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Chapter 22: Problem 41

Predict whether each of the following oxides is acidic, basic, , (d) \(\mathrm{CaO}\) amphoteric, or neutral: (a) \(\mathrm{NO}_{2},\) (b) \(\mathrm{CO}_{2},\) (c) \(\mathrm{Al}_{2} \mathrm{O}_{3}\),

Short Answer

Expert verified
The types of oxides for the given compounds are: (a) \(\mathrm{NO}_{2}\) - Acidic, (b) \(\mathrm{CO}_{2}\) - Acidic, (c) \(\mathrm{Al}_{2} \mathrm{O}_{3}\) - Amphoteric, and (d) \(\mathrm{CaO}\) - Basic.

Step by step solution

01

Understanding the types of oxides

There are four types of oxides: acidic, basic, amphoteric and neutral. Acidic and basic oxides exhibit their respective acid and base behavior when they react with water. Amphoteric oxides can show both acidic and basic behavior. Neutral oxides do not exhibit any acidic or basic character when they react with water. Generally, non-metal oxides are acidic in nature, while metal oxides are basic. However, some metal oxides like Aluminum oxide are amphoteric, and some non-metal oxides are neutral.
02

Predicting the type of oxide for \(\mathrm{NO}_{2}\)

Nitrogen dioxide (\(\mathrm{NO}_{2}\)) is a non-metal oxide. Based on the general rule, non-metal oxides are acidic in nature. Thus, we predict that \(\mathrm{NO}_{2}\) is an acidic oxide.
03

Predicting the type of oxide for \(\mathrm{CO}_{2}\)

Carbon dioxide (\(\mathrm{CO}_{2}\)) is another non-metal oxide. Following the general rule, we predict that \(\mathrm{CO}_{2}\) is an acidic oxide.
04

Predicting the type of oxide for \(\mathrm{Al}_{2} \mathrm{O}_{3}\)

Aluminum oxide (\(\mathrm{Al}_{2} \mathrm{O}_{3}\)) is a metal oxide. However, aluminum is not just any metal; it is considered amphoteric. This means that its oxide can exhibit both acidic and basic properties. Therefore, we predict that \(\mathrm{Al}_{2} \mathrm{O}_{3}\) is an amphoteric oxide.
05

Predicting the type of oxide for \(\mathrm{CaO}\)

Calcium oxide (\(\mathrm{CaO}\)) is a metal oxide. According to the general rule, we predict that \(\mathrm{CaO}\) is a basic oxide. In conclusion, the types of oxides for the given compounds are: (a) \(\mathrm{NO}_{2}\) - Acidic (b) \(\mathrm{CO}_{2}\) - Acidic (c) \(\mathrm{Al}_{2} \mathrm{O}_{3}\) - Amphoteric (d) \(\mathrm{CaO}\) - Basic

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Most popular questions from this chapter

Explain the following observations: (a) \(\mathrm{HNO}_{3}\) is a stronger oxidizing agent than \(\mathrm{H}_{3} \mathrm{PO}_{4}\). (b) Silicon can form an ion with six fluorine atoms, \(\mathrm{SiF}_{6}^{2-}\), whereas carbon is able to bond to a maximum of four, \(\mathrm{CF}_{4}\). (c) There are three compounds formed by carbon and hydrogen that contain two carbon atoms each \(\left(\mathrm{C}_{2} \mathrm{H}_{2}, \mathrm{C}_{2} \mathrm{H}_{4},\right.\) and \(\left.\mathrm{C}_{2} \mathrm{H}_{6}\right),\) whereas silicon forms only one analogous compound \(\left(\mathrm{Si}_{2} \mathrm{H}_{6}\right)\).

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q),(\mathbf{b})\) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+},(\mathrm{c})\) aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) to mercury metal. Write balanced equations for these reactions.

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) calcium hypobromite, (b) bromic acid, (c) xenon trioxide, (d) perchlorate ion, (e) iodous acid, (f) iodine pentafluoride.

A friend tells you that the "neon" in neon signs is a compound of neon and aluminum. Can your friend be correct? Explain.

Explain the following observations: (a) For a given oxidation state, the acid strength of the oxyacid in aqueous solution decreases in the order chlorine \(>\) bromine \(>\) iodine. (b) Hydrofluoric acid cannot be stored in glass bottles. (c) HI cannot be prepared by treating NaI with sulfuric acid. (d) The interhalogen \(\mathrm{ICl}_{3}\) is known, but \(\mathrm{BrCl}_{3}\) is not.
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