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Chapter 7: Problem 82

As we move across a period of the periodic table, why do the sizes of the transition elements change more gradually than those of the representative elements?

Short Answer

Expert verified
The more gradual change in atomic size for transition elements across a period compared to representative elements is mainly due to greater electron shielding experienced by transition elements. This occurs because transition elements have their outer electrons in more diffuse d orbitals, which partially neutralize the increased nuclear charge, allowing for a more gradual change in atomic size as we move across a period.

Step by step solution

01

Understanding Atomic Size

Atomic size refers to the distance between the nucleus and the outermost electrons of an atom. As we move across a period in the periodic table, the atomic size typically decreases. This decrease is due to an increase in the nuclear charge (number of protons), which pulls the electrons closer to the nucleus.
02

Differences between Representative and Transition Elements

Representative elements, also called main group elements, belong to groups 1, 2, and 13 to 18 of the periodic table. In contrast, transition elements are found in groups 3 to 12. The key difference between these two types of elements lies in their electron configurations. Representative elements gain or lose electrons to achieve a stable, full outer electron shell, while transition elements tend to fill their inner d subshells.
03

Electron Shielding in Transition Elements

As we move across a period, the electrons occupy the same energy level but in different orbitals for transition elements. This means that these electrons are in a d subshell apart from the outermost s orbital, while the representative elements' outermost electrons occupy the s or p orbitals in the same energy level. Since the d subshell has more diffused and less tightly held electrons than the s and p orbitals, transition elements experience greater electron shielding. This shielding effect partially neutralizes the increase in nuclear charge, as it keeps the outer electrons from being pulled in as tightly.
04

Gradual Change in Atomic Size for Transition Elements

Due to the greater electron shielding experienced by transition elements, their atomic size does not shrink as rapidly as representative elements as we move across a period. The more diffuse d orbitals mitigate the increased nuclear charge's effect, which causes a more gradual change in atomic size among transition elements. In summary, the sizes of transition elements change more gradually than those of the representative elements across a period because of the greater electron shielding experienced by transition elements due to their d subshell electron configurations.

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Most popular questions from this chapter

(a) Use orbital diagrams to illustrate what happens when an oxygen atom gains two electrons. (b) Why does \(\mathrm{O}^{3-}\) not exist?

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Ozone decomposes to dioxygen. (b) Xenon reacts with fluorine. (Write three different equations.) (c) Sulfur reacts with hydrogen gas. (d) Fluorine reacts with water.

(a) One of the alkali metals reacts with oxygen to form a solid white substance. When this substance is dissolved in water, the solution gives a positive test for hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}.\) When the solution is tested in a burner flame, a lilac-purple flame is produced. What is the likely identity of the metal? (b) Write a balanced chemical equation for the reaction of the white substance with water.

Which quantity must be determined experimentally in order to determine the bonding atomic radius of an atom? (a) The distance from the nucleus where the probability of finding an electron goes to zero. (b) The distance between the nuclei of two atoms that are bonded together. (c) The effective nuclear charge of an atom.

The electron affinities, in \(\mathrm{kJ} / \mathrm{mol},\) for the group 1 \(\mathrm{B}\) and group 2 \(\mathrm{B}\) metals are as follows: (a) Why are the electron affinities of the group 2 \(\mathrm{B}\) elements greater than zero? (b) Why do the electron affinities of the group 1 \(\mathrm{B}\) elements become more negative as we move down the group? [Hint: Examine the trends in the electron affinities of other groups as we proceed down the periodic table.]
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