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Chapter 8: Problem 71

How do the chemical properties of oxides change from left to right across a period? From top to bottom within a particular group?

Short Answer

Expert verified
Oxides change from being basic to acidic as we move from left to right across a period, starting with metallic basic oxides and ending with non-metallic acidic oxides. Within a group from top to bottom, the oxides' properties change less significantly, usually maintaining a similar nature due to the elements having the same number of valence electrons.

Step by step solution

01

Understanding the Periodic Table and Oxides

Chemistry students should already be familiar with the structure of the periodic table. It's divided into periods (which run from left to right) and groups (which run from top to bottom). An oxide is a chemical compound that contains at least one Oxygen atom and one other element. Most elements form oxides.
02

Changes Across a Period (Left to Right)

As you move from left to right across a period, the nature of the oxides changes. On the left side of the periodic table, there are metallic elements that form basic oxides. For example, Sodium (Na), a metal, forms Sodium Oxide (\(Na_2O\)) which is a basic oxide. As we move towards the right, we encounter non-metallic elements that form acidic oxides. For example, Sulphur (S) forms Sulphur Dioxide (\(SO_2\)) which is an acidic oxide. At the center of the table, you have elements that form amphoteric oxides (having both the properties of acidic and basic), like Aluminium Oxide (\(Al_2O_3\)).
03

Changes Within a Group (Top to Bottom)

As you move from top to bottom within a particular group, there is generally very little change in the nature of the oxides. This is because elements within the same group have the same number of valence electrons, resulting in similar chemical properties. The size of the elements, however, does increase down the group, which can sometimes result in differing physical properties.

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Most popular questions from this chapter

Give equations to show that molecular hydrogen can act both as a reducing agent and an oxidizing agent.

Arrange the following in order of increasing first ionization energy: \(\mathrm{F}, \mathrm{K}, \mathrm{P}, \mathrm{Ca},\) and \(\mathrm{Ne} .\)

Element \(\mathrm{M}\) is a shiny and highly reactive metal (melting point \(\left.63^{\circ} \mathrm{C}\right)\), and element \(\mathrm{X}\) is a highly reactive nonmetal (melting point \(-7.2^{\circ} \mathrm{C}\) ). They react to form a compound with the empirical formula MX, a colorless, brittle white solid that melts at \(734^{\circ} \mathrm{C} .\) When dissolved in water or when in the molten state, the substance conducts electricity. When chlorine gas is bubbled through an aqueous solution containing MX, a reddish-brown liquid appears and \(\mathrm{Cl}^{-}\) ions are formed. From these observations, identify \(\mathrm{M}\) and \(\mathrm{X}\). (You may need to consult a handbook of chemistry for the melting-point values.)

Specify which of the following elements you would expect to have the greatest electron affinity and which would have the least: \(\mathrm{He}, \mathrm{K}, \mathrm{Co}, \mathrm{S}, \mathrm{Cl}\)

List the following ions in order of increasing ionic radius: \(\mathrm{N}^{3-}, \mathrm{Na}^{+}, \mathrm{F}^{-}, \mathrm{Mg}^{2+}, \mathrm{O}^{2-}\)
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