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Chapter 8: Problem 73

State whether each of these properties of the representative elements generally increases or decreases (a) from left to right across a period and (b) from top to bottom in a group: metallic character, atomic size, ionization energy, acidity of oxides.

Short Answer

Expert verified
In general, from left to right across a period: metallic character and atomic size decrease, while ionization energy and acidity of oxides increase. From top to bottom in a group: metallic character, atomic size increase, while ionization energy decreases. The acidity of oxides usually decreases, but it depends on the specific group.

Step by step solution

01

Analyze the Trend from Left to Right Across a Period

For metallic character, it decreases from left to right across a period. Atomic size also decreases from left to right across a period, as electrons added to the same energy level experience an increased positive charge from the nucleus. Ionization energy, the energy necessary to remove an electron, increases across a period because as atomic radii decrease, the electrons get closer to the nucleus and are therefore held more tightly. Acidity of oxides increases across a period, where elements tend to form more acidic oxides.
02

Analyze the Trend from Top to Bottom in a Group

For metallic character, it generally increases from top to bottom in a group due to the increase in energy levels, which makes the outer electrons less attracted to the nucleus, making it easier for the elements to lose electrons. Atomic size also increases down a group because additional energy levels are being added. Ionization energy decreases down a group because as atomic size increases, the outer electrons are less tightly held by the nucleus. The trend of acidity of oxides is more complex and depends upon the specific group of elements, but in general, the acidity decreases down a group, where elements tend to form more basic oxides.

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Most popular questions from this chapter

Use the alkali metals and alkaline earth metals as examples to show how we can predict the chemical properties of elements simply from their electron configurations.

Which oxide is more basic, \(\mathrm{MgO}\) or \(\mathrm{BaO}\) ? Why?

How does atomic radius change as we move (a) from left to right across the period and (b) from top to bottom in a group?

Match each of the elements on the right with its description on the left: (a) A greenish-yellow gas \(\quad\) Nitrogen \(\left(\mathrm{N}_{2}\right)\) that reacts with water \(\quad\) Boron (B) (b) A soft metal that reacts Aluminum (Al) with water to produce Fluorine \(\left(\mathrm{F}_{2}\right)\) hydrogen Sodium (Na) (c) A metalloid that is hard and has a high melting point (d) A colorless, odorless gas (e) A more reactive metal than iron, which does not corrode in air

Arrange the following isoelectronic species in order of (a) increasing ionic radius and (b) increasing ionization energy: \(\mathrm{O}^{2-}, \mathrm{F}^{-}, \mathrm{Na}^{+}, \mathrm{Mg}^{2+}\).
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