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Chapter 8: Problem 34

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

Short Answer

Expert verified
(a) The atomic radius generally decreases from left to right across a period, and (b) The atomic radius generally increases from top to bottom down a group.

Step by step solution

01

Analyzing Atomic Radius Across a Period

As you move from left to right across a period, the atomic radius generally decreases. This happens because as you move across a period, the number of protons in the nucleus increases which attracts the electrons in the outer orbitals towards the nucleus and decreases the size of the atomic radius.
02

Analyzing Atomic Radius Down a Group

When you move from top to bottom down a group, the atomic radius generally increases. This is because as you move down a group, new electron shells are added. Each subsequent electron shell is further away from the nucleus proving more shielding effect, thus increasing the size of the atomic radius.
03

Appreciating trends in Atomic Radius

These discussed trends in atomic radius (decreasing from left to right across a period and increasing from top to bottom down a group) arise due to the balance between nuclear charge and electron shielding. Across a period, increase in nuclear charge overshadows electron shielding, curtailing the atomic radius. Down a group, addition of new electron shells enhances shielding effect and dominates over nuclear charge, scaling up the atomic radius.

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Most popular questions from this chapter

Use the second period of the periodic table as an example to show that the size of atoms decreases as we move from left to right. Explain the trend.

Based on knowledge of the electronic configuration of titanium, state which of the following compounds of titanium is unlikely to exist: \(\mathrm{K}_{3} \mathrm{TiF}_{6}, \mathrm{~K}_{2} \mathrm{Ti}_{2} \mathrm{O}_{5}\) \(\mathrm{TiCl}_{3}, \mathrm{~K}_{2} \mathrm{TiO}_{4}, \mathrm{~K}_{2} \mathrm{TiF}_{6}\)

The first four ionization energies of an element are approximately \(579 \mathrm{~kJ} / \mathrm{mol}, 1980 \mathrm{~kJ} / \mathrm{mol}, 2963 \mathrm{~kJ} /\) mol, and \(6180 \mathrm{~kJ} / \mathrm{mol}\). To which periodic group does this element belong?

Write a balanced equation that predicts the reaction of rubidium (Rb) with (a) \(\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{Cl}_{2}(g)\) (c) \(\mathrm{H}_{2}(g)\)

Predict the products of the following oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}, \mathrm{~N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions. Specify whether the oxides are acidic, basic, or amphoteric.
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