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Chapter 8: Problem 46

Explain which of these anions is larger, and why: \(\mathrm{Se}^{2-}\) or \(\mathrm{Te}^{2-}\)

Short Answer

Expert verified
The \( \mathrm{Te}^{2-} \) anion is larger. This is due to the fact that atomic size increases as we move down the periodic table. Tellurium (Te) is located below Selenium (Se) on the table, meaning it has more electron energy levels and therefore, a larger atomic size.

Step by step solution

01

Understanding the Periodic Table

The first thing to remember is that in the Periodic Table, as we move down a group (vertical column), the atomic size or atomic radius increases. This is because each period represents a new energy level in the electron cloud around the nucleus. As such, \( \mathrm{Se}^{2-} \) and \( \mathrm{Te}^{2-} \) are in the same group, with selenium (Se) above tellurium (Te).
02

Analyzing the Atomic Number

Tellurium (Te) has a greater atomic number than Selenium (Se), indicating that there are more protons in the nucleus of Tellurium and also more electrons in its electron cloud. This increased number of energy levels in the electron cloud means that the distance from the nucleus to the outermost energy level of Te will be greater than that of Se.
03

Comparing the size of anions

Considering the above points, we can see that \( \mathrm{Te}^{2-} \) will be larger than \( \mathrm{Se}^{2-} \). Because as we add more energy levels (each additional period on the table), the atomic size increases.

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Most popular questions from this chapter

A neutral atom of a certain element has 17 electrons. Without consulting a periodic table, (a) write the ground-state electron configuration of the element, (b) classify the element, (c) determine whether the atoms of this element are diamagnetic or paramagnetic.

Write ground-state electron configurations for these ions, which play important roles in biochemical processes in our bodies: (a) \(\mathrm{Na}^{+},\) (b) \(\mathrm{Mg}^{2+},\) (c) \(\mathrm{Cl}^{-}\) (d) \(\mathrm{K}^{+},\) (e) \(\mathrm{Ca}^{2+},\) (f) \(\mathrm{Fe}^{2+},(\mathrm{g}) \mathrm{Cu}^{2+},\) (h) \(\mathrm{Zn}^{2+}\)

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

State whether each of the elements listed here is a gas, a liquid, or a solid under atmospheric conditions. Also state whether it exists in the elemental form as atoms, as molecules, or as a three-dimensional network: \(\mathrm{Mg}, \mathrm{Cl}, \mathrm{Si}, \mathrm{Kr}, \mathrm{O}, \mathrm{I}\) \(\mathrm{Hg}, \mathrm{Br}\).

In which of these are the species written in decreasing radius? (a) \(\mathrm{Be}, \mathrm{Mg}, \mathrm{Ba}\) (b) \(\mathrm{N}^{3-}, \mathrm{O}^{2-}, \mathrm{F}^{-}\) (c) \(\mathrm{Tl}^{3+}, \mathrm{Tl}^{2+}, \mathrm{Tl}^{+}\)
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