine which have noble-gas configurations: (a) \(\mathrm{Cr}^{3+}\), (b) \(\mathrm{N}^{3-},(\mathrm{c}) \mathrm{Sc}^{3+},(\mathrm{d}) \mathrm{Cu}^{2+}\) (e) \(\mathrm{Tl}^{+}\), (f) \(\mathrm{Au}^{+}\).

Consider \(\mathrm{S}, \mathrm{Cl}\), and \(\mathrm{K}\) and their most common ions. (a) List the atoms in order of increasing size. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.

(a) Because an exact outer boundary cannot be measured or even calculated for an atom, how are atomic radii determined? (b) What is the difference between a bonding radius and a nonbonding radius? (c) For a given element, which one is larger? (d) If a free atom reacts to become part of a molecule, would you say that the atom gets smaller or larger?

Based on their positions in the periodic table, predict which atom of the following pairs will have the smaller first ionization energy: (a) \(\mathrm{Cl}, \mathrm{Ar} ;\) (b) \(\mathrm{Be}, \mathrm{Ca}\) (c) \(\mathrm{K}\), Co; (d) \(\mathrm{S}, \mathrm{Ge} ;\) (e) Sn. Te.

Explain the following variations in atomic or ionic radii: (a) \(\Gamma>\mathrm{I}>\mathrm{I}^{+},(\mathrm{b}) \mathrm{Ca}^{2+}>\mathrm{Mg}^{2+}>\mathrm{Be}^{2+}\) (c) \(\mathrm{Fe}>\mathrm{Fe}^{2+}>\mathrm{Fe}^{3+}\)
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