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Chapter 22: Problem 60

Give an account of the various kinds of oxides that exist and illustrate each type by two examples.

Short Answer

Expert verified
There are four types of oxides: basic, acidic, amphoteric, and neutral. Examples of basic oxides are Sodium Oxide and Calcium Oxide, acidic oxides examples include Carbon Dioxide and Sulfur Dioxide, Aluminum Oxide and Zinc Oxide are examples of amphoteric oxides, while examples of neutral oxides are Nitrous Oxide and Carbon Monoxide.

Step by step solution

01

Identify Basic Oxides

Basic oxides, also known as alkaline oxides, are oxides that react with water to form a base or with an acid to form a salt. Examples of basic oxides include Sodium Oxide (\(Na_2O\)) and Calcium Oxide (\(CaO\)).
02

Identify Acidic Oxides

Acidic oxides, at times called acid anhydrides, are oxides that react with water to form an acid or with a base to form a salt. Examples of acidic oxides are Carbon Dioxide (\(CO_2\)) and Sulfur Dioxide (\(SO_2\)).
03

Identify Amphoteric Oxides

Amphoteric oxides can behave as both acidic and basic oxides, reacting either with an acid to form a salt or with a base to also form a salt. Examples are Aluminum Oxide (\(Al_2O_3\)) and Zinc Oxide (\(ZnO\)).
04

Identify Neutral Oxides

Neutral oxides show neither basic nor acidic properties and hence do not form salts when reacted with acids or bases. Examples include Nitrous Oxide (\(N_2O\)) and Carbon Monoxide (\(CO\)).

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Most popular questions from this chapter

Give an example of hydrogen as (a) an oxidizing agent and (b) a reducing agent.

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 \(\left.\mathrm{Ca}(\mathrm{OH})_{2} .\right]\)

Explain why (a) \(\mathrm{NH}_{3}\) is more basic than \(\mathrm{PH}_{3}\) (b) \(\mathrm{NH}_{3}\) has a higher boiling point than \(\mathrm{PH}_{3}\), (c) \(\mathrm{PCl}_{5}\) exists but \(\mathrm{NCl}_{5}\) does not, \((\mathrm{d}) \mathrm{N}_{2}\) is more inert than \(\mathrm{P}_{4}\).

Without referring to Figure \(22.1,\) state whether each of the following elements are metals, metalloids, or nonmetals: (a) \(\mathrm{Cs},(\mathrm{b}) \mathrm{Ge},(\mathrm{c}) \mathrm{I},\) (d) \(\mathrm{Kr},\) (e) \(\mathrm{W}\), (f) \(\mathrm{Ga},(\mathrm{g}) \mathrm{Te},(\mathrm{h}) \mathrm{Bi}\)

Hydrogen peroxide is unstable and decomposes readily: $$2 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)$$ This reaction is accelerated by light, heat, or a catalyst. (a) Explain why hydrogen peroxide sold in drugstores comes in dark bottles. (b) The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from \(15.0 \mathrm{~g}\) of a 7.50 percent hydrogen peroxide solution?
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